Class 12 Chemistry — Chapter 2: Electrochemistry
98 practice questions · 33 Easy · 33 Medium · 32 Hard
Practise Class 12 Chemistry Chapter 2, "Electrochemistry", with 98 NCERT-aligned multiple-choice questions. The set is split into 33 Easy, 33 Medium and 32 Hard questions, so you can warm up on the fundamentals and then push into the exam-level problems that separate top scorers in CBSE Board exams, JEE Main, JEE Advanced and NEET UG.
"Electrochemistry" is one of the chapters where reactions, named concepts, and balanced numerical work really pays off. Each MCQ on this chapter is timed and uses exam-grade marking (+2 correct, −1 wrong, 0 skipped), training the same accuracy-under-pressure that real papers demand. Every question carries a short explanation, so a wrong answer becomes a quick lesson rather than a dead end — the fastest way to close gaps before a test.
Use this chapter as targeted revision: attempt the Easy set first to confirm your basics on Electrochemistry, then move to Medium and Hard to test application and problem-solving. Your accuracy, streaks and XP save automatically, and the chapter feeds into your overall Class 12 Chemistry mastery score. A few sample questions are shown below; sign in free to practise all 98.
Key concepts: Electrochemistry (Class 12 Chemistry)
This chapter covers galvanic and electrolytic cells, electrode potentials, the Nernst equation, conductance, and the relation between cell potential and Gibbs energy.
- Galvanic cell
- Converts chemical energy to electrical energy via a spontaneous redox reaction; oxidation at the anode, reduction at the cathode.
- Electrode potential & EMF
- Cell EMF = E°cathode − E°anode (standard); a positive EMF means a spontaneous reaction.
- Nernst equation
- Gives electrode/cell potential at non-standard concentrations: E = E° − (0.059/n) log Q at 298 K.
- Conductance
- Molar conductivity Λm increases on dilution; Kohlrausch's law lets us find Λm° for weak electrolytes.
- EMF and thermodynamics
- ΔG = −nFE°cell links cell potential to Gibbs energy and the equilibrium constant.
Key formulas — Electrochemistry
💡 Exam tips for Electrochemistry
- A positive E°cell ⇒ spontaneous reaction (and negative ΔG).
- Molar conductivity rises on dilution; for weak electrolytes use Kohlrausch's law to get Λm°.
Sample questions
In a galvanic cell, oxidation occurs at the:
Anode = oxidation (loss of electrons). Cathode = reduction.
Standard emf of a cell is given by:
E°_cell = E°_cathode − E°_anode (both as reduction potentials).
How many faradays are required to deposit 1 mol of Al from molten Al₂O₃?
Al³⁺ + 3e⁻ → Al. So 3 mol electrons = 3 F per mol of Al.
Electrochemistry — FAQs
What are the key concepts in Class 12 Chemistry Electrochemistry?+
This chapter covers galvanic and electrolytic cells, electrode potentials, the Nernst equation, conductance, and the relation between cell potential and Gibbs energy. Key ideas include Galvanic cell, Electrode potential & EMF, Nernst equation, Conductance, EMF and thermodynamics.
What does Class 12 Chemistry Chapter 2 (Electrochemistry) cover on XamBaaz?+
It covers 98 NCERT-aligned MCQs on "Electrochemistry" — 33 Easy, 33 Medium and 32 Hard — each with a timed quiz and an instant explanation, suitable for CBSE Board exams, JEE Main, JEE Advanced and NEET UG.
Are these "Electrochemistry" questions free to practise?+
Yes — sign in with Google to practise "Electrochemistry" free. Full unlimited access is ₹999/year (limited-time launch price), with no per-chapter charges.
How should I revise "Electrochemistry" for the exam?+
Start with the Easy quiz to confirm your fundamentals, then attempt Medium and Hard for application-level practice. Review each explanation, retry the questions you miss, and track your accuracy on this chapter until it is consistently high.
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