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NEET Electrochemistry: 5 practice MCQs with answers

By the PrepMatic team · Updated 9 Oct 2026 · 4 min read

Electrochemistry links chemical change to electrical energy and conductance, and it is one of the most formula-driven chapters of Class 12 Chemistry. The five MCQs below test cell potential, Faraday's law, the Nernst equation, molar conductivity and Kohlrausch's law, at NCERT level.

What this chapter covers in the NEET syllabus

In the NMC syllabus this belongs to the combined unit Redox Reactions and Electrochemistry, and the redox half is on NEET Redox Reactions. The electrochemistry topics, matching the NCERT Class 12 chapter, are:

• Electrolytic and metallic conduction, specific and molar conductivity, and how they vary with concentration.
• Kohlrausch's law and its applications.
• Electrochemical cells: galvanic and electrolytic cells, electrode potentials and the standard hydrogen electrode.
• EMF of a cell, the Nernst equation and its applications, and the relation between cell potential and Gibbs energy.
• Faraday's laws of electrolysis.
• Dry cell, lead accumulator and fuel cells.

Five practice MCQs on Electrochemistry

Question 1

Given E° (Zn²⁺/Zn) = −0.76 V and E° (Cu²⁺/Cu) = +0.34 V, the standard EMF of the Daniell cell is:

• A. 0.42 V
• B. −1.10 V
• C. 1.10 V
• D. 0.76 V

Question 2

A charge of 9650 coulombs is passed through a solution of AgNO₃. The mass of silver deposited is (Ag = 108 g/mol; F = 96500 C/mol):

• A. 10.8 g
• B. 108 g
• C. 1.08 g
• D. 5.4 g

Question 3

The electrode potential of a Cu²⁺/Cu half-cell with [Cu²⁺] = 0.01 M at 298 K is (E° = +0.34 V; use 0.059/n log form):

• A. 0.399 V
• B. 0.34 V
• C. 0.22 V
• D. 0.281 V

Question 4

A 0.1 M solution of an electrolyte has a conductivity of 0.012 S cm⁻¹. Its molar conductivity is:

• A. 1.2 S cm² mol⁻¹
• B. 12 S cm² mol⁻¹
• C. 120 S cm² mol⁻¹
• D. 1200 S cm² mol⁻¹

Question 5

Given Λ°m values (S cm² mol⁻¹): CH₃COONa = 91, HCl = 426, NaCl = 126. The limiting molar conductivity of acetic acid is:

• A. 643
• B. 391
• C. 301
• D. 217

Answers and explanations

1. C. E°cell = E°cathode − E°anode = 0.34 − (−0.76) = 1.10 V. Copper has the higher reduction potential, so it is the cathode and zinc the anode.
2. A. Moles of electrons = 9650/96500 = 0.1 mol. Ag⁺ + e⁻ → Ag needs one electron per atom, so 0.1 mol of Ag is deposited: 0.1 × 108 = 10.8 g.
3. D. For Cu²⁺ + 2e⁻ → Cu, E = E° − (0.059/2) log(1/[Cu²⁺]) = 0.34 − 0.0295 × log(100) = 0.34 − 0.059 = 0.281 V. Option A has the sign wrong, and option C uses n = 1 instead of 2.
4. C. Λm = κ × 1000/M, with κ in S cm⁻¹ and M in mol L⁻¹: 0.012 × 1000/0.1 = 120 S cm² mol⁻¹. The factor 1000 converts litres to cm³.
5. B. By Kohlrausch's law, Λ°m(CH₃COOH) = Λ°m(CH₃COONa) + Λ°m(HCl) − Λ°m(NaCl) = 91 + 426 − 126 = 391 S cm² mol⁻¹. Adding all three (643) is a classic error.

How to prepare Electrochemistry

• Learn to build a cell from two half-cells. The electrode with the higher reduction potential is the cathode. E°cell = E°cathode − E°anode, and a positive value means a spontaneous cell. Write the overall reaction by adding the two half-reactions after balancing electrons.
• Master the Nernst equation in its 298 K form: E = E° − (0.059/n) log Q. Practise it for both single electrodes and full cells, and know that E = 0 at equilibrium, where Q = K.
• Connect to thermodynamics. ΔG° = −nFE°cell and ΔG° = −RT ln K. These links often appear as short calculations.
• For Faraday's laws, track moles of electrons. Q = I × t, moles of e⁻ = Q/F, then use the stoichiometry of the half-reaction. Write the electrode reaction before you start.
• Know how conductivity changes. Conductivity falls on dilution (fewer ions per volume) but molar conductivity rises. Strong electrolytes are extrapolated to limiting values, and weak electrolytes need Kohlrausch's law.
• Memorise the batteries and fuel cells: what happens at each electrode of a lead storage battery and an H₂-O₂ fuel cell.

Two or three sessions of mixed numericals make this chapter dependable. Read about Physical Chemistry planning in the NEET Chemistry preparation guide, and about the unit list in the NEET syllabus.

Take a full Electrochemistry test on PrepMatic

Formula-heavy chapters are where negative marking hurts most, so practise under test conditions. PrepMatic's topic tests run about 15 questions in 30 minutes and score +4 for a correct answer and −1 for a wrong one, as in NEET. Topic tests are included in the free Basic plan, and more chapters are on the practice hub.

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