- iamal
- February 14, 2026
Ultimate Electrochemical Cell Anode Cathode and EMF MCQs: Proven Practice to Maximize Your Exam Score
Electrochemistry is one of the most scoring yet conceptually demanding chapters in senior secondary chemistry. Among the most frequently tested areas are electrochemical cell anode cathode and emf mcqs, because they examine both theoretical clarity and numerical skill. Aspirants preparing for board exams, NEET, JEE, or other competitive tests often encounter electrochemical cell anode cathode and emf mcqs that test sign conventions, spontaneity, and electrode identification.
To master electrochemical cell anode cathode and emf mcqs, one must first understand the fundamental structure of an electrochemical cell. A galvanic (voltaic) cell converts chemical energy into electrical energy through a spontaneous redox reaction. In such a cell, oxidation occurs at the anode and reduction occurs at the cathode. This principle is central to solving electrochemical cell anode cathode and emf mcqs accurately.
A common point of confusion in electrochemical cell anode cathode and emf mcqs is the sign of the electrodes. In a galvanic cell, the anode is negative because it releases electrons, while the cathode is positive because it gains electrons. However, in an electrolytic cell, the signs are reversed due to the presence of an external power source. Recognizing this distinction is crucial when practicing electrochemical cell anode cathode and emf mcqs.
The electromotive force (emf) of a cell represents the maximum potential difference between the two electrodes when no current flows. It is calculated using the standard electrode potentials:
E°cell = E°cathode − E°anode
This formula appears repeatedly in electrochemical cell anode cathode and emf mcqs, and aspirants must apply it carefully. Errors often arise when learners subtract in the wrong order or misidentify oxidation and reduction half-reactions. Regular practice of electrochemical cell anode cathode and emf mcqs helps eliminate these mistakes.
Spontaneity of the reaction is directly related to emf. When E°cell is positive, the reaction is spontaneous and the standard Gibbs free energy change is negative. The relationship is given by:
ΔG° = −nFE°cell
Understanding this equation is essential for advanced electrochemical cell anode cathode and emf mcqs that combine thermodynamics with redox chemistry. Many electrochemical cell anode cathode and emf mcqs require aspirants to calculate equilibrium constants using this relationship.
Under non-standard conditions, the emf changes according to the Nernst equation:
Ecell = E°cell − (0.0591/n) log Q (at 298 K)
The Nernst equation is frequently applied in electrochemical cell anode cathode and emf mcqs involving concentration changes. Questions may involve dilution, varying ion concentrations, or reaction quotients. Comfort with logarithmic calculations improves performance in electrochemical cell anode cathode and emf mcqs.
Cell notation is another important aspect. By convention, the anode is written on the left and the cathode on the right. For example:
Zn | Zn²⁺ || Cu²⁺ | Cu
Here, zinc is the anode and copper is the cathode. Correctly interpreting such notation is a recurring theme in electrochemical cell anode cathode and emf mcqs. Aspirants who quickly identify half-reactions gain a time advantage in exams.
Salt bridges maintain electrical neutrality by allowing ion migration between half-cells. Though they do not directly affect emf, misunderstandings about their function often appear in electrochemical cell anode cathode and emf mcqs. Clear conceptual understanding prevents confusion.
Temperature dependence of emf is also occasionally tested. The temperature coefficient relates to entropy change of the reaction. Such conceptual extensions are sometimes integrated into higher-level electrochemical cell anode cathode and emf mcqs.
In summary, success in electrochemical cell anode cathode and emf mcqs depends on mastering oxidation and reduction concepts, understanding electrode signs, applying emf formulas correctly, using the Nernst equation confidently, and interpreting cell notation accurately. Consistent practice and conceptual clarity ensure strong performance in electrochemical cell anode cathode and emf mcqs, making this topic both manageable and highly scoring for competitive examinations.
