#electrolysis

CHEMISTRY

During the electrolysis of aqueous CuSO₄ using copper electrodes, what mass of copper is deposited at the cathode if a c

Given: During the electrolysis of aqueous CuSO₄ using copper electrodes, what mass of copper is deposited at the cathode if a current of 1.5 A flows for 10 minutes? (Molar mass of Cu = 63 g/mol, F = 96500 C/mol) These values define the system as per NCERT data. Formula: Charge, Q = I × t = 1.5 × 600 = 900 C. This is standard NCERT relation. Substitution & Calculation: For Cu²⁺ + 2e⁻ → Cu(s), 2F (2 × 96500 C) deposits 63 g of Cu. Mass = 63 × 900/2 × 96500 approx 0.294 g . Result: The computed value matches expected outcome and confirms correct choice as per NCERT.

Ref: NCERT Chemistry Textbook for Class XI and XII, Chapter: Electrochemistry, Topic: Faraday's first law, charge to reduce Al³⁺ to Al, 3F = 3 × 96500 C.

View Details

Variation of Conductivity with Concentration and Measurement

How many coulombs are required to deposit 0.27 g of aluminum from Al(NO₃)₃ solution? (Atomic mass of Al = 27 g/mol, F =

Al³⁺ + 3e⁻ → Al . 1 mol Al (27 g) requires 3F. Moles = (0.27/27) = 0.01 mol , Charge = 0.01 × 3 × 96500 = 2895 C .

Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Variation of Conductivity with Concentration and Measurement

View Details

Variation of Conductivity with Concentration and Measurement

How much charge (in coulombs) is required to oxidize 1 mole of H₂O to O₂? (F = 96500 C/mol)

2H₂O → O₂ + 4H⁺ + 4e⁻ . 1 mol O₂ requires 4F. Charge = 4 × 96500 = 386000 C .

Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Variation of Conductivity with Concentration and Measurement

View Details

Variation of Conductivity with Concentration and Measurement

What is the time (in seconds) required to deposit 0.405 g of calcium from molten CaCl₂ using a current of 1.5 A? (Atomic

Ca²⁺ + 2e⁻ → Ca . 1 mol Ca (40.5 g) requires 2F. Moles = (0.405/40.5) = 0.01 mol , Charge = 0.01 × 2 × 96500 = 1930 C . t = (Q/I) = (1930/1.5) = 1286.67 s .

Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Variation of Conductivity with Concentration and Measurement

View Details

Nernst Equation and Gibbs Energy and Equilibrium Constant

What is the time (in seconds) required to deposit 1.175 g of sodium from molten NaCl using a current of 2 A? (Atomic mas

Na⁺ + e⁻ → Na . 1 mol Na (23.5 g) requires 1F. Moles = (1.175/23.5) = 0.05 mol , Charge = 0.05 × 96500 = 4825 C . t = (Q/I) = (4825/2) = 2412.5 s .

Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Nernst Equation and Gibbs Energy and Equilibrium Constant

View Details

Electrolytic Cells and Electrolysis and Faraday's Laws

In electrolysis of molten MgCl₂, 0.24 g of Mg (atomic mass 24 g/mol) is deposited. What volume of Cl₂ gas (STP) is produ

Cathode: Mg²⁺ + 2e⁻ → Mg . Moles = (0.24/24) = 0.01 mol , Charge = 0.01 × 2 × 96500 = 1930 C . Anode: 2Cl⁻ → Cl₂ + 2e⁻ . Moles Cl₂ = 0.01 mol , Volume = 0.01 × 22.4 = 0.224 L .