Questions on Voltaic Cells
Voltaic Cells – Multiple Choice Questions
Questions
1. What is a voltaic cell?
A) A cell that stores energy in a magnetic field
B) A cell that uses light to produce electricity
C) A device that converts chemical energy into electrical energy through a spontaneous redox reaction
D) A cell that consumes electrical energy to cause a chemical change
E) A type of capacitor
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2. What type of reaction occurs in a voltaic cell?
A) Neutralization
B) Non-spontaneous redox
C) Spontaneous redox
D) Precipitation
E) Combustion
3. In a voltaic cell, where does oxidation occur?
A) At the cathode
B) In the salt bridge
C) At the anode
D) In the electrolyte
E) In both electrodes equally
4. In a voltaic cell, where does reduction occur?
A) At the cathode
B) In the wire
C) At the anode
D) In the electrolyte
E) In the salt bridge
5. Which of the following components allows the flow of ions between half-cells?
A) Electrode
B) Wire
C) Light bulb
D) Salt bridge
E) Battery
6. What flows through the external circuit of a voltaic cell?
A) Ions
B) Protons
C) Electrons
D) Neutrons
E) Atoms
7. In a voltaic cell, the anode is:
A) Positive
B) Neutral
C) Negative
D) Depends on the reaction
E) Unreactive
8. In a voltaic cell, the cathode is:
A) Where oxidation occurs
B) Always made of copper
C) Positive
D) Negative
E) Not involved in redox
9. Which of the following metals is most likely to be used as an anode in a voltaic cell?
A) Gold (Au)
B) Silver (Ag)
C) Copper (Cu)
D) Zinc (Zn)
E) Platinum (Pt)
10. What is the standard potential (E°) of a voltaic cell?
A) The pH of the solution
B) The potential at which water boils
C) The difference between the cathode and anode potentials
D) The total number of electrons transferred
E) The average mass of the electrodes
11. What is the purpose of the salt bridge in a voltaic cell?
A) To complete the electrical circuit by allowing ion flow
B) To prevent oxidation
C) To generate electrons
D) To act as a reducing agent
E) To convert ions into gas
12. What species is the reducing agent in a voltaic cell?
A) The one that gains electrons
B) The one that loses electrons
C) The one with the most mass
D) The one that has the highest charge
E) The salt in the salt bridge
13. In the cell notation: Zn(s) | Zn²⁺(aq) || Cu²⁺(aq) | Cu(s), which is the cathode?
A) Zn(s)
B) Zn²⁺(aq)
C) Cu²⁺(aq)
D) Cu(s)
E) The salt bridge
14. In the cell mentioned above, which metal is being oxidized?
A) Copper
B) Zinc
C) Both
D) Neither
E) Hydrogen
15. In a voltaic cell, electrons flow from:
A) Cathode to anode
B) Salt bridge to cathode
C) Anode to cathode
D) Electrolyte to wire
E) None of the above
16. Which component of the voltaic cell supplies the electric current to an external device?
A) Salt bridge
B) Electrolyte
C) Electrodes
D) The redox reaction
E) A power supply
17. If the cell potential (E°cell) is positive, the reaction is:
A) Non-spontaneous
B) Spontaneous
C) Reversible
D) Incomplete
E) Acid-base neutralization
18. In a voltaic cell, what happens to the mass of the anode over time?
A) It increases
B) It remains the same
C) It decreases
D) It turns into gas
E) It becomes magnetic
19. Why does the cathode increase in mass in some voltaic cells?
A) Oxidation of the metal
B) Reduction of metal ions to solid metal
C) Evaporation of electrolyte
D) Accumulation of salt
E) Flow of electrons
20. The voltaic cell will stop working when:
A) The wire breaks
B) The temperature drops
C) One electrode dissolves completely
D) The salt bridge is disconnected
E) All of the above
Answer Key with Explanations
1. C – A voltaic cell converts chemical energy into electrical energy via a spontaneous redox reaction.
2. C – The redox reaction in a voltaic cell occurs spontaneously.
3. C – Oxidation occurs at the anode (loss of electrons).
4. A – Reduction occurs at the cathode (gain of electrons).
5. D – The salt bridge allows ion flow to maintain charge balance.
6. C – Electrons flow through the external wire from anode to cathode.
7. C – The anode is negative because it is the source of electrons.
8. C – The cathode is positive in a voltaic cell.
9. D – Zinc is commonly used as an anode due to its high reactivity.
10. C – E°cell = E°(cathode) – E°(anode).
11. A – The salt bridge completes the circuit by allowing ion flow.
12. B – The reducing agent is the species that loses electrons.
13. D – In the notation, the right side is the cathode, which is Cu(s).
14. B – Zinc is oxidized, going from Zn to Zn²⁺.
15. C – Electrons move from anode to cathode.
16. D – The redox reaction generates the current.
17. B – A positive cell potential means the reaction is spontaneous.
18. C – The anode loses mass as it dissolves into the solution.
19. B – Metal ions gain electrons and deposit on the cathode, increasing its mass.
20. E – Any of these issues can stop the voltaic cell from functioning
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