Honors Chemistry: 2nd Semester Practice Tests; Dr. H

3 mole NaOH

6 NaOH + 2 Al → 2 Na3AlO3 + 3 H2 How many moles of NaOH are required to produce 3 grams of hydrogen?

aluminum phosphate

AlPO4

37.6 g AlCl3; 82.4% yield

Aluminum chloride, AlCl3, can be made by the reaction of aluminum with chlorine according to the following equation: 2 Al + 3 Cl2 → 2 AlCl3 What is the limiting reactant if 20.0 grams of Al and 30.0 grams of Cl2 are used, and how much AlCl3 can theoretically form? If 31.0 g of AlCl3 is actually produced, what is the percent yield?

130. g aspirin; 26.3 g C4H6O3 remain

Aspirin (C9H8O4) is produced by the reaction of salicylic acid (C7H6O3) and acetic anhydride (C4H6O3) C7H6O3(s) + C4H6O3(l) → C9H8O4(s) + CH3CO2H(aq) [Molar masses: 138.1 102.1 180.1 60.05] If you mix 100. g of each of the reactants, what is the maximum mass of aspirin that can be obtained? What mass of the excess reactant remains when the limiting reactant is consumed?

466.4 g BaSO4

BaO + H2SO4 → BaSO4 + H2O What mass of BaSO4 can be formed from 196.0 g of H2SO4?

242 g CaCO3

Burning coal and oil in a power plant produces pollutants such as sulfur dioxide, SO2. The sulfur-containing compound can be removed from other waste gases, however, by the following reaction: 2 SO2(g) + 2 CaCO3(s) + O2(g) → 2 CaSO4(s) + 2 CO2(g) [Molar masses: 64.07 100.1 32.00 136.2 44.01] What mass of CaCO3 is required to remove 155 g of SO2?

calcium carbonate

CaCO3

C2H6As

Cacodyl, a compound containing arsenic, was reported by the German Chemist Bunsen. Cacodyl has an almost intolerable garlic-like odor. its molar mass is 210 g.mol and 22.88% C, 5.76% H, and 71.365 As. determine the empirical formula

C4H12As2

Cacodyl, a compound containing arsenic, was reported by the German Chemist Bunsen. Cacodyl has an almost intolerable garlic-like odor. its molar mass is 210 g.mol and 22.88% C, 5.76% H, and 71.365 As. determine the molecular formula

94.2% yield

Calcium carbonate is decomposed by heating to form calcium oxide and carbon dioxide gas. What is the percent yield of this reaction if 24.8 g of CaCO3 is heated to give 13.1 g of CaO? CaCO3 → CaO + O2

cobalt (II) phosphate

Co3(PO4)2

67.1% yield

Diborane, B2H6, is a valuable compound in the synthesis of new organic compounds. One of several ways this born compound can be made is by the reaction 2 NaBH4(s) + I2(s) → B2H6(g) + 2 NaI(s) + H2(g) [Molar masses: 37.84 253.8 27.67 149.9 2.02] Suppose you use 1.203 g of NaBH4 with an excess of iodine and obtain 0.295 g of B2H6. What is the percent yield of B2H6?

67.3 g S2Cl2; 35.7 g Cl2 remain

Disulfur dichloride, S2Cl2, is used to vulcanize rubber. It can be made by treating molten sulfur with gaseous chlorine: S8(l) + 4 Cl2(g) → 4 S2Cl2(l) [Molar masses: 256.6 70.91 135.0] Starting with a mixture of 32.0 g of sulfur and 71.0 g of Cl2, which is the limiting reactant? What mass of S2Cl2 (in grams) can be produced? What mass of the excess reactant remains when the limiting reactant is consumed?

52.2% yield

Disulfur dichloride, which has a revolting smell, can be prepared by directly combining S8 and Cl2, but it can also be made by the following reaction: 3 SCl2(l) + 4 NaF(s) → SF4(g) + S2Cl2(l) + 4 NaCl(s) [Molar masses: 103.0 41.99 108.1 135.0 58.46] Assume you begin with 5.23 g of SCl2 and excess NaF. What is the theoretical yield of S2Cl2? If only 1.19 g of S2Cl2 is obtained, what is the percent yield of the compound?

576.0 g O2

Given the following equation: 2 NaClO3 → 2 NaCl + 3 O2 12.00 moles of NaClO3 will produce how many grams of O2?

