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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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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2.
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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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3.
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Aluminum reacts with oxygen to
produce aluminum oxide.
4 Al(s) + 3 O2(g) → 2
Al2O3(s)
If 5.0 moles of Al react with excess O2, how many moles of
Al2O3 can be formed? a. | 1.0 mol | b. | 2.0 mol | c. | 2.5 mol | d. | 5.0 mol | e. | 10.0 mol | | |
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4.
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The compound
P4S3 is used in matches. It reacts with oxygen to produce
P4O10 and SO2. The unbalanced chemical equation is shown
below.
P4S3(s) + O2(g) →
P4O10(s) + SO2(g)
What mass of O2 will react with
0.641 grams of P4S3? a. | 0.0466 g | b. | 0.0932 g | c. | 0.186 g | d. | 0.372 g | e. | 0.746 g | | |
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5.
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What is a correct method for
determining how many grams of oxygen react with 1.00 gram of pentane?
C5H12(g) + 8
O2(g) → 5 CO2(g) + 6
H2O(g)
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6.
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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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7.
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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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8.
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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(λ)
→ C9H8O4(s) +
C2H4O2(λ)
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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9.
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Under certain conditions the
reaction of ammonia with excess oxygen will produce a 38.2% yield of NO. How many grams of
NH3 must be reacted with excess oxygen to yield 17.5 g of NO?
4 NH3(g) + 5 O2(g)
→ 4 NO(g) + 6 H2O(g)
a. | 3.79 g | b. | 9.93 g | c. | 26.0 g | d. | 32.2 g | e. | 45.8 g | | |
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10.
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A 4.65 g sample of an oxide of
copper, when heated in a stream of hydrogen, produces Cu(s) and 0.585 g H2O. What is
formula for the compound? a. | Cu2O | b. | CuO | c. | CuO2 | d. | Cu2O3 | e. | Cu3O4 | | |
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