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CHM 123 Final Exam Study Info

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percent ionization equation

% ionization = (acid ionized/ initial acid) *100

what is the average rate for the following equation Br2(aq) + HCOOH(aq) --> 2Br-(aq) + 2H+ + CO2(g)

((Δ[Br2])/Δt) = ([Br2]final - [Br2]initial)/tfinal - t initial

atomic number 34 (Se)

Selenium

Chemical analysis of a gaseous compound showed that it contained 33.0 percent silicon (Si) and 67.0 percent fluorine (F) by mass. At 35° C, 0.210 L of the compound exerted a pressure of 1.70 atm. If the mass of 0.210 L of the compound was 2.38 g, calculate the molecular formula of the compound

Si2F6

atomic number 14 (Si)

Silicon

atomic number 50 (Sn)

Tin

atomic number 22 (Ti)

Titanium

atomic number 23 (V)

Vanadium

Classify the following compounds as weak acids (W) or strong acids (S): benzoic acid nitric acid acetic acid

WSW

w system equation

Wsys = -PΔV

atomic number 30 (Zn)

Zinc

for a zero order reaction, a plot of ______ versus ______ is linear

[A] t

0 order half life

[A]o/2k

0 order integrated rate law

[A]t = -kt + [A]0

give the relationship between [H+] and [OH-] if a solution is basic

[H+] < [OH-]

a 1.000L flask is filled with 1.00 mol of H2(g) and 2.00 mol of I2(g) at 488C. Given a K = 50.5 @ 448C, what are the equilibrium concentrations of H2, I2, and HI?

[H2] = .065M [I2] = 1.065 M [HI] = 1.87 M

Which of the following solutions is acidic? [H3O+] = 1.0 x 10-7 M [H3O+] = 1.5 x 10-10 M [H3O+] < 1.0 x 10-7 M [H3O+] > 7.0 x 10-7 M [H3O+] = 1.0 x 10-14 M

[H3O+] > 7.0 x 10-7 M

In acidic solution, [H3O+] _________ [OH-]

[H3O+] > [OH-]

The standard Gibbs free energy of formation of ________ is zero. (a) Mn (s) (b) I2 (s) (c) Cu (s)

abc

acid dissociation constant

activation energy

A Br∅nsted-Lowry acid is defined as a substance that ________.

acts as a proton donor

soluble compounds key

alkali metals, ammonium ion, nitrates, acetates, bicarbonates, chlorates, perchlorates, halides, sulfates

isotope

an element with a different # of neutrons

strong electrolyte

any compound whose dilute aqueous solutions conduct electricity well; this is due to the presence of all or almost all of the dissolved compound in the form of ions

Consider the following reaction at equilibrium: 2NH3 (g) N2 (g) + 3H2 (g) Le Châtelier's principle predicts that the moles H2 of in the reaction container will increase with some removal of from the reaction vessel (V and T constant) B) a decrease in the total pressure (T constant) C) addition of some to the reaction vessel (V and T constant) D) a decrease in the total volume of the reaction vessel (T constant) E) an increase in total pressure by the addition of helium gas (V and T constant)

Which reaction produces an increase in the entropy of the system? A) Ag+ (aq) + Cl- (aq) → AgCl (s) B) CO2 (s) → CO2 (g) C) H2 (g) + Cl2 (g) → 2 HCl (g) D) N2 (g) + 3 H2 (g) → 2 NH3 (g) E) H2O (l) → H2O (s)

The equilibrium constant for the gas phase reaction N2 (g) + 3H2 (g) >< 2NH3 (g) is Keq = 4.34 × 10-3 at 300 °C. At equilibrium, ________. A) products predominate B) reactants predominate C) roughly equal amounts of products and reactants are present D) only products are present E) only reactants are present

b. reactants predominate

constant volume

bomb calorimeter

The compound HPO42− is ____ bronsted

both a Bronsted acid and base.

The compound HPO42− is

both a bronsted acid and base

the passage of electricity through an electrolyte solution is caused by the movement of:

both cations and anions

∆H

change in enthalpy

A + B -> C

combination reaction

what type of reaction is this CxHy + O2 --> CO2 + H2O

combustion

soluble exceptions

compounds containing alkali metal ions and the ammonium ion compounds containing alkali metal ions and the Ba2+ ion

reactions between acids and bases always yield their...

conjugate bases and acids

based on the solubility rules, which of the following should be soluble in water? A) Ag3PO4 B) Ca3(PO4)2 C) Mg3(PO4)2 D) (NH4)3PO4 E) AlPO4

deca

identify the redox reaction Fe + H2SO4 → FeSO4 + H2

displacement

Which of the following is consistent with a reaction at equilibrium? a. ΔG < 0, Q = K b. ΔG > 0, Q = K c. ΔG° = 0, Q < K d. ΔG° = 0, Q > K e. ΔG = 0, Q = K

rate law

expresses the relationship of the rate of a reaction to the rate constant and the concentrations of the reactants raised to some powers

The quantity of energy gained by a system equals the quantity of energy gained by its surroundings.

false

True or False: NH4NO3 is a weak electrolyte

false

true or false a mole of NaNO3 contains a mole of oxygen formula weight

false

true or false in pure water, molecules can only act as bases or only act as acids

false in pure water, a few molecules act as bases and a few act as acids

gases and liquids tend to react _______ than solids

faster

the equilibrium constant for the reaction 2NO(g) + Br2(g) >< 2NOBr(g) is k = 2.0x10^-2 at certain temps 1. at this temp does the equilibrium favor NO and Br2, or NOBr?

favors 2NO(g) + Br2(g)

hepta

hydroiodic acid

least

hypo root ite

How to tell if it's a base

if it gains electrons after the reaction then it is a base

How to tell if it's an acid

if it loses electrons after the reaction then it is an acid

An exothermic reaction causes the surroundings to

increase in temperature

as temp increases, rate ______

increases

internal energy

arrhenius equation

k=Ae^(-Ea/RT)

arrhenius equation

k=Ae^(-Ea/RT) ln(k2/k1)=Ea/R(1/T1-1/T2)

The decomposition of [A] in solution at 55 °C proceeds via first order: A (aq) → B (aq) What is the rate law for the reaction?

k[A]

[A](M) [B](M) initial rate 0.451 .885 1.13 0.451 1.77 1.13 1.35 .855 10.17 the rate law for A + B --> C is

k[A]^2

the collisions model is based on the _________ theory

kinetic molecular

acidic ph

less than 7

first order integrated rate law

ln[A]t=-kt+ln[A]0

activation energy can be determined graphically by organizing the equation:

lnk = -(Ea/RT) + lnA or ln(k1/k2) = Ea/R (1/T2 - 1/T1)

Deviations from the ideal gas law are greater at

low temperatures and high pressures

rate units

m/s

amu

mass of element

entropy

measure of disorder (s)

what kind of reaction is this Mg(NO3)2(aq) + 2 NaOH(aq) → Mg(OH)2(s) + 2 NaNO3(aq)

metathesis

molar heat capacity

molarity =

moles/liters

mono

if Q < K

more solid can dissolve, so no precipitate forms

what kind of reaction 2 KOH + H2SO4 (aq)→ K2SO4 + 2 H2O (l)

neutralization

what type of reaction is this HX(aq) + YOH(aq) -> H2O(l) + YX

neutralization

HNO3

nitric acid

isolated system

no exchange of energy or matter

If Ksp > Q

no precipitate will form

loss of electrons

oxidation

What is the pH of a 0.40 M ammonia solution? kb = 1.8 x 10^-5

pH = 11.43

Determine the pH of a 0.065 M benzoic acid (C6H5COOH) solution.

pH = 2.70

Which solution below has the highest concentration of hydronium ions? A) pH = 3.0 B) pH = 10 C) pH = 7 D) pH = 6.4 E) pH = 11.2

pH = 3.0

What is the pH of a solution in which [H+]=5.8×10^−7 M? What is the pOH of this solution?

pH = 6.24 pOH = 7.76

In the reaction: 2H2O(l) >< H3O+(aq) + OH- (aq) the conjugate acid-base pairs are

pair 1: H2O and OH- pair 2: H2O and H3O+

penta

the most

per root ate

HClO4

perchloric acid

what kind of reaction PbCl2 + Na2S (aq)→ PbS (s)+ 2 NaCl (aq)

precipitation

the larger Ka the more it favors

products

The equilibrium constant for the gas phase reaction 2SO2 (g) + O2 (g) ⇌ 2SO3 (g) is Keq = 2.80 × 10^2 at 999 K. At equilibrium, ________.

products predominate

specific heat capacity equation

q=m∆T

qsol calorimetetry equation

qcal = Ccal x ∆T

we can calculate ∆H for the reaction with this equation

qsoln = Cs x msoln x ∆T

qsolution and q reaction relationship

qsolution = -qreaction

combustion reactions

rapid reactions that produce a flame

rate of A -> B

rate = - Δ[A]/ Δt rate = Δ[B]/ Δt

what kind of reaction PbS(s) + 4 H2O2(aq) → PbSO4(aq) + 4H2O(l)

redox

identify the reducing and oxidizing agents and determine the species that is oxidized and the species that is reduced. H2 + CH2=CH2--> CH3CH3

reducing agent: H2 Oxidizing agent: CH2=CH2 species being reduced: CH2=CH2 species being oxidized: H2

gain of electrons

reduction

root ate

in every acid-base reaction, equilibrium favors transfer of the proton from the ______________ to the _____________ to form the ____________ acid and the ______________ base

stronger stronger weaker weaker

H2SO4

sulfuric acid

first order half life

t1/2 = 0.693/k

2nd order half life

t1/2 = 1/k[A]o

what does the "p" in pH tell you

tells you to take the -log10 of a quantity

gases have an average ________, but each individual molecule has its own _______

temp energy

conjugate acid

the particle formed when a base gains a hydrogen ion

conjugate base

the particle that remains when an acid has donated a hydrogen ion

equivalence point

the point at which the two solutions used in a titration are present in chemically equivalent amounts

system

the portion of the universe that is singled out for study

autoionization

the process by which water acts as an acid and a base with itself

limiting reactants

the reactant present in the smallest stoich amount

hess's law

the ∆Hrxn is the sum of the individual steps

because ionic compounds are strong electrolytes

they dissociate completely to the extent that they dissolve

tri

True or False Ethanol (CH3CH2OH) is a nonelectrolyte.

true

volume

the magnitude of Kw indicates that

water autonizes only to a very small extent

because [H3O+][OH-] = Kw = 1.0x10^-14

we can take the -log of the equation which results in pH + POH = 14

CH3COOh is a ______ electrolyte

weak

what type of electrolyte is -><-

weak

Identify the following compounds as a weak or strong acid or base: H3PO4

weak acid

weak acid (hydroflouric acid)

HNO2

weak acid (nitrous acid)

Identify the following compounds as a weak or strong acid or base: NH3

weak base

ammonia is a

weak base

Identify each of the following substances as a strong electrolyte, weak electrolyte, or nonelectrolyte: (d) CH3COOH

weak electrolyte

the stronger the acid, the ________ the conjugate base

weaker

work

work being performed by surroundings on system

-w

work is being performed by system on the surroundings

Which energy difference in the energy profile below corresponds to the activation energy for the forward reaction?

x (activation energy in the forward direction)

will a ppt form? Q --> K. What is [Ag] remaining 250ml 0.33 M Na2CrO4 250ml 0.12 M AgNO3 Ksp = AgCr2O4 = 1.1 x 10^-12 what is the concentration of the silver ion remaining

yes [Ag] = 2.9 x 10^-6

will a precipitate form (ppt) when 300 mL of 5.0 x 10^-5 M AgNO3 are added to 200mL of 2.5 x 10^-7M NaBr? Answer yes or no, and identify the precipitate if there is one Ksp = 7.7 x 10^-13

yes AgBr

Will a precipitate (ppt) form when 20.0 mL of 1.1 × 10-3 M Ba(NO3)2 are added to 80.0 mL of 8.4 × 10-4 M Na2CO3? The solubility product constant for the solid is 1.17 x 10^-10

yes the ppt is BaCO3

the entropy of a pure crystalline substance at absolute zero is

zero

The graphs below all refer to the same reaction. What is the order of this reaction?

zero order

equilibrium equation

ΔG = -RTlnK k=e^-ΔG/RT

relationship between the equilibrium state, k, and free energy (G)

ΔG = ΔG + RT lnQ

how is spontaneity measured

ΔG = ΔH - TΔS

reversible

ΔSuni = ΔSsys + ΔSsurr = 0

irreversible

ΔSuni = ΔSsys + ΔSsurr > 0

which one of the following is always positive when a spontaneous process occurs

ΔSuniverse

ΔU equation

ΔU = q + w

For the reaction A + 3B → 2C, the rate of disappearance of B given by (Δ[B]/Δt) may also be expressed as

Δ[B]/Δt = 3 Δ[A]/Δt.

rate of irreversible (spontaneous reaction) A(aq) + B(aq) --> C(g)

Δ[C]/Δt = k[A]^1[B]^1

enthalpy of a state function equation

∆Hrxn = Σn∆Hf products - Σm∆Hf reactants

Which one of the following is a Br∅nsted-Lowry base? A) (CH3)3N B) CH3COOH C) HF D) HNO2 E) none of the above

(CH3)3N

van der waals equation

(P+n^2a/V^2)(V-nb)=nRT

write the equilibrium constant expression 2NO >< N2 + O2

([N2][O2]) [NO]^2

methanol (CH3OH) is used as a fuel in race cars calculate the heat produced by combustion per liter of methanol (methanol has a density of .791 g/ml) ΔH = -638.5 kJ/mol CH3OH(l) + 3/2O2(g) ---> CO2(g) + 2H2O(l)

-1.58 x 10^4 kJ/L

Under constant-pressure conditions a sample of hydrogen gas initially at 71.00°C and 9.60 L is cooled until its final volume is 2.30 L. What is its final temperature?

-190.7 C

a 1.8g sample of solid phenol (C6H5OH (s)) was burned in a bomb calorimeter, which has a total heat capacity of 11.66kJ/C. The temp of the colorimeter plus its contents increased from 21.36C to 26.37C. what is the change in enthalpy per mole of phenol

-3057 kJ/mol

-32.45 kJ/g

You are given the following data: H2(g) → 2H(g) ΔHo= 436.4 kJ/mol Br2(g) → 2Br(g) ΔHo= 192.5 kJ/mol H2(g) + Br2(g) → 2HBr(g) ΔHo= −72.4 kJ/mol Calculate ΔHo for the reaction H(g) + Br(g) → HBr(g)

-350.65 kJ/mol

Calcium oxide (CaO) is used to remove sulfur dioxide generated by coal-burning power stations: 2CaO(s) + 2SO2(g) +O2(g) → 2CaSO4(s) Calculate the enthalpy change for this if 6.70 × 105 g of SO2 are removed by this process every day.

-5.24 x 10^6 kJ

When 1.933 g of naphthalene (C10H8) is burned in a constant-volume bomb calorimeter at 298 K, 77.70 kJ of heat is evolved. Calculate ΔU and w for the reaction on a molar basis. ΔU =

-5153 kJ/mol 0 kJ/mol

The standard enthalpies of formation of ions in aqueous solutions are obtained by arbitrarily assigning a value of zero to H ions; that is, ΔHof[H+(aq)] = 0. a) for the following reaction HCl(g) H+(aq) + Cl−(aq) ΔHorxn = -74.9 kJ/mol b)Given that ΔHof for OH− ions is −229.6 kJ/mol, calculate the enthalpy of neutralization when 1 mole of a strong monoprotic acid (such as HCl) is titrated by 1 mole of a strong base (such as KOH) at 25°C.

-56.2 kJ/mol

when 0.560g of Na(s) reacts with excess F2(g) to form NaF(s), 13.8 kJ of heat is evolved at standard state conditions. What is the standard enthalpy of formation (ΔHf) of NaF(s)?

-570 kJ/mol

Calculate the heat (in kJ) associated with 311 g of white phosphorus burning in air according to the equation P4(s) + 5O2(g) → P4O10(s) ΔH = −3013 kJ / mol

-7564 kJ

consider the following reactions: 2Mg(s) + O2 (g) --> 2MgO(s) ∆H = -1204 calculate the amount of heat transferred when 3.57g of Mg(s) react at constant pressure.

-88.4 kJ

The combustion of how many moles of ethane (C2H6) would be required to heat 951 g of water from 25.0°C to 83.0°C? (Assume liquid water is formed during the combustion.)

.148 mol ethane

The combustion of how many moles of ethane (C2H6) would be required to heat 797 g of water from 25.0°C to 98.0° C? (Assume liquid water is formed during the combustion.)

.156 mol ethane

What is the molarity of an HCl solution if 27.3 mL of it neutralizes 134.5 mL of 0.0165 M Ba(OH)2?

.163 M HCl

The formula for rust can be represented by Fe2O3. How many moles of Fe are present in 28.6 g of the compound?

0.358 mol Fe

A solution of 116 mL of 0.180 M KOH is mixed with a solution of 260 mL of 0.210 M NiSO4 . 1. Write the balanced chemical equation for the reaction that occurs. 2. What precipitate forms? 3. What is the limiting reactant? 4. What is the concentration of Ni2+ that remains in solution? 5. How many grams of this precipitate form?

1. 2KOH + NiSO4 -> K2SO4 + NiOH2 2. NiOH2 3. KOH 4. .117 M Ni 5..968 g Ni(OH)2

A 0.10 M aqueous solution of the weak base B at 25.0 °C has a pH of 8.00. The value of Kb for B is ________.

1.0 x 10^-11

A 0.15 M solution of a weak acid has pH of 5.87. Calculate the Ka of this acid.

1.2 x 10^-11

A solution of NaF is added dropwise to a solution that is 0.0122 M in Ba^2+. When the concentration of F- exceeds ________ M, BaF2 will precipitate. Neglect volume changes. For BaF2, Ksp = 1.7x10^-6.

1.2 x 10^-2

how many sodium atoms are there in 6.0g of Na3N

1.349E23 atoms

How many grams of KHP are needed to neutralize 73.48 ml of a 0.1055 M NaOH solution?(molar mass of KHP = 204.2 g/mol)

1.583

How many grams of KHP are needed to neutralize 73.48 mL of a 0.1055 M NaOH solution?(molar mass of KHP = 204.2 g/mol)

1.583 g

Calculate the molarity of each of the following solutions: 7.85 g of sodium chloride (NaCl) in 84.0 mL of solution

1.599

the Ksp for CaF2 is 3.9 x 10^-11 @ 25C what is the molarity solubility (g/L) of CaF2(s)?

1.6 x 10^-2 g/L

The solubility of lead (II) chloride (PbCl2) is 1.6x10-2. What is the Ksp of PbCl2?

1.6 x 10^-5

Calculate the pH of a 0.26 M methylamine solution

12.03

Determine the pH of a 0.35 M aqueous solution of CH3NH2 (methylamine). The Kb of methylamine is 4.4 x 10^-4

12.09

Calculate the pH of a 1.8 × 10^−2 M Ba(OH)2 solution.

12.56

Calculate the mass of KI in grams required to prepare 5.00 × 102 mL of a 2.3 M solution.

190.9

polyprotic acid

2 or more protons to donate or accept several Ka to worry about

What is the pH of a 0.122 M monoprotic acid whose Ka is 5.7 × 10^−4?

2.09

Calculate the number of grams of Al in 411 g of Al2O3

217 grams

The reaction between aluminum and iron(III) oxide can generate temperatures approaching 3000°C and is used in welding metals: 2Al + Fe2O3 → Al2O3 +2Fe In one process, 115 g of Al are reacted with 601 g of Fe2O3. Calculate the mass (in grams) of Al2O3 formed, and determine the amount of excess reagent left at the end of the reaction. mass of Al2O3 formed:

217 grams

A city's water supply is contaminated with a toxin at a concentration of 0.63 mg/L. For the water to be safe for drinking, the concentration of this toxin must be below 1.5 x 10-3 mg/L. Fortunately, this toxin decomposes to a safe mixture of products by first-order kinetics with a rate constant of 0.27 day-1 . How long will it take for the water to be safe to drink?

22 days

how many grams of KO2 are needed to form 8.0g of O2

24 g KO2

when a 4.25g sample of solid ammonium nitrate dissolves in 60.0g of water in a coffee-cup calorimeter, the temp drops form 22.0C to 16.9C. calculate ∆H (in kJ/mol NH4NO3) for the solution process NH4NO3(s) ---> NH4(aq) + NO3(aq) assume the specific heat of the solution is the same as that of pure water (4.184 J/gC)

26 kJ/mol

balance the following equation C + O2 --> CO

2C + O2 --> 2CO

Butane is reacted with oxygen gas to form carbon dioxide and water. Write the balanced reaction (omit state symbols (s), (l), (g), (aq), etc.). C4H10 + O2 ---> CO2 + H2O

2C4H10 + 13O2 → 8CO2 + 10H2O

Write the balanced net ionic equation for the following reaction? Identify the spectator ions? Cr2 (SO4 )3 (aq) + (NH4 )2CO3 (aq) →

2Cr^3+(aq) + 3CO3^2-(aq) --> Cr2(CO3)3(s)

Balance the following equation K + H2O --> KOH + H2

2K + 2H2O --> 2KOH + H2

balance the chemical equation K + H2O -> H2 + KOH

2K + 2H2O -> H2 + 2KOH

which ions remain in solution, unreacted, after each of the following pairs of solutions is mixed ammonium phosphate and calcium chloride

2PO4^3- + 3Ca^2+ --> Ca3(PO4)2

predict what heppens when a potassium phosphate (K3PO4) solution is mixed with a calcium nitrate [Ca(NO3)2] solution. write a net ionic equation for the reaction

2PO4^3- + 3Ca^2+ -> Ca3(PO4)2

assign the correct oxidation number to each species in the redox reaction below. 2PbO2(s) + 2H+(aq) + 2HSO4-(aq) -><- 2PbSO4(s) + 2H2O(l) + O2(g)

2Pb: +4 4O: -2 2H+: +1 2H: +1 2S: +6 8O: -2 2Pb: +2 2S: +6 8O: -2 4H: +1 2O: -2 2O: 0

Calculate the number of atoms in 0.236 g of potassium (K).

