CHEM134 C003 Lesson 7 Quiz | Questions
and Answers – spring 2026 | 100%
Correct - American Public University.
SECTION 1: VOLTAIC/GALVANIC CELLS
1. Which of the following statements correctly describes the function of the salt
bridge in a voltaic cell?
A) It acts as a resistor to slow down the reaction.
B) It provides a pathway for the migration of ions to maintain electrical neutrality in the
half-cells.
C) It is the site where oxidation occurs.
, D) It provides a direct flow of electrons between the two half-cells.
Correct Answer: B
Rationale: As the cell operates, the anode half-cell accumulates positive ions (cations)
from oxidation, and the cathode half-cell becomes depleted of them. The salt bridge
contains inert ions that migrate into the half-cells to neutralize these changes, preventing
the buildup of charge that would stop the reaction .
2. Given the standard reduction potentials below, which species is the strongest
reducing agent?
Half-Reaction E° (V)
Ag⁺ + e⁻ → Ag(s) +0.80
Zn²⁺ + 2e⁻ → Zn(s) -0.76
A) Ag⁺(aq)
B) Ag(s)
C) Zn²⁺(aq)
D) Zn(s)
Correct Answer: D
, Rationale: A reducing agent is a species that loses electrons (is oxidized). The more
negative the reduction potential of a half-reaction, the greater the tendency of the
reactant to be oxidized. Therefore, the species that is oxidized (Zn(s)) is a stronger reducing
agent than Ag(s) .
3. For the spontaneous cell reaction: 2 Ag⁺(aq) + Cu(s) → 2 Ag(s) + Cu²⁺(aq), what
is the correct cell notation?
A) Cu(s) | Cu²⁺(aq) || Ag⁺(aq) | Ag(s)
B) Ag(s) | Ag⁺(aq) || Cu²⁺(aq) | Cu(s)
C) Cu²⁺(aq) | Cu(s) || Ag(s) | Ag⁺(aq)
D) Cu(s) | Cu²⁺(aq) || Ag(s) | Ag⁺(aq)
Correct Answer: A
Rationale: By convention, cell notation is written as Anode || Cathode. The anode is where
oxidation occurs (Cu(s) → Cu²⁺(aq) + 2e⁻) and is written on the left. The cathode is where
reduction occurs (Ag⁺(aq) + e⁻ → Ag(s)) and is written on the right. A single vertical line (|)
represents a phase boundary .
4. Calculate the standard cell potential (E°cell) for the reaction in Question 3.
Given: Ag⁺ + e⁻ → Ag(s) E° = +0.80 V; Cu²⁺ + 2e⁻ → Cu(s) E° = +0.34 V
A) 0.46 V
B) 1.14 V
, C) -0.46 V
D) -1.14 V
Correct Answer: A
Rationale: The cathode is where reduction occurs (Ag⁺/Ag, E° = +0.80 V). The anode is
where oxidation occurs (Cu/Cu²⁺, reverse the reduction potential: -0.34 V). E°cell =
E°cathode - E°anode = 0.80 V - 0.34 V = 0.46 V .
5. In a voltaic cell, the half-cell where reduction occurs is called the:
A) Anode
B) Cathode
C) Salt bridge
D) External circuit
Correct Answer: B
Rationale: Reduction always takes place at the cathode. Oxidation occurs at the anode .
6. Which statement about a standard hydrogen electrode (SHE) is true?
A) It has an assigned potential of exactly 0 V at all temperatures.
and Answers – spring 2026 | 100%
Correct - American Public University.
SECTION 1: VOLTAIC/GALVANIC CELLS
1. Which of the following statements correctly describes the function of the salt
bridge in a voltaic cell?
A) It acts as a resistor to slow down the reaction.
B) It provides a pathway for the migration of ions to maintain electrical neutrality in the
half-cells.
C) It is the site where oxidation occurs.
, D) It provides a direct flow of electrons between the two half-cells.
Correct Answer: B
Rationale: As the cell operates, the anode half-cell accumulates positive ions (cations)
from oxidation, and the cathode half-cell becomes depleted of them. The salt bridge
contains inert ions that migrate into the half-cells to neutralize these changes, preventing
the buildup of charge that would stop the reaction .
2. Given the standard reduction potentials below, which species is the strongest
reducing agent?
Half-Reaction E° (V)
Ag⁺ + e⁻ → Ag(s) +0.80
Zn²⁺ + 2e⁻ → Zn(s) -0.76
A) Ag⁺(aq)
B) Ag(s)
C) Zn²⁺(aq)
D) Zn(s)
Correct Answer: D
, Rationale: A reducing agent is a species that loses electrons (is oxidized). The more
negative the reduction potential of a half-reaction, the greater the tendency of the
reactant to be oxidized. Therefore, the species that is oxidized (Zn(s)) is a stronger reducing
agent than Ag(s) .
3. For the spontaneous cell reaction: 2 Ag⁺(aq) + Cu(s) → 2 Ag(s) + Cu²⁺(aq), what
is the correct cell notation?
A) Cu(s) | Cu²⁺(aq) || Ag⁺(aq) | Ag(s)
B) Ag(s) | Ag⁺(aq) || Cu²⁺(aq) | Cu(s)
C) Cu²⁺(aq) | Cu(s) || Ag(s) | Ag⁺(aq)
D) Cu(s) | Cu²⁺(aq) || Ag(s) | Ag⁺(aq)
Correct Answer: A
Rationale: By convention, cell notation is written as Anode || Cathode. The anode is where
oxidation occurs (Cu(s) → Cu²⁺(aq) + 2e⁻) and is written on the left. The cathode is where
reduction occurs (Ag⁺(aq) + e⁻ → Ag(s)) and is written on the right. A single vertical line (|)
represents a phase boundary .
4. Calculate the standard cell potential (E°cell) for the reaction in Question 3.
Given: Ag⁺ + e⁻ → Ag(s) E° = +0.80 V; Cu²⁺ + 2e⁻ → Cu(s) E° = +0.34 V
A) 0.46 V
B) 1.14 V
, C) -0.46 V
D) -1.14 V
Correct Answer: A
Rationale: The cathode is where reduction occurs (Ag⁺/Ag, E° = +0.80 V). The anode is
where oxidation occurs (Cu/Cu²⁺, reverse the reduction potential: -0.34 V). E°cell =
E°cathode - E°anode = 0.80 V - 0.34 V = 0.46 V .
5. In a voltaic cell, the half-cell where reduction occurs is called the:
A) Anode
B) Cathode
C) Salt bridge
D) External circuit
Correct Answer: B
Rationale: Reduction always takes place at the cathode. Oxidation occurs at the anode .
6. Which statement about a standard hydrogen electrode (SHE) is true?
A) It has an assigned potential of exactly 0 V at all temperatures.