0.567 moles

Given the reaction S + O2 → SO2 How many moles of sulfur must be burned to give 0.567 moles of SO2?

sulfurous acid

H2SO3

hydrofluoric acid

HF

d

HNO3 will most likely dissolve in a. CCl4 (l), which is a nonpolar solvent b. CCl4 (l), which is a polar solvent c. H2O (l), which is a nonpolar solvent d. H2O (l), which is a polar solvent

27.2 g ZnCl2; 6 g Zn remain

If 19 g of zinc are reacted with 19 g magnesium chloride, zinc chloride and magnesium are formed. Zn + MgCl2 → Mg + ZnCl2 a. Calculate the mass of the zinc chloride produced. b. Calculate the mass of the excess reactant that remains unreacted.

tetraphosphorous tetrachloride

P4Cl4

tetraselenium hexabromide

Se4Br6

true

T or F: gases are more easily compressed than either liquids or solids

false

T or F: gases have less space between particles than liquids

false

T or F: gases tend to be more dense than solids

false

T or F: the properties of liquids are more affected by pressure than gases

false

T or F: there are more attractive forced between gaseous particles than liquid particles

3.42 x 10^24 atoms

The equation for one of the reactions in the process of reducing iron ore to the metal is Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g) [Molar masses: 159.7 28.01 55.85 44.01] How many atoms of iron can be obtained from 454 g of iron(III) oxide?

376 g H2

The reaction of methane and water is one way to prepare hydrogen: CH4(g) + H2O(g) → CO(g) + 3 H2(g) [Molar masses: 16.04 18.02 28.01 2.02] If you begin with 995 g of CH4 and 2510 g of water, what is the maximum possible yield of H2?

3 x 10^24 H2O molecules

Using the following equation: 2 NaOH + H2SO4 → 2 H2O + Na2SO4 How many molecules of water will be formed if you start with 200 grams of sodium hydroxide and you have an excess of sulfuric acid?

the shape of molecules

VSEPR theory is a model for predicting what?

0.28 g Arginine

Your body deals with excess nitrogen by excreting it in the form of urea, NH2CONH2. The reaction producing it is the combination of arginine (C6H14N4O2) with water to give urea and ornithine (C5H12N2O2). C6H14N4O2 + H2O → NH2CONH2 + C5H12N2O2 [Molar masses: 174.2 18.02 60.06 132.2] If you excrete 95 mg of urea, what quantity of arginine must have been used?

18.7 atm He, 1.87 atm Ar, 20.6 atm total

a 15.0 g sample of He gas is added to a 15.0 g sample of Ar gas at 31 C in a 5.00 L container. calculate the partial pressure of each gas and the total pressure

10440

a 25.00 gram sample of ice at 0C melts and then warms up to 20C. how much energy is absorbed?

3.9 atm H2, 0.45 atm O2, 0.20 atm CO2, 4.6 atm total

a 252 mL container has 0.082 g of hydrogen, 0.15 g of oxygen, and 0.092 g of carbon dioxide. the temperature is 22.52 C. what is the partial and total pressures of the gas in the container?

49.0 C

a 63.0 g piece of aluminum (specific heat = 0.899) at 25 C is warmed by the addition of 1360 J of energy. find the final temperature of the aluminum

20.5 C

a 65.0 g of iron at 525 C is put into 635 grams of water at 15 C. what is the final temperature of the water and the iron (specific heat of metal = 0.449)

proton donor

a Bronsted-Lowry acid is a(n) __________________

1500 G

a certain mass of water was heated with 41,840 J, raising its temperature from 22 to 28.5 C. find the mass of the water, in grams

CH2Br

a compound contains 12.8% C, 2.1% H, and 85.1% Br. calculate the empirical formula of the compound given that the molar mass is 282 g/mol

C3H6Br3

a compound contains 12.8% C, 2.1% H, and 85.1% Br. calculate the molecular formula of the compound given that the molar mass is 282 g/mol

C5H5O2

a compound has a molar mass of about 100 g/ml and is 63.15% carbon and 5.30% hydrogen. the remainder is oxygen. determine the empirical formula

C5H5O2

a compound has a molar mass of about 100 g/ml and is 63.15% carbon and 5.30% hydrogen. the remainder is oxygen. determine the molecular formula

9.00 atm

a container holds three gases: oxygen, carbon dioxide, and helium. the partial pressures of the three gases are 2.00 atm, 3.00 atm, and 4.00 atm, respectively. what is the total pressure inside the container?

745.5 (746) mm Hg

a eudiometer tube holds hydrogen gas with a pressure of 735.5 mm Hg and water vapor with a pressure of 10.0 mm Hg. what is the total pressure in the tube?

