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Electrochemistry WBJEE MCQ & Practice Questions

Practice Electrochemistry MCQs for WBJEE Chemistry with answers, explanations, chapter revision and related ChemNexa mock tests.

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Electrochemistry Revision Guide for WBJEE Chemistry

Electrochemistry connects chemical change with electrical energy. For exam preparation, students should be comfortable with galvanic and electrolytic cells, electrode potentials, cell notation, conductance and electrolysis. The most useful approach is to understand what each equation represents before applying it to numerical problems.

For WBJEE Chemistry, revise the sign conventions for anode and cathode, standard electrode potential, the Nernst equation, molar conductivity and Faraday laws. After concept revision, solve mixed conceptual and numerical MCQs so that formula selection becomes automatic under time pressure.

Important Topics

  • Electrochemical and galvanic cells
  • Standard electrode potential and cell EMF
  • Nernst equation and reaction quotient
  • Conductance, conductivity and molar conductivity
  • Kohlrausch law and limiting molar conductivity
  • Electrolysis and Faraday laws

Important Formulae & Relationships

  • Ecell = Ecathode − Eanode
  • E = E° − (RT/nF) ln Q
  • At 298 K: E = E° − (0.0591/n) log Q
  • Λm = κ × 1000 / C
  • m = (MIt)/(nF)

Use formulas only after checking the required units, sign convention and assumptions for the question.

What to practise in Electrochemistry

Concept Revision

Revise definitions, principles, equations, trends and core ideas from Electrochemistry before attempting MCQs.

Exam-style MCQs

Use chapter-focused multiple-choice practice to improve accuracy, recall and application for WBJEE Chemistry.

Performance Practice

Attempt ChemNexa tests, review results and return to weak areas for another round of targeted revision.

Top 20 Electrochemistry MCQs with Answers

These public questions are selected from the exact Electrochemistry chapter, screened for topic relevance and deduplicated so repeated versions of the same MCQ are not shown publicly. Use them for quick revision, then sign in to attempt the complete test experience with more questions, results and performance review.

WBJEE Chemistry · Electrochemistry · Very Very Hard

1. Consider: (I) oxidation occurs at anode; (II) E°cell=E°cathode-E°anode; (III) ΔG=-nFE; (IV) molar conductivity usually increases on dilution. Which are correct?

  • A. I, III and IV only
  • B. I, II, III and IV
  • C. I and II only
  • D. II and III only
Answer: B
Explanation: All four statements are correct.

WBJEE Chemistry · Electrochemistry · Very Very Hard

2. Electrochemistry concept check: Consider: (I) oxidation occurs at anode; (II) E°cell=E°cathode-E°anode; (III) ΔG=-nFE; (IV) molar conductivity usually increases on dilution. Which are correct?

  • A. I and II only
  • B. II and III only
  • C. I, III and IV only
  • D. I, II, III and IV
Answer: D
Explanation: All four statements are correct.

WBJEE Chemistry · Electrochemistry · Very Very Hard

3. Standard cell potential is calculated as:

  • A. E°cathode + E°anode always
  • B. E°anode/E°cathode
  • C. E°cathode - E°anode
  • D. E°anode - E°cathode
Answer: C
Explanation: Using standard reduction potentials, E°cell=E°cathode-E°anode.

WBJEE Chemistry · Electrochemistry · Very Very Hard

4. Electrochemistry concept check: Standard cell potential is calculated as:

  • A. E°cathode - E°anode
  • B. E°anode - E°cathode
  • C. E°cathode + E°anode always
  • D. E°anode/E°cathode
Answer: A
Explanation: Using standard reduction potentials, E°cell=E°cathode-E°anode.

WBJEE Chemistry · Electrochemistry · Very Very Hard

5. WBJEE advanced: Standard cell potential is calculated as:

  • A. E°cathode + E°anode always
  • B. E°anode/E°cathode
  • C. E°cathode - E°anode
  • D. E°anode - E°cathode
Answer: C
Explanation: Using standard reduction potentials, E°cell=E°cathode-E°anode.

WBJEE Chemistry · Electrochemistry · Very Very Hard

6. In a galvanic cell, oxidation occurs at the:

  • A. Anode
  • B. Cathode
  • C. Salt bridge
  • D. Electrolyte only
Answer: A
Explanation: The anode is the site of oxidation.

WBJEE Chemistry · Electrochemistry · Very Very Hard

7. In a galvanic cell, reduction occurs at the:

  • A. Anode
  • B. Salt bridge
  • C. External wire
  • D. Cathode
Answer: D
Explanation: The cathode is the site of reduction.

WBJEE Chemistry · Electrochemistry · Very Very Hard

8. In a spontaneous galvanic cell, electrons flow externally from:

  • A. Salt bridge to anode
  • B. Electrolyte to salt bridge
  • C. Anode to cathode
  • D. Cathode to anode
Answer: C
Explanation: Electrons generated at the anode travel to the cathode.

