Electrochemistry Quiz. Electrochemistry studies chemical reactions that produce or use electricity, focusing on redox reactions, electrochemical cells, and the movement of electrons. Understanding these concepts is crucial for solving problems involving galvanic and electrolytic cells, cell potentials, and practical applications of redox reactions. This quiz is designed to test your knowledge of redox reactions in cells, electron flow, electrode potentials, and related calculations.
Electrochemistry Quiz
1. In a galvanic cell, which electrode is the site of oxidation?
A. Cathode
B. Anode
C. Salt bridge
D. Electrolyte
2. Which of the following is reduced in the reaction Zn + Cu²⁺ → Zn²⁺ + Cu?
A. Zn
B. Cu²⁺
C. Zn²⁺
D. Electrons
3. In a Daniell cell, what is the direction of electron flow?
A. From Cu to Zn
B. From Zn to Cu
C. From salt bridge to anode
D. From electrolyte to cathode
4. Which statement about the anode is correct in a galvanic cell?
A. It is positive and site of reduction
B. It is negative and site of oxidation
C. It is positive and site of oxidation
D. It is negative and site of reduction
5. Which of the following is an example of an electrolytic cell?
A. Daniell cell
B. Voltaic cell
C. Electrolysis of water
D. Galvanic cell
Electrochemistry Quiz
6. The standard electrode potential of a metal is used to determine:
A. The rate of reaction
B. The spontaneity of a redox reaction
C. The color of solution
D. The mass of the metal
7. In the reaction 2Ag⁺ + Cu → 2Ag + Cu²⁺, which species is the reducing agent?
A. Ag⁺
B. Cu
C. Cu²⁺
D. Ag
8. What is the role of a salt bridge in a galvanic cell?
A. To oxidize the anode
B. To reduce the cathode
C. To maintain electrical neutrality by allowing ion flow
D. To conduct electrons from anode to cathode
9. In an electrolytic cell, which electrode is positive?
A. Anode
B. Cathode
C. Both
D. None
10. What is the main difference between galvanic and electrolytic cells?
A. Galvanic cells are non-spontaneous, electrolytic are spontaneous
B. Galvanic cells produce electricity, electrolytic use electricity
C. Galvanic cells use salt bridges, electrolytic do not
D. Both are identical in all aspects
Electrochemistry Quiz
11. Which of the following increases the rate of electrolysis?
A. Increasing electrode surface area
B. Decreasing electrolyte concentration
C. Using less conductive solution
D. Lowering applied voltage
12. In the reaction 2H₂O → 2H₂ + O₂, at which electrode is hydrogen produced?
A. Anode
B. Cathode
C. Salt bridge
D. Electrolyte
13. Which of these metals is more likely to be reduced in a redox reaction?
A. Metal with lower standard electrode potential
B. Metal with higher standard electrode potential
C. Metal in excess
D. Metal with highest density
14. What happens to the mass of the cathode in a galvanic cell during operation?
A. Increases due to deposition
B. Decreases due to oxidation
C. Remains constant
D. Fluctuates randomly
15. Which law relates the amount of substance deposited at an electrode to the quantity of electricity passed?
A. Boyle’s Law
B. Faraday’s First Law of Electrolysis
C. Charles’s Law
D. Avogadro’s Law
Electrochemistry Quiz
16. In the electrolysis of molten NaCl, what is produced at the cathode?
A. Cl₂ gas
B. Na metal
C. Na⁺ ions
D. H₂ gas
17. Which of the following is true for the cell potential of a spontaneous reaction?
A. Ecell < 0
B. Ecell = 0
C. Ecell > 0
D. Ecell can be negative or zero
18. What is oxidized in the reaction 2Fe²⁺ → 2Fe³⁺ + 2e⁻?
A. Fe²⁺
B. Fe³⁺
C. Electrons
D. None
19. The cathode in a galvanic cell is:
A. Positive and site of reduction
B. Positive and site of oxidation
C. Negative and site of reduction
D. Negative and site of oxidation
20. Which of the following is a correct description of a redox reaction?
A. Only oxidation occurs
B. Only reduction occurs
C. Oxidation and reduction occur simultaneously
D. No electron transfer occurs
Electrochemistry Quiz
21. In a cell notation Zn | Zn²⁺ || Cu²⁺ | Cu, which is the anode?
A. Zn
B. Cu
C. Cu²⁺
D. Zn²⁺
22. Which of the following is an application of electrochemistry?
A. Electroplating
B. Gas law calculations
C. Stoichiometry
D. Solubility equilibrium
23. In the electrolysis of acidified water, the ratio of H₂:O₂ produced is:
A. 1:1
B. 2:1
C. 1:2
D. 3:1
24. If E°cell = 1.10 V for a Zn/Cu galvanic cell, the reaction is:
A. Spontaneous
B. Non-spontaneous
C. At equilibrium
D. Cannot determine
25. Which species loses electrons in a redox reaction?
A. Oxidizing agent
B. Reducing agent
C. Cathode
D. Electrolyte
Electrochemistry Quiz Answers and Explanations:
1. Answer: B
Explanation: The anode is the site of oxidation in a galvanic cell.
2. Answer: B
Explanation: Cu²⁺ gains electrons (reduction), Zn loses electrons (oxidation).
3. Answer: B
Explanation: Electrons flow from Zn (anode) to Cu (cathode) externally.
4. Answer: B
Explanation: Anode is negative and where oxidation occurs.
5. Answer: C
Explanation: Electrolytic cells require external electricity to drive non-spontaneous reactions.
6. Answer: B
Explanation: Standard electrode potentials indicate the tendency for a species to be reduced; positive potential favors spontaneity.
7. Answer: B
Explanation: Cu loses electrons → reducing agent.
8. Answer: C
Explanation: Salt bridge maintains electrical neutrality by allowing ion flow.
9. Answer: A
Explanation: In electrolytic cells, anode is positive and attracts anions.
10. Answer: B
Explanation: Galvanic cells generate electricity spontaneously, electrolytic cells consume electricity.
11. Answer: A
Explanation: Increasing electrode surface area increases current and rate of electrolysis.
12. Answer: B
Explanation: Hydrogen is produced at the cathode by reduction.
13. Answer: B
Explanation: Metal with higher standard electrode potential is more easily reduced.
14. Answer: A
Explanation: Cathode gains mass as cations deposit during reduction.
15. Answer: B
Explanation: Faraday’s First Law states mass deposited ∝ charge passed.
16. Answer: B
Explanation: Na⁺ ions gain electrons at the cathode → Na metal.
17. Answer: C
Explanation: Spontaneous reactions have positive cell potential.
18. Answer: A
Explanation: Fe²⁺ loses electrons → oxidation.
19. Answer: A
Explanation: Cathode is positive in galvanic cells and site of reduction.
20. Answer: C
Explanation: Redox reactions always involve simultaneous oxidation and reduction.
21. Answer: A
Explanation: Zn (left) is oxidized → anode.
22. Answer: A
Explanation: Electroplating uses electrochemical principles.
23. Answer: B
Explanation: Electrolysis of H₂O produces 2 moles H₂ for 1 mole O₂.
24. Answer: A
Explanation: Positive E°cell indicates a spontaneous reaction.
25. Answer: B
Explanation: Reducing agent loses electrons and causes another species to be reduced.
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