150 mm Hg

a gas mixture is created by blending 0.2 mols CO2, 2.0 mols O2, and 7.8 mols N2. is the total pressure is 750 mm Hg, calculate the partial pressure of oxygen

32.0 g/mol

a gaseous sample of the compound has a density of 0.977 g/L at 710 torr and 373 K. what is the molecular mass of the compound?

c

a given mass of gas in a rigid container is heated from 100 C to 500 C. which of the following responses best describes what will happen to the pressure of the gas? a. the pressure will decrease by a factor of five b. the pressure will increase by a factor of five c. the pressure will increase by a factor of about two d. the pressure will increase by a factor of about eight

CoCl2 o 6H2O

a hydrate is determined to be 45.43% water and 54.57% CoCl2. find the chemical formula

MgSO4 o 7H2O

a hydrate of magnesium sulfate has a mass of 13.52 g. this sample is heated until no water remains. the MgSO4 anhydrate has a mass of 6.60g. find the formula

1.36 atm H2, 0.629 atm N2, 0.0123 atm O2

a mixture of 14.0 grams of hydrogen, 90.0 grams of nitrogen, and 2.00 grams of oxygen are placed in a flask. the total pressure in the flask is 2.00 atm. what is the partial pressure of each component?

molecule

a neutral group of atoms held together by covalent bonds

a region of positive charge and a region of negative charge

a polar molecule contains ____________________________

C3H6O2

a sample contains 145.9 g C, 24.3 g H, and 129.8 g O. what is the empirical formula?

i and iii

a sample of a metal is heated. which of the following are needed to calculate the heat absorbed by the sample? i. the mass ii. the density iii. the specific heat

CuSO4 o 5H2O

a sample of copper (II) sulfate hydrate has a mass of 3.97 g. after heating, the CuSO4 that remains has a mass of 2.54 g. determine the correct formula

745 torr

a sample of hydrogen gas is collected over water at 22 C. the pressure of the resultant mixture is 765 torr. what is the pressure that is exerted by the dry hydrogen alone?

285 g

a sample of nitrogen gas is collected over water at 20 C and a pressure of 1.00 atm. the volume of the collected gas is 250.0 L. what mass of N2 is collected?

covalent bond

a shared bond of valence electrons of different atoms that binds the atoms together

b

a solvent dissolves an ionic compound by a. strongly repelling solute ions b. strongly attracting solute ions c. weakly attracting solute ions d. weakly repelling solute ions

d

a strong electrolyte is a solute that a. dissolves in water as molecules only b. does not dissolve in water c. dissolves in water as molecules and ions d. dissolves in water as ions only

0.392 J/gC

a student determines that 20.4 J of heat are required to raise the temperature of 6.67 g of an unknown metal from 35 C to 42.8 C. what is the specific heat?

strong acid

a substance that ionizes nearly completely in aqueous solutions and produces H3O+ is a ___________________

d

according to Avogadro's law, 1 L of H2 (g) and 1 L of O2 (g) at the same temperature and pressure a. have the same mass b. have unequal volumes c. contain 1 mol of gas each d. contain equal number of molecules

b

according to the kinetic-molecular theory, gases are highly compressible because the particles a. lose energy when they collide with each other b. are very apart from each other c. experience a strong force of attraction d. experience a strong force of repulsion

a

according to the kinetic-molecular theory, particles of matter a. are in constant motion b. have different shapes c. have different colors d. are always fluid

sour

acids taste ________

confirm that the total number of valence electrons used equals the number available

after drawing a Lewis structure, one should _____________________________________________________________

30. C

an iron nail with a mass of 12.37 g absorbs 15 J of heat. if the nail was initially at 28 C, what is its final temperature? (specific heat of iron = 0.449)

decrease, more

as atoms bond with each other they ____________ their potential energy, thus creating _______-stable arrangements of matter

at relatively high potential energy

as independent particles, most atoms are _________________________________

a

as the H3O+ in a solution decreases, the OH- a. increases and the pH increases b. increases and the pH decreases c. decreases and pH increases d. decreases and the pH decreases

temperature

as the kinetic energy of an object increases so does its __________

b

at constant temperature and pressure, gas volume is directly proportional to the a. molar mass of the gas b. number of moles of gas c. density of the gas at STP d. rate of diffusion

c

at room temperature, F2 and Cl2 are gases, Br2 is a liquid, and I2 is a solid. this is because ________ a. dispersion interactions increase with molecular size and polarity increases with molecular size b. dipole-dipole interactions increase with molecular size c. dispersion interactions increase with molecular size d. polarity increases with molecular size

toward low potential energy

atoms naturally move _________________________________________

slippery

bases feel __________

bitter

bases taste _________

resonance

bonding in molecules or ions that cannot be correctly represented by a single Lewis structure

Ca(ClO3)2

calcium chloroate

Ca(OH)2

calcium hydroxide

1 x 10^-12 M

calculate the H3O+ in a 0.010M solution of OH-

31269.5

calculate the energy absorbed when 10 g of ice at -20C are converted into steam at 135C

1.07 g

calculate the mass of 1.50 L of CH4 at STP

1880 grams (1.88 x 10^3)

calculate the mass of 12.2 mol of carbon tetrachloride, CCl4

1.33 L

calculate the number of L of 2.00 M HNO3 solution required to react with 216 grams of Ag according to the following equation: 3 Ag (s) + 4 HNO3 (aq) ----> 3 AgNO3 (aq) + NO (g) + 2 H2O (l)