3.63 x 10^21

The Keq for the equilibrium below is 7.52 × 10-2 at 480.0 °C. 2Cl2 (g) + 2H2O (g) 4HCl (g) + O2 (g) What is the value of Keq at this temperature for the following reaction? 2HCl (g) + ½ O2 (g) Cl2 (g) + H2O (g)

3.65

10.1 g CaO is dropped into a styrofoam coffee cup containing 157g H2O at 18.0 C If the following reaction occurs, what temperature ill the water reach, assuming that the cup is a perfect insulator and that the cup absorbs only a negligible amount of heat? (the specific heat of water is 4.18 J/gC) CaO(s) + H2O(l) --> Ca(OH)2(s) ΔHrxn = -64.8 kJ/mol

35.8 C

ΔH for the reaction: IF5(g) ---> IF3(g) + F2(g) is _______ kJ. given the data below. IF(g) + F2(g) -->IF3(g) ΔH = -390kJ IF(g) + 2F2(g) --> IF5(g) ΔH = -745kJ

355

at what temperature will a sample of oxygen gas with a volume of .110 L at 12 C and 822 mmHg occupy a volume of 345 mL at a pressure of 578 mmHg? Assume the amount of the oxygen gas does not change

355 C

what is the molar heat capacity (in J/mol*k) of liquid bromine? the specific heat of liquid bromine is .226 J/g*k

36.1J/mol*k

What volume (mL) of a 0.2450 M KOH (aq) solution is required to completely neutralize 55.25 mL of a .5440 M H3PO4 solution

368 ml

Calculate the number of grams of lead (Pb) in 22.4 moles of lead.

4640 grams

Consider the reaction 2H2O(g) → 2H2(g) + O2(g)ΔH = 483.6 kJ / mol If 2.0 moles of H2O(g) are converted to H2(g) and O2(g) against a pressure of 1.0 atm at 165°C, what is ΔU for this reaction?

472 kJ

Fermentation is a complex chemical process of wine making in which glucose is converted into ethanol and carbon dioxide: C6H12O6 → 2C2H5OH + 2CO2 Starting with 930.6 g of glucose, what is the maximum amount of ethanol in grams and in liters that can be obtained by this process (density of ethanol = 0.789 g/mL)?

476.1 g .603 L

Consider the reaction 2H2O(g) → 2H2(g) + O2(g)ΔH = 483.6 kJ / mol If 2.0 moles of H2O(g) are converted to H2(g) and O2(g) against a pressure of 1.0 atm at 185°C, what is ΔU for this reaction?

479 kJ

consider the reaction 2H2O(g) → 2H2(g) + O2(g)ΔH = 483.6 kJ / mol If 2.0 moles of H2O(g) are converted to H2(g) and O2(g) against a pressure of 1.0 atm at 155C, what is ΔU for this reaction?

480 kJ

what is the mass of 1.223 mol of Iron(III) sulfate

489.0 grams Fe2(SO4)3

What is the pH of 0.626 M anilinium hydrochloride (monoprotic acid form: C6H5NH3^+Cl- ) solution in water, given that Kb for aniline (the conjugate base of anilinium hydrochloride) is 3.83 x 10^-4 ?

5.39

What is the pH of a 0.023 M solution of HCN (Ka = 4.9 x 10-10)?

5.47

Determine the number of atoms of each element in the empirical formula of a compound with the following composition: 54.95 percent C, 8.455 percent H, 36.60 percent O.

6 C atoms 11 H atoms 3 O atoms

The first-order decomposition, A → products, has a rate constant of 0.150 s-1. Starting with [A]o = 0.350 M, how much time is required for [A]t = 0.125 M?

6.86 s

how many grams of CO2 are used when 8.0 g of O2 are produced

7.3 g CO2

calculate the standard enthalpy change for the following: 2CuO (s) + NO (g) --> Cu2 (s) + NO2 (g)

87.1

Ammonia is a principal nitrogen fertilizer. It is prepared by the reaction between hydrogen and nitrogen. 3H2(g) + N2(g)→ 2NH3(g) In a particular reaction, 6.00 moles of NH3 were produced. How many moles of H2 and how many moles of N2 were reacted to produce this amount of NH3?

9 mol H2 3 mol N2

What is the pH of a 0.080 M solution of the weak base pyridine (C5H5N; Kb = 1.7 x 10-9)?

9.07

If 5.17 g of Ag2O is sealed in a 75.0-mL tube filled with 760 torr of N2 gas at 32 °C, and the tube is heated to 350°C, the Ag2O decomposes to form oxygen and silver. What is the total pressure inside the tube assuming the volume of the tube remains constant?

9.67 atm

A gas occupying a volume of 619.0 mL at a pressure of 0.803 atm is allowed to expand at constant temperature until its pressure reaches 0.534 atm. What is its final volume?

931 mL

Which of the following equations does not represent an oxidation-reduction reaction? A) Cu(NO3)2 (aq) + Zn(s) → Zn(NO3)2(aq) + Cu(s) B) 3 Al(s) + 6 HCl(l) → 3 H2 (g) + AlCl3 (s) C) 2 NaCl(aq) + Pb(NO3)2 (aq) → PbCl2 (s) + 3 NaNO3 (aq) D) 2 NaI(aq) + Br2 (l) → 2 NaBr (aq) + I2 (s) E) 2 H2O (l) → 2 H2 (g) + O2 (g)

Which of the following represents an acid-base neutralization reaction? A) LiOH(aq) + HNO3(aq) → LiNO3(aq) + H2O(l) B) SO2(g) + H2O(l) → H2SO3(g) C) 2KBr(aq) + Cl2(g) → 2KCl(aq) + Br2(l) D) CaBr2(aq) + H2SO4(aq) → CaSO4(s) + 2HBr(g) E) 2Al(s) + 3H2SO4(aq) → Al2(SO4)3(aq) + 3H2(g)

A/B X label the parts of an element table thing

A = mass # B = atomic # X = element name

solvent

A liquid substance capable of dissolving other substances

arrhenius plot

A plot of the natural log of the rate constant (ln k) versus the inverse of the temperature in kelvins (1/T) that yields a straight line with a slope of -Ea/R and a y-intercept of ln A.

solute

A substance that is dissolved in a solution.

A- + H2O ⇌ HA + OH-

A- = base HA = conjugate acid

Consider the reaction A + B → Products From the following data obtained at a certain temperature, determine the order of the reaction. Enter the order with respect to A, the order with respect to B, and the overall reaction order. [A](M) [B](M) Rate (M/s) 1.50 1.50 3.20 x 10^-1 1.50 2.50 3.20 x 10^-1 3.00 1.50 6.40 x 10^-1

A: 1 B: 0 Reaction: 1

Identify the correct net ionic equation for the reaction that occurs when solutions of AgNO3 and NH4Cl are mixed.

Ag+(aq) + Cl-(aq) → AgCl(s)

insoluble exceptions

Ag+, Hg22+, Pb2+, Ca2+, Sr2+, Ba2+, Hg22+, and Pb2+

Which statement is false?

All molecules of an ideal gas have the same kinetic energy at constant temperature.

Which statement is false? the average kinetic energies of molecules from samples of different "ideal" gases are the same at the same temperature. The molecules of an ideal gas are relatively far apart. All molecules of an ideal gas have the same kinetic energy at constant temperature. Molecules of a gas undergo many collisions with each other and the container walls. Molecules of greater mass have a lower average speed than those of less mass at the same temperature.

All molecules of an ideal gas have the same kinetic energy at constant temperature.

atomic number 13 (Al)

Aluminum

electrolyte

An ionic compound whose aqueous solution conducts an electric current

Predict whether the following solutions will be acidic, basic, or nearly neutral: (a) LiClO4, (b) Na3PO4, (c) Bi(NO3)3, (d) NH4CN.

Answer (a) pH ≈ 7, (b) pH > 7, (c) pH < 7, (d) pH > 7.

At equilibrium, ________. A) all chemical reactions have ceased B) the rates of the forward and reverse reactions are equal C) the rate constants of the forward and reverse reactions are equal D) the value of the equilibrium constant is 1 E) the limiting reagent has been consumed

Answer: B

The value of Keq for the equilibrium H2 (g) + I2 (g) 2HI (g) is 794 at 25 °C. At this temperature, what is the value of Keq for the equilibrium below? HI (g) 1/2 H2 (g) + 1/2 I2 (g) A) 1588 B) 28 C) 397 D) 0.035 E) 0.0013

Answer: D

atomic number 18 (Ar)

Argon

atomic number 33 (As)

Arsenic

A reaction that is spontaneous as written ________. A) is very rapid B) will proceed without outside intervention C) is also spontaneous in the reverse direction D) has an equilibrium position that lies far to the left E) is very slow

The spectator ions in the reaction between aqueous perchloric acid and aqueous barium hydroxide are ________.

Ba and ClO4

atomic number 4 (Be)

Beryllium

atomic number 5 (B)

Boron

atomic number 35 (Br)

Bromine

Select the factors that will change when additional A(g) is added to the following system at equilibrium. A + B >< 2C

C increases A increases B decreases Equilibrium shits to the right

the percent comp by mas of a compound is 76% c , 12.8% H, 11.2% O. The molar mass is 284.5 g/mol. What is the molar mass

C18H36O2

it is composed of 40.92% carbon, 4.58% hydrogen and 54.50% O by mass 1. determine its imperical formula 2. determine its molecular formula if the molecular weight of ascorbic acis is 176.006 g/mol^2

C3H4O3 C6H8O6

the characteristics odor of pineapple is due to ethyl butyrate, Cl compound contaning carbon, hydrogen, and oxygen. Combustion of 3.06 mg of ethyl butrate produces 6.95 mg of CO2 and 2.84 mg of H2O. What is the empirical formula of the compound?

C3H6O

which of the following has the largest entropy at 25C and 1 atm a)C3H4 b)C3H6 c)C3H8 d)H2 e)C2H6

C3H8

A certain anesthetic contains 64.9 percent C, 13.5 percent H, and 21.6 percent O by mass. At 122°C and 782 mmHg, 1.00 L of the gaseous compound weighs 2.36 g. What is the molecular formula of the compound?

C4H10O

Assuming that each metal ion is 0.10 M, place the following hyrdroxide salts in order of precipitation with increasing pH: Ca(OH)2 Ksp = 6.5 x 10^−6 Fe(OH)2 Ksp = 4.1 x 10^−15 Mn(OH)2 Ksp = 1.6 x 10^−13 Cu(OH)2 Ksp = 2.2 x 10^−20 Co(OH)2 Ksp = 1.3 x 10^−15 Zn(OH)2 Ksp = 3 x 10^−16

Ca(OH)2 Ksp = 6.5 x 10^−6 Mn(OH)2 Ksp = 1.6 x 10^−13 Fe(OH)2 Ksp = 4.1 x 10^−15 Co(OH)2 Ksp = 1.3 x 10^−15 Zn(OH)2 Ksp = 3 x 10^−16 Cu(OH)2 Ksp = 2.2 x 10^−20

What is the formula for the ionic compound containing Calcium ions and sulfate ions?

CaSO4

atomic number 20 (Ca)

Calcium

atomic number 6 (C)

Carbon

hypochlorite

ClO-

chlorite

ClO2 -

chlorate

ClO3 -

perchlorate

ClO4 -

atomic number 27 (Co)

Cobalt

atomic number 29 (Cu)

Copper

dichromate

Cr2O7 2-

chromate

CrO4 2-

qsolution =

Cs * msolution * ∆T

specific heat capacity equation (solving for specific heat)

Cs= q/(∆T*m)

net ionic equation of CuCl2(aq) + Pb(s) -> Cu(s) + PbCl2

Cu2+(aq) + 2Cl-(aq) + Pb(s) -> Cu(s) + PbCl2(s)

A 10.1 g sample of NaOH is dissolved in 250.0 g of water in a coffee-cup calorimeter. The temperature increases from 23.0 °C to ________°C. Specific heat of liquid water is 4.18 J/g-K and ΔH for the dissolution of sodium hydroxide in water is - 44.4 kJ/mol. A) 35.2 B) 24.0 C) 33.7 D) 33.3 E) 40.2

A decrease in the entropy of the system is observed for the reaction ________. A) 4 NH3 (g) + 5 O2 (g) → 4 NO (g) + 6 H2O (g) B) 2 HgO (s) → 2 Hg (l) + O2 (g) C) UF6 (s) → U (s) + 3F2 (g) D) K (s) + 1/2 I2 (g) → KI (s) E) H2O (s) → H2O (g)

At what temperature will a reaction be spontaneous? ΔH = +22.2 kJ/mol and ΔS = +81.1 J/K-mol and assume both do not vary with temperature. A) at T > 298 K B) at T < 274 K C) at T < 298 K D) at T > 274 K E) at all temperatures

Given the following reactions N2 (g) + O2 (g) → 2NO (g) ΔH = +180.7 kJ 2N2O (g) → O2 (g) + 2N2 (g) ΔH = -163.2 kJ the enthalpy of reaction for 2N2O (g) → 2NO (g) + N2 (g) is ________ kJ. A) 145.7 B) 343.9 C) -343.9 D) 17.5 E) -145.7

HA is a weak acid. Which equilibrium corresponds to the equilibrium constant Kb for A-? A) HA (aq) + H2O (l) ⇌ H2A + (aq) + OH-(aq) B) A- (aq) + H3O + (aq) ⇌ HA (aq) + H2O (l) C) HA (aq) + OH- (aq) ⇌ H2O (l) + H+ (aq) D) A- (aq) + H2O (l) ⇌ HA (aq) + OH- (aq) E) A- (aq) + OH- (aq) ⇌ HOA2- (aq)

The internal energy of a system ________. A) is the sum of the kinetic energy of all of its components B) is the sum of the rotational, vibrational, and translational energies of all of its components C) refers only to the energies of the nuclei of the atoms of the component molecules D) is the sum of the potential and kinetic energies of the components E) none of the above

The signs of ΔH° and ΔS° must be ________ and ________, respectively, for a reaction to be spontaneous at high temperatures but nonspontaneous at low temperatures. A) +, - B) -, + C) -, - D) +, + E) +, 0

The specific heat capacity of lead is 0.13 J/g-K. How much heat (in J) is required to raise the temperature of 15g of lead from 22 °C to 37 °C? A) 2.0 J B) -0.13 J C) 5.8 × 10-4 J D) 29 J E) 0.13 J

A 50.0-g sample of liquid water at 25.0 °C is mixed with 23.0 g of water at 79.0 °C. The final temperature of the water is ________ °C. A) 123 B) 27.3 C) 52.0 D) 231 E) 42.0

The combustion of acetylene in the presence of excess oxygen yields carbon dioxide and water: 2C2H2 (g) + 5O2 (g) → 4CO2 (g) + 2H2O (l) The value of ΔS° for this reaction is ________ J/K ∙ mol. A) +689.3 B) +122.3 C) +432.4 D) -122.3 E) -432.4

The combustion of titanium with oxygen produces titanium dioxide: Ti (s) + O2 (g) → TiO2 (s) When 0.610 g of titanium is combusted in a bomb calorimeter, the temperature of the calorimeter increases from 25.00 °C to 50.50 °C. In a separate experiment, the heat capacity of the calorimeter is measured to be 9.84 kJ/K. The heat of reaction for the combustion of a mole of Ti in this calorimeter is ________ kJ/mol. A) 2.09 B) 4.14 C) -311 D) -0.154 E) -1.98 × 10⁴

The ΔU of a system that absorbs 12.4 J of heat and does 4.2 J of work on the surroundings is ________ J. A) 16.6 B) 12.4 C) 4.2 D) -16.6 E) 8.2

Which one of the following is a BrØnsted-Lowry acid? A) (CH3)3NH + B) CH3CO2H C) HF D) HNO2 E) all of the above

in which of the following reactions would increase pressure @ constant temperature not change the concentration of reactants and products, based on la chatelier's principle? A) N2(g) + 2O2(g) >< 2NO2(g) B) N2O4(g) >< 2NO2(g) C) 2N2(g) + O2(g) >< 2N2O(g) D) N2(g) + 3H2(g) >< 2NH3(g) E) N2(g) + O2(g) >< 2NO(g)

The second-order rate constant has been measured at different temperatures for the decomposition of nitrous oxide (N2O) into a nitrogen molecule and an oxygen atom. k(1/M · s) T(°C) 1.87 × 10−3 600.0 0.0113 650.0 0.0569 700.0 0.244 750.0 Determine the activation energy for the reaction.

Ea = 241.2 kJ/mol

second law of thermodynamics

Every energy transfer or transformation increases the entropy of the universe.

iron metal reacts with hydrochloric acid to produce iron (III) chloride and hydrogen gas. identify the balanced reaction that describes this process

Fe + 2HCl --> FeCl2 + H2

iron metal reacts with hydrochloric adic to produce iron (ii) chloride and hydrogen gas. Identify the balanced equation

Fe + 2HCl -> FeCl2 + H2

atomic number 9 (F)

Fluorine

atomic number 31 (Ga)

Gallium

atomic number 32 (Ge)

Germanium

atomic number 79 (Au)

Gold

enthalpy change

When H2SO4 is neutralized by NaOH in aqueous solution, the net ionic equation is

H+ + OH- -> H2O

diatomic elements

H, N, O, F, Cl, Br, I

What is the conjugate acid of HCO3 - ?

H2CO3

What is the conjugate acid of HCO3-?

H2CO3

List in order of decreasing concentration all the ionic and molecular species in the following base solutions: (i) NH3, (ii) KOH.

H2O > NH3 > NH4+, OH− > H+. (ii) H2O > K+, OH− > H+.

List in order of decreasing concentration all the ionic and molecular species in the following acid solutions: (i) HNO3, (ii) HF.

H2O >H+, NO3− > OH−. (ii) H2O > HF > H+, F− > OH−

which is the more negative quantity at 25°C: ΔHof H2O(l) or ΔHof for H2O(g)?

H2O(l)

Nitric acid is a strong oxidizing agent. State which of the following species is least likely to be produced when nitric acid reacts with a strong reducing agent such as zinc metal: N2O4 NO2 N2O N2O5 NO NH4+

H2O5

dihydrogen phosphate

H2PO4 -

In which of the following species does the sulfur atom have the highest oxidation number? H2S S8 H2SO4 S2−

H2SO4

HA + H2O --> H3O+ + A-

HA = acid A- = conjugate base

bicarbonate

HCO3 -

Hydrochloric acid is a strong acid. This means that ________.

HCl dissociates completely to H+ and Cl- when it dissolves in water

In the reaction HSO4-(aq) + OH-(aq) ⇌ SO4^2-(aq) + H2O(l), the conjugate acid-base pairs are

HSO4- and SO42- H2O and OH-

Heat energy (heat flow)

atomic number 2 (He)

Helium

mercury (I)

Hg2 2+

Acetylene (C2H2) and benzene (C6H6) have the same empirical formula. In fact, benzene can be made from acetylene as follows: 3C2H2(g) → C6H6(l) The enthalpies of combustion for C2H2 and C6H6 are −1299.4 kJ/mol and −3267.4 kJ/mol, respectively. Calculate the standard enthalpies of formation of C2H2 and C6H6. Assume that the products of the combustions are CO2(g) and H2O(l). Hof(C2H2) = Hof(C6H6) =

Hof(C2H2) = 226.6 kJ/mol Hof(C6H6) = 49.0 kJ/mol

what are the names if the strong acids

Hydrochloric Acid, HCl Hydrobromic Acid, HBr Hydroiodic Acid, HI Chloric Acid, HClO3 Perchloric Acid, HClO4 Nitric Acid, HNO3 Sulfuric Acid, H2SO4

Concerning the decomposition of A, A → products, which of the following methods could be used to determine the order of the reaction with respect to A? I. Plot [A] vs time, ln[A] vs time, and 1/[A] vs time and identify which plot yields a straight line. II. Vary the concentration of A and note by what factor the rate changes. III. Identify if successive half lives of A double, halve, or stay constant.

I, II, III

Which of the following has a ΔH°f= 0 kJ/mol? O3(g) Cl-(aq) I2(s) NH3(aq) CO2(g)

I2(s)

How to tell if it's an acid

If the number of hydrogens has decreased that substance is the acid (gives up hydrogen ions).

