Electrolysis of an acetate solution produces ethane according to the reaction: 2CH3COO^– - C2H6(g) + 2CO2(g) + 2e^–. What total volume of ethane and CO2 would be produced at 0°C and 1 atm, if a curre

Question

Electrolysis of an acetate solution produces ethane according to the reaction: 2CH3COO^– -> C2H6(g) + 2CO2(g) + 2e^–. What total volume of ethane and CO2 would be produced at 0°C and 1 atm, if a current of 0.5 A is passed through the solution for 482.5 min? Assume current efficiency 80%.

Prashant Kotian · Accepted Answer

Correct answer: C. Total charge Q = I × t × efficiency = 0.5 × (482.5 × 60) × 0.80 = 11580 C. Faradays passed = 11580 / 96500 = 0.12 F. The reaction produces 1 mole of C2H6 and 2 moles of CO2 (total 3 moles of gas) for every 2 Faradays of charge. Total moles of gas = (3/2) × 0.12 = 0.18 mol. Volume at STP = 0.18 mol × 22.4 L/mol = 4.032 L. Therefore, correct answer is C.

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