semester 2 final chem

355

Calculate delta H for the reaction IF5 (g) --> IF3 (g) + F2 (g) delta H = Given these thermochemical equations: IF (g) + F2 (g) --> IF3 (g) delta H= -390 kJ IF (g) + 2F2 (g) --> IF5 (g) delta H = -745 kJ

gases

Pressure has an appreciable affect on the solubility of ____________ in liquids

1.8 x 10^-10

The pH of a solution was measured to equal 9.75. Determine the [H3O+].

-579.9 kJ

The value of delta H° for the reaction below is -482 kJ. Calculate the heat (kJ) released to the surroundings when 38.5 g of O2 (g) reacts with excess CO. 2CO (g) + O2 (g) 2CO2 (g)

hydrogen gas

When an acid reacts with a metal, what is one of the usual products?

0.10 m Na2SO4

Which of the following aqueous solutions will have the highest boiling point? 0.10 m Na2SO4 0.20 m glucose 0.25 sucrose 0.10 NaCl 0.10 m SrSO4

contains dissolved solute in equilibrium with undissolved solute

a saturated solution _____________

aromatic hydrocarbons are not very stable

all are true about aromatic hydrocarbons except: the structure has a 6 carbon ring many of the compounds have notable odors a circle or ring is typically placed inside a hexagon to represent alternating single and double bonds aromatic hydrocarbons are not very stable many polycyclic aromatic hydrocarbons make outstanding dyes

more separated, less

as a solid element melts, the atoms become ________________ and they have ______________ attraction for one another

decreases

as temperature increases, solubility of gases in liquids

NaCl

of the following, a 0.2 M aqueous solution of ____________ will have the highest freezing point (NH40PO4 Pb(NO3)2 Na3PO4 Mg(NO3)2 NaCl

F2

of the following, delta h of fusion is not zero for O2 (G) C (Graphite) N2 (G) F2 (S) Cl2 (G)

13.04

what is the pH of a 0.055 M Ba(OH)2

vinegar

which of the following is not a colloid? jello fog milk shaving cream vinegar

kekule

which of these scientists is credited with the discovery of carbon's tendency toe form four bonds? wohler lewis kekule dalton bohr

H2O (l) and K2SO4 (aq)

A neutralization reaction between KOH (aq) and H2SO4 (aq) would give which two products?

[H3O+] < [OH-]

In order for a solution to be basic:

CH4

Of the following, _______________ is the most volatile CBr4 CCl4 CF4 CH4 C6H14

0.60

The mole fraction of He in a gaseous solution prepared from 4.0 of He, 6.5 g of Ar, and 10.0 g of Ne is _______________

23.4

The vapor pressure of pure water at 25C is 23.8 torr. what is the capor pressure (torr) of water above a solution prepared by dissolving 18.0 g of glucose ( a non electrolyte, MW = 180.0 g/mol) in 95.0 g of water?

london dispersion forces

What is the predominant intermolecular force in CBr4

75.9kJ

calculate the enthalpy change associated with the conversion of 25.0 grams of ice at -4.00 C to water vapor at 110.0 C. the specific heat of ice, water, and steam are 2.09 J/g-K, 4.18 J/g-K, and 1.84 J/g-K, respectively. for H2), delta Hfus = 6.01 kj/mol and delta Hvap = 40.67 kJ/mol

-1.37 C

calculate the freezing point of a solution containing 15.0 grams of CaCl2 and 550 grams of water

alkynes

hydrocarbons containing carbon-carbon triple bonds are called ____________

alkanes

hydrocarbons containing only single bonds between the carbons atoms are called

13

if the [H+] in a solution is 1.0 x 10^-1 mol/L what is the [OH-]

basic

if the hydrogen ion concentraion is 10^-10M what class is it

1

if the hydrogen ion concentration is 1.0 x 10^-13M what is the pOH of the solution

2

if the hydroxide ion concentration is 1.0x10^-12M what is the pH of the solution

equal to [OH-]

in a neutral solution the h+ is

the point of neutralization has been reached

in a titration, when the number of moles of hydrogen ions equals the number of moles of hydroxide ions, what is said to have happened?

released

in an exothermic reaction, is heat released or absorbed?