How to tell if it's a base

If the number of hydrogens has increased that substance is the base (accepts hydrogen ions).

atomic number 53 (I)

Iodine

atomic number 26 (Fe)

Iron

at equilibrium Q =

Predict whether the equilibrium constant for the following reaction is greater than or smaller than 1

K > 1

consider the two gaseous equilibria: SO2(g) + 1/2O2(g) >< SO3(g) K1 2SO3(g) >< 2SO2(g) + O2(g) K2 the values of the equilibrium constants K1 and K2 are related by

K2 = 1/K1^2

when the equilibrium constant is less than 1

K<1 favors reactants

when the equilibrium constant is greater than 1

K>1 favors products

In the following chemical reaction the oxidizing agent is 5S + 6KNO3 + 2CaCO3 -> 3K2SO4 + 2CaSO4 + CO2 + 3N2

KNO3

The equilibrium expression for the hydrolysis of a weak base, A-, in water is:

Kb = [OH-][HA]/[A-]

5.00 mol of ammonia are introduced into a 5.00 L reactor vessel in which it partially dissociates at high temperatures. 2NH3(g) >< 3H2(g) + N2(g) At equilibrium and a particular temperature, 1.00 mole of ammonia remains. Calculate Kc for the reaction.

Kc = 17.3

the equilibrium expression for aA + bB >< dD + eE would be:

Kc = [D]^d[E]^e/[A]^a[B]^b

atomic number 3 (Li)

Lithium

k units

M-1 x S-1

Given the rate law for a reaction, rate = k[A]^2 , where rate is measured in units of M min^-1 , what are the units for the rate constant k?

M-1min-1

Concerning the rate law, Rate = k[A]0, what are appropriate units for the rate constant k?

M/s

molarity equation

M=mol/L

what is being oxidized and reduced in 4NH3 + 3Ca(ClO)2 -> 2N2 + 6H2O + 3CaCl2

N is oxidized Cl is reduced

ammonia

NH3

nitrite

NO2 -

nitrate

NO3 -

NaHCO3 (aq) + HBr(aq) ->>

NaBr(aq) + CO2(g) + H2O(l)

which of the following ionic compounds are soluble? CuS NaOH Zn(NO3)2 Ca(OH)2

NaOH Zn(OH)2

What are the two different ions present in the compound Na2S?

Na^+ S^2-

atomic number 10 (Ne)

Neon

atomic number 28 (Ni)

Nickel

atomic number 7 (N)

Nitrogen

atomic mass

Number of protons and neutrons

peroxide

O2 2-

Using the data in the table, which of the conjugate bases below is the strongest base? HOAc.........................1.8 x 10^-5 HC7H5O2................6.3 x 10^-5 HNO2........................4.5 x 10^-4 HF................................6.8 x 10^-4

OAc-

hydroxide

OH-

atomic number 8 (O)

Oxygen

Oxidation numbers in PBr3

P +3 Br -1

Assign oxidation numbers to all elements in the following compound and ion: (a)PBr3

P: +3 Br: -1

Be sure to answer all parts.A sample of natural gas contains 6.768 moles of methane (CH4), 0.749 moles of ethane (C2H6), and 0.449 moles of propane (C3H8). If the total pressure of the gases is 3.20 atm, what are the partial pressures of the gases? PCH4 PC2H6 PC3H8

PCH4 = 2.72 PC2H6 = .301 PC3H8 = .180

Suppose dry air near sea level has the following composition by volume: N2, 78.08 percent; O2, 20.94 percent; Ar, 0.93 percent; CO2, 0.05 percent. If the atmospheric pressure is 1.000 atm, calculate the partial pressure of each gas in atm.

PN2 = 0.7808 atm PO2 = .2094 atm PAr = .0093 atm PCO2 = .0005 atm

phosphate

PO4 3-

ideal gas law

PV=nRT

Which ions remain in solution, unreacted, after each of the following pairs of solutions is mixed? Lead(II) nitrate and lithium sulfide

Pb + S --> PbS

What compound is the Oxidizing Agent in the following reaction? Pb(s) + PbO2 (s) + 2 H2SO4 (aq) --> 2 PbSO4 (s) + 2 H2O (l)

Pb(s) is oxidized PbO2(s) is the oxidixing agent

which ions remain in solution, unreacted, after each of the following pairs of solutions is mixed lead (ii) nitrate and lithium sulfide

Pb^2+ + S^2- -> PbS

atomic number 15 (P)

Phosphorus

atomic number 78 (Pt)

Platinum

rate law equation

Rate = k [A]ⁿ

1st order rate

Rate = k[A]

A + B -><- C forward reaction info

Ratef = k[A][B]

A + B -><- C reverse reaction info

Rater = [C]^1 ^C ^ rate

The van der Waals equation is a modification of the ideal gas equation. What two factors does this equation account for?

Real gas molecules exert forces on each other. Gas molecules have volume.

sulfite

SO3 2-

Which of the following processes is endothermic, given the following: S(s) + O2(g) →SO2(g) ΔH = -299 kJ/mol S(s) + 3/2 O2(g) →SO3(g) ΔH = -395 kJ/mol S(s) + 3 O2(g) →2 SO3(g) 2 S(s) + 5/2 O2(g) → SO2(g) + SO3(g) SO3(g) →S(s) + 3/2 O2(g) 2 S(s) + 2 O2(g) →2 SO2(g) ½ S(s) + ½ O2(g) →½ SO2(g)

SO3(g) →S(s) + 3/2 O2(g)

sulfate

SO4 2-

The conjugate base of HSO4- is ________.

SO4^2-

partial pressure equation

(n1/ntotal)xPtotal

H oxidation number

oxidation number of Cl in ClF

oxidation number of Cs in Cs2O

oxidation number Pt in PtCl4^2-

How many moles of magnesium (Mg) are there in 97.3 g of Mg?

4.00 mol Mg

time: 0.0 5.0 10.0 15.0 20.0 [A] (M): 0.2 0.14 0.10 .071 .040 What is the concentration (M) of [A] after 80s

4.06x10^-4

chlorine gas reacts with phosphorus to produce phosphorus pentachloride. How many grams of PCl5 are produced from 3.5g of Cl2 and excess P

4.1 g

specific heat of water

4.184 J/gC

What is the concentration of Ca(OH)2 in a solution if the pH is 7.92?

4.2 x 10^-7

hat is the mass of 4.50 x 10^22 Cu atoms?

4.75 g

An unknown compound with a molar mass of 223.94 g/mol consists of 32.18% C, 4.50% H, and 63.32% Cl. Find the molecular formula for the compound.

C6H10Cl4

A 0.813 g sample of an unknown vapor occupies 294 mL at 140.°C and 847 mmHg. The empirical formula of the compound is CH2. What is the molecular formula of the compound?

C6H12

An unknown compound with a molar mass of 155.06 g/mol consists of 46.47% C, 7.80% H, and 45.72% Cl. Find the molecular formula for the compound.

C6H12Cl2

C6H5OH + 7O2 --> 6CO2 + 3H2O

acetate

CH3COO-

atomic number 36 (Kr)

Krypton

what is the equilibrium constant for the following equation: BaSO4(s) ⇌ Ba^2+(aq) + SO4^2- (aq)

Ksp = [Ba^2+] [SO4^2-]

what is the equilibrium constant for the following equation: Ba3(PO4)2(s) ⇌ Ba^2+(aq) + 2PO4^2-(aq)

Ksp = [Ba^2+]^3[PO4^3-]^2

calculate the Ksp for: Mg(OH)2 (s) ⇌ Mg^2+(aq) + 2OH- (aq)

Ksp = [Mg^2+] [OH-]^2

Which is the correct Ksp expression for MnCl4 (s) dissolving in water?

Ksp = [Mn^4+] [Cl-]^4

Which is the correct Ksp expression for PbCl2 (s) dissolving in water?

Ksp = [Pb2+] [Cl-]2

relationship between Ka and Kb

Kw = Ka × Kb = 1.0 × 10⁻¹⁴

Le Chatelier's Principle

States that if a stress is applied to a system at equilibrium, the system shifts in the direction that relieves the stress.

KOH

Strong Base (Potassium Hydroxide)

RbOH

Strong Base (Rubidium Hydroxide)

Sr(OH)2

Strong Base (Strontium Hydroxide)

atomic number 16 (S)

Sulfur

Which reaction will shift to the right in response to a decrease in volume? A) N2 (g) + 3H2 (g) >< 2NH3 (g) B) H2 (g) + Cl2 (g) >< 2 HCl (g) C) 2 SO3 (g) >< 2 SO2 (g) + O2 (g) D) 2HI (g) >< H2 (g) + I2 (g) E) 2 Fe2O3 (s) >< 4 Fe (s) + 3O2 (g)

combination reaction

a chemical change in which two or more substances react to form a single new substance

two formulas that differ by H+ are called...

a conjugate acid-base pair

Predict whether the equilibrium constant for the following reaction is greater than or smaller than 1: CH3COOh + HCOO >< CH3COO- + HCOOH

smaller than 1

when an equilibrium equation is written, the __________ is the reactants and the ______ in solution are the products

solid ions

what is Ksp

solubility product constant

specific heat capacity

given that following table of thermodynamic data, H2(g) -136.3 kJ/mol 232.6 kJ/mol*k H2(l) -187.8 kJ/mol 110 J/mol*k complete the following sentence. The vaporization of H2

spon @ highT nonspon @ low temp

2C4H10(g) + 13O2(g) --> 8CO2(g) + 10H2O(g) ΔH is -125 kJ/mol and ΔS is +253 J/kmol. This reaction is _______.

spontaneous

HNO3 is a _______ electrolyte

strong

what type of electrolyte is ->

strong

ka = 1x10^3

strong acid

HBr

strong acid (hydrobromic acid)

strong acid (hydroiodic acid)

HNO3

strong acid (nitric acid)

HClO4

strong acid (perchloric acid)

H2SO4

strong acid (sulfuric acid)

HCl

strong acid, (hydrochloric acid)

Ba(OH)2

strong base (barium hydroxide)

given the following information: 2A(g) + B(g) >< A2B(g) Kp1 2A(g) + C2(g) >< 2AC(g) Kp2 3/2A2(g) + B(g) + C(g) >< AC(g) + A2B(g) Kp3 Which relationship represents the equilibrium constant for the reaction: 3A2(g) + 3B(g) + 2C(g) >< 3A2B(g) + C2(g) Knet =

(Kp1 Kp3^2)/ Kp2

Based on the solubility rules, which of the following should be soluble in water? •A) Ag3PO4 •B)(NH4)3PO4 •C) AlPO4 •D) Ca3(PO4)2 •E) Mg3(PO4)2

(NH4)3PO4

Select the oxidation number for the indicated atom in the following molecules and ions: Pt in PtCl4^2-

oxidation number of Cr in K2Cr2O4

oxidation number of phosphorus in H3PO3

Select the oxidation number for the indicated atom in the following molecules and ions: Pt in PtCl6^2-

oxidation number of B in NaBH4

a 0.1326g sample of magnesium was burned in an oxygen bomb calorimeter. The total heat capacity o the calorimeter plus water was 5760 J/C. If the temperature rise of the calorimeter with water was 0.570 C. calculate the enthalpy of combustion of magnesium Mg(s) + 1/2O2(g) --> MgO(s)

-602 kJ/mol

Water is added to 25.0 mL of a 0.911 M KNO3 solution until the volume of the solution is exactly 500.0 mL. What is the concentration of the final solution?

.0455

A sample of oxygen gas initially at 0.470 atm is cooled from 21°C to −60°C at constant volume. What is its final pressure (in atm)?

.341 atm

O2 oxidation number

molarity of 7.95 g of sodium chloride (NaCl) in 79.4 mL of solution

1.71

How many grams of KHP are needed to neutralize 83.28 mL of a 0.1087 M NaOH solution?(molar mass of KHP = 204.2 g/mol)

1.849

2nd order integrated rate law

1/[A]t = kt + 1/[A]0

How many moles of magnesium (Mg) are there in 69.3 g of Mg?

2.85 mol Mg

calculate the mass of KI in grams required to prepare 5.00 x 10^2 mL of a 2.9 M solution

240.7

neutral ph

Determine [H+] in a solution in which pOH=10.93.

8.51 x 10^-4

Of the following acids, ________ is not a strong acid. A) HNO2 B) H2SO4 C) HNO3 D) HClO4 E) HCl

ammonium

NH4 +

4Al(s) + 3O2(g) --> 2Al2O3(s) ΔH = -3351 kJ is _____________, and thermal heat is __________ by the reaction

exothermic released

what does rate law relate

relates rate and reactant concentration

Select the oxidation number for the indicated atom in the following molecules and ions: Ti in TiO2

oxidation number Pt in PtCl6^2-

oxidation number of C in NaHCO3

oxidation number of Ti in TiO2

The oxidation number of N in NaNO3 is

oxidation number of I in NaIO3

oxidation number of P in H4P2O7

oxidation number of P in PF6^-

oxidation number of phosphorus in H3PO4

oxidation number of phosphorus in H5P3O10

oxidation number of phosphorus in HPO3

Select the oxidation number for the indicated atom in the following molecules and ions: Mo in MoO4^2-

The oxidation numbers of Cr in Cr2O7 2-

oxidation number Mo in MoO4^2-

oxidation number of Mo in MoO4^2−

oxidation number of S in K2SO4

the oxidation number of Cr in Cr2O7^2- is

The oxidation number of Mn in KMnO4 is

oxidation number of I in IF7

what does it mean to establish an equilibrium state

- concentration of reactants and products no longer change with time - products and reactants cannot escape the reaction - equilibrium state is reversible and can be reached from either the forward or reverse direction

common ion effect

- if one of the ions in a solution equilibrium is already dissolved in the solution, the solubility of the salt will decrease - if either calcium ions or fluoride ions are present, then calcium flouride will be less soluble

choose equivalent expressions for the rate of the reaction in terms of the appearance or disappearance of the two substances B---> 2A

- Δ[B]/Δt = 1/2 Δ[A]/Δt

Consider the reaction 4PH3(g) → P4(g) + 6H2(g) Suppose that, at a particular moment during the reaction, molecular hydrogen is being formed at rate of 0.230 M/s. At what rate is PH3 changing?

-.153

F oxidation number is always

-1

O oxidation number in H2O2

-1

Determine the amount of heat (in kJ) associated with the production of 5.64 × 104 g of ammonia according to the following equation. N2(g) + 3H2(g) ---> 2NH3 ΔH°rxn = −92.6 kJ Assume that the reaction takes place under standard-state conditions at 25°C.

-1.53 x10^5

what if the equation is not 1:1 2O3(g) --> 3O2(g)

-1/2 Δ[O3]/ Δt = 1/3 Δ[O2]/Δt

For a substance that remains a gas under the conditions listed, deviation from the ideal gas law would be most pronounced at 100°C and 2.0 atm. 0°C and 2.0 atm. -100°C and 2.0 atm. -100°C and 4.0 atm. 100°C and 4.0 atm.

-100 C and 4 atm

For a substance that remains a gas under the conditions listed, deviation from the ideal gas law would be most pronounced at

-100 C and 4.0 atm

for the reaction 3H2(g) + N2(g) >< 2NH3(g) k= 9.0 @ 350C calculating ΔG at 350C

-11.381 kJ/mol

Calculate the heats of combustion for the following reactions. Use the standard enthalpies of formation. b) 2H2S(g) + 3O2(g) → 2H2O(l) + 2SO2(g)

-1144.68 kJ/mol

Calculate the heat (in kJ) associated with 496 g of white phosphorus burning in air according to the equation P4(s) + 5O2(g) → P4O10(s) ΔH = −3013 kJ / mol

-12,063 kJ

Calculate the heats of combustion for the following reactions. Use the standard enthalpies of formation. (a) C2H4(g) + 3O2(g) → 2CO2(g) + 2H2O(l)

-1410.9 kJ/mol

-167.2 kJ/mol

Under constant-pressure conditions a sample of hydrogen gas initially at 71.00°C and 9.60 L is cooled until its final volume is 2.30 L. What is its final temperature?

-190.6 C

A sample of nitrogen gas expands in volume from 1.2 to 6.0 L at constant temperature. Calculate the work done in joules if the gas expands against a constant pressure of 4.9 atm:

-2.38 x 10^3 J

A balloon 17.0 m in diameter is inflated with helium at 25°C. Calculate the work done (in kJ) during the inflation process if the atmospheric pressure is 97.7 kPa.

-2.51 x 10^5 kJ

A balloon 17.0 m in diameter is inflated with helium at 21°C. Calculate the work done (in kJ) during the inflation process if the atmospheric pressure is 97.7 kPa.

-2.51 x10^5 kJ

at elevated temperatures, dinitrogen pentoxide decompses to nitrogen dioxide and oxygen: 2N2O5(g) --> 4NO2(g) + O2(g) when the rate of formation of NO2 is 5.5x10^-4 M/s, the rate of decomposition of N2O5 is ________ M/s

-2.8 x 10^-4

A sample of nitrogen gas expands in volume from 1.3 to 6.5 L at constant temperature. Calculate the work done in joules if the gas expands against a constant pressure of 5.5 atm:

-2.9 x 10^3

Calculate the heat (in kJ) associated with the cooling of 391 g of mercury from 65.9°C to 12.0°C.

-2.93 kJ

H2 + F2 --> 2HF ΔHf = -537 kJ C + 2F2 --> CF4 ΔHf = -680 kJ 2C + 2H2 --> C2H4 ΔHf = 52.3 kJ calculate the ΔHrxn for the reaction of enthylene with F2: C2H4 + 6F2 ---> 2CF4 + 4HF

-2486.3 kJ

calculate the heat combustion for the following reaction 2C2H2 (g) + 5O2 (g) --> 4CO2 (g) + 2H2O (l)

-2598.8

find ΔHrxn for the reaction: 2Na(s) + 2H2O(l) --> 2NaOH(aq) + 2H2(g) (ΔHfNaOH = -426.8 kJ/mol ; ΔHf H2O = -285.5 kJ/mol)

-282.6 kJ

A gas expands from 248 mL to 974 mL at a constant temperature. Calculate the work done (in joules) by the gas if it expands (a) against a constant pressure of 4.00 atm w =

-294 J

Calculate the heat (in kJ) associated with the cooling of 305 g of mercury from 84.1°C to 12.0°C.

-3.057 kJ

Calculate the heat (in kJ) associated with the cooling of 348 g of mercury from 79.9°C to 12.0°C.

-3.296 kJ

A sample of nitrogen gas expands in volume from 1.2 to 6.0 L at a constant temperature. Calculate the work done in joules if the gas expands against a constant pressure of 0.73 atm:

-3.35 x 10^2 J

A sample of nitrogen gas expands in volume from 1.3 to 6.5 L at constant temperature. Calculate the work done in joules if the gas expands against a constant pressure of 0.68 atm:

-3.6 x 10^2 J

when solutions containing silver ions and chloride ions are mixed, silver chloride precipitates: Ag+(aq) + Cl-(aq) ---> AgCl (s) ∆H=-65.5 kj calculate ∆H for the formation of 8.00g of AgCl

-3.65 kJ

when solutions containing silver ions and chloride ions are mixed, silver chloride precipitates: Ag+(aq) + Cl-(aq) ---> AgCl (s) ∆H=-65.5 kj calculate ∆H for formation of 0.46 mol of AgCl by this reaction?

-30.13 kJ

The first step in the industrial recovery of zinc from the zinc sulfide ore is roasting-that is, the conversion of ZnS to ZnO by heating: 2ZnS(s) + 3O2(g) →2ZnO(s) + 2SO2(g) ΔH = −879 kJ Calculate the heat (in kJ) associated with roasting 1 gram of zinc sulfide.

-4.51 kJ

-4.51kJ

Determine the amount of heat (in kJ) associated with the production of 1.77 × 104 g of ammonia according to the following equation. N2(g) + 3H2(g) 2NH3 ΔH°rxn = −92.6 kJ assume that the reaction takes place under standard-state conditions at 25°C. Enter your answer in scientific notation.

-4.81 x 10^4 kJ

a certain gas expands in volume from 2.0L to 6.0L at constant temperature. Calculate the work done by the gas if it expands a) against a constant pressure of 1.2 atm

-4.9x10^2

Benzene (C6H6) burns in air to produce carbon dioxide and liquid water. Calculate the change in heat (in kilojoules) per gram of the compound reacted with oxygen. The standard enthalpy of formation of benzene is 49.04 kJ/mol.

-41.83 kJ/g

When 1.703 g of naphthalene (C10H8) is burned in a constant-volume bomb calorimeter at 298 K, 68.45 kJ of heat is evolved. Calculate ΔU and w for the reaction on a molar basis. ΔU =

-5,152.8 kJ/mol

Calcium oxide (CaO) is used to remove sulfur dioxide generated by coal-burning power stations: 2CaO(s) + 2SO2(g) +O2(g) → 2CaSO4(s) Calculate the enthalpy change for this if 6.50 × 105 g of SO2 are removed by this process every day.