5.73 g

calculate the number of grams of AgCl formed when 200. mL of 0.200 M AgNO3 reacts with excess of CaCl2: 2 AgNO3 (aq) + CaCl2 (aq) ----> 2 AgCl (s) + Ca(NO3)2 (aq)

0.0246 mole

calculate the number of moles contained in 550 mL of carbon dioxide at STP

4.62 x 10^-6 moles

calculate the number of moles of S in 2.78 x 10^18 atoms of S

75.3 L

calculate the volume in liters of 50.0 grams of nitrogen dioxide at 445 torr and 28.0 C

0.53 L

calculate the volume of hydrogen gas produced by the reaction of 0.52 grams of solid magnesium with excess hydrochloric acid at 25 C and 0.989 atm. Mg + 2 HCl --> MgCl2 + H2

HClO2

chlorous acid

0.0597

clculate the mass of water (in grams) that will be vaporized by 135 J of energy

b

complete this sentence: the molecules of different samples of an ideal gas have the same average kinetic energies at the same _________________ a. pressure b. temperature c. volume d. density

SO4-2

conjugate base of HSO4-

H2O

conjugate base to H3O+

570 mm Hg

convert 0.75 atm to mm Hg (use SF)

130,000 Pa

convert 1.3 atm to Pa (use SF)

1750 mm Hg

convert 2.3 atm into mm Hg (use SFs)

55 mm Hg

convert 55 torr to mm Hg (use SF)

SF2

determine the empirical formula of a compound containing 54.2% F and 45.8% S

35.00%

determine the percentage composition of N in NH4NO3

32.69%

determine the percentage composition of S in H2SO4

H+ and Cl-

dissolving HCl in water produces __________

nitrogen

equal mass of oxygen and nitrogen gas are present in a container. which gas exerts the larger partial pressure and by what factor?

as mass increases, so do melting points

explain the melting points of fluorine, chlorine, bromine, and iodie

because it needs activation energy to start

explain why no reaction takes place between methane and chlorine at room temperature unless the reactants are sparked, exposed to UV light or heated

50.3 grams

find the mass in grams of 2.00 x 10%23 molecules of C10H15O

26.6 grams

find the mass of 8.90 x 10^23 molecules of water

10 M

find the molarity: 0.5 moles of NaCl is dissolved to make 0.05 liters of solution

2.67 M

find the molarity: 734 grams of Li2SO4 are dissolved to make 2.500 L of solution

b

for which substance would you predict the highest heat of vaporization? a. F2 b. H2O c. HF d. Br2

a

formic acid is a weak acid because it a. does not dissociate completely b. is always dilute c. contains two hydrogen atoms d. cannot form hydrogen bonds e. is slightly basic

a

gases tend to deviate from the ideal gas law at a. high pressures b. low pressures c. high temperatures d. high pressures and temperatures

dipole dipole

give the bonds/forces in the following: between the molecules of HCl in liquid HCl

ldf

give the bonds/forces in the following: between the molecules of carbon dioxide, CO2 in dry ice

h-bond

give the bonds/forces in the following: between water molecule in ice

ionic

give the bonds/forces in the following: in a crystal of the salt NaCl

covalent network

give the bonds/forces in the following: in diamond

metallic

give the bonds/forces in the following: in tungsten metal

covalent

give the bonds/forces in the following: within a water molecule H2O

709 g

given the following reaction: CuO (s) + H2 (g) --> Cu (s) + H2O (g), if 250. L of hydrogen gas are used to reduce copper (II) oxide at STP, what mass of copper is to be expected?

25.0 L

given the following reaction: NH4NO2 (s) --> N2 (g) + 2H2O (g). how many liters of nitrogen gas is produced if 50.0 L of water is produced at STP?

1.35 x 10^24 atoms

how many atoms are in 0.750 moles of water?

3.480 x 10^24 atoms

how many atoms of C are in 5.778 moles of C?

8

how many electrons must be shown in the Lewis structure of the hydroxide ion, OH-?

3

how many extra electrons are in the Lewis structure of the phosphate ion PO4-3?

0.50 g

how many grams of BeCl2 are needed to make 125 mL of a 0.050 M solution?

24.97 grams

how many moles of H2O are in 450.0 g of H2O?

0.23 mole

how many moles of HCl are present in 0.70 L of a 0.33 M HCl solution?

3.69 x 10^21 particles

how many particles are there in 1.43 g of a molecular compound with a molar mass of 233 g?

24737.2

how much energy is required to melt 42 g of ice at -18C, and bring the liquid water up to 52C?

836

how much energy must be absorbed by 20 g of steam to increase its temperature from 283 C to 303 C?

22600 J

how much heat is released when 100 grams of steam condenses at 100C?

5010 J

how much heat is required to melt 15 grams of ice at 0C?

39,000 J

how much heat must be absorbed by 375 grams of water to raise its temperature by 25 C?

