Test Bank General Chemistry, 10th edition 21
75. The net ionic equation for the reaction between aqueous ammonia and hydrobromic acid is
A)
HBr(aq) + NH3(aq) → NH4Br(aq).
B)
H+(aq) + OH–(aq) → H2O(l).
C)
HBr(aq) + OH–(aq) → Br–(aq) + H2O(l).
D)
H+(aq) + NH3(aq) → NH4+(aq).
E)
H+(aq) + Br–(aq) + NH3(aq) → NH4+(aq) + Br–(aq).
76. Which of the following best represents the molecular equation for the reaction of aqueous
ammonia with sulfuric acid?
A)
2NH3(aq) + H2SO4(aq) → (NH4)2SO4(aq)
B)
NH3(aq) + H2SO4(aq) → NH4SO4(aq)
C)
NH4OH(aq) + H2SO4(aq) → NH4SO4(aq) + H2O(l)
D)
2NH4+(aq) + H2SO4(aq) → (NH4)2SO4(aq) + 2H+(aq)
E)
2NH4+(aq) + H2SO4(aq) → (NH4)2SO4(aq) + H2(g)
77. The net ionic equation for the reaction of nitrous acid with lithium hydroxide is
A)
H+(aq) + OH–(aq) → H2O(l).
B)
HNO2(aq) + OH–(aq) → NO2–(aq) + H2O(l).
C)
HNO3(aq) + LiOH(aq) → LiNO3(aq) + H2O(l).
D)
HNO3(aq) + LiOH(aq) → Li+(aq) + NO3–(aq) + H2O(l).
E)
H+(aq) + NO2–(aq) + Li+(aq) + OH–(aq) → Li+(aq) + NO2–(aq) + H2O(l).
78. What is the net ionic equation for the reaction that occurs between nitrous acid and
strontium hydroxide?
A)
HNO2(aq) + OH–(aq) → NO2–(aq) + H2O(l)
B)
2HNO2(aq) + Sr(OH)2 → Sr(NO2)2(aq) + H2O(l)
C)
2H+(aq) + 2NO2–(aq) + Sr2+(aq) + 2OH–(aq) → Sr(NO2)2(aq) + H2O(l)
D)
2H+(aq) + 2NO2–(aq) + Sr2+(aq) + 2OH–(aq) → Sr2+(aq) + 2NO2–(aq) + 2H2O(l)
E)
H+(aq) + OH–(aq) → H2O(l)
79. In the reaction of acetic acid with aqueous sodium hydroxide, what is the spectator ion?
A)
OH–(aq)
B)
There is no spectator ion.
C)
C2H3O2–(aq)
D)
Na+(aq)
E)
H+(aq)
80. The balanced net ionic equation for the reaction of magnesium sulfite with nitric acid is
A)
MgSO3(s) + 2H+(aq) → Mg2+(aq) + SO2(g) + H2O(l).
B)
Mg2+(aq) + CO32–(aq) + 2H+(aq) + 2NO3–(aq) → Mg(NO3)2(aq) + SO2(g) +
H2O(l).
C)
MgSO3(s) + 2HNO2(aq) → Mg2+(aq) + 2NO2–(aq) + SO2(g) + H2O(l).
D)
Mg(HSO3)2(s) + 2HNO3(aq) → Mg2+(aq) + 2NO3–(aq) + SO2(g) + 2H2O(l).
E)
MgSO3(s) + 2HNO3(aq) → Mg2+(aq) + 2NO3–(aq) + SO2(g) + H2O(l).
81. Which of the following concerning oxidation-reduction reactions is/are correct?
1.
Oxidation-reduction reactions always form gaseous products.
2.
At least one substance is oxidized and one substance is reduced in an
oxidation-reduction reaction.
3.
The species that is oxidized loses one or more electrons in an oxidation-
reduction reaction.
A)
1 only
B)
2 only
C)
3 only
D)
1 and 3
E)
2 and 3
82. Which of the following is an oxidation–reduction reaction?
A)
PbCO3(s) + 2HNO3(aq) → Pb(NO3)2(aq) + CO2(g) + H2O(l)
B)
Na2O(s) + H2O(l) → 2NaOH(aq)
C)
SO3(g) + H2O(l) → H2SO4(aq)
D)
CO2(g) + H2O(l) → H2CO3(aq)
E)
C2H4(g) + H2(g) → C2H6(g)
83. All the following are oxidation–reduction reactions except
A)
H2(g) + F2(g) → 2HF(g).
B)
Ca(s) + H2(g) → CaH2(s).
C)
2K(s) + 2H2O(l) → 2KOH(aq) + H2(g).
D)
6Li(s) + N2(g) → 2Li3N(s).
