For the electrolysis of aqueous KCl solution using inert electrodes, chlorine gas is evolved at one electrode and hydrogen gas is evolved at the other electrode. The solution around the electrode at which hydrogen gas is evolved becomes basic as the

1
For the electrolysis of aqueous KCl solution
using inert electrodes, chlorine gas is evolved
at one electrode and hydrogen gas is evolved at
the other electrode. The solution around the
electrode at which hydrogen gas is evolved
becomes basic as the electrolysis proceeds. Which
of the following describe, or are applicable to,
the cathode and the reaction that occurs at the
cathode? I. the positive electrode II. 2H2O
image O2 4H 4e- III. the negative electrode
IV. 2H2O 2e- image H2 2OH- V. 2Cl- image
Cl- 2e- VI. electrons enter external circuit
(wire) VII. Cl2 2e- image 2Cl- VIII.
electrons leave external circuit (wire) IX.
oxidation X. reduction

1. III, IV, VIII, and IX
2. I, II, VI, and IX
3. II, III, VI, and X
4. I, IV, VIII, and X
5. None of the first four responses is correct.

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2
For the electrolysis of aqueous KCl solution
using inert electrodes, chlorine gas is evolved
at one electrode and hydrogen gas is evolved at
the other electrode. The solution around the
electrode at which hydrogen gas is evolved
becomes basic as the electrolysis proceeds. Which
of the following describe, or are applicable to,
the electrode at which chlorine is produced and
its reaction? I. the positive electrode II. 2H2O
image O2 4H 4e- III. the negative
electrode IV. 2H2O 2e- image H2 2OH- V. 2Cl-
image Cl2 2e- VI. electrons enter external
circuit (wire) VII. Cl2 2e- image 2Cl- VIII.
electrons leave external circuit (wire)IX.
oxidation X. reduction

1. III, V, VIII, and X
2. III, V, VI, and X
3. I, VII, VIII, and X
4. I, V, VI, and IX
5. None of the first four responses is correct.

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3
How many faradays (F) are passed through a cell
if 4.50 amperes of current are passed through the
cell for 2.50 hours?

1. 6.82 F
2. 0.0207 F
3. 302 F
4. 0.420 F
5. 6.99 x 10-3 F

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4
What mass of chromium could be deposited by
electrolysis of an aqueous solution of
Cr2(SO4)3for 60.0 minutes using a steady current
of 10.0 amperes?

1. 3.25 g
2. 6.47 g
3. 17.3 g
4. 0.187 g
5. 0.373 g

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5
How many mL of chlorine gas can be obtained at
STP by the electrolysis of molten NaCl using a
0.350 ampere current for 20.0 minutes?

1. 195 mL
2. 48.7 mL
3. 133 mL
4. 97.5 mL
5. 582 mL

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6
A cell is constructed by immersing a strip of
iron in a solution that is 1.0 M in Fe2 ions and
connecting this electrode to a standard hydrogen
electrode using a wire and a salt bridge. The
following observations can be made. The strip of
iron loses mass, and the concentration of Fe2
ions increases. In the standard hydrogen
electrode, the concentration of hydrogen ions
decreases. Which of the following is the
strongest reducing agent?

1. Fe2
2. H
3. Fe
4. H2
5. Fe3

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7
A table
of standard electrode potentials is necessary for
many of the questions below.
Which of the following is the
strongest oxidizing agent?

1. Al3
2. Al
3. F2
4. F-
5. H2

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8
Which of the following species is the strongest
oxidizing agent?

1. Zn2
2. Zn
3. Hg2
4. Hg
5. Na

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9
Which of the following species is the strongest
reducing agent?

1. Zn2
2. Zn
3. Hg2
4. Hg
5. Ag

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10
Which of the following is the strongest reducing
agent?

1. Na
2. Au
3. Cu2
4. F2
5. Cd

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11
What is the cell potential for a cell constructed
by immersing a strip of copper in a 1.0 M CuSO4
solution and a strip of tin in a 1.0 M SnSO4
solution and completing the circuit by a wire and
a salt bridge?

1. -0.19 V
2. 0.19 V
3. -0.48 V
4. 0.48 V
5. 0.54 V

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12
Calculate the cell potential of the following
voltaic cell. ZnZn2(1.0 x 10-8 M)Cu2(1.0 x
10-6 M)Cu

1. 1.06 V
2. 1.10 V
3. 1.03 V
4. 1.14 V
5. 1.16 V

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13
A voltaic cell is constructed by immersing a
strip of copper metal in 1.0 M CuSO4solution and
a strip of aluminum in 0.50 M Al2(SO4)3 solution.
A wire and a salt bridge complete the circuit.
The aluminum strip loses mass, and the
concentration of aluminum ions in the solution
increases. The copper electrode gains mass, and
the concentration of copper ions decreases.
Calculate the equilibrium constant at 25C for
the cell reaction. (F 96,500 J/Vmol e- and R
8.314 J/molK) (Round off errors are large!!!)

1. 4 x 1041
2. 2 x 1083
3. 6 x 1095
4. 3 x 10101
5. 9 x 10202

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