3.70 kJ

how much heat will be released when 1.48 g of chlorine reacts with excess phorphorus according to: 2P + 5Cl2 ---> 2PCl5 -886 kJ

88 kJ

how much heat will be released when 13.7 g of nitrogen reacts with excess O2 according to: N2 + O2 ---> 2NO -393.5 kJ

17.4 kJ

how much heat will be released when 38.2 g of bromine reacts with excess H2 according to: H2 + Br2 ---> 2HBr 72.80 kJ

155 kJ

how much heat will be released when 4.72 g of carbon reacts with excess O2 according to: C + O2 ---> CO2 -393.5 kJ

79.5 kJ

how much heat will be released when 6.44 g of sulfur reacts with excess O2 according to: 2 S + 3 O2 ---> 2SO3 -791.4 kJ

add 7.5 mL

how much water is added to 15.0 mL of a 0.75 M solution to produce a 0.5 M solution?

0.6 M

if 50 mL of water are added to 200 mL of a 0.75 M K2SO4 solution, what will the molarity of the diluted solution be?

3.7 C

if 57 J of heat are added to an aluminum can with a mass of 17.14 g, what is its temperature change? (specific heat of aluminum = 0.899)

basic

if H3O+ of a solution is less than OH-, the solution is __________

9.9%

if I make a solution by adding 82 grams of NaOH to 750 g of water, what is the mass percent of NaOH?

13%

if I make a solution by adding water to 35 g of methanol until the final volume of the solution is 275 g, what is the mass percent?

5 atm

if I place 3 moles of N2 and 4 moles of O2 in a 35 L container at a temperature of 25 C, what will the pressure of the resulting mixture of gases be?

32.4 C

if a piece of copper with a mass of 37.60 g and a temperature of 100 C is dropped into 25 g of water at 23 C, what will be the final temperature of the system? (specific heat of copper = 0.385)

2.00 x 10^23 atoms

if a sample of calcium has a mass of 13.3 grams, how many atoms of calcium are present?

a

if equal masses of O2 (g) and HBr (g) are in separate containers of equal volume and temperature, which one of the following statements are true? a. the pressure in the O2 container is greater than that in the HBr container b. there are more HBr molecules than O2 molecules c. the average kinetic energy of HBr molecules is greater than that of O2 molecules d. the pressures of both gases are the same

a

if pressure is constant, the relationship between temperature and volume is a. direct b. inverse

polar

if the atoms that share electrons have an unequal attraction for the electrons, the bond is ____________

1/2

if the pressure of a gas sample is quadrupled and the absolute temperature is doubles, by what factor does the volume of the sample change?

4/3

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

1/2

if the volume of a gas increases by a factor of four and the temperature doubles, what happens to the pressure?

nonpolar covalent

if two covalently bonded atoms are identical, the bond is ____________________________

0.32 M

if water is added to 175 mL of a 0.45 KOH solution until the volume is 250 mL, what will the molarity of the diluted solution be?

8

in a molecule of fluorine, the two shared electrons give each fluorine atom how many electrons in the outer energy level?

H

in the formula H = mCT, which variable is measured in Joules

chlorine

in the three molecules, O2, HCl, and F2, what atoms would have a partial negative charge?

a

in water solutions of HCl, the free H+ ion is a. present in very large quantities b. present in moderate quantities c. present in small quantities d. not present

a

in which one of the following will dipole-dipole attractions play the most significant role as the intermolecular attraction? a. HCl b. H2O c. NH3 d. Kr

strong

is HCl a weak or strong acid?

polar

is NH3 polar or nonpolar?

NO2

nitrogen dioxide

one atom usually attracts electrons more strongly than the other

nonpolar covalent bonds are not common because ___________________________________________________________

c

one way to increase pressure on a gas is to a. decrease temperature b. increase volume c. increase the number of gas particles d. lower the kinetic energy of the gas molecules

HClO4

perchloric acid

c

polar water molecules are attracted to a. positive ions b. negative ions c. both positive and negative ions d. nether positive or negative ions

1,4,6,2,5,3

rank the following from lowest to highest: melting point of argon boiling point of argon boiling point of CaBr2 melting point of HF boiling point of HF melting point of CaBr2

Na2O

sodium oxide

X to Y

solid x at 10C is placed in contact with solid Y. heat will flow spontaneously from ___ to ____

b

strong bases are more __________ than weak bases a. dense b. highly ionized c. nonmetallic d. molecular

Br4F7

tetrabromine heptafluoride

pascals

the SI unit of pressure

c

the compounds Br2 and ICl have almost identical molecular weights, yet ICl boils at 97 C and Br2 boils at 59 C. the best explanation for the difference is a. ICl is an ionic compound and Br2 is covalent b. ICl is a nonpolar molecule and Br2 is polar c. ICl has a measurable dipole moment (is polar) and Br2 is not (is nonpolar) d. ICl has a stonger bond than that in Br2

VSEPR theory

the concept that electrostatic repulsion between electron pairs surrounding an atom causes these pairs to be separated as far as possible

ClO3-

the conjugate base of HClO3

3

the electron configuration of nitrogen is 1s2 2s2 2p3. how many more electrons does nitrogen need to satisfy the octet rule?

valence electrons

the electrons involved in the formation of a chemical bond

ionic bond

the electrostatic attraction between positively charged nuclei and negatively charged electron permits two atoms to be held together by a(n) ___________________

C4H4O4

the empirical formula for maleic acid is CHO. its molar mass is 116.1 g/mol. what is the molecular formula?