-5.08 x 10^6 kJ

The standard enthalpies of formation of ions in aqueous solutions are obtained by arbitrarily assigning a value of zero to H ions; that is, ΔHof[H+(aq)] = 0. HCl(g) --> H+(aq) + Cl−(aq) ΔHorxn= −74.9 kJ/mol Given that ΔHof for OH− ions is −229.6 kJ/mol, calculate the enthalpy of neutralization when 1 mole of a strong monoprotic acid (such as HCl) is titrated by 1 mole of a strong base (such as KOH) at 25°C.

-56.2 kJ/mol

A 0.1326 g sample of magnesium was burned in an oxygen bomb calorimeter. The total heat capacity of the calorimeter plus water was 5,760 J/°C. If the temperature rise of the calorimeter with water was 0.570°C, calculate the enthalpy of combustion of magnesium. Mg(s) + 1/2O2(g) →MgO(s)

-602 kJ/mol

-630.8 kJ/mol

Given that 2Al(s) + 3/2O2(g) → Al2O3(s) ΔHorxn=−1601 kJ/mol 2Fe(s) + 3/2O2(g) → Fe2O3(s) ΔHorxn =−821 kJ/mol calculate the standard enthalpy change for the following reaction: 2Al(s) + Fe2O3(s) → 2Fe(s) + Al2O3(s)

-7.8 x 10^2 kJ

Given that 2Al(s) + 32O2(g) → Al2O3(s) ΔHorxn=−1601 kJ/mol and. 2Fe(s) + 3/2O2(g) → Fe2O3(s) ΔHorxn=−821 kJ/mol calculate the standard enthalpy change for the following reaction: 2Al(s) + Fe2O3(s) → 2Fe(s) + Al2O3(s)

-7.8 x 10^2 kJ

A quantity of 1.922 g of methanol (CH3OH) was burned in a constant-volume bomb calorimeter. Consequently, the temperature rose by 4.92°C. If the heat capacity of the bomb plus water was 9.77 kJ / °C, calculate the molar heat of combustion of methanol.

-801 kJ / mol

A quantity of 1.922 g of methanol (CH3OH) was burned in a constant-volume bomb calorimeter. Consequently, the temperature rose by 5.76°C. If the heat capacity of the bomb plus water was 8.51 kJ / °C, calculate the molar heat of combustion of methanol.

-817 kJ / mol

C(graphite) + O2(g) → CO2(g) ΔHorxn = −393.5 kJ/mol H2(g) + 1/2O2(g)→ H2O(l) ΔHorxn=−285.8 kJ/mol 2C2H6(g) + 7O2(g) → 4CO2(g) + 6H2O(l) ΔHorxn = −3119.6 kJ/mol calculate the enthalpy change for the reaction below: 2 C(graphite) + 3H2(g) → C2H6(g)

-84.6 kJ

Enter your answer in the provided box. From the following data, C(graphite) + O2(g) →CO2(g) ΔHrxn = −393.5 kJ/mol H2(g) + 1/2O2(g) → H2O(l) ΔHrxn = −285.8 kJ/mol 2C2H6(g) + 7O2(g) → 4CO2(g) + 6H2O(l) ΔHrxn = −3119.6 kJ/mol calculate the enthalpy change for the reaction below: 2 C(graphite) + 3H2(g) → C2H6(g)

-84.6 kJ

Enter your answer in the provided box.A quantity of 1.922 g of methanol (CH3OH) was burned in a constant-volume bomb calorimeter. Consequently, the temperature rose by 5.52°C. If the heat capacity of the bomb plus water was 9.32 kJ / °C, calculate the molar heat of combustion of methanol.

-858 kJ / mol

Calculate the heat (in kJ) associated with 371 g of white phosphorus burning in air according to the equation P4(s) + 5O2(g) → P4O10(s)ΔH = −3013 kJ / mol

-9023 kJ

H2(g) + 1/2 O2(g) --> H2O(l) ΔHf = -285.8 kJ/mol H2O2(l) --> H2(g) +O2(g) ΔHrxn = 187.6 kJ/mol calculate ΔHfHrxn for the reaction H2O2 (l) --> H2O(l) + 1/2O2 (g)

-98.2 kJ

Given the following ΔH° values, H2(g) + 1/2O2(g) → H2O(l) ΔH°f = -285.8 kJ/mol H2O2(l) → H2(g) + O2(g) ΔH°rxn = 187.6 kJ/molcalculate ΔH°rxn for the reaction H2O2(l) → H2O(l) + 1/2O2(g).

-98.2 kJ/mol

if Kw = [H+][OH-]...

-logKw = -log[H+][OH-] pKw = pH + pOH

pOH

-log[OH-]

the internal energy can be increased by...

-transferring heat from the surroundings to the system -doing work on the system

Calcium carbonate, CaCO3 (s), the principal compound in limestone, decomposes upon heating to CaO(s) and CO2 (g). A sample of CaCO3 is decomposed, and the carbon dioxide is collected in a 250-mL flask. After decomposition is complete, the gas has a pressure of 1.3 atm at a temperature of 31 °C. How many moles of CO2 gas were generated?

.01303 mol CO2

Ethyl iodide (C2H5I) decomposes at a certain temperature in the gas phase as follows: C2H5I(g) → C2H4(g) + HI(g) From the following data determine the order of the reaction and the rate constant. Time (min) [C2H5I] (M) 0.0 2.00 15.0 1.76 30.0 1.52 48.0 1.23 75.0 0.80 rate constant:

.016

Consider the reaction 4PH3(g) → P4(g) + 6H2(g) Suppose that, at a particular moment during the reaction, molecular hydrogen is being formed at rate of 0.230 M/s. At what rate is P4 changing?

.0383

Water is added to 25.0 mL of a 0.911 M KNO3 solution until the volume of the solution is exactly 500.0 mL. What is the concentration of the final solution?

.0455 M

A flask is charged with 0.124 mol of A and allowed to react to form B according to the reaction A(g) →B(g). The following data are obtained for [A] as the reaction proceeds: time: 0.00 10.0 20.0 30.0 40.0 moles of A .124 .110 .088 .073 .054 how many moles of B are present at 30s

.051

when solutions containing silver ions and chloride ions are mixed, silver chloride precipitates: Ag+(aq) + Cl-(aq) ---> AgCl (s) ∆H=-65.5 kj calculate ∆H when 9.25 x 10^-4 mol of AgCl dissolves in water

.06059 kJ

The hydrogen gas generated when calcium metal reacts with water is collected over water at 20.°C. The volume of the gas is 641 mL and the pressure is 988 mmHg. What is the mass (in grams) of the hydrogen gas obtained? The vapor pressure of water at 20.°C is 17.54 mmHg.

.0686 g

.0699 g

A quantity of 19.68 mL of a KOH solution is needed to neutralize 0.2938 g of KHP. What is the concentration (in molarity) of the KOH solution?(The molar mass of KHP is 204.2 g/mol.)

.07311

A quantity of 19.68 mL of a KOH solution is needed to neutralize 0.2938 g of KHP. What is the concentration (in molarity) of the KOH solution?(The molar mass of KHP is 204.2 g/mol.)

.07312 M

the rate of disappearance of HBr in the gas phase reaction 2HBr(g) --> H2(g) + Br2(g) is -.190 Ms^-1 at 150 C. The rate of appearance of Br2 is _______ Ms^-1

.095

Acetic acid (HC2H3O2) is an important ingredient of vinegar. A sample of 50.0 mL of a commercial vinegar is titrated against a 1.00 M NaOH solution. What is the concentration (in M) of acetic acid present in the vinegar if 5.45 mL of the base is needed for the titration?

.109

In a titration experiment, a student finds that 23.48 mL of a NaOH solution are needed to neutralize 0.5468 g of KHP. What is the concentration (in molarity) of the NaOH solution? C8H5O4K

.1140 M

A quantity of 11.68 mL of a KOH solution is needed to neutralize 0.2788 g of KHP. What is the concentration (in molarity) of the KOH solution?(The molar mass of KHP is 204.2 g/mol.)

.1169

17.5 mL of a 0.1050 M Na2CO3 solution is added to 46.0 mL of 0.1250 M NaCl. What is the concentration of sodium ion in the final solution?

.148

Calculate the concentration (in molarity) of an NaOH solution if 25.0 mL of the solution is needed to neutralize 15.9 mL of a 0.261 M HCl solution.

.1660

Dry ice is solid carbon dioxide. A 1.33−g sample of dry ice is placed in an evacuated 3.45−L vessel at 26.0°C. Calculate the pressure inside the vessel after all the dry ice has been converted to CO2 gas.

.215 atm

A piece of silver with a mass 427 g has a heat capacity of 101.2 J/°C. What is the specific heat of silver?

.237 J/g ·°C

A piece of silver with a mass 313 g has a heat capacity of 74.2 J/°C. What is the specific heat of silver?

.237 J/g·°C

A piece of silver with a mass 316 g has a heat capacity of 74.9 J/°C. What is the specific heat of silver?

.2370 J/g·°C

At elevated temperatures, molecular hydrogen and molecular bromine react to partially form hydrogen bromide: H2 (g) + Br2 (g) 2HBr (g) A mixture of 0.682 mol of H2 and 0.440 mol of Br2 is combined in a reaction vessel with a volume of 2.00L. At equilibrium at 700 K, there are 0.546 mol of H2 present. At equilibrium, there are ________ mol of Br2 present in the reaction vessel.

.304

At elevated temperatures, molecular hydrogen and molecular bromine react to partially form hydrogen bromide: H2 (g) + Br2 (g) ⇌ 2 HBr (g) A mixture of 0.682 mol of H2 and 0.440 mol of Br2 is combined in a reaction vessel with a volume of 2.00L. At equilibrium at 700 K, there are 0.546 mol of H2 present. At equilibrium, there are ________ mol of Br2 present in the reaction vessel.

.304

Calculate the concentration (in molarity) of an NaOH solution if 25.0 mL of the solution is needed to neutralize 16.9 mL of a 0.453 M HCl solution.

.306 M

Calculate the concentration (in molarity) of an NaOH solution if 25.0 mL of the solution is needed to neutralize 16.9 mL of a 0.453 M HCl solution.

.3062

the reaction potassium superoxide, KO2, and CO2, is used as a source of O2 and absorber of CO2 in self-contained breathing equipment used by rescue workers how many moles of O2 are produced when .425 mol of KO2 reacts in the fashion

.319 mol O2

calculate the molarity of each of the following solutions. 8.05 g of calcium chloride (CaCl2) in 2.20 x 102 mL of solution:

.330

Calculate the molarity of each of the following solutions. 8.05 g of calcium chloride (CaCl2) in 2.20 × 102 mL of solution:

.330 mol/L

A sample of oxygen gas initially at 0.470 atm is cooled from 21°C to −60°C at constant volume. What is its final pressure (in atm)?

.341 atm

Calculate the molarity of each of the following solutions. 8.84 g of calcium chloride (CaCl2) in 2.20 × 102 mL of solution:

.3621

Calculate the number of moles of cesium in 50.0 g of cesium

.376 mol

A piece of copper with a mass of 218 g has a heat capacity of 83.9 J/°C. What is the specific heat of copper?

.385 J/gC

The reaction between nitric oxide (NO) and oxygen to form nitrogen dioxide (NO2) is a key step in photochemical smog formation: 2NO(g) + O2(g) → 2 NO2(g) How many grams of O2 are needed to produce 1.41 g of NO2?

.490 grams

The reaction 2NO2 → 2NO + O2 follows second-order kinetics. At 300 °C, [NO2] drops from 0.0100 M to 0.00650 M in 100.0 s. The rate constant for the reaction is ________ M-1s-1.

.54

how many moles of aluminum are present in an Al cylinder with a mass of 15g

.556 mol

4.46 moles Ne, .74 moles Ar, 2.15 moles Xe, calculate the partial pressure of each gas Pt = 2.00 atm

.585

calculate the molarity of each of the following solutions. 6.66 g of naphthalene (C10H8) in 85.2 mL of benzene solution:

.610

Calculate the molarity of each of the following solutions. 6.66 g of naphthalene (C10H8) in 85.2 mL of benzene solution:

.610 mol/L

molarity of 17.4 g of sucrose (C12H22O11) in 80.0 mL of solution

.638

Calculate the molarity of each of the following solutions: (b) 17.4 g of sucrose (C12H22O11) in 80.0 mL of solution

.638 M

Calculate the molarity of each of the following solutions. 8.18 g of naphthalene (C10H8) in 85.2 mL of benzene solution:

.7491

.7808 atm .2094 atm .0093 atm .0005 atm .0348 M .00934 M .00041 M 2.2 x10-5

molarity of 18.0 g of ethanol (C2H5OH) in 485 mL of solution

.806

Calculate the molarity of each of the following solutions: (a) 18.0 g of ethanol (C2H5OH) in 485 mL of solution

.806 M

an 6.11g sample of CaCO3(s) absorbs 84J of heat at constant pressure, upon which the temp of the sample increases from 19.2 C to 35.9 C. What is the specific heat of calcium carbonate?

.8232

Calculate the molarity of each of the following solutions: 24.6 g of sucrose (C12H22O11) in 83.0 mL of solution

.8658

Nitric oxide (NO) reacts with oxygen gas to form nitrogen dioxide (NO2), a dark brown gas: 2NO(g) + O2(g) → 2NO2(g) In one experiment, 0.879 mol of NO is mixed with 0.511 mol of O2. Determine which of the two reactants is the limiting reactant. Calculate also the number of moles of NO2 produced. Moles of NO2 produced:

.879 moles

A sample of air occupies 2.70 L when the pressure is 2.20 atm. (a) What volume does the sample occupy at 6.70 atm at the same temperature? (b) What pressure is required in order to compress it to 0.0790 L at the same temperature?

.887 75.2

A sample of air occupies 2.70 L when the pressure is 2.20 atm. (a) What volume does the sample occupy at 6.70 atm at the same temperature?

.890 L

the temperature of a sample of argon gas in a 365 mL container at 740 mmHg and 25C is lowered to 12C. Assuming the volume of the container and the amount of gas is unchanged, calculate the new pressure of the argon

.931 atm

A 2.21-L flexible flask at 15°C contains a mixture of N2, He, and Ne at partial pressures of 0.321 atm for N2, 0.157 atm for He, and 0.455 atm for Ne. (a) Calculate the total pressure of the mixture. (b) Calculate the volume in liters at STP occupied by He and Ne if the N2 is removed selectively.

.933 1.28

.933 atm

Ethyl iodide (C2H5I) decomposes at a certain temperature in the gas phase as follows: C2H5I(g) → C2H4(g) + HI(g) From the following data determine the order of the reaction and the rate constant. Time (min) [C2H5I] (M) 0.0______________2.00 15.0______________1.76 30.0______________1.52 48.0______________1.23 75.0______________0.80 reaction order:

Zn oxidation number

a certain gas expands in volume from 2.0L to 6.0L at constant temperature. Calculate the work done by the gas if it expands a) against a vacuum

oxidation number of As4

oxidation number of Se8

A gas expands from 248 mL to 974 mL at a constant temperature. Calculate the work done (in joules) by the gas if it expands (a) against a vacuum. w =

0 J

When 1.703 g of naphthalene (C10H8) is burned in a constant-volume bomb calorimeter at 298 K, 68.45 kJ of heat is evolved. Calculate ΔU and w for the reaction on a molar basis. w =

0 kJ/mol

at equilibrium ΔQ =

0 kJ/mol

∆Hf of any element is

0 kj/mol

In which of the following aqueous solutions would you expect AgF to have the highest solubility? A) 0.00750 M LiF B) 0.030 M AgNO3 C) 0.023 M NaF D) 0.015 M KF E) AgF will have the same solubility in all solutions.

0.00750 M LiF

AgBr would have the lowest solubility in ________. A) 0.040 M SrBr2 B) pure H2O C) 0.040 M NaBr D) 0.040 M KBr E) 0.010 M AgNO3

0.040 M SrBr2

Consider the reaction: N2(g) + 3H2(g) → 2NH3(g) Suppose that a particular moment during the reaction, molecular hydrogen is reacting at a rate of −0.0600 M/s. At what rate is ammonia being formed?

0.0400 M/s

at 1285C the equilibrium constant for the reaction Br2(g) >< 2Br(g) is k=1.04x10^-3 a .200L vessel containing an equilibrium mixture of the gases has .246g of Br2(g) initially. What is the mass in grams of Br(g) in the vessel at equilibrium

0.0412g

Consider the reaction: A → B The rate of the reaction is 1.6 × 10−2 M/s when the concentration of A is 0.35 M. Calculate the rate constant if the reaction is first order in A.

0.046

0.109 M

The formula for rust can be represented by Fe2O3. How many moles of Fe are present in 25.2 g of the compound?

0.316 mol Fe

Consider the reaction X + Y → Z From the data in the table, obtained at 360 K, determine the overall order of the reaction Initial rate of disappearance of X [X] [Y] 0.053 0.10 0.50 0.127 0.20 0.30 1.02 0.40 0.60 0.254 0.20 0.60 0.509 0.40 0.30 (b) determine the initial rate of disappearance of X when the concentration of X is 0.40 M and that of Y is 0.20 M.

0.34 M/s

Nitric oxide (NO) reacts with oxygen gas to form nitrogen dioxide (NO2), a dark brown gas: 2NO(g) + O2(g) → 2NO2(g) In one experiment, 0.885 mol of NO is mixed with 0.511 mol of O2. Determine which of the two reactants is the limiting reactant. Calculate also the number of moles of NO2 produced. Moles of NO2 produced

0.885 moles

integrated rate laws

0th order reaction: [A]t = -kt + [A]0 1st order reaction: ln[A]t = -kt + ln[A]0 2nd order reaction: 1/[A]t = kt + 1/[A]0

2 ClO2 (aq) + 2 OH- (aq) → ClO3- (aq) + ClO2- (aq) + H2O (l) [ClO2](M) [OH-](M) initial rate 0.06 .030 .0248 0.02 .030 .00276 0.02 .090 .00828 what is the order of the reaction with respect to OH-

How many moles of hydrogen gas would be produced for every mole of magnesium added into the HCl solution?

Balance the following equation and list the coefficients in order from left to right. __ SF4 (s) + __ H2O(l) → __ H2SO3(aq) + __ HF(aq)

1 3 1 4

monoprotic acid

1 proton to donate or accept also only one Ka to worry about

If the H+ ion concentration in an aqueous solution is 0.0010 M, why is it not possible for the OH− ion concentration to be 1.0 × 10^−10 M ?

1.0 x 10^-11 M

how many atoms of He gas are present in a 450 mL container at 35 C and 740 mmHg

1.0 x 10^22

Determine the equilibrium constant (Kp) at 25°C for the reaction CO(g) + H2O(g) CO2(g) + H2(g). ΔG° = -28.5 kJ/mol

1.0 x 10^5

Given that Ea for a certain biological reaction is 48 kJ/mol and that the rate constant is 2.5 × 10-2 s -1 at 15°C, what is the rate constant at 37°C?

1.0 × 10^-1s^-1

Determine the Ksp for magnesium hydroxide (Mg(OH)2) where the solubility of Mg(OH)2 is 1.4 x 10-^4.

1.1 x 10^-11

A certain reaction A → products is second order with respect to A. If it takes 45 min to reduce the concentration of A from 0.350 M to 0.125 M, what is the rate constant for this reaction

1.1 x 10^-1M^-1min^-1

The first-order rate constant for the reaction of methyl chloride (CH3Cl) with water to produce methanol (CH3OH) and hydrochloric acid (HCl) is 3.32 × 10−10 s−1 at 25°C. Calculate the rate constant at 49.3°C if the activation energy is 116 kJ/mol.

1.13 x 10^-8 s-1

How many moles of cobalt (Co) atoms are there in 7.00 × 10^9 (7.00 billion) Co atoms?

1.16 x 10^-14 mol

Cyclobutane decomposes to ethylene according to the equation: C4H8(g) → 2C2H4(g) Determine the value of the rate constant for the reaction based on the following pressures, which were recorded when the reaction was carried out at 430°C in a constant-volume vessel. ______ 1/s Time mmHg 0 400 2000 316 4000 248 6000 196 8000 155 10000 122

1.18 x 10^-4 1/s

Cyclobutane decomposes to ethylene according to the equation: C4H8(g) → 2C2H4(g) Determine the value of the rate constant for the reaction based on the following pressures, which were recorded when the reaction was carried out at 430°C in a constant-volume vessel. Time mmHg 0 400 2000 316 4000 248 6000 196 8000 155 10000 122

1.19 x 10^-4 1/s

A 2.21-L flexible flask at 15°C contains a mixture of N2, He, and Ne at partial pressures of 0.321 atm for N2, 0.157 atm for He, and 0.455 atm for Ne. (b) Calculate the volume in liters at STP occupied by He and Ne if the N2 is removed selectively.

1.28 L

the reaction between ethyl iodide and hydroxide ion in ethanol (alc) solution, C2H5I (alc) + OH-(alc) --> C2H4OH(l) + I-(alc) has an activation energy of 86.8 kJ/mol and a frequency factor of 2.10x10^11 M-1S-1. Predict the rate constant at 25C

1.28 x 10^-4 m-1s-1

Calculate the hydrogen ion concentration in a solution of iced tea with lemon having a pH of 2.87.