179.6 J

iron metal has a specific heat of 0.449 J/(g*C). How much heat is transferred to a 5.00 g piece of iron, initially at 20.0 C when it is placed in a pot of boiling water? Assume that the temperature of the water is 100.00 C and that the water remains at this temperature, which is the final temperature of the iron

extreme brittleness

metallic solids do not exhibit

vitalism

the belief that only living organisms could make organic compounds is known as

alkene

the compound below is an H2C==CH-CH3

2.70

the concentration of nitrate ions in a solution that contains 0.900 M aluminum nitrate is _______M

ethane

the correct name for the molecule CH3CH3 is

H+

the formula of the hydrogen ion is often written as

tetrahedral

the molecular geometry of each carbon atom in an alkane is

false

true or false: aldehydes have an -ide ending

false

true or false: amines contain at least one sulfur atom

bitter taste

what is a property of a base

proton

what is transferred between a conjugate acid base pair

a chlorinated hydrocarbon

what kind of functional group is known for being harmful to our atmosphere

diprotic

what type of acid is sulfric acid

ion-dipole

when NaCl dissolves in water, aqueous Na+ and Cl- ions result. The force of attraction that exists between Na+ abd H2) is called a __________________ interaction

a

which of the following is a statement of Hess's law: a. If a reaction is carried out in a series of steps, the delta H for the reaction will equal the sum of the enthalpy changes for the individual steps. b. If a reaction is carried out in a series of steps, the delta H for the reaction will equal the product of the enthalpy changes for the individual steps. c.The delta H for a process in the forward direction is equal in magnitude and opposite in sign to the delta H for the process in the reverse direction d.The delta H for a process in the forward direction is equal to the delta H for the process in the reverse direction. e.The delta H of a reaction depends on the physical states of the reactants and product

NH4+ and NH3

which of the following represents a Bronsted-Lowry conjugate acid base pair? SO3^2- and SO2 CO3^2- and CO H30 and H2 NH4+ and NH3

1.88 kJ/mol

calculate the heat absorbed by 15.0 g of water to raise its temperature from 20.0 C to 50.0 C

3, acidic

calculate the hydrogen ion concentration [H+] for an aqueous solution in which [OH=] is 1.0 x 10 -11 mol/L. Is this solution acidic basic or neutral?

1.74

calculate the pH. Assume 25 C 0.018 M hydrochloric acid

12.54

calculate the pH. Assume 25 C 0.035 M NaOH

12.20

calculate the pH. Assume 25 C 7.9 x 10^-3 calcium hydroxide

2

calculate the pH. Assume 25 C 9.9 x 10^-3 M nitric acid

the concentration of the solute particles

colligative properties depend on

the increase of reaction rates with increase in temperature

colligative properties of solutions does not include

scatter light

colloids

highly ordered structures

crystalline solids have

OH = 2.24 x 10^-13 pH = 1.35

determine the OH of a 0.045 M HCL Calculate pH

nonpolar and water is polar

gasoline and water do not mix because gasoline is

CH4

of the following substances, only ______________ has london dispersion forces as its only intermolecular force CH30H NH3 H2S CH4 HCl

Br2

of the following, _____________ has the highest boiling point N2 Br2 H2 Cl2 O2

the freezing point

on a phase diagram, the melting point is the same as

miscible

pairs of liquids that will mix in all proportions are called _________ liquids

water boils at a lower temperature at high altitudes than low altitudes

some things take longer to cook at high altitudes than at low altitudes because

13.2

the enthalphy change for converting 1.00 mol of ice at -50 0 C to water at 70.0 C is __________ kJ. The specific heats of ice, water, and steam are 2.09 J/g-K, 4 18J/g-k, and 1.84 J/g-K, respectively. For H2O, delta Hfus = 6.01kJ/mol, and delta Hvap = 40.67 kJ/mol

acetic acid

the primary ingredient in vinegar is

titration

the process of adding a known amount of solution of known concentration to determine the concentration of another solution is called ___________

solvation

the process of solute particles being surrounded by solvent particles is known as

