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
combustion of propane produces carbon dioxide and steam.
C3H8(g) + 5 O2(g)
→ 3
CO2(g) + 4 H2O(g)
All of the following statements concerning this reaction are correct
EXCEPT a. | three molecule
of carbon dioxide are formed per one molecule of propane consumed. | b. | five molecules
of oxygen are consumed per one molecule of propane consumed. | c. | four moles of
steam are formed per five moles of oxygen consumed. | d. | the combined
mass of reactants consumed equals the mass of products formed. | e. | three grams of
carbon dioxide are formed per five grams of oxygen consumed. | | |
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2.
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Ammonia is prepared by reacting nitrogen and hydrogen gases at high temperature
according to the unbalanced chemical equation below.
__ N2(g) + __ H2(g)
→ __
NH3(g)
What are the respective coefficients when the equation
is balanced with the smallest whole numbers? a. | 1, 1, 1 | b. | 1, 3,
1 | c. | 1, 3,
2 | d. | 2, 1,
2 | e. | 2, 3,
2 | | |
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3.
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When
methanol undergoes complete combustion, the products are carbon dioxide and
water.
__ CH3OH(l) + __
O2(g) → __ CO2(g) + __
H2O(g)
What are the respective coefficients when the equation
is balanced with the smallest whole numbers? a. | 1, 1, 1, 1 | b. | 1, 2, 1,
2 | c. | 2, 2, 2,
4 | d. | 2, 3, 2,
4 | e. | 2, 4, 6,
4 | | |
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4.
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The
reaction of calcium with elemental chlorine yields calcium chloride. Write a balanced chemical
equation for this reaction. a. | Ca(s) + Cl2(g) → CaCl(s) +
Cl(g) | b. | Ca(s) + Cl2(g) →
CaCl2(s) | c. | Ca(s) + 2 Cl2(g) →
CaCl4(s) | d. | 2 Ca(s) + Cl2(g) → 2
CaCl(s) | e. | 4 Ca(s) + Cl2(g) → 2
Ca2Cl(s) | | |
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5.
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Metals react with oxygen to give oxides with the general formula
MxOy. Write a balanced chemical equation for the reaction of iron with oxygen
to yield iron(III) oxide. a. | Fe(s) + O2(g) →
FeO2(s) | b. | 2 Fe(s) + 3 O2(g) →
Fe2O3(s) | c. | 3 Fe(s) + O2(g) →
Fe3O2(s) | d. | 4 Fe(s) + 3 O2(g) → 2
Fe2O3(s) | e. | 6 Fe(s) + O2(g) → 2
Fe3O(s) | | |
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6.
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The
products of the complete combustion of a hydrocarbon are carbon dioxide and water. Write a balanced
chemical equation for the combustion of pentane, C5H12. a. | C5H12(g) + 8 O2(g) → 5
CO2(g) + 6 H2O(g) | b. | C5H12(g) → 5 C(s) + 6
H2(g) | c. | C5H12(g) + 9 O2(g)
→ 4
CO2(g) + 5 H2O(g) | d. | C5H12(g) + 11 O2(g)
→
C5O10(g) + 6 H2O(g) | e. | C5H12(g) + 11 O2(g) → 5
CO2(g) + 12 H2O(g) | | |
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7.
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The
balanced equation for the complete combustion of benzene, C6H6,
is a. | C6H6(l) → 6 C(s) + 3 H2(g) | b. | C6H6(l) + 12 H2O(l) → 6 CO2(g) + 15 H2(g) | c. | C6H6(l) + O2(g) → CO2(g) + H2O(g) | d. | 2
C6H6(l) + 9 O2(g) → 12 CO (g) + 6 H2O(g) | e. | 2
C6H6(l) + 15 O2(g) → 12 CO2(g) + 6 H2O(g) | | |
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8.
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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 4.6 moles of
Fe? a. | 2.3
mol | b. | 2.8
mol | c. | 4.6
mol | d. | 6.9
mol | e. | 9.2
mol | | |
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9.
