E)
4.54 mol
117. Calculate the number of moles of O2 required to react with phosphorus to produce 4.76 g of
P4O6. (Molar mass P4O6 = 219.9 g/mol)
A)
0.0216 mol
B)
0.149 mol
C)
0.0649 mol
D)
0.0433 mol
E)
0.130 mol
118. Elemental sulfur can be converted to sulfur dioxide by combustion in air. Sulfur dioxide
will react with water to form sulfurous acid (see balanced equation below).
SO2(g) + H2O(l) → H2SO3(l)
What mass of sulfur dioxide is needed to prepare 36.86 g of H2SO3(l)?
A)
28.77 g
B)
47.23 g
C)
0.5754 g
D)
0.4491 g
E)
36.86 g
119. One step in the isolation of pure rhodium metal (Rh) is the precipitation of rhodium(III)
hydroxide from a solution containing rhodium(III) sulfate according to the following
balanced chemical equation:
Rh2(SO4)3(aq) + 6NaOH(aq) → 2Rh(OH)3(s) + 3Na2SO4(aq)
If 2.40 g of rhodium(III) sulfate reacts with excess sodium hydroxide, what mass of
rhodium(III) hydroxide may be produced?
A)
1.50 g
B)
4.80 g
C)
2.40 g
D)
0.374 g
E)
2.99 g
120. Pure copper may be produced by the reaction of copper(I) sulfide with oxygen gas as
follows:
Cu2S(s) + O2(g) → 2Cu(s) + SO2(g)
What mass of copper(I) sulfide is required in order to prepare 0.610 kg of copper metal?
A)
0.610 kg
B)
0.305 kg
C)
0.459 kg
D)
1.53 kg
E)
0.764 kg
121. One step in the isolation of pure rhodium metal (Rh) is the precipitation of rhodium(III)
hydroxide from a solution containing rhodium(III) sulfate according to the following
balanced chemical equation:
Rh2(SO4)3(aq) + 6NaOH(aq) → 2Rh(OH)3(s) + 3Na2SO4(aq)
What mass of sodium hydroxide is required to precipitate 74.0 g of rhodium(III) hydroxide
from a solution containing excess rhodium(III) sulfate?
A)
6.41 g
B)
57.7 g
C)
19.2 g
D)
222 g
E)
74.0 g
122. Pure copper may be produced by the reaction of copper(I) sulfide with oxygen gas as
follows:
Cu2S(s) + O2(g) → 2Cu(s) + SO2(g)
If 0.680 kg of copper(I) sulfide reacts with excess oxygen, what mass of copper metal may
be produced?
A)
0.680 kg
B)
0.136 kg
C)
0.271 kg
D)
0.543 kg
E)
1.36 kg
Test Bank General Chemistry, 10th edition 34
123. One step in the isolation of pure rhodium metal (Rh) is the precipitation of rhodium(III)
hydroxide from a solution containing rhodium(III) sulfate according to the following
balanced chemical equation:
Rh2(SO4)3(aq) + 6NaOH(aq) → 2Rh(OH)3(s) + 3Na2SO4(aq)
If 0.620 g of rhodium(III) hydroxide is produced, what mass of sodium sulfate is also
produced?
A)
0.572 g
B)
0.930 g
C)
0.858 g
D)
0.620 g
E)
0.381 g
124. The balanced equation for the combustion of ethanol is
2C2H5OH(g) + 7O2(g) → 4CO2(g) + 6H2O(g)
How many grams of dioxygen are required to burn 5.9 g of C2H5OH?
A)
14 g
B)
21 g
C)
4.1 g
D)
38 g
E)
55 g
125. 2Al(s) + 6HCl(aq) → 2AlCl3(aq) + 3H2(g)
According to the equation above, how many grams of aluminum are needed to completely
react with 3.83 mol of hydrochloric acid?
A)
310 g
B)
46.6 g
C)
34.4 g
D)
3.83 g
E)
103.3 g
Test Bank General Chemistry, 10th edition 35
126. A chemical reaction has the equation: 2A + B → C. In which case is B the limiting
reactant?
A)
II
B)
I
C)
III
D)
IV
E)
none of these
127. Consider an initial mixture of CH4 and O2 represented in the container below:
Given the reaction CH4 + 2O2 → CO2 + 2H2O, which of the following represents a
stoichiometric picture of the container after the reaction has gone to completion?
A)
Test Bank General Chemistry, 10th edition 36
B)
C)
D)
E)
none of the above
128. Which of the following statements concerning the limiting reactant is/are correct?
1.
The mass of the limiting reactant is the always the lowest mass of all reactant
masses.
2.
The theoretical yield depends on the amount of limiting reactant.
3.
The moles of limiting reactant is always the lowest moles of all reactants.
A)
2 only
B)
3 only
C)
1 and 3
D)
2 and 3
E)
1, 2, and 3
129. The limiting reactant is the reactant
Test Bank General Chemistry, 10th edition 37
A)
that has the lowest coefficient in the balanced equation.
B)
that has the lowest molar mass.
C)
that is left over after the reaction has gone to completion.
D)
for which there is the lowest mass in grams.
E)
none of the above
130. The commercial production of phosphoric acid, H3PO4, can be represented by the equation
1500 g
307 g
1180 g
300 g
Ca3(PO4)2 +
5C +
5O2 +
3H2O
→ 3CaSiO3 + 5CO2 + 2H3PO4
310 g/mol
12.0 g/mol
32.0 g/mol
18.0 g/mol
The molar mass for each reactant is shown below the reactant, and the mass of each reactant
for this problem is given above. Which substance is the limiting reactant?