OH- and H+

the products of self ionization of water are

acetylene

the simplest alkyne is

0.12

the solubility of oxygen gas in water at 25* C and 1.0 atm pressure of oxygen is 0.041 g/L. The solubility of oxygen in water at 3.0 atm and 25 *C is __________ g/L

-one

the suffix used for organic molecules containing the ketone functional group is

kJ

the units of specific heat are

1 atm

the vapor pressure of any substance at its normal boiling point is

complete ionization in water

what characterizes a strong acid or base

carbon

what element is the basis for organic chemistry

sour taste

what is a property of acids

the negative log of the hydrogen ion concentration

what is ph

Basic

what is the best description of a solution with a hydroxide concentration of 1 x 10^-4M

1+

what is the charge on the hydronium ion

39.2 C

what is the final temperature of 365 g aluminum when it absorbs 5.56 kJ of heat and its intial temperature is 22.3 C. The specific heat of aluminum is 0.901 J/(g*c)

rcooh

what is the general form for a carboxylic acid

2 x 10^-4

what is the hydrogen ion concentration is the pH is 3.7

1.0 x 10^-14 at 25 C

what is the ion product constant for water?

12.82

what is the pH of a 0.066M KOH(aq)

1.66

what is the pOH of a 0.011 M calcium hydroxide aqueous solution at 25 C

12.64

what is the pOH of a 0.044 M perchloric acid solution

scattering of light by colloid particles

what is the tyndall effect?

-45.7

when a 9.55 g sample of solid sodium hydroxide dissolves in 100.0 mL of water in a coffee-cup calorimeter, the temperature rises from 23.6 C to 47.4 C,. calculate toe delta h for this reaction in kJ/mol NaOH. assume the specific heat and density of the solution is that of pure water

h2o

which compound can act as both a bronsted lowry acid and a bronsted lowry base

molarity

which of the following concentration units varies with temperature molarity mass percent mole fraction molality all of the above

alcohols

which of the following does not contain a c==o bond alcohols aldehydes carboxylic acids esters

all of the above

which of the following is true of a hydrocarbon? it consists of carbon and hydrogen atoms it can form a ring structure it is a good fuel for combustion reactions it can contain double or triple bonds all of the above

SiH4

which of the following should have the lowest boiling point? PH3 H2S HCl SiH4 H2O

C10H22

which of the following substances would be the most soluble in CCl4? CH3CH2OH H2O NH3 C10H22 NaCL

amine

which of these does not always have a double bond? amine aldehyde ketone alkene carboxylic acid

alcohols

which of these functional groups does not contain a c==o in its general form aldehydes alcohols esters carboxylic acids ketones

all of these are correct

which of these is not a subfamily of the hydrocarbon family? alkenes alkynes alkanes all of these are correct

CH3CH2CH2CH3

which of these is the correct condensed structural formula for butane? CH2CH2CH3 CH3CH2CH2CH3 CH3CH2=CH2CH3 CH3CH2HC=CHCH3

