SCH 4U1
Chapter 9 Test
Part 1: Multiple Choice (25 marks)
Identify the choice that best completes the statement or answers the question. Record your answers onto the Google Form.
1. In the half-reaction Ag +(aq) + e–
a.
b.
c.
d.
Ag(s), Ag +(aq) is
oxidized
reduced
the reducing agent
none of the above
2. In a reaction, a reducing agent
a.
b.
c.
d.
is reduced
gains electrons
is oxidized
causes oxidation
3. In which of the following does nitrogen have an oxidation number of –3?
a.
b.
c.
d.
N2O
NH4Cl
NaNO3
N2
4. In the unbalanced reaction equation Ag 2S(s) + Al(s)
a.
b.
c.
d.
Al2S3(s) + Ag(s),
aluminum loses electrons
silver loses electrons
silver metal is the oxidizing agent
aluminum is reduced
5. What does a half-reaction equation represent?
a.
b.
c.
d.
a reduction reaction
the oxidation part or the reduction part of a redox reaction
the balanced chemical equation
an oxidation reaction
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6. When the equation for the redox reaction H2S(g) + O2(g)
correct coefficients, in order?
a.
b.
c.
d.
2, 1, 1, 2
2, 1, 2, 2
2, 2, 1, 2
2, 2, 1, 1
7. In the unbalanced reaction equation H2S(g) + O2(g)
a.
b.
c.
d.
S(s) + H2O(l),
sulfur is oxidized
oxygen is the oxidizing agent
hydrogen is reduced
sulfur is the oxidizing agent
8. For the unbalanced equation CH3OH(aq) + MnO4–(aq)
a.
b.
c.
d.
H2(g) + Ca(NO3)2(aq), what is the correct equation for
Ca2+(aq) + 2 e–
Ca(s)
+
H2(g)
H (aq) + e–
Ca(s)
Ca2+(aq) + 2 e–
+
H (aq) + e–
H2(g)
10. For the equation, Zn(s) + HNO3(aq)
a.
b.
c.
d.
Zn(NO3)2(aq) + NH4NO3(aq),
ammonium is reduced
zinc is oxidized
nitrogen is the reducing agent
zinc is reduced
11. For the unbalanced reaction equation MnO4–(aq) + Cl–(aq)
a.
b.
c.
d.
CO32–(aq) + MnO42–(aq),
carbon is reduced
the oxidation number of carbon changes from +4 to 0
oxygen is reduced
manganese gains 1 electron
9. For the unbalanced equation Ca(s) + HNO3(aq)
the reduction half-reaction?
a.
b.
c.
d.
S(s) + H2O(l) is balanced, what are the
Mn2+(aq) + Cl2(g),
8 water molecules must be added to balance the equation
chlorine is the oxidizing agent
10 hydrogen ions must be added to balance the equation
when charge is balanced, the total number of electrons transferred is 8
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12. For the unbalanced equation Zn(s) + HNO3(aq)
Zn(NO3)2(aq) + NH4NO3(aq), what are the oxidation
numbers of nitrogen on the reactant and product sides of the equation, in order?
a.
b.
c.
d.
+5, +5, –3, +5
+5, +2, –3, +5
0, +5, +2, –3
0, +2
Cr2O72–(aq) + I–(aq)
Cr3+(aq) + IO3–(aq)
13. From the unbalanced equation above, what is the correct balanced half-reaction equation for the
oxidation half-reaction in an acidic medium?
a.
b.
c.
d.
I–(aq) + 3 H2O(l)
IO3–(aq) + 6 e– + 6 H+(aq)
I–(aq)
IO3–(aq) + 6 e–
Cr2O72–(aq) + 6 e– + 14 H+(aq)
2 Cr3+(aq) + 7 H2O(aq)
2–
–
3+
Cr2O7 (aq) + 3 e
Cr (aq)
14. In the reaction equation given above, what is the oxidation number of iodine in the iodate ion?
a.
b.
c.
d.
+6
–1
+3
+5
15. From the unbalanced equation above, what is the correct balanced half-reaction equation for the
reduction half-reaction in an acidic medium?
a.
b.
c.
d.
Cr2O72–(aq) + 3 e–
Cr3+(aq)
I–(aq)
IO3–(aq) + 6 e–
–
I (aq) + 3 H2O(l)
IO3–(aq) + 6 e– + 6 H+(aq)
Cr2O72–(aq) + 6 e– + 14 H+(aq)
2 Cr3+(aq) + 7 H2O(aq)
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Au3+(aq) + 3 e– ↔ Au(s),
Sn2+(aq) + 2 e– ↔ Sn(s),
= +1.50 V
= –0.14 V
Co2+(aq) + 2 e– ↔ Co(s),
= –0.28 V
Ca2+(aq) + 2 e– ↔ Ca(s),
= –2.76 V
16. In the list of half-reactions and reduction potentials above, which metal or ion is the strongest reducing
agent?
a.
b.
c.
d.
gold ion
gold metal
calcium ion
calcium metal
17. In the list of half-reactions and reduction potentials above, which metal or ion is the weakest reducing
agent?
a.
b.
c.
d.
calcium ion
calcium metal
gold ion
gold metal
18. From the table above, a spontaneous reaction will occur if gold ion reacts with what?
a.
b.
c.
d.