E)
Mg3N2(s) + 6H2O(l) → 3Mg(OH)2(s) + 2NH3(g).
84. Which of the following chemical reactions is an oxidation–reduction reaction?
A)
Zn(s) + S(s) → ZnS(s)
B)
H2SO4(aq) + 2NaOH(aq) → Na2SO4(aq) + 2H2O(l)
C)
NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(l)
D)
AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq)
E)
CO2(aq) + H2O(aq) → H2CO3(aq)
85. Which one of the following is necessary in order for a metal to be oxidized?
A)
addition of electrons
B)
removal of electrons
C)
addition of oxygen
D)
removal of oxygen
E)
addition of hydrogen
86. Which of the following reactions is an oxidation–reduction reaction?
A)
CaCO3(s) + 2HCl(aq) → CaCl2(aq) + H2O(l) + CO2(g)
B)
NH4NO3(aq) → N2O(g) + 2H2O(l)
C)
AgNO3(aq) + KI(aq) → AgI(s) + KNO3(aq)
D)
CaO(s) + SO3(g) → CaSO4(s)
E)
H2SO4(aq) + 2NaOH(s) → Na2SO4(aq) + 2H2O(l)
87. Which of the following chemical reactions is an oxidation–reduction reaction?
A)
Mg(s) + CO2(g) → MgO(s) + CO(g)
B)
H2SO4(aq) + Ba(OH)2(aq) → BaSO4(s) + 2H2O(l)
C)
Pb(NO3)2(aq) + 2HCl(aq) → PbCl2(s) + 2HNO3(aq)
D)
CO2(aq) + H2O(l) → H2CO3(aq)
E)
NH3(g) + HCl(g) → NH4Cl(s)
88. Which of the following is best described as an oxidation–reduction reaction?
A)
SO2(g) + H2O(l) → H2SO3(aq)
B)
2Cl(g) → Cl2(g)
C)
3O2(g) → 2O3(g)
D)
2NO2(g) → N2O4(g)
E)
SO2(g) + O2(g) → SO3(g)
89. Which of the following reactions involves neither oxidation nor reduction?
A)
N2(g) + 3H2(g) → 2NH3(g)
B)
NH4NO2(s) → N2(g) + 2H2O(l)
C)
Cu(s) + 2Ag+(aq) → Cu2+(aq) + 2Ag(s)
D)
2CrO42–(aq) + 2H+(aq) → Cr2O72–(aq) + H2O(l)
E)
C2H4(g) + H2(g) → C2H6(g)
Test Bank General Chemistry, 10th edition 25
90. Which of the following conversions is not an oxidation–reduction reaction?
A)
conversion of Mn2O3 to MnO2
B)
conversion of K to KCl
C)
conversion of NaBr to Br2
D)
conversion of CaCO3 to CaO
E)
conversion of VO2+ to VO2+
91. All the following species can be reduced except
A)
ClO2.
B)
F–.
C)
NO3–.
D)
H+.
E)
Fe3+.
92. Which of the following species cannot function as an oxidizing agent?
A)
S
B)
Br–
C)
H+
D)
MnO4–
E)
Mn2+
93. What is the oxidation number of each O in BaFeO4?
A)
+6
B)
+2
C)
-2
D)
+3
E)
0
94. Which of the following species cannot function as an oxidizing agent?
Test Bank General Chemistry, 10th edition 26
A)
Co3+
B)
O2
C)
Cr2O72–
D)
MnO4–
E)
O2–
95. What is the oxidation number of each H in NH4(H2PO4)?
A)
-3
B)
-2
C)
+1
D)
+5
E)
0
96. The oxidation number of nitrogen given for all the following species is correct except
A)
N2H4 (–2).
B)
N2O (+1).
C)
NH2OH (–1).
D)
HNO2 (+3).
E)
HN3 (–1).
97. In which one of the following is the oxidation number of nitrogen given incorrectly?
A)
N2H4 (–2)
B)
NaN3 (–1)
C)
HNO2 (+3)
D)
N2O3 (+3)
E)
H2N2O2 (+1)
98. What is the average oxidation number of C in C6H12O6?
A)
–2
B)
0
C)
+1
D)
+2
E)
–1
99. The oxidation number of carbon in the formate ion, HCOO–, is
A)
0.
B)
–2.
C)
+2.
D)
–1.
E)
+1.
100. The oxidation numbers of nitrogen in N2O and N2F4 are, respectively,
A)
–2 and +2.
B)
–2 and –3.
C)
+1 and +2.
D)
+1 and –1.
E)
+1 and –3.
101. The sum of all the oxidation numbers in cysteine, , is
A)
–1.
B)
+4.
C)
0.
D)
–2.
