Multiple
Choice
Identify the letter of the choice that best completes the statement or answers the
question.
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1.
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The balanced equation for the
complete combustion of benzene, C6H6, is a. | C6H6(l) + 12 H2O → 6
CO2(g) + 15 H2(g) | b. | C6H6(l) → 6 C(s)
+ 3 H2(g) | c. | 2 C6H6(l) + 9 O2(g) → 12 CO (g) + 6 H2O(g) | d. | C6H6(l) + O2(g) →
CO2(g) + H2O(g) | e. | 2 C6H6(l) + 15 O2(g) → 12 CO2(g) + 6 H2O(g) | | |
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2.
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Iron reacts with hydrochloric
acid to produce iron (II) chloride and hydrogen gas.
Fe(s) + 2 HCl(aq) → FeCl2(aq) + H2(g)
How many moles of HCl will react with 3.5
moles of Fe? a. | 1.0 mol | b. | 1.8 mol | c. | 2.0 mol | d. | 7.0 mol | e. | 8.5 | | |
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3.
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Copper reacts with nitric acid
to produce copper nitrate, nitrogen dioxide gas, and water.
Cu(s) + 4 HNO3(aq) → Cu(NO3)2(aq) + 2 NO2(g) + 2
H2O(l)
If you have 0.60 moles of Cu, a. | you need at least 2.4 moles of
HNO3 to produce 1.2 moles of NO2. | b. | you need at least 0.60 moles of HNO3 to produce 0.60 moles of
Cu(NO3)2. | c. | you need at least 2.4 moles of
HNO3 to produce 2.4 moles of NO2. | d. | you need at least 0.15 moles of HNO3 to produce 0.60 moles of
Cu(NO3)2. | e. | you need at least 0.30 moles of
HNO3 to produce 0.60 moles of NO2. | | |
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4.
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The complete combustion of 2.0
moles of butane gas, C4H10, will a. | consume 13 mol O2 and produce 8.0 mol
H2O. | b. | consume 5.0 mol O2 and produce
13 mol CO2. | c. | consume 7.0 mol O2 and produce
8.0 mol CO2. | d. | produce 8 mol CO2 and 5.0 mol
H2O. | e. | consume 13 mol O2 and produce
8.0 mol CO2. | | |
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5.
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How many moles of
Fe2O3(s) is produced from the reaction of 0.34 mol Fe(s) with 0.30 mol
O2(g)? a. | 0.17 mol | b. | 0.20 mol | c. | 0.34 mol | d. | 0.51 mol | e. | 0.68 mol | | |
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6.
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Aspirin is produced by the
reaction of salicylic acid (molar mass = 138.1 g/mol) and acetic anhydride (molar mass = 102.1 g/mol).
C7H6O3(s) +
C4H6O3(l)
→ C9H8O4(s) +
C2H4O2(l)
If you mix 10.0 grams of each reactant, how many grams of aspirin (molar mass = 180.2 g/mol) can theoretically by obtained?
a. | 7.30 g | b. | 7.66 g | c. | 9.32 g | d. | 12.7 g | e. | 13.0 g | | |
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7.
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Nitroglycerine decomposes
violently according to the unbalanced chemical equation below. How many total moles of gases are
produced from the decomposition of 1.00 mol
C3H5(NO3)3?
C3H5(NO3)3(l) →
CO2(g) + N2(g) + H2O(g) + O2(g) a. | 4.00 mol | b. | 7.25 mol | c. | 16.5 mol | d. | 26.0 mol | e. | 29.0 mol | | |
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8.
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Aspirin is produced by the
reaction of salicylic acid (molar mass = 138.1 g/mol) and acetic anhydride (molar mass = 102.1 g/mol).
C7H6O3(s) +
C4H6O3(l)
→ C9H8O4(s) +
C2H4O2(l)
If 1.02 g of C9H8O4 (molar mass = 180.2 g/mol) is
produced from the reaction of 3.00 g C7H6O3 and 5.40 g
C4H6O3, what is the percent yield? a. | 7.11% | b. | 11.6% | c. | 15.9% | d. | 26.1% | e. | 43.1% | | |
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9.
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Which one of the following
compounds is a weak electrolyte when dissolved in water? a. | CH3CO2H | b. | NaCH3CO2 | c. | KNO3 | d. | Na2SO4 | e. | sugar | | |
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10.
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Which of the following
compounds are likely to be soluble in water: Ni(OH)2, ZnCl2, CuS,
Fe2(CO3)3, AgCl, and
Pb(NO3)2? a. | ZnCl2 | b. | ZnCl2 and Pb(NO3)2 | c. | CuS and AgCl | d. | Fe2(CO3)3
and Ni(OH)2 | e. | none of the compounds are
soluble | | |
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11.
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A precipitate will form when an
aqueous solution of iron(III) chloride is added to ________. a. | Ca(NO3)2 | b. | NaOH | c. | HCl | d. | NaCH3CO2 | e. | KClO4 | | |
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12.
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What is the net ionic equation
for the reaction of calcium carbonate with a strong acid?
a. | Ca(s) + 2 H+(aq) → Ca2+(aq) + H2(g) | b. | CaO(s) + 2 H+(aq) →
Ca2+(aq) + H2O(l) | c. | CaCO3(s) + 2 HCl(aq)
→ CaCl2(aq) +
H2CO3(aq) | d. | CaCO3(s) + 2 H+(aq)
→ Ca2+(aq) +
H2CO3(s) | e. | CaCO3(s) + 2 H+(aq)
→ Ca2+(aq) + CO2(g) + H2O(l) | | |
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13.
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Sulfuric acid is the product of
the reaction of ________ and H2O. a. | SO2 | b. | SO3 | c. | SO32- | d. | SO4- | e. | SO42- | | |
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14.