calcium metal
cobalt metal
tin metal
all of the above
19. From the table above, a spontaneous reaction will occur if tin ion reacts with what?
a.
b.
c.
d.
cobalt metal
cobalt ion or calcium ion
cobalt metal or calcium metal
cobalt metal, calcium metal, or gold metal
20. What is the best indication of whether a spontaneous redox reaction will occur or not?
a.
b.
c.
d.
nature of reactants
the relative positions of the reducing agent and the oxidizing agent in the redox table
presence of a catalyst
temperature of solution
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Hg2+(aq) + 2 e– ↔ Hg(l),
= +0.80 V
Ag+(aq) + e– ↔ Ag(s),
= +0.80 V
Cu+(aq) + e– ↔ Cu(s),
= +0.52 V
Cd2+(aq) + 2 e– ↔ Cd(s),
= –0.40 V
21. Use the list of half-reactions and reduction potentials above to select the entity that would react
spontaneously with silver metal.
a.
b.
c.
d.
silver ion
mercury ion
copper ion
cadmium ion
22. What is the strongest oxidizing agent in the list of half-reactions and reduction potentials above?
a.
b.
c.
d.
silver metal
cadmium metal
mercury ion
copper ion
23. What is the strongest reducing agent in the list of half-reactions and reduction potentials above?
a.
b.
c.
d.
copper metal
silver ion
cadmium metal
mercury ion
24. Use the list of half-reactions and reduction potentials above to select the entity that would react
spontaneously with mercury metal.
a.
b.
c.
d.
copper ion
silver metal
cadmium ion
none of the above
25. Use the list of half-reactions and reduction potentials above to select the entity that would react
spontaneously with copper metal.
a. cadmium ion
b. silver ion
c. mercury ion and silver ion
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d. mercury ion
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26. The following equation represents a reaction that took place in an acidic medium. The correct balanced
equation is
(5 marks)
MnO4–(aq) + SO32–(aq)
a.
b.
c.
d.
Mn2+(aq) + SO42–(aq)
3 MnO4–(aq) + 5 SO32–(aq) + 6 H+(aq)
3 Mn2+(aq) + 5 SO42–(aq) + 3 H2O(l)
MnO4–(aq) + 5 SO32–(aq) + 6 H+(aq)
Mn2+(aq) + 5 SO42–(aq) + 3 H2O(l)
–
2–
+
2 MnO4 (aq) + 5 SO3 (aq) + 6 H (aq)
2 Mn2+(aq) + 5 SO42–(aq) + 3 H2O(l)
2 MnO4–(aq) + 4 SO32–(aq) + 6 H+(aq)
2 Mn2+(aq) + 4 SO42–(aq) + 3 H2O(l)
27. The correctly balanced half-reaction in basic solution is
N2O(g)
a.
b.
c.
d.
N2(g)
H2O(l) + 3 N2O(g) + 6 e–
3 N2(g) + 2 OH–(aq)
2 H2O(l) + N2O(g) + 4 e–
N2(g) + 4 OH–(aq)
2 H2O(l) + 3 N2O(g) + 6 e–
3 N2(g) + 4 OH–(aq).
H2O(l) + N2O(g) + 2 e–
N2(g) + 2 OH–(aq)
28. The correctly balanced half-reaction in an acidic solution is
NO3–(aq)
a.
b.
c.
d.
(3 marks)
(3 marks)
NO2–(aq)
2 H+(aq) + NO3–(aq) + 2 e–
NO2–(aq) + H2O(l)
4 H+(aq) + NO3–(aq) + 4 e–
NO2–(aq) + 2 H2O(l)
+
–
–
H (aq) + NO3 (aq) + e
NO2–(aq) + H2O(l)
2 H+(aq) + NO3–(aq) + e–
NO2–(aq) + 2 H2O(l)
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29. Which of the following statements is true based on the reactions below?
Cl2(g) + 2 e–
2 Cl–(aq);
= +1.36 V
Br2(l) + 2 e–
2 Br–(aq);
= +1.09 V
2 H+(aq) + 2 e–
H2(g);
2 H2O(l) + 2 e–
H2(g) + 2 OH–(aq);
a.
b.
c.
d.
(4 marks)
= 0.00 V
= –0.83 V
The strongest oxidizing agent is hydrogen gas and the strongest reducing agent is bromide ion. Since
hydrogen gas and bromide ion form a downward diagonal to the right in the given reduction potential
equations, this reaction is spontaneous.
The strongest oxidizing agent is chlorine gas and the strongest reducing agent is bromide ion. Since chlorine
gas and bromide ion form a downward diagonal to the right in the given reduction potential equations, this
reaction is spontaneous.
The strongest oxidizing agent is bromine gas and the strongest reducing agent is chloride ion. Since bromine
gas and chloride ion form a downward diagonal to the right in the given reduction potential equations, this
reaction is spontaneous.
none of the above
30. Which of the following statements pertaining to the reactions below is false?
Ag+(aq) + e–
Ag(s);
= +0.80 V
2 H2O(l) + 2 e–
H2(g) + 2 OH–(aq);
Al3+(aq) + 3 e–
Al(s);
a.
b.
c.
d.
= –0.83 V
= –1.66 V
The entities present in the reaction are Al(s), Ag+(aq), and H2O(l).
From the given information, silver ion is the strongest oxidizing agent
From the given information, aluminum metal is the strongest reducing agent
none of the above
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