E)
+2.
102. The oxidation number of barium in BaO is
A)
+1.
B)
+4.
C)
–1/2.
D)
+2.
E)
–2.
103. The oxidation number of chromium in sodium chromite, NaCrO2, is
A)
–1.
B)
–2.
C)
+2.
D)
+1.
E)
+3.
104. In which of the following molecules or ions does the underlined element have an oxidation
number of –3?
A)
NO2
B)
PH4+
C)
CrO2Cl2
D)
HNO2
E)
Zn(OH)42–
105. Which of the following is a correct set of oxidation numbers for the atoms in calcium
dihydrogen phosphate, Ca(H2PO4)2?
A)
Ca = +2, H = +1, P = +5, O = –2
B)
Ca = +2, H = 0, P = +7, O = –8
C)
Ca = +2, H = –1, P = +4, O = –2
D)
Ca2+ = +2, H2PO4– = –1
E)
Ca = +2, H = +1, P = +3, O = –2
Test Bank General Chemistry, 10th edition 29
106. Assign oxidation numbers to each atom in nitrous acid.
A)
H = +1, N = +5, O = –1
B)
H = +1, N = +5, O = –2
C)
H = +1, N = +3, O = –1
D)
H = +1, N = +3, O = 0
E)
H = +1, N = +3, O = –2
107. In basic solution the chromate ion, CrO42–, can be converted to the chromite, CrO2–, ion. The
number of electrons gained or lost by the chromium atom is
A)
0.
B)
3 electrons lost.
C)
2 electrons lost.
D)
3 electrons gained.
E)
2 electrons gained.
108. What is the reduction half-reaction for the reaction of zinc with hydrochloric acid?
Zn(s) + 2H+(aq) + 2Cl–(aq) → Zn2+(aq) + 2Cl–(aq) + H2(g)
A)
Zn(s) → Zn2+(aq) + 2e–
B)
2H+(aq) + 2e– → H2(g)
C)
2H+(aq) + 2e–(aq) → H2(g) + 2Cl–(aq)
D)
2H+(aq) + 2Cl–(aq) → H2(g) + 2e– + 2Cl–(aq)
E)
Zn(s) → Zn2+(aq) + 2Cl–(aq) + 2e–
109. What is the reduction half-reaction for the reaction between iron(II) sulfate and potassium
permanganate in a sulfuric acid solution?
5Fe2+(aq) + MnO4–(aq) + 8H+(aq) → 5Fe3+(aq) + Mn2+(aq) + 4H2O(l)
Test Bank General Chemistry, 10th edition 30
A)
MnO4–(aq) + 3e– → Mn2+(aq) + 4H2O(l)
B)
MnO4–(aq) + 8H+(aq) + 5e– → Mn2+(aq) + 4H2O(l)
C)
5Fe2+(aq) → 5Fe3+(aq) + 5e–
D)
Fe2+(aq) + 2e– → Fe(s)
E)
MnO4–(aq) + 5e– → Mn2+(aq) + SO42–(aq)
110. What is the balanced oxidation half-reaction for the following reaction?
Cu2+(aq) + Fe(s) → Cu(s) + Fe2+(aq)
A)
Cu(s) + 2e– → Cu(s)
B)
Cu2+(aq) + 2e– → Cu(s)
C)
Fe2+(aq) + 2e– → Fe(s)
D)
Cu(s) → Cu2+(aq) + 2e–
E)
Fe(s) → Fe2+(aq) + 2e–
111. Consider the reaction of sulfur dioxide and water, which is represented by the following
equation:
2SO2(g) + 2H2O(g) → 2H2S(g) + 3O2(g)
How many moles of electrons are transferred according to the equation that is written?
A)
2
B)
6
C)
4
D)
12
E)
8
112. In the following reaction, which species is oxidized?
3Na2S(s) + 8H+(aq) + 2NO3–(aq) → 6Na+(aq) + 3S(s) + 2NO(g) + 4H2O(l)
A)
NO3–
B)
Na2S
C)
Na+
D)
NO
E)
H+
113. For the reaction that occurs in a lead storage battery,
Pb(s) + PbO2(s) + 2H+(aq) + 2HSO4–(aq) → 2PbSO4(s) + 2H2O(l)
the oxidizing agent is
A)
HSO4–.
B)
PbSO4.
C)
Pb.
D)
PbO2.
E)
H+.
114. In the balanced equation
3Na+(aq) + 3OH–(aq) + P4(s) + 3H2O(l) → 3Na+(aq) + 3H2PO2–(aq) + PH3(g)
what is the reducing agent?