1.3 x 10^-3

The annual production of sulfur dioxide from burning coal and fossil fuels, auto exhaust, and other sources is about 26 million tons. The equation for the reaction is S(s) + O2(g) →SO2(g) If 2.68 × 107 tons of sulfur dioxide formed, how many tons of sulfur were present in the original materials? Assume 100% yield.

1.34 x 10^7 tons

Lactic acid (CH3CH(OH)COOH) has one acidic hydrogen. A 0.10 M solution of lactic acid has a pH of 2.44. Calculate Ka.

1.37 x 10^-4

a .10 M solution of chloracetic acid (ClCH2COOH) is 11.0% ionized. Using this information, calculate [ClCH2C00-], [H+], [ClCH2COOH], and the Ka for this equilibrium

1.4 x 10^-3

A man ate 0.552 pound of cheese (an energy intake of 3.50 × 103 kJ). Suppose that none of the energy was stored in his body. What mass (in grams) of water would he need to perspire in order to maintain his original temperature? (It takes 44.0 kJ to vaporize 1 mole of water.) Enter your answer in scientific notation.

1.43 x 10^3g

Calculate the molarity of each of the following solutions. 7.04 g of methanol (CH3OH) in 1.50 × 102 mL of solution:

1.465

the data below refer to the following reaction: 2NO(g) + Br2(g)>< 2NOBr(g) Concentration NO Br2 NOBr initial 2.5 5.0 1.0 equilibrium 2.0 find the concentration of NOBr when the system reaches equilibrium

1.5 M

calculate the molarity of each of the following solutions. 7.31 g of methanol (CH3OH) in 1.50 x 102 mL of solution:

1.52

Calculate the molarity of each of the following solutions. 7.31 g of methanol (CH3OH) in 1.50 × 102 mL of solution:

1.52 mol/L

the solubility of lead (II) chloride (PbCl2) is 1.6 x 10^-2 M. What is the Ksp of PbCl2?

1.64 x 10^-5

Calculate the molarity of each of the following solutions: 34.0 g of ethanol (C2H5OH) in 4.40 × 10^2 mL of solution

1.677

Calculate the molarity of each of the following solutions: (c) 7.95 g of sodium chloride (NaCl) in 79.4 mL of solution

1.71 M

What volume of sulfur dioxide gas at 45 C and 723 mmHg will react completely with .870 L of oxygen gas at constant temperature and pressure? 2SO2(g) + O2(g) -> 2SO3(g)

1.74 L

the molar solubility of Magnesium(II) carbonate is 4.2 x 10^-6 M. What is Ksp for this compound

1.76 x 10^-11

27) Acetic acid is a weak acid that dissociates into the acetate ion and a proton in aqueous solution: HC2H3O2 (aq) >< C2H3O2- (aq) + H+ (aq) At equilibrium at 25 °C a 0.100 M solution of acetic acid has the following concentrations: [HC2H3O2] = .0990M, [C2H3O2-]= 1.33x10^-3 M, and [H+] = 1.33 x10^-3 and The equilibrium constant, Keq, for the ionization of acetic acid at 25 C is ________.

1.79 x 10^-5

The pH of a 0.60 M aqueous solution of formic acid, HCHO2, at 25.0 °C is 1.98. What is the value of Ka for formic acid?

1.8 x 10^-4

the pH of a .60 M aq solution of formic acid, HCHO2, at 25 C is 1.98. What is the value of Ka for formic acid?

1.8 x 10^-4

The "concentration" of water is 55.5 M. Calculate the percent ionization of water.

1.8 x 10^-7

An unknown organic acid has Ka = 5.6 × 10-6. What is the Kb of the conjugate base?

1.8 x 10^-9

A man ate 0.725 pound of cheese (an energy intake of 4.60 × 103 kJ). Suppose that none of the energy was stored in his body. What mass (in grams) of water would he need to perspire in order to maintain his original temperature? (It takes 44.0 kJ to vaporize 1 mole of water.) Enter your answer in scientific notation.

1.88 x 10^3 g

A 45.0−mL sample of 0.513 M glucose (C6H12O6) solution is mixed with 170.0 mL of 2.33 M glucose solution. What is the concentration of the final solution? Assume the volumes are additive.

1.950

2nd order half life

1/ (k[A]0)

The equilibrium constant for reaction 1 is K. The equilibrium constant for reaction 2 is ________. (1) SO2 (g) + (1/2) O2 (g) >< SO3 (g) (2) 2SO3 (g) >< 2SO2 (g) + O2 (g)

1/K^2

describe the graph that shows the correct relationship between concentration and time for a reaction that is second order in [A]?

1/[A] vs time positive

For many years chloroform (CHCl3) was used as an inhalation anesthetic in spite of the fact that it is also a toxic substance that may cause severe liver, kidney, and heart damage. Calculate the percent composition by mass of this compound to four significant figures. The following molar masses should be used in your calculation: H = 1.008 g/mol, C = 12.01 g/mol, Cl = 35.45 g/mol.

10.06% C .8444% H 89.09% Cl

What is the pOH of an aqueous solution at 25.0 °C that contains 2.50 × 10-4 M hydronium ion?

10.4

a certain first order reaction A -> B is 25% composition in 42 min @ 25C. What is the 1/2 life of the reaction?

101.17 minutes

1L x atm is how many J

101.3 J

The variation of the rate constant with temperature for the first-order reaction 2N2O5(g) → 2N2O4(g) + O2(g) is given in the following table. Determine graphically the activation energy in kJ/mol for the reaction. T (K) k(s−1) 298 1.74 × 10−5 308 6.61 × 10−5 318 2.52 × 10−4 328 7.59 × 10−4 338 2.40 × 10−3

103 kJ/mol

angstrom

10^-10

pico

10^-12

centi

10^-2

milli

10^-3

micro

10^-6

nano

10^-9

tera

10^12

kilo

10^3

mega

10^6

giga

10^9

What is the pH of a 0.74 M solution of potassium cyanide (KCN)?

11.3

what is the pH of a .0011M Ca(OH)^2(aq) solution?

11.3

the molarity of an aqueous solution containing 75.3 g of glucose in 35.5 mL of solution is _______ M

11.8

The molarity of an aqueous solution containing 75.3 g of glucose (C6H12O6 ) in 35.5 mL of solution is ________ (mol/L).

11.8M

how many milliliters of concentrated hydrochloric acid solution (36% HCL by mass, density = 1.18 g/ml) are required to produce 20.0L of a solution that has a pH of 2.16?

11.9 mL HCl solution

A sealed 1.0 L flask is charged with 0.500 mol of I2 and 0.500 mol of Br2. An equilibrium reaction ensues: I2 (g) + Br2 (g) 2IBr (g) When the container contents achieve equilibrium, the flask contains 0.84 mol of IBr. The value of Keq is ________.

110

What is the mass of the solid NH4Cl formed when 75.5 g of NH3 is mixed with an equal mass of HCl? What is the volume of the gas remaining, measured at 14.0°C and 752 mmHg? What gas is it? NH3(g) + HCl(g) → NH4Cl(s) What is the mass of the NH4Cl produced? Which gas remains What is the volume of the gas remaining

110.75 g NH3 56.2 L

What is the mass of the solid NH4Cl formed when 75.5 g of NH3 is mixed with an equal mass of HCl? What is the volume of the gas remaining, measured at 14.0°C and 752 mmHg? (a) What gas is it? NH3(g) + HCl(g) →NH4Cl(s) What is the mass of the NH4Cl produced? (b) WHich gas remains? (c) What is the volume of the gas remaining?

110.75g NH3 56.3 L

The average adult male has a total blood volume of 5.0 L. After drinking a few beers, he has a blood alcohol concentration (x grams ethanol /100mL of Blood) of 0.22. What is the mass of alcohol circulating in his blood?

11g

What is the coefficient of H2O when the following equation is properly balanced?

determine the pH of a .35 M solution of CH3NH2 (methylamine). The Kb of methylamine is 4.4x10^-4

12.1

Determine how many grams of each of the following solutes would be needed to make 4.80 × 102 mL of a 0.100 M solution. cesium iodide (CsI)

12.47

Calculate the heat required when 2.50 mol of A reacts with excess B and A2B according to the reaction: 2A + B + A2B → 2AB + A2 Given: 2A + B --> A2B H= -25.0 kJ/mol 2A2B --> 2AB + A2 H= 35.0 kJ/mol

12.5 kJ

Assume the atomic mass of element X is 22.99 amu. A 23.77−g sample of X combines with 131.21 g of another element Y to form a compound XY. Calculate the atomic mass of Y.

126.9 amu

what is the pOH of a 0.1M HNO3 solution?

Calculate the percent ionization of formic acid in a 0.010 M HCOOH solution.(Ka = 1.7 × 10-4)

13%

What is the density (in g/L) of uranium hexafluoride (UF6) at 773 mmHg and 60°C?

13.1 g/L

What is the density (in g/L) of uranium hexafluoride (UF6) at 773 mmHg and 60°C?

13.14 g/L

A small bubble rises from the bottom of a lake, where the temperature and pressure are 8° C and 6.4 atm, to the water's surface, where the temperature is 8° C and the pressure is 1.0 atm. Calculate the final volume (in mL) of the bubble if its initial volume was 2.1 mL.

13.44 mL

Consider the combustion of butane (C4H10): 2C4H10(g) + 13O2(g) → 8CO2(g) + 10H2O(l) In a particular reaction, 3.40 moles of C4H10 are reacted with an excess of O2. Calculate the number of moles of CO2 formed.

13.6 mol CO2

An aqueous solution contains 0.500 M NaOH at 25.0 °C. The pH of the solution is ___________.

13.7

What is the minimum mass of sulfur dioxide necessary to produce 200. g of sulfuric acid in the following reaction? 2SO2 + O2 + 2H2O → 2H2SO4

131 g

Calculate the molar mass of (NH4)2SO4

132.15

Calculate the molar mass of (NH4)2SO4.

132.15 g/mol

what is the molar mass of Freon-11 gas if its density is 6.13 g/L at STP

137 g/mol

Convert 105 mmHg to kilopascals

14.0

Convert 105 mmHg to kilopascals.

14.0 kPa

Determine how many grams of each of the following solutes would be needed to make 4.80 × 102 mL of a 0.100 M solution. potassium dichromate (K2Cr2O7):

14.12

In the first step of the industrial process for making nitric acid, ammonia reacts with oxygen in the presence of a suitable catalyst to form nitric oxide and water vapor. 4 NH3 (g) + 5 O2 (g) → 4 NO (g) + 6 H2O (g) How many liters of NH3 (g) at 850 °C and 5.00 atm are required to react with 1.00 mol of O2 (g) in this reaction?

14.7

Calculate the mass of FeS formed when 9.42 g of iron reacts with 8.50 g of sulfur according to the following reaction. Fe(s) + S(s) → FeS(s)

14.8 grams

Calculate the number of grams of Al in 271 g of Al2O3

143.4

Calculate the molecular mass or formula mass (in amu) of each of the following substances: (a) NaI

149.9 amu

At what temperature (in K) will a reaction become spontaneous? ΔH is 115.0 kJ/mol and ΔS is 75.00 J/K ∙ mol.

1533

Consider the combustion of butane (C4H10): 2C4H10(g) + 13O2(g) → 8CO2(g) + 10H2O(l) In a particular reaction, 4.00 moles of C4H10 are reacted with an excess of O2. Calculate the number of moles of CO2 formed.

16 mol CO2

Calculate the molecular mass or formula mass (in amu) of each of the following substances: (a) CH4

16.04 amu

using the data in the table, estimate the temp at which the free-energy change for the transformation form I2(s) to I2(g) is zero. express the temp in C I2(g) 62.25 kJ/mol 260.57 J/mol*k I2(s) 0 kJ/mol 116.73 J/mol*k

160C

The isomerization of methyl isocyanide, CH3NC → CH3CN, follows first-order kinetics. The half-lives were found to be 161 min at 199°C and 12.5 min at 230°C. Calculate the activation energy for this reaction.

163 kJ/mol

consider the following reactions: 2Mg(s) + O2 (g) --> 2MgO(s) ∆H = -1204 how many grams of MgO are produced during an enthalpy change of -239kJ

16g

The analysis of a compound gives the following percent composition by mass: C: 58.08 percent; H: 10.04 percent; S: 9.123 percent; O: 22.76 percent. What is its molecular formula given that its molar mass is 351.5 g?

17 C atoms 35 H atoms 1 S atoms 5 O atoms

calculate the grams of SO2 gas present at STP in a 5.9 L container

17 g

what is the % comp of N in Ca(NO3)2

17.07%

In an experiment, 0.42 mol of CO (g) and 0.42 mol of H2 (g) were placed in a 1.00-L reaction vessel to yield an equilibrium mixture with gaseous methanol (CH3OH (g)). What is the equilibrium constant (K) for this experiment if there was 0.29 mol of CO (g) remaining at equilibrium?

17.5

Calculate the number of grams of Al in 321 g of Al2O3

170 grams

Calculate the molecular mass or formula mass (in amu) of each of the following substances: K2SO4

174.27 amu

A reaction is experimentally found to follow the rate law, Rate = k[A]2 where k = 0.130 M-1min-1 . Starting with 2.50 M of A, how many seconds will it take for the concentration of A to reach 1.25 M? 1

185s

A reaction is experimentally found to follow the rate law, Rate = k[A]2 where k = 0.130 M-1min-1. Starting with [A]o = 2.50 M, how many seconds will it take for [A]t = 1.25 M?

185s

A reaction is experimentally found to follow the rate law, Rate = k[A]2 where k = 0.130 M1min-1 . Starting with 2.50 M of A, how many seconds will it take for the concentration of A to reach 1.25 M? 1

185s

1.018 g of Freon-113 gas is trapped in a 145 mL container at 760. mmHg and 50.0C. What is the molar mass of Freon-113?

186 g/mol

2 ClO2 (aq) + 2 OH- (aq) → ClO3- (aq) + ClO2- (aq) + H2O (l) [ClO2](M) [OH-](M) initial rate 0.06 .030 .0248 0.02 .030 .00276 0.02 .090 .00828 what is the order of the reaction with respect to ClO2

The pH of a 0.55 M aqueous solution of hypobromous acid, HBrO, at 25.0 °C is 4.48. What is the value of Ka for HBrO?

2.0 x 10^-9

2NaOH + CO2 -> Na2CO3 + H2O a) which reagent is the limiting reactant when 2.02 mol NaOH and 1.1 mol CO2 b) how many moles of Na2CO3 can be produced c) how many moles of the excess reactant remain after the completion of the reaction

2.02 mol NaOH is limiting 1.01 mol NaOH .09 excess mol CO2

what is the mass in grams of a single atom of Sb

2.023 x 10^-22

An aqueous solution of NaF is prepared by dissolving 0.350 mol of NaF in sufficient water to yield 1.0 L of solution. The pH of the solution was 8.93 at 25.0 °C. The Kb of F- is ________.

2.1 x 10^-10

2.2 x 10^-3

The pH of a 0.060 M weak monoprotic acid is 3.44. Calculate the Ka of the acid.

2.2 x 10^-6

What is the concentration of H+ in a 2.5 M HCl solution?

2.5 M

The molar solubility of lead(II) iodate in water is 4.0 × 10^-5 mol/L. Calculate Ksp for lead(II) iodate.

2.6 x 10^-13

Calculate the concentration (in M) of hydroxide ions in a solution at 25.0 °C with a pOH of 3.58.

2.63 x 10^-4

Consider the combustion of carbon monoxide (CO) in oxygen gas: 2CO(g) + O2(g) → 2CO2(g) Starting with 2.85 moles of CO, calculate the number of moles of CO2 produced if there is enough oxygen gas to react with all the CO.

2.85 mol CO2

a solution of KOH in ethanol is made up by dissolving 0.314 KOH in ethanol to form 251.0 mL of solution. Similarly, 1.451 g of C2H5I is dissolved in ethanol to form 251.0mL of solution. Equal volumes of the 2 solutions are mixed. Assuming the rxn is first order, what is the initial rate @ 25C

2.9 x 10^-8

Consider the following reaction: 3A → 2B The average rate of appearance of B is given by Δ[B]/Δt. Comparing the rate of appearance of B and the rate of disappearance of A, we get Δ[B]/Δt = _________ x (Δ[A]/Δt)

2/3

What volume of concentrated nitric acid (15.0 M) is required to make 100. mL of a 3.0 M nitric acid solution?

20 mL

When heated, lithium reacts with nitrogen to form lithium nitride: 6Li(s) + N2(g) → 2Li3N(s) What is the theoretical yield of Li3N in grams when 12.2 g of Li is heated with 33.3 g of N2?

20.4

If 0.86 mole of MnO2 and 43.0 g of HCl react, how many grams of Cl2 will be produced? MnO2 + 4HCl → MnCl2 + Cl2 + 2H2O

20.9 grams

When heated, lithium reacts with nitrogen to form lithium nitride: 6Li(s) + N2(g) → 2Li3N(s) What is the theoretical yield of Li3N in grams when 12.8 g of Li is heated with 34.9 g of N2?

21.4 grams

A quantity of 5.40 × 102 mL of 0.650 M HNO3 is mixed with 5.40 × 102 mL of 0.325 M Ba(OH)2 in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of both solutions is the same at 18.46°C. The heat of neutralization when 1.00 mol of HNO3 reacts with 0.500 mol Ba(OH)2 is −56.2 kJ/mol. Assume that the densities and specific heats of the solution are the same as for water (1.00 g/mL and 4.184 J/g · °C, respectively). What is the final temperature of the solution?

22.8 °C

Methanol (CH3OH) burns in air according to the equation 2CH3OH + 3O2 →2CO2 + 4H2O If 203 g of methanol are used up in a combustion process, what is the mass of H2O produced?

228 grams

If 0.86 mole of MnO2 and 48.3 g of HCl react, how many grams of Cl2 will be produced? MnO2 + 4HCl → MnCl2 + Cl2 + 2H2O

23.5 grams

A quantity of 5.40 × 102 mL of 0.850 M HNO3 is mixed with 5.40 × 102 mL of 0.425 M Ba(OH)2 in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of both solutions is the same at 18.46°C. The heat of neutralization when 1.00 mol of HNO3 reacts with 0.500 mol Ba(OH)2 is −56.2 kJ/mol. Assume that the densities and specific heats of the solution are the same as for water (1.00 g/mL and 4.184 J/g · °C, respectively). What is the final temperature of the solution?

23.8 °C

How many grams of silver nitrate are necessary to react completely with 7.000 moles of copper? Cu + 2 AgNO3 → Cu(NO3 )2 + 2 Ag

2379 g

A quantity of 3.10 × 102 mL of 0.900 M HNO3 is mixed with 3.10 × 102 mL of 0.450 M Ba(OH)2 in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of both solutions is the same at 18.46°C. The heat of neutralization when 1.00 mol of HNO3 reacts with 0.500 mol Ba(OH)2 is −56.2 kJ/mol. Assume that the densities and specific heats of the solution are the same as for water (1.00 g/mL and 4.184 J/g · °C, respectively). What is the final temperature of the solution?

24.5 °C

When heated, lithium reacts with nitrogen to form lithium nitride: 6Li(s) + N2(g) → 2Li3N(s) If the actual yield of Li3N is 5.65 g, what is the percent yield of the reaction?

26.4%

261 g

calculate the heat released (kJ) in the reaction of 3.50 g of acetylene (C2H2) and excess hydrogen gas to form ethane gas: C2H2(g) + 2H2(g) --> C2H6(g) given: 2C2H2(g) +5O2(g) --> 4CO2(g) + 2H2O(g) ΔH = -2320 kJ/mol 2C2H6(g) + 7O2(g) ---> 4CO2(g) + 6H2O(g) ΔH = -3040 kJ/mol 2H2(g) + O2(g) --> 2H2O(g) ΔH = -572 kj/mol

28.5

What is the volume (in liters) occupied by 47.1 g of HCl at STP? Assume ideal behavior.

28.9 L

The isomerization of cyclopropane to form propene is a first-order reaction. At 760 K, 15% of a sample of cyclopropane changes to propene in 6.8 min. What is the half-life of cyclopropane at 760 K? t1/2 =0.693/k

29 min

What is the volume (in liters) occupied by 47.1 g of HCl at STP? Assume ideal behavior.

29.0 L

at elevated temps, nitrogen dioxide decomposes to nitrogen oxide and oxygen: NO2(g) --> NO(g) + 1/2 O2(g). The reaction is second order in NO2 with a rate constant of .543 M-1S-1 at 300C. If the initial [NO2] is 0.260 M, it will take _____s for the concentration to drop to .050M

29.7 s

Calculate the pressure exerted by 4.13 moles of molecular chlorine confined in a volume of 2.15 L at 32°C. The van der Waals constants for Cl2 are a = 6.49 atm · L2/mol2 and b = 0.0562 L/mol.P = atmCompare the pressure with that calculated using the ideal equation.

29.94 The pressure calculated using the van der Waals equation is smaller than the pressure calculated using the ideal gas equation.

Hsolid sodium peroxide (Na2O2) reacts with liquid water yielding aqueous sodium hydroxide and oxygen gas how much heat is released when 250.0 L of oxygen gas is produced from the reaction of sodium peroxide and water if the reaction is carried out in an open container at 1.00 atm pressure and 25C? Given ΔHf [Na2O(s)] = -510.9 kJ/mol ΔHf [NaOH(aq)] = -469.2 kJ/mol ΔHf [H2O(l)] = -285.8 kj/mol

2900 kJ

Write the net ionic equation for the reaction between AgNO3(aq) and Na2SO4(aq). Be sure to include states of matter in your answer.