142

the equations: Cu(s) + O2(g) ----> CuO(s) H = -156 2Cu(s) + O2(g) ----> Cu2O(s) H = -170 what is the value of H in: 2CuO(s) ----> Cu2O(s) + O2(g)

H3O+

the formula for the hydronium ion

10.0 mm Hg

the gas in a eudiometer has a total pressure of 750.0 mm Hg. if 740.0 mm Hg is due to pressure of hydrogen gas, what pressure is due to water vapor?

ionic character

the greater the electronegativity difference between two bonded atoms, the greater the percentage of __________________________________ in the bond

c

the intermolecular forces in a liquid X are greater than those in a liquid Y. comparing the two liquids, it could be expected that liquid X would have ________ a. the higher rate of evaporization b. the higher vapor pressure at a given temperature c. the higher boiling temperature d. no conclusions can be states

crystal lattice

the ions in most ionic compounds are organized into a __________________

Boyle's law

the law that relates the pressure and volume of a gas to each other is known as ______________

single

the longest bond length

B

the only property listed below that is not a characteristics of gases is: a. the ability to flow easily b. very high density c. an indeterminate shape d. large space between particles

7

the pH of a neutral solution

6.3 x 10^-10 M

the pH of a solution is 4.80. what is the concentration of hydroxide ions in this solution?

less than 7

the pH of an acidic solution is _________________

1 x 10^-3

the pOH of a solution of NaOH is 11. what is the H+ for this solution

c

the pair of elements that forms a bond with the least ionic character is: a. Na and Cl b. K and Cl c. O and Cl d. Mg and Cl

d

the phrase "like dissolves like" refers to the fact that ______________ a. polar solvents dissolve nonpolar solutes and vice versa b. solvents can only dissolve solutes of similar molar mass c. gases can only dissolve other gases d. polar solvents dissolve polar solutes and nonpolar solvents dissolve nonpolar solvents

459 mm Hg

the pressure of a 70.0 L sample of gas is 600. mm Hg at 20.0 C. if the temperature drops to 15.0 C and the volume expands to 90.0 L, what will the pressure of the gas be?

40 atm

the pressure of a sample of helium in a 200 mL container is 2.0 atm. if the helium is compressed to a volume of 10. mL without changing the temperature, what would be the pressure of the gas?

tetrahedral

the shape of CI4

linear

the shape of CO2

trigonal-pyramidal

the shape of ClO3-

linear

the shape of HCl

trigonal-pyramidal

the shape of NH3

b

the solubility of most solid solutes _____________ as the temperature increases a. decreases b. increases c. remains constant d. increases then decreases

conjugate acid

the species that is formed by the addition of a proton to a base

7600 J

the specific heat of ethanol is 2.46. find the heat required to raise the temperature of 193 g of ethanol from 19 to 35 C

c

the substance whose Lewis structure shows three covalent bonds is a. H2O b. CH2Cl2 c. NH3 d. CCl4

9.0

the temperature of a 2.0 g sample of aluminum increased from 25C to 30C. how many joules of heat energy were added (specific heat of Al = 0.900)

423 K

the volume of a gas at 7.00 C is 49.0 mL. if the volume increases to 74.0 mL and the pressure is constant, what will the temperature of the gas be?

236 l

the volume of a gas is 120. L is 0.500 atm and 15.0 C. what volume will it occupy at 0.250 atm and 10.0 C?

SnS2

tin (IV) sulfide

d

to dissolve a substance, a solvent must attract particles of the substance more strongly than the ____________ attract each other a. solvent particles b. water molecules c. ions d. solute particles

number of valence electrons in each atom

to draw a Lewis structure, one must know the ____________________________________

1030 mL

to what volume will you have to dilute 30.0 mL of a 12.0 M HCl solution to make a 0.350 M HCl solution?

c

two moles of chlorine gas at 20.0 C are heated to 350 C while the volume is kept constant. the density of the gas a. increases b. decrease c. remains the same d. not enough information is given to correctly answer the question

d

under the same conditions of temperature and pressure, a liquid differs from a gas because the particles of the liquid a. are in constant straight-line motion b. take the shape of the container they occupy c. have no regular arrangement d. have stronger forces of attraction between them

130

using the equations below: C (s) + O2 (g) ---> CO2 (g) -390 kJ Mn (s) + O2 (g) ---> MnO2 (S) -520 kJ what is H for the following: MnO2(s) + C(s) --> Mn(s) + CO2(g)

c

water can dissolve charges particles because a. it is an ionic compound b. it is solid at 0C c. its atoms have partial charges d. it has a low molecular weight

glass

water has a specific heat f 4.184 while glass has one of 0.780. if 10 J of heat is added to 1.00 g of each of these, which will experience the larger increase of temperature?