WBJEE Chemistry · Electrochemistry · Very Very Hard

9. At equilibrium, the cell potential of a reversible cell is:

  • A. Zero
  • B. Always positive
  • C. Always negative
  • D. Equal to 1 V
Answer: A
Explanation: At equilibrium ΔG=0 and therefore Ecell=0.

WBJEE Chemistry · Electrochemistry · Very Very Hard

10. Electrochemistry concept check: In a galvanic cell, oxidation occurs at the:

  • A. Salt bridge
  • B. Electrolyte only
  • C. Anode
  • D. Cathode
Answer: C
Explanation: The anode is the site of oxidation.

WBJEE Chemistry · Electrochemistry · Very Very Hard

11. Electrochemistry concept check: In a galvanic cell, reduction occurs at the:

  • A. External wire
  • B. Cathode
  • C. Anode
  • D. Salt bridge
Answer: B
Explanation: The cathode is the site of reduction.

WBJEE Chemistry · Electrochemistry · Very Very Hard

12. Electrochemistry concept check: In a spontaneous galvanic cell, electrons flow externally from:

  • A. Anode to cathode
  • B. Cathode to anode
  • C. Salt bridge to anode
  • D. Electrolyte to salt bridge
Answer: A
Explanation: Electrons generated at the anode travel to the cathode.

WBJEE Chemistry · Electrochemistry · Very Very Hard

13. Electrochemistry concept check: At equilibrium, the cell potential of a reversible cell is:

  • A. Always negative
  • B. Equal to 1 V
  • C. Zero
  • D. Always positive
Answer: C
Explanation: At equilibrium ΔG=0 and therefore Ecell=0.

WBJEE Chemistry · Electrochemistry · Very Very Hard

14. WBJEE advanced: In a galvanic cell, oxidation occurs at the:

  • A. Anode
  • B. Cathode
  • C. Salt bridge
  • D. Electrolyte only
Answer: A
Explanation: The anode is the site of oxidation.

WBJEE Chemistry · Electrochemistry · Very Very Hard

15. WBJEE advanced: In a galvanic cell, reduction occurs at the:

  • A. Anode
  • B. Salt bridge
  • C. External wire
  • D. Cathode
Answer: D
Explanation: The cathode is the site of reduction.

WBJEE Chemistry · Electrochemistry · Very Very Hard

16. WBJEE advanced: In a spontaneous galvanic cell, electrons flow externally from:

  • A. Salt bridge to anode
  • B. Electrolyte to salt bridge
  • C. Anode to cathode
  • D. Cathode to anode
Answer: C
Explanation: Electrons generated at the anode travel to the cathode.

WBJEE Chemistry · Electrochemistry · Very Very Hard

17. WBJEE advanced: At equilibrium, the cell potential of a reversible cell is:

  • A. Zero
  • B. Always positive
  • C. Always negative
  • D. Equal to 1 V
Answer: A
Explanation: At equilibrium ΔG=0 and therefore Ecell=0.

WBJEE Chemistry · Electrochemistry · Very Very Hard

18. For a spontaneous galvanic cell under operating conditions, Ecell is:

  • A. Negative
  • B. Always zero
  • C. Infinite
  • D. Positive
Answer: D
Explanation: A spontaneous cell reaction has positive cell potential.

WBJEE Chemistry · Electrochemistry · Very Very Hard

19. The Nernst equation relates electrode/cell potential to:

  • A. Only density
  • B. Only electrode area
  • C. Reaction quotient and temperature
  • D. Only molar mass
Answer: C
Explanation: Nernst equation gives the concentration/activity dependence of potential.

WBJEE Chemistry · Electrochemistry · Very Very Hard

20. The relation between E°cell and equilibrium constant K at 298 K is:

  • A. E°=(0.0591/n)log K
  • B. E°=-(0.0591/n)log K
  • C. E°=n/0.0591 log K
  • D. E°=0.0591n/K
Answer: A
Explanation: Combining ΔG°=-nFE° with ΔG°=-RT ln K gives this relation.

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Electrochemistry Practice Tests

Electrochemistry Frequently Asked Questions

What should I revise first in Electrochemistry?

Start with oxidation and reduction, electrode notation, anode/cathode conventions and standard electrode potential. Then move to the Nernst equation, conductance and electrolysis.

Why is the Nernst equation important?

It relates electrode or cell potential to concentration and the reaction quotient, so it is central to many conceptual and numerical electrochemistry problems.

How should I practise Electrochemistry MCQs?

Mix direct concept questions with short calculations. Review every wrong answer and identify whether the error came from a sign convention, unit conversion, formula choice or concept gap.

Continue with another chapter to build connected concepts and strengthen your overall Chemistry preparation.

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