Questions about Electrochemical Reactions
Electrochemical Reactions – Multiple-Choice Questions
Questions
1. What is an electrochemical reaction?
A) A reaction involving only acids and bases
B) A reaction involving electron transfer
C) A reaction with no energy change
D) A combustion reaction
E) A reaction that always produces heat
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2. Which of the following devices uses electrochemical reactions to generate electricity?
A) Generator
B) Transformer
C) Battery
D) Light bulb
E) Capacitor
3. What is the function of a salt bridge in an electrochemical cell?
A) To supply electrons
B) To absorb energy
C) To maintain electrical neutrality
D) To produce light
E) To store ions
4. In an electrochemical cell, oxidation occurs at the:
A) Anode
B) Cathode
C) Salt bridge
D) Electrolyte
E) Wire
5. In an electrochemical cell, reduction occurs at the:
A) Anode
B) Wire
C) Electrolyte
D) Cathode
E) Salt bridge
6. What flows through the external wire in a galvanic cell?
A) Ions
B) Protons
C) Neutrons
D) Electrons
E) Atoms
7. In a galvanic cell, the anode is:
A) Positive
B) Neutral
C) Negative
D) Always larger
E) Made of copper
8. What is the oxidizing agent in an electrochemical reaction?
A) The species that loses electrons
B) The species that gains electrons
C) The anode
D) The salt bridge
E) The electrode
9. A Daniell cell uses which pair of electrodes?
A) Na and Cl
B) Cu and Zn
C) Fe and Ag
D) H and O
E) Al and Fe
10. Which of the following correctly shows a spontaneous redox reaction?
A) Cu²⁺ + Zn → Zn²⁺ + Cu
B) Zn²⁺ + Cu → Cu²⁺ + Zn
C) Cu + Cu²⁺ → Cu
D) Zn + Zn²⁺ → Zn
E) H₂O + O₂ → H₂O₂
11. Which of the following is true for a galvanic cell?
A) It consumes electricity to drive the reaction
B) It requires a strong acid to operate
C) It converts chemical energy to electrical energy
D) It has no redox reactions
E) It stops once ions are formed
12. What is the standard electrode potential (E°) a measure of?
A) Reaction time
B) Ion concentration
C) Tendency to gain or lose electrons
D) Number of protons
E) Temperature
13. The voltage of an electrochemical cell is determined by:
A) Type of salt bridge used
B) Electrode size
C) Temperature
D) The difference in electrode potentials
E) Concentration of oxygen
14. What happens at the cathode during electrolysis?
A) Oxidation
B) Electron loss
C) Ion transfer
D) Reduction
E) No reaction
15. In electrolysis, the anode is usually:
A) Negative
B) Positive
C) Neutral
D) Uncharged
E) Replaced by salt
16. Which of these metals is most likely to be oxidized in an electrochemical cell?
A) Cu
B) Au
C) Zn
D) Ag
E) Pt
17. A cell with a positive standard potential (E° > 0) is:
A) Non-spontaneous
B) Spontaneous
C) Neutral
D) Unstable
E) Always endothermic
18. In an electrochemical cell, ions move through:
A) The wire
B) The voltmeter
C) The electrodes
D) The salt bridge
E) The light bulb
19. Which of the following reactions could occur at the cathode?
A) Zn → Zn²⁺ + 2e⁻
B) Fe → Fe²⁺ + 2e⁻
C) Cu²⁺ + 2e⁻ → Cu
D) Na → Na⁺ + e⁻
E) Al → Al³⁺ + 3e⁻
20. What is the role of the electrolyte in an electrochemical cell?
A) Generate electricity
B) Carry electrons
C) Maintain ion flow
D) Block reactions
E) Insulate the system
Answer Key with Explanations
1. B – Electrochemical reactions involve the transfer of electrons, typically in redox processes.
2. C – A battery uses electrochemical reactions to produce electricity.
3. C – The salt bridge maintains electrical neutrality by allowing ion flow.
4. A – Oxidation occurs at the anode (loss of electrons).
5. D – Reduction (gain of electrons) occurs at the cathode.
6. D – Electrons flow through the external wire.
7. C – In a galvanic cell, the anode is negative.
8. B – The oxidizing agent gains electrons (gets reduced).
9. B – The Daniell cell uses zinc (Zn) and copper (Cu) electrodes.
10. A – Zinc displaces copper in solution: spontaneous reaction.
11. C – A galvanic cell converts chemical to electrical energy.
12. C – E° values show the tendency to gain/lose electrons.
13. D – The difference in electrode potentials gives cell voltage.
14. D – Reduction occurs at the cathode in electrolysis.
15. B – In electrolysis, the anode is positive.
16. C – Zinc (Zn) is more easily oxidized than the other listed metals.
17. B – Positive E° means the reaction is spontaneous.
18. D – Ions move through the salt bridge to balance charges.
19. C – Cu²⁺ gains 2e⁻ → Cu: a reduction at the cathode.
20. C – Electrolytes maintain ion flow in the system.
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