2Ag+(aq) + SO4^2-(aq) -> Ag2SO4(s)

Write the net ionic equation for the reaction between AgNO3(aq) and Na2SO4(aq). Be sure to include states of matter in your answer.

2Ag^+(aq)+SO4^2-(aq)->Ag2SO4(s)

Identify the major ionic species present in an aquesous solution of K2SO4

2K+ SO4 2-

Predict what happens when a potassium phosphate (K3 PO4 ) solution is mixed with a calcium nitrate [Ca(NO3 )2 ] solution. Write a net ionic equation for the reaction.

2PO4 + 3Ca --> Ca3(PO4)2

Which ions remain in solution, unreacted, after each of the following pairs of solutions is mixed? ammonium phosphate and calcium chloride

2PO4 + 3Ca --> Ca3(PO4)2

Consider the reaction X + Y → Z From the data in the table, obtained at 360 K, determine the overall order of the reaction Initial rate of disappearance of X [X] [Y] 0.053______0.10____0.50 0.127_______0.20____0.30 1.02_________0.40____0.60 0.254______0.20_____0.60 0.509______0.40_____0.30 (a) determine the overall order of the reaction

What is the coefficient of H2O when the equation below is properly balanced?___ PCl3(l) + ___ H2O(l) → ___ H3PO3(aq) + ___ HCl(aq)

what is the coefficient of H2So4 when the following equation is properly balanced Ca3(PO4)2 + H2SO4 -> CaSO4 + H3PO4

Calculate the pH of (a) a 1.0×10−3 M HCl solution and (b) a 0.020 M Ba(OH)2 solution.

3 12.60

what is the ph of 1 x 10^-3 M hydronium ion what is OH

3 1x10^-11 (or pH 11?)

The concentration of iodide ions in a saturated solution of lead (II) iodide is ________ M. The solubility product constant of PbI2 is 1.4 x 10^-8

3.0 x 10^-3

The concentration of iodide ions in a saturated solution of lead (II) iodide is ________ M. The solubility product constant of PbI2 is 1.4x10^-8.

3.0 x 10^-3

consider the decomposition of ammonium chloride at a certain temp. NH4Cl(s) >< NH3(g) + HCl(g) calculate the equilibrium constant Kp if the total pressure is 6.10 atm at the temp

3.05 atm

what is the molar solubility of CaF2 in .010 M Ca(NO3)2? Ksp = 3.9 x 10^-11

3.1 x 10^-5

What mass of Na2SO4 is needed to prepare 350. mL of a solution having a sodium ion concentration of 0.125M?

3.11 g

What mass of Na2SO4 is needed to prepare 350. mL of a solution having a sodium ion concentration of 0.125M?

3.11g

The molar solubility of magnesium carbonate is 1.8 × 10^-4 mol/L. What is Ksp for this compound?

3.2 x 10^-8

The equation for the metabolic breakdown of glucose (C6H12O6) is the same as the equation for the combustion of glucose in air: C6H12O6(s) + 6O2(g) → 6CO2(g) + 6H2O(l) Calculate the volume of CO2 produced at 37°C and 1.00 atm when 3.83 g of glucose is used up in the reaction.

3.24 L

The equation for the metabolic breakdown of glucose (C6H12O6) is the same as the equation for the combustion of glucose in air: C6H12O6(s) + 6O2(g) → 6CO2(g) + 6H2O(l) Calculate the volume of CO2 produced at 37 °C and 1.00 atm when 3.83 g of glucose is used up in the reaction.

3.25 L

The rate constant of a first-order process that has a half-life of 3.50 min is ________ s-1.

3.30x10^-3

What is the magnitude of k for a first-order reaction at 75.0 °C if Ea= 95.1 kj/mol and rate constant is 1.35 × at 25.0 °C?

3.36 x10^4

What mass of Li3PO4 is needed to prepare 500. mL of a solution having a lithium ion concentration of 0.175 M?

3.38

Calculate the pH of a carbonated beverage in which the hydrogen ion concentration is 3.4 × 10-4 M.

3.47

Calculate the number of atoms in 0.245 g of potassium (K).

3.77 x 10^21

What is the pOH of a solution in which [H+]=9.1×10^−11 M?

3.96

Calculate the pressure exerted by 4.13 moles of molecular chlorine confined in a volume of 2.15 L at 32°C. The van der Waals constants for Cl2 are a = 6.49 atm · L^2/mol^2 and b = 0.0562 L/mol.

30 atm

calculate the molar mass of a gaseous substance if 0.125g of the gas occupies 93.3 mL at STP.

30.0 g/mol

A mixture of three gases has a total pressure of 1,380 mmHg at 298 K. The mixture is analyzed and is found to contain 1.27 mol CO2, 3.04 mol CO, and 1.50 mol Ar. What is the partial pressure of CO2?

302 mmHg

When heated, lithium reacts with nitrogen to form lithium nitride: 6Li(s) + N2(g) → 2Li3N(s) If the actual yield of Li3N is 6.49 g, what is the percent yield of the reaction?

31.8%

Calculate the molecular mass or formula mass (in amu) of each of the following substances: Ca3(PO4)2

310.18

What volume (mL) of a 0.3428 M HCl(aq) solution is required to completely neutralize 23.55 mL of a 0.2350 M Ba(OH)2(aq) solution?

32.39 mL

Calculate the mass in grams of iodine (I2) that will react completely with 22.9 g of aluminum (Al) to form aluminum iodide (AlI3).

323.1 g I2

Calculate the mass in grams of iodine (I2) that will react completely with 23.2 g of aluminum (Al) to form aluminum iodide (AlI3).

327 grams I2

Calculate the mass in grams of iodine (I2) that will react completely with 23.3 g of aluminum (Al) to form aluminum iodide (AlI3).

329 grams I2

A 22.0 g block of copper at 45°C absorbs 2.50 kJ of heat. Given the specific heat of Cu is 0.385 J/g·°C what will be the final temperature of the Cu?

340 C

NH3(g) + HCl(g) --> NH4Cl(s) Given the following table of thermodynamic data, determine the temp (C) above which reaction is nonspontaneous NH3(g) -46.19 kJ/mol 192.5 J/mol*K HCl(g) -92.30 kJ/mol 186.69 J/mol*K NH4Cl(s) -314.4 kJ/mol 94.6 J/mol*K

345C

from the data for the 1st order gas phase isomerization of CH3NC @ 215C, graph and calculate the 1st order rate constant and 1/2 life for the reaction times pressure 0 502 2000 335 5000 180 8000 95.5 12000 41.7 15000 22.4

3465 seconds or 3418 seconds

ammonia reacts with oxygen to form nitric oxide and water vapor: 4NH3 + 5O2 --> 4NO + 6H2O when 20.0 g NH3 and 50.0 g O2 are allowed to react, what is the limiting?

35.24 grams NH3

When acetaldehyde (CH3CHO) at a pressure of 364 mmHg is initially introduced into an evacuated 500. mL flask at 518°C, the half-life for the second-order decomposition process is 410 s. CH3CHO (g) → CH4 (g) + CO (g) What will the total pressure in the flask be after 1.00 hour?

37 mmHg

calculate the standard enthalpy change for the following: Mg(OH)2 (s) --> MgO(s) + H2O (l)

37.06

the normal boiling point of methanol is 64.7 C and the molar enthalpy of vaporization if 71.8kJ/mol. The value of ΔS wjem 1.75 mol of CH3OH(l) vaporizes at 64.7 C is ____ J/k

372 J/K???

The rate constant of a first-order reaction is 2.65 × 10−4 s−1 at 350.°C. If the activation energy is 137 kJ/mol, calculate the temperature at which its rate constant is 8.90 × 10−4 s−1.

380C

Fermentation is a complex chemical process of wine making in which glucose is converted into ethanol and carbon dioxide: C6H12O6 → 2C2H5OH + 2CO2 Starting with 754.5 g of glucose, what is the maximum amount of ethanol in grams and in liters that can be obtained by this process (density of ethanol = 0.789 g/mL)?

385.9 g .489 L

Identify the correct net ionic equation for the reaction that occurs when solutions Na3PO4 and Ca(NO3)2 mix

3Ca2+(aq) + 2PO43-(aq) -> Ca3(PO4)2(s)

identify the correct net ionic equation for the reaction that occurs when solutions when solutions of Na3PO4 and Ca(NO3)2 are mixed

3Ca^2+(aq) + 2PO4^3-(aq) --> Ca3(PO4)2(s)

balance the following equation KOH + H3PO4 --> K3PO4 + H2O

3KOH + H3PO4 --> K3PO4 + 3 H2O

One cup of fresh orange juice contains 134 mg 9 of ascorbic acid (vitamin C, C6H8O6 ). Given that one cup = 255.8 mL, calculate the molarity of vitamin C in orange juice.

3x10^-3 M

Determine [H+] in a solution where [OH-] = 2.3 × 10^−5 M.

4.3 x 10^-10

The Ka of hypochlorous acid (HClO) is 3.0 x10-8 at 25.0 °C. Calculate the pH of a 0.0385 M hypochlorous acid solution.

4.47

the activation energy for the following reaction is 60 kJ/mol Sn^2+ + 2CO^3+ --> Sn^4+ + 2CO^2+ by what factor will the rate constant increase when the temp is raised from 10C to 28 C

4.6

Determine how many grams of each of the following solutes would be needed to make 4.80 × 102 mL of a 0.100 M solution. sulfuric acid (H2SO4)

4.708

If the pressure of a gas sample is tripled and the absolute temperature is quadrupled, by what factor will the volume of the sample change?

4/3

sodium carbonate can be made by heating sodium bicarbonate 2NaHCO3(s) --> Na2CO3(s)+ CO2(g) + H2O(g) given that ΔH = 128.9 kJ/mol and ΔG = 33.1 kJ/mol at 25 C, above what minimum temp will the reaction become spontaneous under state conditions

401K

what is the theoretical yeild of H2O that can be obtained from the reaction of 4.5 grams H2 and excess O2

40g

The thermal decomposition of acetaldehyde, CH3CHO → CH4 + CO, is a second-order reaction. The following data were obtained at 518°C. Time,s Pressure CH3CHO2 mmHg 0 364 42 330 105 290 720 132 Based on the data given, what is the half-life for the disappearance of acetaldehyde?

410

A sample of oxygen gas has a volume of 302 mL at 35°C. The gas is heated to 151ºC at constant pressure in a container that can contract or expand. What is the final volume of the oxygen gas?

416 mL

The density of a gaseous organic compound is 3.28 g/L at 44.0°C and 1.95 atm. What is its molar mass?

43.8 g/mol

Ammonium nitrite undergoes decomposition to produce only gases as shown below. NH4NO2(s) → N2(g) + 2H2O(g) How many liters of gas will be produced by the decomposition of 22.1 g of NH4NO2 at 525°C and 1.5 atm?

45 L

Calculate the molecular mass or formula mass (in amu) of each of the following substances: (b) NO2

46.01 amu

What mass of C12H22O11 (sucrose) is needed to prepare 255 mL of a 0.570 M solution of sucrose in water?

49.8 g

A 15.0 L cylinder contains 4.0 g of hydrogen and 28 g of nitrogen. If the temperature is 27°C what is the total pressure of the mixture in kPa?

498 kPa

ion: Mass number: 4 Protons: 2 Neutrons: electrons: 0

4He 2

The OH- concentration in a 2.5 × 10-3 M Ba(OH)2 solution is

5.0 x 10^-3

Determine how many grams of each of the following solutes would be needed to make 4.80 × 102 mL of a 0.100 M solution. sodium carbonate (Na2CO3):

5.088

The enthalpy of combustion of benzoic acid (C6H5COOH) is commonly used as the standard for calibrating constant-volume bomb calorimeters; its value has been accurately determined to be −3226.7 kJ/mol. When 2.7117 g of benzoic acid are burned in a calorimeter, the temperature rises from 21.84°C to 26.67 °C. What is the heat capacity of the bomb? (Assume that the quantity of water surrounding the bomb is exactly 2250 g.)

5.42 kJ/°C

what is the pH of a .023 M solution of HCN. (Ka = 4.9x10^-10)?

5.47

Calculate the pOH for a solution with [H3O+] = 3.1 x 10-9 M.

5.49

A modern penny weighs 2.5500 g but contains only 0.0585 g of copper (Cu). How many copper atoms are present in a modern penny?

5.54 x 10^20 Cu atoms

[A](M) [B](M) initial rate 0.451 .885 1.13 0.451 1.77 1.13 1.35 .855 10.17 the magnitude of this rate constant is

5.56

Calculate the H+ ion concentration in a 8.8 × 10-4 M Ca(OH)2 solution.

5.7 x 10^-12

how many moles of chloride ions are in .255g of aluminum chloride

5.737 x 10^-3 mol Cl

the rate constant for a particular zero order reaction is 0.075 ms-1. if the initial concentration of reaction is 0.537 M it takes _______s for the concentration to decrease to .100 M

5.8 secands

Calculate the density of Br2 (g) at 59.0°C and 1.00 atm pressure.

5.83 g/L 1.41

A modern penny weighs 2.7150 g but contains only 0.0615 g of copper (Cu). How many copper atoms are present in a modern penny?

5.83 x 10^20 Cu atoms

the equilibrium constant for the reaction 2NO(g) + Br2(g) >< 2NOBr(g) is k = 2.0x10^-2 at certain temps 2. calculate K1 for 2NOBr(g) >< 2NO(g) + Br2(g)

the equilibrium constant Kp is 209 at a certain temp. calculate Po2 if PNO = .503 atm and PNO2 = .259 atm. K = 209 2NO2 >< 2NO(g) + O2(g)

55.4

what is the theoretical yield of ammonia that can be obtained from the reaction of 10g H2 and excess N2? N2 + 3h2 -> 2NH3

56.3 g

refer to the (unbalanced) equation CS2 + CaO -> CO2 + CaS How many grams of CaO are required to react completely with 38 grams of CS2

56g CaO

The rate at which tree crickets chirp is 2.20 × 102 per minute at 27°C but only 41.9 per minute at 6.5°C. From these data, calculate the activation energy for the chirping process.

57 kJ/mol

The pH of a 0.15 M aqueous solution of NaBrO (the sodium salt of HBrO) is 10.7. What is the Ka for HBrO?

6.0 x 10^-9

what is the # of molecules in 1x10^-6 mol CH3CH2OH

6.022 x 10^17 molecules

Enter your answer in the provided box. The enthalpy of combustion of benzoic acid (C6H5COOH) is commonly used as the standard for calibrating constant-volume bomb calorimeters; its value has been accurately determined to be −3226.7 kJ/mol. When 3.4737 g of benzoic acid are burned in a calorimeter, the temperature rises from 20.84°C to 26.67°C. What is the heat capacity of the bomb? (Assume that the quantity of water surrounding the bomb is exactly 2250 g.)

6.33 kJ/°C

Calculate the molar solubility of CaF2 in a 0.25 M solution of NaF(aq). (Ksp (CaF2) = 4.0 x 10^-11)

6.4 x 10^-10

What is the mass in grams of a single atom of He?

6.647 x 10^-24 grams

Consider the chemical reaction 2NH3(g) >< N2(g) + 3H2(g) The equilibrium is to be established in a 1.0 L container at 1,000 K, where Kc = 4.0 × 10^-2. Initially, 1,220 moles of NH3(g) are present. Estimate the equilibrium concentration of N2(g).

6.8 M

The first-order decomposition, A → products, has a rate constant of 0.150 s-1 . Starting with an initial concentration of A = 0.350 M, how much time is required to leave 0.125 M of A remaining?

6.86s

the value of ΔH for the reaction below is -126 kJ. _________kJ are released when 2 mol of NaOH is formed in the reaction. 2Na2O2(s) + 2H2O(l) --> 4NaOH(s) + O2(g)

63 kJ

The atomic masses of the two stable isotopes of copper, 63Cu29 (69.17 percent) and 65Cu29 (30.83 percent), are 62.9296 amu and 64.9278 amu, respectively. Calculate the average atomic mass of copper.

63.55 amu

What is the pressure of the sample of gas trapped in the open-tube mercury manometer shown below if atmospheric pressure is 736 mmHg and h = 9.2 cm?

644 mmHg

In alcohol fermentation, yeast converts glucose to ethanol and carbon dioxide: C6H12O6(s) → 2C2H5OH(l) + 2CO2(g) If 7.75 g of glucose are reacted and 1.44 L of CO2 gas are collected at 293 K and 0.984 atm , what is the percent yield of the reaction?

67.3%

68.5%

Calculate the density of Ar(g) at -264°C and 1.42 bar

69.7 g/L

Determine the number of atoms of each element in the empirical formula of a compound with the following composition: 65.08 percent C, 10.14 percent H, 24.77 percent O.

7 C atoms 13 H atoms 2 O atoms

How would you prepare 70.0 mL of 0.400 M HNO3 from a stock solution of 4.00 M HNO3? What volume (in mL) of the 4.00 M HNO3 solution will you need?

7.00

How would you prepare 70.0 mL of 0.400 M HNO3 from a stock solution of 4.00 M HNO3? What volume (in mL) of the 4.00 M HNO3 solution will you need?

7.00 mL

A gas at 847 mmHg and 31°C occupies a volume of 7.05 L. Calculate its volume at STP.

7.03

A gas at 847 mmHg and 31°C occupies a volume of 7.05 L. Calculate its volume at STP.

7.06 L

the equilibrium constant for the reaction 2NO(g) + Br2(g) >< 2NOBr(g) is k = 2.0x10^-2 at certain temps 3. calculate k2 for NOBr(g) >< NO(g) + 1/2 Br2(g)

7.07

The base-dissociation constant, Kb, for an unknown base is 1.4x10-9. The acid-dissociation constant, Ka, for the conjugate ion is ________.

7.1 x 10^-6

What is the concentration (in M) of hydronium ions in a solution at 25.0 °C with pH = 4.146?

7.15 x 10^-5

) For the reaction BrO3 - (aq) + 5 Br- (aq) + 6H+ → 3 Br2 + 3H2O at a particular time, ∆[𝐵rO3^−]/∆𝑡 = - 1.5 × 10-2 M/s. What is ∆[𝐵r−] ∆𝑡 at the same instant?

7.5 x 10^-2 M/s

Determine how many grams of each of the following solutes would be needed to make 4.80 × 102 mL of a 0.100 M solution. potassium permanganate (KMnO4):

7.58

A second-order reaction has a half-life of 18 s when the initial concentration of reactant is 0.71 M. The rate constant for this reaction is ________ M-1s-1.

7.8 x10^2

time: 0.0 5.0 10.0 15.0 20.0 [A] (M): 0.2 0.14 0.10 .071 .040 What is the rate constant (s-1) for this reaction?

7.8 x10^2

The reaction of 60.0 g of aluminum oxide with 30.0 g of carbon produced 22.5 g of aluminum. What is the percent yield for this reaction? Al2O3 + 3C → 2Al + 3CO

70.9%

The reaction of 60.0 g of aluminum oxide with 30.0 g of carbon produced 22.5 g of aluminum. What is the percent yield of Al (s) for this reaction? Al2O3 (s) + 3C (s) → 2Al (s) + 3CO (g)

70.9%

The distinctive odor of vinegar is due to acetic acid, CH3COOH, which reacts with sodium hydroxide in the following fashion: CH3COOH(aq) + NaOH (aq) → H2O(l) + NaC2H3O2 (aq) If 3.85 mL of vinegar needs 42.0 mL of 0.115 M NaOH to reach the equivalence point in a titration, how many grams of acetic acid are in a 1.00 qt sample of this vinegar?

71 g acidic acid

A sample of air occupies 2.70 L when the pressure is 2.20 atm. (b) What pressure is required in order to compress it to 0.0790 L at the same temperature?

75.0 atm

what is the mass % of chloride ions in .255 g aluminum chloride

76.76% Cl-

Assume the atomic mass of element X is 22.99 amu. A 67.98−g sample of X combines with 236.26 g of another element Y to form a compound XY. Calculate the atomic mass of Y.

79.81 amu

The reaction A + 2B → products has the rate law, rate = k[A][B]^3 . If the concentration of B is doubled while that of A is unchanged, by what factor will the rate of reaction increase?

a 3.682 gram sample of KClO3 is dissolved in enough water to give 375 mL of solution. what is the chlorate ion concentration in this solution

8.01 x 10-2 M

A 20.00 mL sample of 0.1015 M nitric acid is introduced into a flask, and water is added until the volume of the solution reaches 250. mL. What is the concentration of nitric acid in the final solution?

8.12 x 10^-3

The half-life of a first-order reaction is 13 min. If the initial concentration of reactant is .085 M, it takes _______ min for it to decrease to 0.055 M.

8.2

Calculate the pH of a 0.24 M sodium formate solution (HCOONa).

8.58

Calculate the number of atoms in 0.564 g of potassium (K).