Electrochemical Cell Anode Cathode and EMF MCQs
1. Other things being equal, the EMF of a Daniel cell may be increased by
A. keeping low temperature
B. using large copper electrodes
C. using large zinc electrodes
D. decreasing concentration of Cu²⁺ ions
Answer: A
2. Match the electrode (Column-I) with its general name (Column-II)
Column-I:
A. Calomel
B. Glass
C. Hydrogen
D. Quinhydrone
Column-II:
-
Reference
-
Redox
-
Membrane
-
Gas
Options:
A. A-1, B-3, C-4, D-2
B. A-3, B-4, C-2, D-1
C. A-3, B-2, C-4, D-1
D. A-2, B-4, C-3, D-1
Answer: A
3. In a Daniell cell constructed in the laboratory, the voltage observed was 0.9 V instead of 1.1 V of the standard cell. A possible explanation is
A. [Zn²⁺] > [Cu²⁺]
B. [Zn²⁺] < [Cu²⁺]
C. Zn electrode has twice the surface of Cu electrode
D. mol ratio of Zn²⁺ : Cu²⁺ = 2 : 1
Answer: A
4. In electrolysis of NaCl when Pt electrode is taken then H₂ is liberated at cathode while with Hg electrode it forms sodium amalgam
A. Hg is more inert than Pt
B. More voltage is required to reduce H⁺ at Hg than at Pt
C. Na is dissolved in Hg while it does not dissolve in Pt
D. Concentration of H⁺ ions is larger when Pt electrode is taken
Answer: B
5. Minimum emf required to carry out electrolysis of Al₂O₃
A. 2.14 V
B. 4.28 V
C. 6.42 V
D. 8.56 V
Answer: A
6. The equilibrium constant of a reaction (E° = 0.295 V, n = 2) is
A. 2.0 × 10¹¹
B. 4.0 × 10¹²
C. 1.0 × 10²
D. 1.0 × 10¹⁰
Answer: D
7. In galvanic cell, the salt bridge is used to
A. complete the circuit
B. reduce the electric resistance in the cell
C. separate cathode from anode
D. carry salts for the chemical reaction
Answer: A
8. Anode reaction of a fuel cell is
A. Zn(Hg) + 2OH⁻ → ZnO + H₂O + 2e⁻
B. Pb + SO₄²⁻ → PbSO₄ + 2e⁻
C. 2H₂ + 4OH⁻ → 4H₂O + 4e⁻
D. 2Fe → 2Fe²⁺ + 4e⁻
Answer: C
9. Correct representation of Sn/Cu cell is
A. Sn | Sn²⁺ (0.1M) || Cu²⁺ (1M) | Cu
B. Sn | Sn²⁺ (1M) || Cu⁺ (1M) | Cu
C. Sn | Sn²⁺ (1M) || Cu²⁺ (1M) | Cu
D. None
Answer: C
10. In electrolysis of aqueous CuSO₄ using copper electrode, at anode
A. SO₄²⁻ → SO₄ + 2e⁻
B. Cu → Cu⁺ + e⁻
C. 2OH⁻ → H₂O + ½O₂ + e⁻
D. Cu → Cu²⁺ + 2e⁻
Answer: D
11. Galvanic cell is a device in which
A. chemical energy is converted into electrical energy
B. electrical energy is converted into chemical energy
C. chemical energy appears as heat
D. thermal energy drives reaction
Answer: A
12. Cell reaction in Daniell cell is
A. Cu + ZnSO₄ → CuSO₄ + Zn
B. Zn + CuSO₄ → Cu + ZnSO₄
C. Ni + ZnSO₄ → NiSO₄ + Zn
D. 2Na + CdSO₄ → Na₂SO₄ + Cd
Answer: B
13. Correct statement is
A. Unit of emf is V cm⁻¹
B. ΔG = -(nF)/E
C. In galvanic cell, chemical energy → electrical energy
D. Oxidation state of Mn in KMnO₄ is +6
Answer: C
14. Cell reaction is spontaneous when
A. E°red is negative
B. E°red is positive
C. ΔG° is negative
D. ΔG° is positive
Answer: C
15. Efficiency of a fuel cell is
A. ΔG/ΔS
B. ΔG/ΔH
C. ΔS/ΔG
D. ΔH/ΔG
Answer: B
16. When an acid cell is charged
A. voltage increases
B. resistance increases
C. electrolyte dilutes
D. All
Answer: A
17. Anode in galvanic cell is
A. negative electrode
B. positive electrode
C. neutral electrode
D. None
Answer: A
18. Regarding sulphuric acid concentration in battery
A. Not in effective range
B. In effective range
C. Hardly in effective range
D. Mechanic decides
Answer: B
19. What flows in the internal circuit of galvanic cell?
A. Ions
B. Electrons
C. Electricity
D. Atoms
Answer: A
20. Correct representation of reaction
2AgCl + H₂ → 2HCl + 2Ag
A. Pt | H₂ | KCl | AgCl | Ag
B. Pt | H₂ | HCl | Ag⁺ | Ag
C. Pt | H₂ | HCl | AgCl | Ag
D. None
Answer: B
21. Molar conductance of 0.1 M HNO₃ (κ = 6.3 × 10⁻²)
A. 6300 Ω⁻¹ cm² mol⁻¹
B. 630 Ω⁻¹ cm² mol⁻¹
C. 63 Ω⁻¹ cm² mol⁻¹
D. 6.3 Ω⁻¹ cm² mol⁻¹
Answer: B
Conclusion on Electrochemical Cell Anode Cathode and EMF MCQs
In summary, success in electrochemical cell anode cathode and emf mcqs depends on mastering oxidation and reduction concepts, understanding electrode signs, applying emf formulas correctly, using the Nernst equation confidently, and interpreting cell notation accurately. Consistent practice and conceptual clarity ensure strong performance in electrochemical cell anode cathode and emf mcqs, making this topic both manageable and highly scoring for competitive examinations.