CHEM134 Practice Exam 11
Electrochemistry Practice Exam
Questions And Correct Answers
(Verified Answers) Plus Rationales
2026 Q&A | Instant Download Pdf
1. Which statement best describes oxidation in an electrochemical
reaction?
A. Gain of electrons
B. Decrease in oxidation number only
C. Loss of electrons
D. Gain of hydrogen atoms
Answer: C. Loss of electrons
Rationale: Oxidation is defined as the loss of electrons. A useful
mnemonic is “OIL”: Oxidation Is Loss. When a species loses
electrons, its oxidation number increases.
2. Which statement best describes reduction?
A. Gain of electrons
B. Loss of electrons
C. Loss of oxygen only
D. Increase in oxidation number
Answer: A. Gain of electrons
,Rationale: Reduction is the gain of electrons, remembered by “RIG”:
Reduction Is Gain. When a species gains electrons, its oxidation
number decreases.
3. In a galvanic cell, oxidation occurs at the:
A. Cathode
B. Salt bridge
C. Anode
D. External wire
Answer: C. Anode
Rationale: Oxidation always occurs at the anode, regardless of whether
the cell is galvanic or electrolytic. In a galvanic cell, the anode is the
negative electrode because oxidation releases electrons into the
external circuit.
4. Reduction occurs at the:
A. Anode
B. Cathode
C. Salt bridge
D. Voltmeter
Answer: B. Cathode
Rationale: Reduction always occurs at the cathode. In a galvanic cell,
electrons flow through the external circuit toward the cathode, where
the reduction half-reaction consumes those electrons.
5. Which process occurs at the anode of an electrochemical cell?
A. Oxidation
B. Reduction
,C. Neutralization
D. Precipitation only
Answer: A. Oxidation
Rationale: The anode is defined by the reaction occurring there:
oxidation. This rule applies to both galvanic cells, which generate
electrical energy, and electrolytic cells, which consume electrical
energy.
6. Which electrode is the site of reduction?
A. Anode
B. Cathode
C. Salt bridge
D. Electrolyte reservoir
Answer: B. Cathode
Rationale: Reduction takes place at the cathode. Remember that
electrode names are based on the chemical process, not on whether the
electrode is positive or negative.
7. In a galvanic cell, the reaction is:
A. Nonspontaneous and requires continuous external power
B. Spontaneous and produces electrical energy
C. Always at equilibrium
D. Unable to transfer electrons
Answer: B. Spontaneous and produces electrical energy
Rationale: A galvanic, or voltaic, cell uses a spontaneous redox
reaction to generate electrical energy. Chemical free energy is
converted into electrical energy as electrons move through the external
circuit.
, 8. An electrolytic cell is primarily used to:
A. Convert electrical energy into chemical energy
B. Convert chemical energy into heat only
C. Produce electricity from a spontaneous reaction
D. Eliminate the need for electrodes
Answer: A. Convert electrical energy into chemical energy
Rationale: Electrolytic cells use an external electrical source to force a
nonspontaneous chemical reaction. Electrical energy is therefore
converted into stored chemical energy.
9. What is the primary function of a salt bridge in a galvanic cell?
A. Supply electrons to the cathode
B. Prevent oxidation
C. Maintain electrical neutrality by allowing ion migration
D. Increase the temperature of the solution
Answer: C. Maintain electrical neutrality by allowing ion migration
Rationale: As oxidation and reduction occur, charge imbalances would
develop in the two half-cells. Ions from the salt bridge migrate into the
appropriate compartments, maintaining electrical neutrality and
allowing current to continue.
10. Electrons in a functioning galvanic cell flow through the
external circuit from:
A. Cathode to anode
B. Salt bridge to cathode
C. Cathode to salt bridge
D. Anode to cathode
Answer: D. Anode to cathode
Electrochemistry Practice Exam
Questions And Correct Answers
(Verified Answers) Plus Rationales
2026 Q&A | Instant Download Pdf
1. Which statement best describes oxidation in an electrochemical
reaction?
A. Gain of electrons
B. Decrease in oxidation number only
C. Loss of electrons
D. Gain of hydrogen atoms
Answer: C. Loss of electrons
Rationale: Oxidation is defined as the loss of electrons. A useful
mnemonic is “OIL”: Oxidation Is Loss. When a species loses
electrons, its oxidation number increases.
2. Which statement best describes reduction?
A. Gain of electrons
B. Loss of electrons
C. Loss of oxygen only
D. Increase in oxidation number
Answer: A. Gain of electrons
,Rationale: Reduction is the gain of electrons, remembered by “RIG”:
Reduction Is Gain. When a species gains electrons, its oxidation
number decreases.
3. In a galvanic cell, oxidation occurs at the:
A. Cathode
B. Salt bridge
C. Anode
D. External wire
Answer: C. Anode
Rationale: Oxidation always occurs at the anode, regardless of whether
the cell is galvanic or electrolytic. In a galvanic cell, the anode is the
negative electrode because oxidation releases electrons into the
external circuit.
4. Reduction occurs at the:
A. Anode
B. Cathode
C. Salt bridge
D. Voltmeter
Answer: B. Cathode
Rationale: Reduction always occurs at the cathode. In a galvanic cell,
electrons flow through the external circuit toward the cathode, where
the reduction half-reaction consumes those electrons.
5. Which process occurs at the anode of an electrochemical cell?
A. Oxidation
B. Reduction
,C. Neutralization
D. Precipitation only
Answer: A. Oxidation
Rationale: The anode is defined by the reaction occurring there:
oxidation. This rule applies to both galvanic cells, which generate
electrical energy, and electrolytic cells, which consume electrical
energy.
6. Which electrode is the site of reduction?
A. Anode
B. Cathode
C. Salt bridge
D. Electrolyte reservoir
Answer: B. Cathode
Rationale: Reduction takes place at the cathode. Remember that
electrode names are based on the chemical process, not on whether the
electrode is positive or negative.
7. In a galvanic cell, the reaction is:
A. Nonspontaneous and requires continuous external power
B. Spontaneous and produces electrical energy
C. Always at equilibrium
D. Unable to transfer electrons
Answer: B. Spontaneous and produces electrical energy
Rationale: A galvanic, or voltaic, cell uses a spontaneous redox
reaction to generate electrical energy. Chemical free energy is
converted into electrical energy as electrons move through the external
circuit.
, 8. An electrolytic cell is primarily used to:
A. Convert electrical energy into chemical energy
B. Convert chemical energy into heat only
C. Produce electricity from a spontaneous reaction
D. Eliminate the need for electrodes
Answer: A. Convert electrical energy into chemical energy
Rationale: Electrolytic cells use an external electrical source to force a
nonspontaneous chemical reaction. Electrical energy is therefore
converted into stored chemical energy.
9. What is the primary function of a salt bridge in a galvanic cell?
A. Supply electrons to the cathode
B. Prevent oxidation
C. Maintain electrical neutrality by allowing ion migration
D. Increase the temperature of the solution
Answer: C. Maintain electrical neutrality by allowing ion migration
Rationale: As oxidation and reduction occur, charge imbalances would
develop in the two half-cells. Ions from the salt bridge migrate into the
appropriate compartments, maintaining electrical neutrality and
allowing current to continue.
10. Electrons in a functioning galvanic cell flow through the
external circuit from:
A. Cathode to anode
B. Salt bridge to cathode
C. Cathode to salt bridge
D. Anode to cathode
Answer: D. Anode to cathode