8.69 x 10^21 atoms

A gas-filled balloon having a volume of 3.70 L at 1.25 atm and 26°C is allowed to rise to the stratosphere (about 30 km above the surface of the Earth), where the temperature and pressure are −44°C and 4.00 × 10−3 atm, respectively. Calculate the final volume of the balloon.

8.86 x 10^2

8.86 x 10^2 L

The density of water is 1.00 g/mL at 4°C. How many water molecules are present in 2.66 mL of water at this temperature?

8.89 x 10^22 molecules

Industrially, vanadium metal, which is used in steel alloys, can be obtained by reacting vanadium(V) oxide with calcium at high temperatures: 5Ca + V2O5 5CaO + 2V In one process, 1.540 ×10^3 g of V2O5 react with 2.000 × 103 g Ca. Calculate the theoretical yield of V

862.6 grams

Industrially, vanadium metal, which is used in steel alloys, can be obtained by reacting vanadium(V) oxide with calcium at high temperatures: 5Ca + V2O5 → 5CaO + 2V In one process, 1.540 × 103 g of V2O5 react with 2.030 × 103 g Ca. (a) Calculate the theoretical yield of V.

863 9/18

At 900.0 K, the equilibrium constant (Kp) for the following reaction is 0.345. 2SO2 (g) + O2(g) 2SO3 (g) At equilibrium, the partial pressure of SO2 is 36.9 atm and that of O2 is 16.8 atm. The partial pressure of SO3 is ________ atm.

88.8

At 900.0 K, the equilibrium constant (Kp) for the following reaction is 0.345. 2SO2 (g) + O2(g) >< 2SO3 (g) At equilibrium, the partial pressure of SO2 is 36.9 atm and that of O2 is 16.8 atm. The partial pressure of SO3 is ________ atm.

88.8

89.61%

Ammonia is a principal nitrogen fertilizer. It is prepared by the reaction between hydrogen and nitrogen. 3H2(g) + N2(g) → 2NH3(g) In a particular reaction, 6.00 moles of NH3 were produced. How many moles of H2 and how many moles of N2 were reacted to produce this amount of NH3?

9.00 mol H2 3.00 mol N2

Consider the formation of nitrogen dioxide from nitric oxide and oxygen: 2 NO(g) + O2(g) → 2 NO2(g) If 9.03 L of NO is combined with excess O2 at STP, what is the volume in liters of the NO2 produced?

9.03 L

Consider the formation of nitrogen dioxide from nitric oxide and oxygen:2 NO(g) + O2(g) → 2 NO2(g)If 9.03 L of NO is combined with excess O2 at STP, what is the volume in liters of the NO2 produced?

9.03 L

The enthalpy of combustion of benzoic acid (C6H5COOH) is commonly used as the standard for calibrating constant-volume bomb calorimeters; its value has been accurately determined to be −3226.7 kJ/mol. When 2.7031 g of benzoic acid are burned in a calorimeter, the temperature rises from 20.84°C to 24.67°C. What is the heat capacity of the bomb? (Assume that the quantity of water surrounding the bomb is exactly 2250 g.)

9.23 kJ/°C

How many milliliters of a stock solution of 6.0 M HNO3 (aq) would you have to use to prepare 110 mL of a 0.500 M HNO3 (aq)

9.2x10^-3

The Goodyear blimp contains 5.74×106 L of helium at 25°C and 1.00 atm. What is the mass in grams of the helium inside the blimp?

9.32 x 10^5 g Hg

Sulfur hexafluoride SF6 is a colorless and odorless gas. Due to its lack of chemical reactivity, it is used as an insulator in electronic equipment. Calculate the pressure (in atm) exerted by 1.82 moles of the gas in a steel vessel of volume 5.43 L at 69.5° C.

9.42 atm

A man ate 0.370 pound of cheese (an energy intake of 2350 kJ). Suppose that none of the energy was stored in his body. What mass (in grams) of water would he need to perspire in order to maintain his original temperature? (It takes 44.0 kJ to vaporize 1 mole of water.) Enter your answer in scientific notation.

9.62 x 10^2 g

Determine the pH of a 0.055 M solution of an unknown weak base: (Kb = 9.1 × 10^-8).

9.85

90.08%

93.5

Predict the value of ΔHof (greater than, less than, or equal to zero) for these elements at 25°C: Br2(l)

Predict the value of ΔHof (greater than, less than, or equal to zero) for these elements at 25°C: Br2(g)

how many grams of Cl2 can be prepared from the reaction of 16 grams MnO2 and 30 grams HCl MnO2 + 4HCl -> MnCl2 + Cl2 + 2H2O

???

A sample of iron absorbs 81.0 J of heat, upon which the temperature of the sample increases from 19.7 ℃ to 28.2℃ If the specific heat of iron is 0.450 J/g-K, what is the mass (in grams) of the sample? A) 21.2 g B) 4.29 g C) -21.2 g D) 0.0472 g E) 3.83 g

AgBr would have the lowest solubility in _____. A) 0.040 M SrBr2 -> 0.08 M Br B) pure H2O C) 0.040 M NaBr -> 0.04 M Br D) 0.040 M KBr -> 0.04 M Br E) 0.010 M AgNO3 -> 0.01 Ag+

CH3OH (l) decomposes into carbon monoxide and hydrogen gas in the presence of heat. How much heat is consumed when 5.75 g of CO (g) is formed? ΔH° = +128.1 kJ. A) 26.3 kJ B) 23.3 kJ C) 62.0 kJ D) 162 kJ E) 8.3 kJ

Given the data in the table below, ΔH°rxn for the reaction 4NH3 (g) + 5O2 (g) → 4NO (g) + 6H2O (l) is ________ kJ. A) -1172 B) -150 C) -1540 D) -1892 E) The ΔH°f of O2 (g) is needed for the calculation.

Given the following reactions Fe2O3 (s) + 3CO (s) → 2Fe (s) + 3CO2 (g) ΔH = -28.0 kJ 3Fe (s) + 4CO2 (s) → 4CO (g) + Fe3O4 (s) ΔH = +12.5 kJ the enthalpy of the reaction of Fe2O3 with CO 3Fe2O3 (s) + CO (g) → CO2 (g) + 2Fe3O4 (s) is ________ kJ. A) -59.0 B) 40.5 C) -15.5 D) -109 E) +109

Given the following reactions N2 (g) + 2O2 (g) → 2NO2 (g) ΔH = 66.4 kJ 2NO (g) + O2 (g) → 2NO2 (g) ΔH = -114.2 kJ the enthalpy of the reaction of the nitrogen to produce nitric oxide N2 (g) + O2 (g) → 2NO (g) is ________ kJ. A) 180.6 B) -47.8 C) 47.8 D) 90.3 E) -180.6

Given the following table of thermodynamic data, complete the following sentence. The vaporization of H2O2 (l) is ________. H2O2(g) H: -136.3 S: 232.6 H2O2(l) H: -187.8 S: 110 A) nonspontaneous at low temperature and spontaneous at high temperature B) spontaneous at low temperature and nonspontaneous at high temperature C) spontaneous at all temperatures D) nonspontaneous at all temperatures E) not enough information given to draw a conclusion

How many joules of heat are absorbed when the temperature of a 13.9 g sample of CaCO3 (s) increases from 21.7 ℃ to 33.3 ℃ Specific heat of calcium carbonate is 0.82 J/g-K . A) 130 J B) 0.68 J C) s-130 J D) -0.68 J E) 9.5 J

How many kJ of heat are released when 15.75 g of Ba (s) reacts completely with oxygen gas to form BaO (s)? ΔH° = -1107 kJ. A) 63.5 kJ B) 20.8 kJ C) 114 kJ D) 70.3 kJ E) 35.1 kJ

Of the following, ΔH°f is not zero for ________. A) Sc (g) B) Si (s) C) P4 (s, white) D) Br2 (l) E) Ca (s)

The temperature of a 24.3 g sample of gold increases from 23.7 ℃ to 31.5℃ If the specific heat of gold is 0.129 J/g-K. How many joules of heat are absorbed? A) 24.5 J B) 0.0414 J C) -24.5 J D) 0.293 J E) 1.01 J

For a given process at constant pressure, w is positive. This means that the process involves ________. A) work being done by the system on the surroundings B) work being done by the surroundings on the system C) no work being done D) an equal amount of work done on the system and by the system E) work being done against a vacuum

For which one of the following reactions is ΔH°rxn equal to the heat of formation of the product? A) N2 (g) + 3H2 (g) → 2NH3 (g) B) (1/2)N2 (g) + O2 (g) → NO2 (g) C) 6C (s) + 6H (g) → C6H6 (l) D) P (g) + 4H (g) + Br (g) → PH4Br (l) E) 12C (g) + 11H2 (g) + 11O (g) → C6H22O11 (g)

The enthalpy change for the following reaction is -483.6 kJ: 2H2 (g) + O2 (g) → 2H2O (g) Therefore, the enthalpy change for the following reaction is ________ kJ. 4H2 (g) + 2O2 (g) → 4H2O (g) A) -483.6 B) -967.2 C) 2.34 × 105 D) 483.6 E) 967.2

The value of ΔG° at 373 K for the oxidation of solid elemental sulfur to gaseous sulfur dioxide is ________ kJ/mol. At 298 K, ΔH° for this reaction is -269.9 kJ/mol, and ΔS° is +11.6 J/K. A) -300.4 B) -274.2 C) -4,597 D) +300.4 E) +4,597

The value of ΔU for a system that performs 151 kJ of work on its surroundings and loses 79 kJ of heat is ________ kJ. A) +230. B) -230. C) +72 D) -72 E) -151

When a system ________, ΔU is always negative. A) absorbs heat and does work B) gives off heat and does work C) absorbs heat and has work done on it D) gives off heat and has work done on it E) None of the above is always negative.

Which one of the following statements regarding Kw is false? A) pKw is 14.00 at 25 °C. B) The value of Kw is always 1.0 × 10-14. C) Kw changes with temperature. D) The value of Kw shows that water is a weak acid. E) Kw is known as the ion product of water.

ΔS is positive for the reaction ________. A) Pb(NO3 )2 (aq) + 2KI(aq) → PbI2 (s) + 2KNO3 (aq) B) 2H2O (g) → 2H2 (g) + O2 (g) C) H2O (g) → H2O (s) D) NO (g) + O2 (g) → NO2 (g) E) Ag⁺ (aq) + Cl⁻ (aq) → AgCl (s)

which chemical equation is consistent with these dat? A increasing at a faster rate B decreasing

B --> 2A

Hydrogen and iodine gas react to produce hydrogen iodide gas. What is the value of for this reaction if at equilibrium the concentrations of , , and HI were and respectively?

B. 34

) The value of ΔH° for the reaction below is -790 kJ. The enthalpy change accompanying the reaction of 0.95 g of S is ________ kJ. 2S (s) + 3O2 (g) → 2SO3 (g) A) 23 B) -23 C) -12 D) 12 E) -790

A- is a weak base. Which equilibrium corresponds to the equilibrium constant Ka for HA? A) HA (aq) + H2O (l) ⇌ H2A+ (aq) + OH- (aq) B) A- (aq) + H3O+ (aq) ⇌ HA (aq) + H2O (l) C) HA (aq) + H2O (l) ⇌ H3O+ (aq) + A- (aq) D) A- (aq) + H2O (l) ⇌ HA (aq) + OH- (aq) E) A- (aq) + OH- (aq) ⇌ HOA2- (aq)

Given the data in the table below, ΔH°rxn for the reaction 2SO2 (g) + O2 (g) → 2SO3 (g) is ________ kJ. A) -99 B) 99 C) -198 D) 198 E) The ΔH°f of O2 (g) is needed for the calculation.

Given the following table of thermodynamic data, complete the following sentence. The vaporization of Ti is ________. Substance: TiCl4(g) TiCl4(1) Delta Hf (kJ/mol) -763.2 -804.2 S (J/mol*K) -804.2 221.9 A) spontaneous at all temperatures B) spontaneous at low temperature and nonspontaneous at high temperature C) nonspontaneous at low temperature and spontaneous at high temperature D) nonspontaneous at all temperatures E) not enough information given to draw a conclusion

In which one of the following solutions is silver chloride the most soluble? A) 0.200 M HCl B) 0.750 M LiNO3 C) 0.0150 M NH3 D) 0.185 M KCl E) pure H2O

Which of the following aqueous solutions has the lowest [OH-]? A) a solution with a pH of 3.0 B) a 1 × 10^-4 M solution of HNO3 C) a solution with a pOH of 12.0 D) pure water E) a 1 × 10-3 M solution of NH4Cl

Which of the following gases has the largest entropy at 25℃ and 1 atm? A) Cl2 B) F2 C) I2 D) Br2 E) O3

Which one of the following processes produces a decrease of the entropy of the system? A) dissolving sodium chloride in water B) sublimation of naphthalene C) dissolving oxygen in water D) boiling of alcohol E) explosion of nitroglycerine

which one of the following equations represents the ionization of a weak monoprotic acid in water A. CN-(aq) + H2O(aq) ⇌ HCN(aq) + OH-(aq) B. HCN(aq) + OH-(aq) ⇌ H2O(l) + CN+(aq) C. HCN(aq) + H2O(l) ⇌ H3O+(aq) + CN-(aq) D. HCN(aq) + NH3(aq) ⇌ HN4CN(aq) E. HCN(aq) + OH-(aq) ⇌ H2O(l) + CN-(aq)

Δ S is positive for the reaction ________. A) Pb(NO3)2 (aq) + 2KI(aq) → PbI2 (s) + 2KNO3 (aq) B) H2O (g) → H2O (s) C) 2H2O (g) → 2H2 (g) + O2 (g) D) NO (g) + O2 (g) → NO2 (g) E) Ag+ (aq) + Cl- (aq) → AgCl (s)

ΔS is positive for the reaction ________. A) CaO (s) + CO2 (g) → CaCO3 (s) B) N2 (g) + 3H2 (g) → 2NH3 (g) C) 2SO3 (g) → 2SO2 (g) + O2 (g) D) Ag⁺ (aq) + Cl⁻ (aq) → AgCl (s) E) H2O (l) → H2O (s)

A compound with an empirical formula of C2H4Br has a molar mass of 215.90 g/mol. What is the molecular formula?

C4H8Br2

methanol (CH3OH) is used as a fuel in race cars write the balanced equation for the combustion of liquid methanol in air

CH3OH(l) + 3/2O2(g) ---> CO2(g) + 2H2O(l)

Consider the following two acids and their ionization constants: HCOOH ...... Ka=1.7×10^−4 HCN ............... Ka=4.9×10^−10 Which conjugate base (HCOO− or CN−) is stronger?

CN-

cyanide

CN-

given the following Ka values, which anion is the strongest base acid.......................Ka HF......................... 7.1 x 10^-4 HCOOH........... 1.7x10^-4 HCN...................... 4.9 x 10^-10 HNO2................... 4.5x10^-4 CH3COOH........ 1.8x10^-5

CN-

Which ions remain in solution, unreacted, after each of the following pairs of solutions is mixed? potassium carbonate and magnesium sulfate

CO3 + Mg --> MgCO3

carbonate

CO3 2-

insoluble compounds

CO32-, PO43-, CrO42-, S2-, OH-

Given the following Ka values, which anion is the strongest base? Acid........................Ka H2CO3................. 4.2x10^-7 HCO3-................. 4.8x10^-11 H2C2O4.............. 6.5 10^-2 HC2O4-................6.1 x 10^-5 H2PO4-................6.2 x 10^-8

CO3^2-

Vanadium(V) oxide reacts with calcium according to the chemical equation below. When 10.0 moles of V2O5 are mixed with 10.0 moles of Ca, which is the limiting reagent?V2O5(s) + 5Ca(l) → 2V(l) + 5CaO(s)

Give the formula of calcium phosphate

Ca3(PO4)2

CaCO3 (s) + HCl(aq) ->>

CaCl2(aq) + CO2(g) + H2O(l)

Formula..................................Ksp CdCO3..................................5.2 x 10^-12 Cd(OH)2...............................2.5 x 10^-14 CaF2.......................................3.9 x 10^-11 AgI..........................................8.3 x 10^-17 ZnCO3..................................1.4 x 10^-11 which compound listed above has the greatest molar solubility in water

CaF2

Identify the reducing agent in the following chemical reaction. Cd(s) + NiO2 (s)+ 2H2O(l) → Cd(OH)2 (aq)+ Ni(OH)2 (aq)

Cd(s)

atomic number 17 (Cl)

Chlorine

atomic number 24 (Cr)

Chromium

which ions remain in solution, unreacted, after each of the following pairs of solutions is mixed potassium carbonate and magnesium sulfate

Co3 + Mg -> MgCO3

Of the acids in the table below, ________ is the strongest acid. A) HCHO2..............1.8 x 10^-5 B) HOAc..................1.8 x 10^-4 C) HClO..................3.0 x 10^-8 D) HF........................6.8 x 10^-4 E) HOAc and HCHO2

The value of ΔS° for the catalytic hydrogenation of acetylene to ethene, C2H2 (g) + H2 (g) → C2H4 (g) is ________ J/K∙ mol. A) +18.6 B) +550.8 C) +112.0 D) -112.0 E) -18.6

Which of the following ions will act as a weak base in water? A) OH- B) Cl- C) NO3 - D) ClO- E) None of the above will act as a weak base in water.

Which of the following is a statement of the first law of thermodynamics? A) Ek = ½ mv² B) A negative ΔH corresponds to an exothermic process. C) ΔU = Ufinal - Uinitial D) Energy lost by the system must be gained by the surroundings. E) 1 cal = 4.184 J (exactly)

Which of the following reactions would have a negative ΔS? A) NH4Cl (s) → NH3 (g) + HCl (g) B) PbCl2 (s) → Pb2+ (aq) + 2Cl- (aq) C) 2C (s) + O2 (g) → 2CO2 (g) D) 2SO2 (g) + O2 (g) → 2 SO3 (g) E) H2O (l) → H2O (g)

Which reaction will shift to the reactants in response to a decrease in volume? (4 Pts) A) 2 HI (g) ⇌ H2 (g) + I2 (g) B) H2 (g) + Cl2 (g) ⇌ 2 HCl (g) C) N2 (g) + 3 H2 (g) ⇌ 2 NH3 (g) D) 2 SO3 (g) ⇌ 2 SO2 (g) + O2 (g) E) 4 Fe (s) + 3 O2 (g) ⇌ 2 Fe2O3 (s)

for the following reaction at equilibrium, which gives a change that will shift the position of equilibrium to favor formation of more products? 2NOBr(g) >< 2NO(g) + Br2(g) ΔH= 30 kJ/mol a) remove NOBr selectively b) increase the total pressure by decreasing the volume c) lower the temperature d) remove Br2 e) add more NO

which of these species has the highest entropy (S) at 25C a) CH3OH(l) b) H2O(l) c) Ni(s) d) CO (g) e) MgCo3(s)

The second-order rate constant has been measured at different temperatures for the decomposition of nitrous oxide (N2O) into a nitrogen molecule and an oxygen atom. k(1/M · s) _____T(°C) 1.87 × 10−3 ___600.0 0.0113 _________650.0 0.0569 _______700.0 0.244 _________750.0 Determine the activation energy for the reaction.

Ea = 241.2 kJ/mol

first law of thermodynamics

Energy can be transferred and transformed, but it cannot be created or destroyed.

strong acids

HCl, HBr, HI, HNO3, H2SO4, HClO3, HClO4

list the 6 strong acids

HCl, HBr, HI, HNO3, H2SO4, HClO4

Of the following acids, ________ is a strong acid. HNO2 H2CO3 HNO3 HClO HF

HNO3

Which of the following compounds is a strong acid? HNO3 CH3CO2H HNO2 HClO2 NaOH

HNO3

monohydrogen phosphate

HPO4 2-

In which of the following species does the sulfur atom have the lowest oxidation number? HS− SO2 SO3

HS-

In which of the following species does the sulfur atom have the lowest oxidation number? HS− SO2 SO3

HS-

hydrogen sulfate

HSO4 -

atomic number 1 (H)

Hydrogen

atomic number 82 (Pb)

Lead

Soluble Compounds

Li+, Na+, K+, NH4+, NO3-, C2H3O2-, HCO3-, ClO3-, ClO4-, Cl-, Br-, I-, SO42-

strong bases

LiOH, NaOH, KOH, RbOH, CsOH, Ca(OH)2, Sr(OH)2, Ba(OH)2

Concerning the rate law, Rate = k[A][B], what are appropriate units for the rate constant k?

M^-1 s^-1

atomic number 12 (Mg)

Magnesium

atomic number 25 (Mn)

Manganese

atomic number 80 (Hg)

Mercury

oxidation numbers in MnO4-

Mn +7 O -2

Assign oxidation numbers to all elements in the following compound and ion: (b)MnO4-

Mn: +7 O: -2

oxidation number of MnO4^-

Mn: +7 O: -2

permanganate

MnO4 -

In the following chemical reaction the oxidizing agent is 5 H2O2 + 2MnO4 - + 6H+ → 2Mn2+ + 8H2O + 5O2

MnO4-

balance the following equation N2 + H2 --> NH3

N2 + 3H2 --> 2NH3

N2O5

oxidation number of NF3

N: +3 F: -1

Using the data in the table, which of the conjugate acids below is the weakest acid? NH3.................................... 1.8 x 1o^-5 C5H5N..............................1.7 x 10^-9 H2NOH.............................1.1 x 10^-8 NH2CH2CH3.................4.2 x 10^-4

NH3CH2CH3+

Which substance is acting as a Brønsted acid in the following reaction? HSO4-(aq) + NH4+ (aq) → H2SO4 (aq) + NH3(aq)

NH4

Ammonium

NH4+

Which of the following does not fit the definition of a Brønsted Base? CO32- NH3 H2O NH4+ HCO3-

NH4+

wite the balanced net ionic equation for the following reaction? identify the spectator ions?

