Electrochemistry Review Quiz
1. Two cells, one containing aqueous
AgNO3 and other containing CuSO4 are set up
in series. In a given electrolysis that results
in depositing 1.25g of silver in the first cell,
how much copper should deposit
simultaneously in the second cell.
A. 1.47g
B. 0.368g
C. 0.736g
D. 2.65g
E. 1.25g
6. If a constant current of 8.00 amperes is
passed through a cell containing Zn2+ for
2.00 hours, how many grams of zinc will plate
out onto the cathode?
A. 126 g
B. 1.43 x 103 g
C. 0.985 g
D. 19.5 g
E. 39.0 g
2. The equilibrium constant (K) for the
reaction below is approximately:
Cl2 + 2e- → 2Cl- (E0 = 1.36v)
Cu+ + e- → Cu (E0 = 0.52v)
A. 10-34
B. 1017
C. 1011
D. 1028
E. 102
2NaCl + 2H2SO4 + MnO2 → Na2SO4 +
MnSO4 + 2H2O + Cl2
A. ClB. Mn4+
C. Na+
D. H+
E. O2-
3.
A.
B.
C.
D.
Reduction potential is:
measured in amperes
an extensive property
always positive
an intensive property
4. The standard hydrogen electrode is
assigned a potential of:
A. v
B. 0.76v
C. -1.00v
D. zero volts
5. How many electrons are transferred in
the following reaction?
2NaCl + 2H2SO4 + MnO2 → Na2SO4 +
MnSO4 + 2H2O + Cl2
A. 4
B. 1
C. 2
D. 8
E. 6
7.
is:
8.
A.
B.
C.
D.
E.
In the reaction below, the oxidizing agent
What value of E do you expect for
Pb(s) → Pb2+ + 2ein 0.015m Pb2+ solution? E0 = +0.13v
E = +0.27v
E = 0.00v
E = +0.83v
E = +0.18v
E = +0.13v
9. In the electrolytic decomposition of water:
2H2O → 2H2 + O2
A. hydrogen is formed at the cathode
and oxygen is formed at the anode
B. hydrogen is formed at the anode and
oxygen is formed at the cathode
C. oxygen is formed at both the anode
and the cathode
D. hydrogen is formed at both the
anode and the cathode
10. Which of the following would be the best
reducing agent?
A. Na
B. Cl2
Electrochemistry Review Quiz
C.
D.
E.
O2Na+
F-
11. This picture of an electrochemical cell can
best be described as:
A.
B.
C.
D.
E.
1.78 x 105 sec
5.35 x 105 sec
2.19 x 104 sec
3.90 x 103 sec
1.68 x 102 sec
15. The equation that represents a reaction
that is not a redox reaction is:
1. 2H2 + O2 → 2H2O
2. Zn + CuSO4 → ZnSO4 + Cu
3. 2H2O2 → 2H2O + O2
4. H2O + CO2 → H2CO3
A.
B.
C.
D.
a complete galvanic cell
a complete electrolytic cell
a galvanic cell, but missing at least
one essential component
an electrolytic cell, but missing at
least one essential component
12. Calculate the value of E0cell for a galvanic
cell that contains the following half
cells:
Cl2 + 2e- → 2Cl- (E0 = 1.36v)
Cu+ + e- → Cu (E0 = 0.52v)
A.
B.
C.
D.
E.
E0cell = 0.32 volts
E0cell = 1.88 volts
E0cell = -0.32 volts
E0cell = 0.84 volts
E0cell = -0.84 volts
13. What is the oxidation state of S in H2SO3?
A. -3
B. +4
C. +6
D. 0
E. +2
14. With a current of 20 amps, how long
would it take to generate 1.00 kilograms of
aluminum by the reaction:
Al3+ + 3e- → Al(s)
A.
B.
C.
D.
E.
All of these are redox reactions
Reaction 4
Reaction 2
Reaction 1
Reaction 3
16. Calculate DG0 for the reaction:
Cl2 + 2e- → 2Cl- (E0 = 1.36v)
Cu+ + e- → Cu (E0 = 0.52v)
A.
B.
C.
D.
E.
-8.1 x 104 J
-6.2 x 104 J
-1.6 x 105 J
-3.1 x 104 J
8.1 x 105 J
17. A mole of electrons has a charge of
96,485 coulombs per mole of electrons. This
quantity is known to chemists as:
A.
B.
C.
D.
E.
1 joule
1 ampere
1 watt
1 volt
1 faraday
18. In all electrochemical cells, the process
that takes place at the anode is
_________________ and the process that
Electrochemistry Review Quiz
takes place at the cathode is
_________________.
A.
B.
C.
D.
reduction, reduction
oxidation, reduction
oxidation, oxidation
reduction, oxidation
19. For the galvanic cell described below, the
correct line notation is:
Cl2 + 2e- → 2Cl- (E0 = 1.36v)
Cu+ + e- → Cu (E0 = 0.52v)
A. Cu(s)|Cu+(aq)||Cl2(g)|2Cl-(aq)|Pt(s)
B. Cu(s)|Cu+(aq)||Cl2(g)|2Cl-(aq)
C. Pt(s)|Cu(s)|Cu+(aq)||Cl2(g)|2Cl-(aq)|Pt
(s)
D. Pt(s)|Cl2(g)|2Cl-(aq)||Cu(s)|Cu+(aq)
E. Pt(s)|Cl2(g)|2Cl-(aq)||Cu(s)|Cu+(aq)|Pt
(s)
20. The current in a given wire is 1.80 amp.
How many coulombs will pass a given point
on the
wire in 1.36 minutes?
A.
B.
C.
D.
E.
253 C
147 C
45.3 C
1.32 C
2.45 C