Calculate the quantity of electricity required to liberate 0.224 dm ^3 of chlorine at STP during the electrolysis of fused sodium chloride?

Step-by-step solution

Electrolysis of fused sodium chloride liberates chlorine gas at the anode: 2 Cl ^- Cl ₂ + 2 e ^- Since one mole of chlorine gas corresponds to two moles of electrons transferred, the moles of Cl ₂ produced are calculated from its volume at STP, where one mole occupies 22.4 dm³. For 0.224 dm³: Moles of Cl ₂ = 0.224 22.4 = 0.01 Moles of electrons required: 0.01 2 = 0.02 Using Faraday’s constant, 1 F = 96500 C per mole of electrons, the charge is: Q = 0.02 96500 = 1930 C The quantity of electricity required is 1930 C,