[H+] = 1x10^-11M

which of these solutions is the most basic? [H+] = 1x10^-2M [OH-] = 1x10^-4M [H+] = 1x10^-11M [OH-] = 1x10^-13M

alkanes are nonflammable

which of these statements about alkanes is not correct? alkanes are non polar alkanes are non flammable carbon must always form four bonds alkanes have a general formula CnH2n

benzene rings are composed of six carbons held together by six double bonds

which of these statements about benzene rings is false? benzene is a particularly stable structure benzene rings are sometimes called aromatic rings benzene is a six membered ring with the formula C6H6 benzene rings are composed of six carbons held together by six double bonds

isomers have essentially the same properties

which of these statements about isomers is incorrect? isomers have the same chemical formula isomers have different structural formulas isomers have essentially the same properties

all of the above

which of these statements about water is correct? water has a high boiling point water expands when it freezes water is the most abundant liquid on the planet water molecules for hydrogen bonds all of the above

all of the above

which of these statements is correct? alkanes are saturated hydrocarbons alkynes are hydrocarbon chains which contain a triple bond unsaturated hydrocarbons contain at least one multiple bond all of the above

table salt

which of these substances is not an organic compound? alcohol aspirin gasoline table salt

urea

which of these was the first organic compound synthesized from an inorganic one

C2I6

which one of the following derivatives of ethane has the highest boiling point? C2Br6 C2F6 C2I6 C2Cl6 C2H6

all

which statements about viscosity are true? i. viscosity increases as temperature decreases ii. viscosity increases as molecular weight increases iii. viscosity increases as intermolecular forces increase

degree of ionization

with solutions of strong acids and strong bases the word strong refers to

exothermic

4Al(s) + 3O2(g) --> 2Al2O3(s) delta H = -3351kJ is this reaction endothermic or exothermic?

a strong base

A 0.10 M solution of an electrolyte has a pH of 4.5. The electrolyte is:

364.79 J

A 25.2g piece of silver is heated from 22.2⁰C to 83.8⁰C. The specific heat of silver = 0.235 J g-1K-1. Calculate the quantity of heat that the piece of silver absorbs.

basic

A solution's [OH-] was determined to be 5.2 x 10-4 M. Is this solution acidic, basic, or neutral at 25°C?

1.22

Calculate the pH when 10.00 mL 0.12M NaOH is mixed with 10.00 mL 0.24M HCl.

1214.5kJ

Calculate ΔHfor the following reaction, 2CH4(g) + 3O2(g) --> 2CO(g) + 4H2O(l) using the following thermochemical equations: 2C(s) + O2(g) --> 2CO(g) ΔH = -221.08 kJ CH4(g) + 2O2(g) --> CO2(g) + 2H2O(l) ΔH = -890.4 kJ C(s) + O2(g) --> CO2(g) ΔH = -393.5 kJ

pH= 13.15 H3O = 7.08x10^-14

Determine the hydronium ion concentration of a 0.14 M KOH. Calculate pH

2.52

Determine the pH of a solution made by taking 25.0 mL of 0.25M HCl and diluting to a total volume of 2.00 L.

29.25J

The specific heat of lead is 0.13 J/g-K. How much heat (in J) is required to raise the temperature of 15 g of lead from 22 °C to 37 °C?

-63 kJ

The value of H° for the reaction below is -126 kJ. Calculate the heat produced when 2.00 mol of NaOH is formed in the reaction. 2Na 2 O 2 (s) + 2H 2 O (l) --> 4NaOH (s) + O 2 (g) ∆H = -126 kJ

-93

The value of delta H° for the reaction below is -186 kJ. H2 (g) + Cl2 (g) --> 2HCl (g) The value of delta H°f for HCl (g) is _________________ kJ/mol.

0.413

The vapor pressure pf pure ethanol at 60* C is 0.459 atm. Raoult's Law predicts that a solution prepared by dissolving 10.0 mmol napthalene (nonvolatile) in 90.0 mmol ethanol will have a vapor pressure of ____________atm

.57M

What is the concentration of HCl determined to be when a titration of 10.00 mL of the acidic solution uses 23.58 mL of a 0.12M Ba(OH)2 solution to neutralize.

