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Cathode: Cu²⁺ + 2e⁻ → Cu . Copper metal is deposited.
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Electrolytic Cells and Electrolysis and Faraday's Laws
Anode: 2Cl⁻ → Cl₂ + 2e⁻ . Chlorine gas is produced due to overpotential.
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Electrolytic Cells and Electrolysis and Faraday's Laws
Cathode: 2H₂O + 2e⁻ → H₂ + 2OH⁻ , Anode: 2H₂O → O₂ + 4H⁺ + 4e⁻ . Total moles = (0.336/22.4) = 0.015 mol (H₂:O₂ = 2:1), H₂ = 0.01 mol, O₂ = 0.005 mol. Charge = (0.01 × 2 + 0.005 × 4) × 96500 = 0.04 × 96500 = 3860 C .
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Electrolytic Cells and Electrolysis and Faraday's Laws
Anode: 2Br⁻ → Br₂ + 2e⁻ . 1 mol Br₂ (22.4 L) requires 2F. Moles = (0.112/22.4) = 0.005 mol , Charge = 0.005 × 2 × 96500 = 965 C .
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Electrolytic Cells and Electrolysis and Faraday's Laws
Anode: 2H₂O → O₂ + 4H⁺ + 4e⁻ . Oxygen gas is produced.
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Electrochemical Cells - Galvanic Cells and Electrode Potential
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