1x10^-11 M

we have a 0.00100 M solution of OH- at 25C. what is the H3O+ in this solution?

0.35

we have a 0.45 M solution of H+. what is the pH of this solution at 25C?

3.33

we have a 4.63 x 10^-4 M solution of H+. what is the pH of this solution at 25C?

c

what are standard temperature and pressure conditions for gases? a. 0 K and 760 torr b. -273 C and 1 atm c. 0 C and 760 torr d. 0 C and 1 torr

the energy transferred between samples of matter because of a difference in their temperature

what best describes heat?

a measure of the average kinetic energy of the particles in a sample of matter

what best describes temperature?

c

what characteristic of a molecular compound is most likely to cause the compound to be very soluble in water? a. hydrogen content b. low boiling point c. high polarity d. small size

energy is released when bonds are formed and absorbed when they are broken

what energy changes occur when chemical bonds are formed and broken?

noble gas

what group of elements satisfies the octet rule without forming compounds?

c

what happens when KBr (s) is dissolved in water? a. Br- ions are attracted to the oxygen atoms of the water molecules b. Br- ions are repelled by the hydrogen atoms of the water molecules c. K+ ions are attracted to the oxygen atoms of the water molecules d. K+ ions are repelled by the oxygen atoms of the water molecules

double-headed arrow

what is placed between a molecule's resonance structure to indicate resonance?

electrons

what is shared in a covalent bond

5.22 x 10^-5

what is the concentration (in M) of hydronium ions in a solution at 25.0 C with pH = 4.282?

2.23 g/L

what is the density of the ethane gas, C2H6, at a pressure of 183.4 kPa and a temperature of 25 C?

8.08 grams

what is the mass of 4 moles of hydrogen gas?

exothermic

what is the name given to the type of a chemical reaction characterized by the release of heat energy?

2q

what is the pH of a solution with a pOH of 12?

2.60

what is the pH of an aqueous solution at 25.0 C in which H+ is 0.00250 M?

8.40

what is the pH of an aqueous solution at 25.0 C that contains 3.98 x 10^-9 M hydronium ion?

5.60

what is the pH of an aqueous solution at 25.0 C that contains 3.98 x 10^-9 hydroxide ion?

11.4

what is the pH of an aqueous solution at 25.0 in which OH- is 0.00250 M?

-0.40

what is the pOH of a 2.5 M OH-?

0.78 L

what is the volume of 2.0 g of CS2 vapor (molar mass = 76.15 g/mol) at 70 C and 736 mm Hg?

1500 g

what mass of propane, C3H8, must be burned in order to produce 76,000 kJ of energy? C3H8 + 5O2 ---> 3CO2 + 4H2O -2200 kJ

54g

what mass or iron mustreact to produce 3600 kJ of energy? 3Fe +2O2 ---> FeO4 -1120 kJ

hydrogen

what type of bonding is responsible for sugar being soluble in water?

26.4 L

what volume of hydrogen gas is produced at 1 atm and 25 C when 15.0 g of lithium is reacted?

0.67 L

what will the volume of a 0.50 M solution be if it contains 25 grams of Ca(OH)2?

d

when CaCl2 dissolves in water, the following will be produced. a. Ca and Cl b. Ca+2 and Cl- c. Ca and Cl2 d. Ca+2 and 2C-

0.19 J/gC

when a 4.0 g sample of glass was heated from 22.6 C to 63.9 C, the glass was found to have absorbed 32 J of heat. what is the specific heat?

the reaction is endothermic and H is positive

when the solid Ba(OH)2 and NH4SCN are mixed, a solution is produced and the temperature drops. what is true about the energies of the reaction?

c

which combination of solid and liquid would likely form a solution? a. ionic solid and non-polar liquid b. non-polar solid and polar liquid c. ionic solid and polar liquid d. polar solid and non-polar liquid

d

which is not a measurable property of gases? a. total volume occupied b. number of moles c. composition d. temperature in Kelvin

all

which is true about endothermic reactions? i. the system absorbs heat ii. the enthalpy change is positive iii. the enthalpy total for the reactants is greater than for the products

b

which of the following accounts for the fact that the boiling points of hydrogen fluoride (19.5 C) is significantly higher than that of hydrogen chloride (-84 C) despite the fact that HCl is the larger molecule? a. HCl has intermolecular hydrogen bonds b. HF has intermolecular hydrogen bonds c. HCl has greater London disperion forces than HF d. HF has greater London dispersion forces than HCl