A)
H2O
B)
C
C)
O2
D)
Ca3(PO4)2
E)
SiO2
131. SO2 reacts with H2S as follows:
2H2S + SO2 → 3S + 2H2O
When 7.50 g of H2S reacts with 12.75 g of SO2, which statement applies?
A)
6.38 g of sulfur is formed.
B)
SO2 is the limiting reagent.
C)
0.0216 mol of H2S remains.
D)
10.6 g of sulfur is formed.
E)
1.13 g of H2S remains.
132. A 15-g sample of lithium is reacted with 15 g of fluorine to form lithium fluoride:
2Li + F2 → 2LiF. After the reaction is complete, what will be present?
A)
0.789 mol of lithium fluoride only
B)
2.16 mol of lithium fluoride only
C)
2.16 mol of lithium fluoride and 0.395 mol of fluorine
D)
0.789 mol of lithium fluoride and 1.37 mol of lithium
E)
none of these
133. When 20.0 g C2H6 and 60.0 g O2 react to form CO2 and H2O, how many grams of water are
formed?
A)
14.5 g
B)
58.0 g
C)
18.0 g
D)
20.0 g
E)
none of these
134. If 48.8 g of O2 is mixed with 48.8 g of H2 and the mixture is ignited, what is the maximum
mass of water that may be produced?
A)
439 g
B)
54.9 g
C)
48.8 g
D)
98 g
E)
86.8 g
135. One step in the isolation of pure rhodium metal (Rh) is the precipitation of rhodium(III)
hydroxide from a solution containing rhodium(III) sulfate according to the following
balanced chemical equation:
Rh2(SO4)3(aq) + 6NaOH(aq) → 2Rh(OH)3(s) + 3Na2SO4(aq)
What is the theoretical yield of rhodium(III) hydroxide from the reaction of 0.590 g of
rhodium(III) sulfate with 0.266 g of sodium hydroxide?
A)
0.341 g
B)
0.266 g
C)
0.184 g
D)
0.856 g
E)
0.368 g
Test Bank General Chemistry, 10th edition 39
136. A 5.95-g sample of AgNO3 is reacted with BaCl2 according to the equation
2AgNO3(aq) + BaCl2(aq) → 2AgCl(s) + Ba(NO3)2(aq)
to give 3.36 g of AgCl. What is the percent yield of AgCl?
A)
44.6 %
B)
33.5 %
C)
66.9 %
D)
56.5 %
E)
100 %
137. The reaction of 11.9 g of CHCl3 with excess chlorine produced 10.2 g of CCl4, carbon
tetrachloride:
2CHCl3 + 2Cl2 → 2CCl4 + 2HCl
What is the percent yield?
A)
85.7 %
B)
100 %
C)
66.5 %
D)
33.3 %
E)
44.3 %
138. Consider the following reaction:
2A + B → 3C + D
3.0 mol A and 2.0 mol B react to form 4.0 mol C. What is the percent yield of this reaction?
A)
75 %
B)
67 %
C)
89 %
D)
50 %
E)
100 %
139. Pure copper may be produced by the reaction of copper(I) sulfide with oxygen gas as
follows:
Cu2S(s) + O2(g) → 2Cu(s) + SO2(g)
If the reaction of 0.630 kg of copper(I) sulfide with excess oxygen produces 0.190 kg of
copper metal, what is the percent yield?
Test Bank General Chemistry, 10th edition 40
A)
75.5 %
B)
39.9 %
C)
30.2 %
D)
151 %
E)
37.8 %
140. One step in the isolation of pure rhodium metal (Rh) is the precipitation of rhodium(III)
hydroxide from a solution containing rhodium(III) sulfate according to the following
balanced chemical equation:
Rh2(SO4)3(aq) + 6NaOH(aq) → 2Rh(OH)3(s) + 3Na2SO4(aq)
If the reaction of 0.650 g of rhodium(III) sulfate with excess sodium hydroxide produces
0.320 g of rhodium(III) hydroxide, what is the percent yield?
A)
316 %
B)
158 %
C)
39.5 %
D)
49.2 %
E)
79.0 %
141. Sulfur trioxide, SO3, is made from the oxidation of SO2, and the reaction is represented by
the equation:
2SO2 + O2 → 2SO3
A 21-g sample of SO2 gives 18 g of SO3. The percent yield of SO3 is .
A)
11 %
B)
69 %
C)
17 %
D)
26 %
E)
100 %
142. Nitric oxide, NO, is made from the oxidation of NH3, and the reaction is represented by the
equation
4NH3 + 5O2 → 4NO + 6H2O
An 9.1-g sample of NH3 gives 12.0 g of NO. The percent yield of NO is .
A)
94 %
B)
46 %
C)
17 %
D)
75 %
E)
28 %
143. Consider the fermentation reaction of glucose:
C6H12O6 → 2C2H5OH + 2CO2
A 1.00-mol sample of C6H12O6 was placed in a vat with 100 g of yeast. If 67.8 g of C2H5OH
was obtained, what was the percent yield of C2H5OH?
A)
73.6 %
B)
36.8 %
C)
67.8 %
D)
100 %
E)
none of these
144. One commercial system removes SO2 emissions from smoke at 95.0°C by the following set
of balanced reactions:
SO2(g) + Cl2 → SO2Cl2(g)
SO2Cl2 + 2H2O → H2SO4 + 2HCl
H2SO4 + Ca(OH)2 → CaSO4(s) + 2H2O
Assuming the process is 95.0 % efficient, how many grams of CaSO4 may be produced
from 100. g of SO2? (molar masses: SO2, 64.1 g/mol; CaSO4, 136 g/mol)
A)
87.2 g
B)
202 g
C)
44.8 g
D)
47.1 g
E)
212 g