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A major use of calcium oxide
(lime. is in pollution control at coal burning power plants. Which reaction below occurs in the
smokestack of a power plant? a. | CaO(s) + SO3(g) → CaSO4(s) | b. | CaO(s) + SO3(g) → Ca(s) + SO2(g) + O2(g) | c. | CaO(s) + SO2(g) → CaS(s)
+ O2(g) | d. | 2 CaO(s) + C(s) → Ca2C(s) + O2(g) | e. | CaO(s) + C(s) → CaCO(s) | | |
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15.
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Which compound is the reducing
agent in the reaction below?
I-(aq) + ClO-(aq) →
IO-(aq) + Cl-(aq) a. | I- | b. | ClO- | c. | H2O | d. | IO- | e. | Cl- | | |
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16.
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Classify the reaction
below.
FeCl3(aq) + 3 NaOH(aq) →
Fe(OH)3(s) + 3 NaCl(aq) a. | gas forming | b. | oxidation-reduction | c. | acid-base | d. | precipitation | e. | decomposition | | |
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17.
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What is the mass, in grams, of
solute in 0.175 L of 3.17 × 10-2 M KCl? a. | 0.00555 g | b. | 0.181 g | c. | 0.255 g | d. | 0.414 g | e. | 13.5 g | | |
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18.
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The pH of 6.0 M KOH is 14.78.
What is the hydrogen ion concentration of this solution? a. | 1.7 × 10-15
M | b. | 2.2 ×
10-14 M | c. | 6.0 ×
10-14 M | d. | 1.0 ×
10-6 M | e. | 1.3 ×
10-1 M | | |
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19.
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Specific heat capacity
is a. | the quantity of heat required to melt 1.00 g of a substance. | b. | the mass of a substance 1.00 J of energy will heat by 1.00
K. | c. | the mass of a substance 1.00 cal of energy will heat by 1.00
K. | d. | the temperature change undergone when 1.00 g of a substance absorbs
1.00 cal. | e. | the quantity of heat needed to change 1.00 g of a substance by 1.00
K. | | |
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20.
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Heat capacity is defined
as a. | the amount of heat required to raise the temperature of a substance by 1
K. | b. | the amount of heat required to raise the temperature of 1 gram of
substance by 1 K. | c. | 4.18
J/g·K. | d. | 4.18 J/K. | e. | 4.18
cal/g·K. | | |
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21.
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Calculate ΔE of a gas for a process in which the gas evolves 27 J of heat and does 24 J of
work on the surroundings (i.e. the gas expands)? a. | -51 J | b. | -3 J | c. | +3 J | d. | 24 J | e. | +51 J | | |
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22.
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Commercial cold packs consist
of solid ammonium nitrate and water. NH4NO3 absorbs 330. J of heat per gram
dissolved in water. In a coffee-cup calorimeter, 3.00 g NH4NO3 is dissolved in
100.0 g of water at 24.0ºC. What
is the final temperature of the solution? Assume that the solution (whose total mass is 103.0 g) has
a specific heat capacity of 4.18 J/g·K. a. | 11.0 °C | b. | 15.9 °C | c. | 19.1 °C | d. | 21.6 °C | e. | 35.9 °C | | |
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23.
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Determine the heat of
vaporization of titanium(IV) chloride given the enthalpies of reaction
below.
Ti(s) + 2 Cl2(g) →
TiCl4(l) | ΔH =
-804.2 kJ | Ti(s) + 2 Cl2(g) →
TiCl 4(g) | ΔH =
-763.2 kJ | | |
a. | -1567.4 kJ | b. | 0.949 kJ | c. | 41.0 kJ | d. | 61.3 kJ | e. | 1567.4 kJ | | |
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24.
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The standard enthalpy change
for the combustion of propane is -2219.9 kJ.
C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(l)
Calculate the standard molar enthalpy of formation for propane based on the following
standard enthalpies of formation.
molecule | ΔHfº (kJ) | CO2(g) | -393.5 | H2O(l) | -285.8 | | |
a. | -103.8 kJ | b. | -102.8 kJ | c. | -74.8 kJ | d. | +52.1 kJ | e. | +1540.6 kJ | | |
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25.
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The standard enthalpy of
formation of CO2(g) is -393.5 kJ. What is the enthalpy change if 4.49 g C(s) reacts with
9.21 g O2(g) to form CO2(g)?
a. | -113 kJ | b. | -92.8 kJ | c. | -87.6 kJ | d. | -42.7 kJ | e. | -27.8 kJ | | |
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Completion
Complete each sentence or statement.
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26.
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The percent yield of a chemical
reaction is calculated by dividing the actual yield by the __________.
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27.
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A ________ agent loses
electrons in an oxidation-reduction reaction.
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28.
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________ acid is produced in a
larger quantity than any other chemical in the United States. This chemical is used in the production
of fertilizers, pigments, alcohol, paper and detergents.
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29.
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The net ionic equation for the
reaction of silver nitrate and sodium chloride is as follows.
Ag+(aq) + Cl-(aq)
→ AgCl(s)
Sodium and nitrate ions are referred to as ________ ions because they
are not involved in the reaction.
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Essay
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30.
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Give the name of an acidic
oxide and write a balanced chemical equation for the reaction of the oxide with water.
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31.
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The pH of a sodium hydroxide
solution gradually decreases if the solution is left in contact with air. In fact, the process can be
hastened if a person exhales over a sodium hydroxide solution. Write a balanced chemical equation
that describes the process by which the sodium hydroxide concentration decreases.
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32.
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You can remove a piece of
aluminum foil from a hot oven without using an oven mitt to protect your hand. Why do you not get
burned?
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33.
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What is one advantage and one
disadvantage of using hydrogen gas as fuel?
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