a

which of the following compounds shows an abnormal boiling point due to hydrogen bonding? a. CH3NH2 b. CH3Cl c. CH3OCH3 d. CH3SH

c

which of the following describes the relationship between H3O+ AND OH-? a. H3O+ x OH- = 14.00 b. H3O+ + OH- = 14.00 c. H3O+ x OH- = 1.0 x 10^-14 d. H3O+ + OH- = 1.0 x 10^-14

d

which of the following gas molecules have the highest average kinetic energy at 25 C? a. H2 b. O2 c. N2 d. all the gases have the same average kinetic energy

a

which of the following gas molecules have the highest average velocity at 25 C? a. H2 b. O2 c. N2 d. all the gases have the same average velocity

d

which of the following indicates very strong intermolecular forces of attraction in a liquid? a. a very low boiling point b. a very low melting point c. a very low heat of vaporization d. a very low vapor pressure

c

which of the following is NOT an acid-base conjugate pair? a. HCN and CN- b. H2O and OH- c. H2S and OH- d. NH4+ and NH3

all

which of the following statements about exothermic reactions are correct? i. they have negative H values ii. the products have a lower enthalpy than the reactants iii. the products are more energetically stable than the reactants

b

which of the following will dissolve in polar solvents? a. non-polar solvents and ionic compounds b. ionic compounds and polar covalent compounds c. non-polar solvents and covalent compounds d. all of the above

a

which of the following would be expected to have the highest heat of vaporization? a. H2O b. HF c. NH3 d. all three are the same

C4H10

which of the following would have the highest volatility?: C4H10 or C5H12

CO

which of the following would have the highest volatility?: CO or NaCl

Cl2

which of the following would have the highest volatility?: Cl2 or Br2

Br2

which of the following would have the highest volatility?: ICl or Br2

PH3

which of the following would have the highest volatility?: NH3 or PH3

Na

which of the following would have the highest volatility?: Na or Al

Na

which of the following would have the highest volatility?: Na or Mg

C5H12

which of the following would you expect to have the higher melting point: C4H10 OR C5H12

Br2

which of the following would you expect to have the higher melting point: Cl2 or Br2

ICl

which of the following would you expect to have the higher melting point: ICl or Br2

NH3

which of the following would you expect to have the higher melting point: NH3 OR PH3

Al

which of the following would you expect to have the higher melting point: Na or Al

Mg

which of the following would you expect to have the higher melting point: Na or Mg

d

which one of the following is a non-electrolyte when dissolved in water? a. calcium chloride b. copper sulfate c. sodium chloride d. sugar

d

which one of the following is least soluble in water? a. CH3OH b. CH3CH2CH2OH c. CH3CH2OH d. CH3CH2CH2CH2CH2OH

b

which one of the following is linked with the correct intermolecular force of attraction? a. H2 - hydrogen bonding b. NH3 - hydrogen bonding c. AlH3 - London dispersion forces d. C2H4 - covalent bonding

b

which one of the following substances exhibits t he strongest intermolecular forces of attraction? a. CH4 b. CH3OH c. C2H6 d. C3H8

c

which one of the following would be an electrolyte when dissolved in water? a. I2 b. CH3I c. Ca(OH)2 d. C12H22O11

c

which solution contains the most dissolved particles? a. 1.0 M NaCl b. 6.0 M C6H12O6 c. 5.0 M NH4OH d. 0.80 M CH3COOH

c

which statement about solutions is INCORRECT? a. liquids that mix to form a single layer are said to be miscible b. solutions can be composed of any combination of the three phases of matter c. in a solution, the solvent is dissolved in the solute d. solutions will not separate under normal circumstances

gas

which states of matter would be characterized by each of the following: high individual molecular speeds

liquid

which states of matter would be characterized by each of the following: molecules close together but having sufficient kinetic energies to overcome the intermolecular forces

liquid

which states of matter would be characterized by each of the following: molecules move with respect to one another but are held together in a condensed state

gas

which states of matter would be characterized by each of the following: totally random molecular order with comparatively great distances between individual molecules

b

which substance below exhibits the weakest IMFs? a. SO2 b. CO2 c. SiO2 d. PH3

because the polarity matches the attractiveness

why do the melting points of the alkali metals decrease as you move down the column, but the halogen melting points increase?

b

with what type of substances do London dispersion forces play the most significant role? a. polar molecules b. non-polar molecules c. metals d. network compounds

CH

write the empirical formula for the following: C6H6

C4H9

write the empirical formula for the following: C8H18

CH3O

write the empirical formula for the following: CH3O

N2O5

write the empirical formula for the following: N2O5

WO2

write the empirical formula for the following: WO2

X3Y

write the empirical formula for the following: X39Y13

58,000 J

you wish to heat water to make coffee. how much heat must be used to raise the temperature of 180 grams of water from 19 to 96 C?