Practice question
Question
In electrolysis of molten CaCl₂, 0.4 g of Ca (atomic mass 40 g/mol) is deposited. What volume of Cl₂ gas (STP) is produced at the anode? (F = 96500 C/mol)
Explanation
Cathode: Ca²⁺ + 2e⁻ → Ca , Moles = (0.4/40) = 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 .
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