Electrochemistry — Class 12 Chemistry NCERT Solutions (Free)

Free step-by-step NCERT solutions for Class 12 Chemistry chapter "Electrochemistry" — 8 important questions with detailed answers for CBSE board exam preparation.

TL;DR: Free step-by-step NCERT solutions for Class 12 Chemistry chapter "Electrochemistry" — 8 important questions with detailed answers for CBSE board exam…

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Key Questions Covered:

  1. Define electrochemistry. What are electrodes and electrolytes?
  2. Write the Nernst equation and explain its significance.
  3. Calculate the standard cell potential for the reaction: Cu²⁺ + Zn → Cu + Zn²⁺…
  4. + 5 more questions in the full chapter

Solutions Summary:

Question Status
Define electrochemistry. What are electrodes and electrol… ✓ Solved
Write the Nernst equation and explain its significance. ✓ Solved
Calculate the standard cell potential for the reaction: C… ✓ Solved

Showing 3 of 8 questions

Q1: Define electrochemistry. What are electrodes and electrolytes?

Electrochemistry is the study of chemical reactions that produce electrical current or the use of electrical current to drive non-spontaneous chemical reactions. Electrode: A conductor (usually metal or graphite) through which current enters or leaves an electrolytic cell or galvanic cell. Types: 1...

Q2: Write the Nernst equation and explain its significance.

The Nernst equation relates cell potential to concentration of reactants and products at non-standard conditions. Nernst Equation: E_cell = E°_cell - (RT/nF) × ln(Q) Alternative form (at 25°C): E_cell = E°_cell - (0.0592/n) × log(Q) where: E_cell = cell potential at non-standard conditions E°_cel...

Q3: Calculate the standard cell potential for the reaction: Cu²⁺ + Zn → Cu + Zn²⁺. (Given: E°(Cu²⁺/Cu) = +0.34 V, E°(Zn²⁺/Zn) = -0.76 V)

Given: Cu²⁺ + Zn → Cu + Zn²⁺ E°(Cu²⁺/Cu) = +0.34 V E°(Zn²⁺/Zn) = -0.76 V Step 1: Identify oxidation and reduction Zn → Zn²⁺ + 2e⁻ (oxidation, occurs at anode) Cu²⁺ + 2e⁻ → Cu (reduction, occurs at cathode) Step 2: Calculate standard cell potential E°_cell = E°(cathode) - E°(anode) E°_cell = E°(Cu²...

Showing 3 of 8 questions. Visit the full page for complete solutions.