1.26

What is the pH of a 0.055M solution of HNO3

A

Which of the following is NOT a property of acids? A) Acids have a slippery feel. B) Acids have a sour taste. C) Acids turn litmus paper red. D) Acids dissolve many metals. E) All of the above are properties of acids.

supercritical

Which of the following is not a type of solid? ionic molecular supercritical metallic covalent-network

NaHCO3

Which of the following is the active ingredient of baking soda? A) NH3 B) NaHC C) KOH D) NaOH E) none of the above

aqueous FeI3

Which of the following liquid will have the lowest freezing point? pure H2O aqueous glucose (0.050 m) aqueous CoI2 (0.030 m) Aqueous FeI3 (0.030 m) aqueous NaI (0.030 m)

acetic acid, sodium hydroxide

Which of the following pairs consists of a weak acid and a strong base? sulfuric acid, sodium hydroxide acetic acid, ammonia acetic acid, sodium hydroxide nitric acid, calcium hydroxide

all

Which of the following statements about acids are TRUE? 1. An acid is used in car batteries. 2. A component of vinegar is an acid. 3. Acids are used for cleaning metals.

e

Which of the following statements about water are TRUE? A) Water can act as an acid. B) Water can act as a base. C) The conjugate base of water is OH-. D) The conjugate acid of water is H3O+. E) All of the above are true.

b

Which solution below has the highest concentration of hydroxide ions? A) pH = 3.21 B) pH = 12.49 C) pH = 7.00 D) pH = 10.12 E) pH = 7.93

basic

Which type of solution is one with a pH of 8?

dilute and weak

a 0.12M solution of an acid that ionizes only slightly in solution would be termed ____________

KCl

a 1.35 m aqueous solution of compound X had a boiling point of 101.4 C. Which one of the following could be compound X? CH3CH2OH C6H12O6 Na3PO4 KCl CaCL2

10^-10

a liter of impure water has 10^-4 mol of hydroxide ions. What is the concentration of hydronium ions in this sample of water?

2001g/mol

a solution of 0.400 g of a polypeptide in 1.00 L of an aqueous solution has an osmotic pressure of 3.74 torr at 27C. what is the molar mass of the polypeptide

will precipitate when a seed crystal is added

a supersaturated solution _______________

readily evaporates

a volatile liquid is one that

a good hydrogen ion acceptor

acetic acid ionizes in water as follow: CH3COOH + H20 ==> CH3COO- + H30+ fewer than 1% of ethanoic acid molecules are ionized at any instant. the acetate ion (CH3COO-) is therefore __________

C-Cl bond

alkyl halides may contain

2.41 x 10^-4

The Henry's law constant for helium gas in water a 30C is 3.70 x 1.^-4 M/atm. when the partial pressure of helium above a sample of water is 0.650 atm, the concentration of helium in teh water is ____________M

OH = 6.0 x 10^-7 pOH = 6.22

The average pH of normal arterial blood is 7.40. At normal body temperature (37°C), Kw= 2.4 x 10-14. Calculate [H+], [OH-], and pOH for blood at this temperature.

0.75

The concentration of HCl in a solution that is prepared by dissolving 5.5 g of HCl in 200 g of C2H6O is _____________ molal

29

The concentration of urea in a solution prepared by dissolving 16 g of urea in 39g of H2O is ___________% by mass. The molar mass of urea is 60.0 g/mol.

-967.2

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)

10.36

The fluorocarbon C2Cl3F3 has a normal boiling point of 47.6 C. the specific heats of C2Cl3F3(l) and C2Cl3F3(g) are 0.91 J/g-K and 0.67 J/g-K, respectively. the heat of vaporization of the compound is 27.49 kJ/mol. The heat required to convert 50.0 g of the compound from the liquid at 5.9 C to the gas at 80.0C is _____________kJ

0.0136

The osmotic pressure of a solution formerd by dissolcing 25.0 mg of aspirin (C9H8O4) in 0.250 L of water at 25 C is ___________ atm

pOH = 5 10^-5

If the pH is 9.00 what is the concentration of hydroxide ions