A)
OH–
B)
Na+
C)
H2O
D)
P4
E)
PH3
115. In the following oxidation–reduction reaction,
8H+(aq) + 6Cl–(aq) + Sn(s) + 4NO3–(aq) → SnCl62–(aq) + 4NO2(g) + 4H2O(l)
what is the oxidizing agent?
A)
Sn
B)
NO3–
C)
H+
D)
Cl–
E)
SnCl62–
Test Bank General Chemistry, 10th edition 32
116. Besides its ability to function as an acid, hydrosulfuric acid, H2S, is able to act as a reducing
agent. Which one of the following equations illustrates this property of H2S?
A)
H2S(aq) + 2OH–(aq) → S2–(aq) + 2H2O(l)
B)
H2S(aq) + 2Na(s) → H2(g) + 2Na+(aq) + S2–(aq)
C)
H2S(aq) + 2AgI(s) → Ag2S(s) + 2H+(aq) + 2I–(aq)
D)
H2S(aq) + Cu2+(aq) → CuS(s) + 2H+(aq)
E)
3H2S(aq) + 2H+(aq) + 2NO3–(aq) → 3S(s) + 2NO(g) + 4H2O(l)
117. In the following reaction,
2H2O2(l) → 2H2O(l) + O2(g)
hydrogen peroxide functions as
A)
an acid.
B)
a reducing agent.
C)
an oxidizing agent.
D)
both an oxidizing agent and a reducing agent.
E)
neither an oxidizing agent nor a reducing agent.
118. Which of the following species would be expected to function as a reducing agent?
A)
Ba2+
B)
Zn2+
C)
ClO4–
D)
Cs+
E)
V2+
119. All of the following reactions are described as decomposition reactions except
A)
CuSO4 • 5H2O(s) CuSO4(s) + 5H2O(g).
B)
2PbO2(s) 2PbO(s) + O2(g).
C)
Fe(CO)5(l) Fe(s) + 5CO(g).
D)
H2SO3(aq) SO2(g) + H2O(l).
E)
NO2(g) + H2O(l) NO(g) + 2HNO3(aq).
120. All of the following reactions can be described as displacement reactions except
A)
Zn(s) + FeCl2(aq) → ZnCl2(aq) + Fe(s).
B)
C6H6(l) + Cl2(g) → C6H5Cl(l) + HCl(g).
C)
2Na(s) + 2H2O(l) → 2NaOH(aq) + H2(g).
D)
Cu(s) + 2AgNO3(aq) → Cu(NO3)2(aq) + 2Ag(s).
E)
CuSO4(aq) + Fe(s) → Cu(s) + FeSO4(aq).
121. All of the following reactions are called combination reactions except
A)
BaO(s) + SO2(g) → BaSO3(s).
B)
C6H10(l) + Br2(l) → C6H10Br2(l).
C)
Br2(l) + H2O(l) → HOBr(aq) + HBr(aq).
D)
CaCl2(s) + 6H2O(l) → CaCl2 • 6H2O(s).
E)
3H2(g) + N2(g) → 2NH3(g).
122. All of the following reactions are described as decomposition reactions except
A)
PCl5(l) → PCl3(g) + Cl2(g).
B)
2CH3OH(l) + 3O2(g) → 2CO2(g) + 4H2O(g).
C)
NH4HS(s) → NH3(g) + H2S(g).
D)
(NH4)2Cr2O7(s) → N2(g) + 4H2O(g) + Cr2O3(s).
E)
2CO2(g) → 2CO(g) + O2(g).
123. All of the following reactions can be described as displacement reactions except
A)
CuSO4(aq) + Ni(s) → NiSO4(aq) + Cu(s).
B)
3CuCl2(aq) + 2Al(s) → 3Cu(s) + 2AlCl3(aq).
C)
Fe(s) + 2HCl(aq) → FeCl2(g) + H2(g).
D)
CH4(g) + Br2(g) → CH3Br(g) + HBr(g).
E)
Mg(s) + Hg(NO3)2(aq) → Mg(NO3)2(aq) + Hg(l).
124. All of the following reactions are described as decomposition reactions except
A)
PCl5(g) → PCl3(g) + Cl2(g).
B)
2H2O(g) → 2H2(g) + O2(g).
C)
BaCl2 • 2H2O(s) → BaCl2(s) + 2H2O(g).
D)
CH4(g) + Cl2(g) → CH3Cl(g) + HCl(g).
E)
CaCO3(s) → CaO(s) + CO2(g).
125. A 5.0-g sample of a white, powdery solid is heated in the presence of air. The solid
remaining after heating now has a mass of 3.2 g. The reaction that took place must have
been a(an)
A)
acid–base reaction.
B)
decomposition reaction.
C)
combination reaction.
D)
precipitation reaction.
E)
displacement reaction.