NH4+, SO4+ = spectators 2Cr^3+ + 3CO3^2- --> Cr3(CO3)3

label the acid, base, conjugate acid, and conjugate base for the following reaction NHO3 + H2O ⇌ H3O + NO3

NHO3: acid H2O: base H3O: conjugate acid NO3: conjugate base

nitric oxide (NO) reacts with O2 to form NO2 2NO + O2 -> 2NO2. In one experiment .877 mol of NO is mixed with .509 mol O2. What is the limiting reactant

PCH4 = 2.72 atm PC2H6 = .301 atm PC3H8 = .180 atm

atomic number 19 (K)

Potassium

Classify the following compounds as weak acids (W) or strong acids (S): hydrobromic acid hydrochloric acid hydrofluoric acid

SSW

atomic number 21 (Sc)

Scandium

chemical analysis of a gaseous compound showed that it contained 33% silicon and 67% F by mass. At 35C, .210 L of the compound exerted a pressure of 1.7 atm. if the mass of .210 L of the compound was 2.38g, calculate the molecular form of the compound

Si2F6

Determine the empirical formula of a compound containing 2.06 g of silicon and 10.4 g of chlorine.

SiCl4

Determine the empirical formula of a compound containing 3.61 g of silicon and 18.2 g of chlorine.

SiCl4

Determine the empirical formula of a compound containing 3.81 g of silicon and 19.2 g of chlorine.

SiCl4

atomic number 47 (Ag)

Silver

atomic number 11 (Na)

Sodium

Which of the following processes always results in an increase in the energy of a system? The system loses heat and does work on the surroundings. The system gains heat and has work done on it by the surroundings. The system loses heat and has work done on it by the surroundings. The system gains heat and does work on the surroundings. None of these is always true.

The system gains heat and has work done on it by the surroundings.

give the relationship between [H+] and [OH-] if a solution is neutral

[H+] = [OH-]

give the relationship between [H+] and [OH-] if a solution is acidic

[H+] > [OH-]

ph =

[H+] @ equilibrium or -log[H+]

Which of the following expressions is the correct equilibrium-constant expression for the reaction below? (NH4)2Se (s) ⇌ 2 NH3 (g) + H2Se (g)

[NH3]^2 [H2Se] / [(NH4)2Se]

Which of the following expressions is the correct equilibrium-constant expression for the reaction below? (NH4)2Se (s) 2NH3 (g) + H2Se (g)

[NH3]^2[H2Se]

Which of the following expressions is the correct equilibrium-constant expression for the equilibrium between dinitrogen tetroxide and nitrogen dioxide? N2O4 (g) >< 2NO2 (g)

[NO2]^2/[N2O4]

what is the acid dissociation constant for the following equation: NHO3 + H2O ⇌ H3O + NO3

[NO3][H3O]/[HNO3]

equilibrium constant equation

[products]/[reactants]

which acid is stronger? HA 1x10^-4 HA 1x10^-6

^-4

combustion reaction

a chemical reaction that occurs when a substance reacts with oxygen, releasing energy in the form of heat and light

consider the following reaction at equilibrium 2SO2(g) + O2(g) >< 2SO3(g) ΔH = -99kJ. La Chatelier's principle predicts that a(n) decrease in temp will result in ______.

a decrease in the partial pressure of SO3 a decrease in Keq no changes in equilibrium partial pressure an increase in the partial pressure of O2 an increase in partial pressure of SO3

empirical formula

a formula that shows the simplest whole number ratio of elements in compounds

transition state

a high-energy intermediate state of the reactants during a chemical reaction that must be achieved for the reaction to proceed

what is pH

a method of reporting hydrogen ion concentration at equilibrium

If Ksp < Q

a precipitate will form

if Q > K

a precipitate will form

decomposition reaction

a reaction in which a single compound breaks down to form two or more simpler substances (C --> A+B)

neutralization reaction

a reaction in which an acid and a base react in an aqueous solution to produce a salt and water (HB(aq) + COH(aq) --> H2O(l) + CB(aq))

precipitation reaction

a reaction in which an insoluble substance forms and separates from the solution (AB(aq) + CD(aq) --> AD(s) + CB(aq))

displacement reaction

a reaction in which one element replaces a similar element in a compound (A + BC --> AC + B)

metathesis reaction

a reaction that involves the exchange of parts between two compounds (AB(aq) + CD(aq) --> AD(aq) + CB(aq) )

nonelectrolyte

a solution that does not conduct electricity

mechanism

a step by step view of the change of reactants to products

base

a substance that, when dissolved in water, increases the concentration of hydroxide ions

acid

a substance that, when dissolving in water, increases the concentration of hydrogen ions

Calculate the solubility in g/L of AgBr in (a) pure water and (b) 0.0026 M NaBr.

a. .00016 g/L b. 5.6 x 10^-8 g/L

consider the following reaction at equilibrium 2SO2(g) + O2(g) >< 2SO3(g) ΔH = -99kJ. La Chatelier's principle predicts that a(n) decrease in temp will result in ______. a decrease in the partial pressure of SO3 a decrease in Keq no changes in equilibrium partial pressure an increase in the partial pressure of O2 an increase in partial pressure of SO3

an increase in partial pressure of SO3

calculate the pH of a strong acid pH of a 0.1 M solution of HCl? HCl + H2O ⇌ H3O + Cl-

assume [HCl] = [H3O] pH = 1

2 ClO2 (aq) + 2 OH- (aq) → ClO3- (aq) + ClO2- (aq) + H2O (l) [ClO2](M) [OH-](M) initial rate 0.06 .030 .0248 0.02 .030 .00276 0.02 .090 .00828 what is the order of the reaction with respect to OH-

balance the chemical equation 2NH4NO3 -> N2 + O2 + H2O

balance the chemical equation 2NH4NO3 -> 2N2 + O2 + 4H2O

the passage of electricity through an electrolyte solution is caused by the movement of

both cations and anions

Which of the following statements is true? A) Processes that are spontaneous in one direction are spontaneous in the opposite direction. B) Processes are spontaneous because they occur at an observable rate. C) Spontaneity can depend on the temperature. D) All of the statements are true.

suppose dry air near sea level has the following composition by volume: N2, 78.08 percent; O2, 20.94 percent; Ar, 0.93 percent; CO2, 0.05 percent. If the atmospheric pressure is 1.000 atm, calculate the partial pressure of each gas in atm. Calculate the concentration of each gas in moles per liter at 0°C.

cN2 = .03484 M cO2 = .00934 M cAr = .00041 M cCO2 = 2 × 10 ^-5 M

open system

can exchange matter and energy with its surroundings

insoluble compounds key

carbonates, phosphates, chromates, sulfides, and hydroxides

reaction rates depend on the presence of a ________

catalyst

ΔG

change in free energy

There are two stable isotopes of chlorine: chlorine-35, with a mass of 34.968853 amu; and chlorine-37, with a mass of 36.965903. Given that the average atomic mass of a chlorine atom is 35.45 amu, which of the following statements is true?

chlorine contains more 35/17 Cl than 37/17 Cl.

constant pressure

coffee cup calorimeter

example of endothermic

cold pack

molecules can only react if they

collide with each other

The rate of a reaction depends on ________.

collision frequency collision energy collision orientation

identify the redox reaction S + 3F2 → SF6

combination

integrated rate law is determined from

data of concentration as time proceeds

arrhenius equation is determined from

data of rate constant and different temps

identify the redox reaction 2CuCl → Cu + CuCl2

decomposition disproportionate

as OH increases, H

decreases

what is rate law determined by

determined from data of rates @ different reaction concentrations

heterogeneous equilibrium

different state/phase

identify the redox reaction 2Ag + PtCl2 → 2AgCl + Pt

displacement

1) Which one of the following is not a valid expression for the rate of the reaction below? 4NH3 + 7O2 → 4NO2 + 6H2O a. -1/7 (Δ[O2]/Δt) b. 1/4 (Δ[NO2]/Δt) c. 1/6 (Δ[H2O]/Δt) d. -1/4 (Δ[NH3]/Δt) e. all of the above

Which of the following statements is true? A) Q does not change with temperature. B) Keq does not change with temperature, whereas Q is temperature dependent. C) K does not depend on the concentrations or partial pressures of reaction components. D) Q does not depend on the concentrations or partial pressures of reaction components. E) Q is the same as Keq when a reaction is at equilibrium.

conducts electricity

electrolyte

oxidizing agent

electron acceptor

reducing agent

electron donor

liquid water to gaseous water

endothermic

q + A >< B

endothermic

solid water to liquid water

endothermic

kinetic energy

energy associated with motion

thermal energy

energy associated with the random motions of atoms and molecules

energy barrier

energy needed to initiate a chemical reaction

chemical energy

energy stored within the structural units of chemical substances

Q=K

equilibrium

A reaction with an equilibrium constant Kc = 1.5 x 10^21 would consist of which of the following at equilibrium:

essentially all products

surroundings

everything that lies outside the system being studied

closed system

exchanges energy but not matter with the surroundings

A>< B + q

exothermic

consider the following reactions: 2Mg(s) + O2 (g) --> 2MgO(s) ∆H = -1204 is the reaction exothermic or endo thermic

exothermic

gaseous water to liquid water

exothermic

liquid water to solid water

exothermic

Q<K

forward reaction proceeds to form more products

increasing entropy

gas > liquid > solid

when a system ________, ΔU is always negative

gives off heat and does work

basic ph

greater than 7

spontaneous

having no external cause, acting on impulse

monoprotic strong acid

having one hydrogen ion

-q

heat flows from system to the surroundings

heat flows from the surroundings to the system

∆ enthalpy

heat of reaction (∆H)

example of exothermic

heat pack

hexa

two types of equilibrium

homogeneous and heterogeneous

chemical equations

how chemists represent chemical reactions on paper

what does rate law tell you

how fast a reaction is

HBr

hydrobromic acid

HCl

hydrochloric acid

reaction rate generally ________ with increased temperature

increases

the entropy of the universe _______ in any spontaneous process

increases

relationship between reactant concentration and reaction rate

increasing reactant concentration generally increases reaction rate

The rate law of the overall reaction A + B → C is rate = k[A]2. Which of the following will not increase the rate of the reaction?

increasing the concentration of reactant B

Which one of the following changes would alter the rate constant (k) for the reaction 2A + B → products?

increasing the temperature

Which one of the following changes would alter the rate constant (k) for the reaction 2A + B → products? increasing the concentration of A increasing the temperature increasing the concentration of B measuring k again after the reaction has run for a while

increasing the temperature

molecular formula

is a formula that shows the element symbol and exact # of each types of atom in a molecular compound

what does it mean that water is amphoteric

it is able to react both as a base and an acid

@ 100C the equilibrium constant for the reaction COCl2(g) >< CO(g) + Cl2(g) has the value k = 2.19 x10^-10. Are the following mixtures of COCl2, CO, and Cl2 @ 100C at equilibrium? If not, indicate the direction that the reaction must proceed to achieve equilibrium based on the following. [COCl2] = 2.00x10^-3 M, [CO] = 3.3x10^-6 M, [Cl2] = 6.62x10^-6 M

k = 2.19x10^-10 Q>K the reaction will proceed left to attain equilibrium

a closed system initially containing 1.00x10^-3 M H2 and 2.00x10^-3 M I2 at 448C is allowed to reach equilibrium. Analysis of the equilibrium mixture shows that the concentration of HI is 1.87x10^-3 M. Calculate Kc at 448C for the reaction taking place, which is H2(g) + I2(g) >< 2HI(g)

k = 51

assuming the frequency factor and activation energy do not change as a function of temp, calculate the rate constant for the reaction @ 50C

k2 = 1.898 x 10^-8 M-1S-1

where does the entropy term of a reaction come to play

molecules often collide without forming products

nona

C12H22O11 is a _____ electrolyte

nonelectrolyte

Identify each of the following substances as a strong electrolyte, weak electrolyte, or nonelectrolyte: (e) C12H22O11

nonelectrolyte

does not conduct electricity

nonelectrolyte

atomic number

number of protons

octa

how do we measure pH

one way to measure pH is with a pH meter another way is calorimetrically with indicators

weak electrolyte

partially dissociates in water

Bronsted-Lowry base

proton acceptor

bronsted base

proton acceptor

Bronsted acid

proton donor

Bronsted-Lowry acid

proton donor

0 order rate

rate = -k

2nd order rate

rate = k[A]^2

Chlorine dioxide reacts in basic water to form chlorite and chlorate according to the following chemical equation: 2 ClO2(aq) + 2OH- (aq) → ClO2 - (aq) + ClO3 - (aq) + H2O(l) A kinetic study of this reaction under a certain set of conditions yielded the data below. Exp # [ClO2]M [OH-]M Initial rate(M/s) 1 0.0500 0.100 5.75x10^-2 2 0.100 0.100 2.30x10^-1 3 0.100 0.0500 1.15x10^-1 Which one of the following is the rate law for this reaction?

rate = k[ClO2]^2[OH-]

Use the following data to determine the rate law for the reaction shown below. 2 NO (g) + H2(g) → N2O (g) + H2O (g) Exp # [NO]M [H2]M Initial rate(M/min) 1 0.021 0.065 1.46 2 0.021 0.260 1.46 3 0.042 0.065 5.84

rate = k[NO]^2

The data below were determined for the reaction shown below. S2O8^2- + 3I^- (aq) → 2SO4^2- + I^3- Exp # [S2O8^2-] [I-] Initial Rate 1 0.038 0.060 1.4x10^-5 M/s 2 0.076 0.060 2.8x10^-5 M/s 3 0.076 0.030 1.4x10^-5 M/s The rate law for this reaction must be:

rate = k[S2O8^2-][I^-]

rate constant

arrhenius equation relates

rate constant and temp

non spontaneous

reaction requires a sustained input of energy

if Q>k

reaction shifts left

if K>Q

reaction shifts right

The van der Waals equation is a modification of the ideal gas equation. What two factors does this equation account for?

real gas molecules exert forces on each other gas molecules have volume

H2 + CH2=CH2 ->> CH3CH3 name the reducing agent, oxidizing agent, species being reduced, and species being oxidized

reducing agent: H2 oxidizing agent: CH2=CH2 species being reduced: CH2=CH2 species being oxidized: H2

identify the reducing and oxidizing agents and determine the species that is oxidized and the species that is reduced. Mg + Fe2+ --> Mg2+ + Fe

reducing agent: Mg Oxidizing agent: Fe2+ species being reduced: Fe2+ species being oxidized: Mg

Mg + Fe2+ -> Mg 2+ + Fe name the reducing agent, oxidizing agent, species being reduced, and species being oxidized

reducing agent: Mg oxidizing agent: Fe 2+ species being reduced: Fe2+ species being oxidized Mg

identify the reducing and oxidizing agents and determine the species that is oxidized and the species that is reduced. Cu2+ + Sn --> Sn2+ + Cu

reducing agent: Sn Oxidizing agent: Cu2+ species being reduced: Cu2+ species being oxidized: Sn

Cu 2+ + Sn -> Sn 2+ + Cu name the reducing agent, oxidizing agent, species being reduced, and species being oxidized

reducing agent: Sn oxidizing agent: Cu2+ species being reduced: Cu2+ species being oxidized: Sn

Q>K

reverse reactions proceeds to form more reactions

less

root ite

homogeneous equilibrium

same state/phase

what is it called when a solution that is in equilibrium with undissolved solute

saturated

Identify the following compounds as a weak or strong acid or base: NaOH

strong base

identify the following compounds as a weak or strong acid or base: NaOH

strong base

Ca(OH)2

strong base (calcium hydroxide)

CsOH

strong base (cesium hydroxide)

LiOH

strong base (lithium hydroxide)

NaOH

strong base (sodium hydroxide)

Identify each of the following substances as a strong electrolyte, weak electrolyte, or nonelectrolyte: (b) KCl

strong electrolyte

Identify each of the following substances as a strong electrolyte, weak electrolyte, or nonelectrolyte: (c) HNO3

strong electrolyte

KCl is a _____ electrolyte

strong electrolyte

the larger Ka the ________ the acid

stronger

weaker the acid, the __________ the conjugate base

stronger

factors that affect reaction rate

temp frequency of collisions orientation of molecules energy needed for the reaction to take place (Ea)

___________ is the only time that you are changing the free energy difference between the products and reactants... thus changing the equilibrium constant (k)

temperature change

tetra

actual yield

the amount it actually produces

integrated rate law relates

the concentration of the reactants to time

solubility product constant

the equilibrium expression for a chemical equation representing the dissolution of a slightly to moderately soluble ionic compound

activation energy (Ea)

the initial energy needed to start a chemical reaction

theoretical yield

the maximum amount of product that can be made based on the limiting reagent

Write the reaction rate expressions for the reaction below in terms of the disappearance of the reactants and the appearance of products. Give the expressions for the disappearance of the reactants first, in the order written in the chemical equation. Then write the expressions for the appearance of the products in the order written in the chemical equation. Write the expressions in order of appearance in the equation in the form. ±(1/X) × (Δ[Α]/Δt) where ± is either a plus OR a minus sign, not both, X is an integer, and A is a chemical species. Do not include the state of matter. 2H2(g) + O2(g) → 2H2O(g)

the rate = -(1/2) x Δ[H2]/Δt -(1/1) x Δ[O2]/Δt +(1/2) x Δ[H2O]/Δt

arrhenius noted...

the relationship between activation energy and temp

strong bases are...

the soluble hydroxides, which are the alkali metal and heavier alkaline earth metal hydroxides

Which is more acidic: a solution where [H+]=2.5×10^−3 M or a solution where pOH=11.6?

the solution with pOH = 11.6

rate reaction

the speed at which reactions take place

chemical kinetics

the study of reaction rate

formula weight

the sum of the atomic weights of the atoms in the chemical formula of the substance

if Q = K

the system is at equilibrium and the solution is saturated

which way does the equilibrium lie in the following reaction and why CH3CO2H(aq) + H2O(l) ⇌ H3O(aq) + CH3CO2-(aq)

to the left acetate us a stronger base than H2O, so the equilibrium favors the left side

which way does the equilibrium lie in the following reaction and why HCl(aq) + H2O(l) -> H3O+ + Cl-(aq)

to the right H2O is a much stronger base than Cl-, so the equilibrium lies far to the right (K >> 1)

True or False, At the same temperature and pressure, Cl2(g) molecules will have an overall slower average molecular speed than H2(g) molecules.

true

True or False: H2O is acting like a Bronsted Acid in the following reaction NH3 + H2O -><- NH4+ OH-

true

Identify the following compounds as a weak or strong acid or base: HCOOH

weak acid

identify the following compounds as a weak or strong acid or base: H3PO4

weak acid

identify the following compounds as a weak or strong acid or base: HCOOH

weak acid

ka = 1x10-3

weak acid

CH3COOH

weak acid (acetic acid)

H2PO4

weak acid (phosphoric acid)

Identify the following compounds as a weak or strong acid or base: NH3

weak base

H2O is a ___ electrolyte

weak electrolyte

Identify each of the following substances as a strong electrolyte, weak electrolyte, or nonelectrolyte: (a) H2O

weak electrolyte

arrhenius equation tells you

what is the rate constant at a given temp

integrated rate law tells you

what the concentration is at a particular time

when does chemical equilibrium occur

when a reaction and its reverse reaction proceed at the same time

Suppose a 50.0 g block of silver (specific heat = 0.2350 J/g·°C) at 100°C is placed in contact with a 50.0 g block of iron (specific heat = 0.4494 J/g·°C) at 0°C, and the two blocks are insulated from the rest of the universe. The final temperature of the two blocks

will be lower than 50C

what is the molar solubility of CaF2 (Ksp = 4x10^-11) in .25M NaF?

x = 6.4 x 10^-10

rate of reaction = k[A]^x[B]^y

xth order in a yth order in b (x+y)th order overall

does a precipitate form when .1L of 8.0 x 10^-3 M Pb(NO3)2 is added to .40L of 5.0 x 10^-3 M Na2SO4? Ksp = 6.3 x 10^-7 (PbSO4) Ksp = 1 x 10^3 (NaNO3)

yes

which of the following is consistent with a reaction that proceeds spontaneously in the reverse direction (assume all variables are in terms of the forward direction only)

ΔG > 0, Q>K

methanol (CH3OH) is used as a fuel in race cars calculate the standard enthalpy change for the combustion reaction assuming that H2O is a product CH3OH(l) + 3/2O2(g) ---> CO2(g) + 2H2O(l)

ΔH = -726.5 kJ/mol

When 1.531 g of naphthalene (C10H8) is burned in a constant-volume bomb calorimeter at 298 K, 61.54 kJ of heat is evolved. Calculate ΔU and w for the reaction on a molar basis.

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