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The
complete combustion of 0.40 moles of butane gas, C4H10, will a. | consume 0.40 mol
O2 and produce 0.20 mol CO2. | b. | consume 0.80 mol
O2 and produce 0.40 mol CO2. | c. | consume 1.3 mol
O2 and produce 0.80 mol CO2. | d. | consume 2.6 mol
O2 and produce 1.6 mol CO2. | e. | consume 5.2 mol
O2 and produce 3.2 mol CO2. | | |
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10.
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The
reaction of water and coal at a high temperature produces a mixture of hydrogen and carbon monoxide
gases. This mixture is known as synthesis gas (or syngas). What mass of hydrogen gas can be formed
from the reaction of 51.3 g of carbon with excess water?
C(s) + H2O(g) → H2(g) + CO(g)
a. | 4.31
g | b. | 8.61
g | c. | 17.2
g | d. | 1.20
´ 102
g | e. | 306
g | | |
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11.
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What
mass of carbon dioxide is produced by the complete combustion of 5.50 grams of hexane,
C6H14? a. | 0.468 g | b. | 2.81
g | c. | 3.06
g | d. | 16.9
g | e. | 33.7
g | | |
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12.
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What
mass of oxygen is consumed by the complete combustion of 23.0 grams of
ethylene?
C2H4(g) + 3 O2(g)
→ 2
CO2(g) + 2 H2O(g)
a. | 8.75 g | b. | 26.2
g | c. | 60.5
g | d. | 69.0
g | e. | 78.7
g | | |
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13.
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What
is a correct method for determining how many moles of calcium oxide are produced in the reaction of
10.0 g calcium with excess oxygen?
2 Ca(s) +
O2(g) → 2 CaO(s)
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14.
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How
many moles of potassium bromide can be produced from the reaction of 2.92 moles of potassium with
1.78 moles of bromine gas?
2 K(s) +
Br2(g) →
2
KBr(s)
a. | 1.46
mol | b. | 1.78
mol | c. | 2.92
mol | d. | 3.56
mol | e. | 5.84
mol | | |
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15.
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How
many moles of Fe2O3(s) can be produced from the reaction of 0.45 mol Fe(s) with
0.30 mol O2(g)? a. | 0.15 mol | b. | 0.20
mol | c. | 0.23
mol | d. | 0.45
mol | e. | 0.75
mol | | |
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16.
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Nitric oxide is made from the oxidation of ammonia. How many moles of nitric oxide can
be made from the reaction of 3.80 mol NH3 with 5.15 mol
O2?
4 NH3(g) + 5 O2(g)
→
4 NO(g) + 6
H2O(g)
a. | 3.80 mol | b. | 4.12
mol | c. | 5.15
mol | d. | 6.44
mol | e. | 8.95
mol | | |
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17.
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Sulfur trioxide is made from the reaction of sulfur dioxide and oxygen. How many grams
of SO3 can be made from the reaction of 3.00 g SO2 with 2.02 g
O2?
2 SO2(g) + O2(g)
→ 2
SO3(g)
a. | 2.53 g | b. | 3.75
g | c. | 5.02
g | d. | 5.05
g | e. | 10.1
g | | |
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18.
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Magnesium reacts with iodine gas at high temperatures to form magnesium iodide. What
mass of MgI2 can be produced from the reaction of 4.44 g Mg and 13.4 g
I2? a. | 2.76
g | b. | 14.7
g | c. | 16.0
g | d. | 17.8
g | e. | 50.8
g | | |
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19.
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The
reaction of 10.0 g H2(g) with 10.0 g O2(g) yields 8.43 g H2O(g).
What is the percent yield of this reaction? a. | 9.43% | b. | 27.3% | c. | 42.2% | d. | 66.8% | e. | 74.9% | | |
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20.
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Aspirin is produced by the reaction of salicylic acid (M = 138.1 g/mol) and
acetic anhydride (M = 102.1 g/mol).
C7H6O3(s) +
C4H6O3(l) → C9H8O4(s) +
C2H4O2(l)
If 2.04 g of C9H8O4
(M = 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. | 14.2% | b. | 21.4% | c. | 24.3% | d. | 52.1% | e. | 68.0% | | |
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