The electrolysis of acetate solution produces ethane according to the reaction:2CH3COO- --> C2H6(g) + 2CO2(g) + 2e-The current efficiency of the process is 80%. What volume of gases would be produced at 27oC and 740 torr, if the current of 0.5 amp is passed through the solution of 96.45 min?

Explanation

Q V/F From the chemical equation, 2 moles of electrons produce 3 moles of gases (C2H6 + 2CO2)Now, Q = ItAs given, I = 0.5At = 96.45 min = 96.45 x 60 = 5787 sQ = 0.5 x 5787 = 2893.5However, the system is only 80% efficient or has an efficiency of 0.8. So, Actual Q = 0.8 x Q= 0.8 x 2893.5= 2314.8 CNow, according to the formulaN = actual Q/F (where F = Faraday's constant = 96485 C/mol, and n = no. of electrons)So, n = 2314.8 / 96485= 0.024As 3 moles of gases are produced, then 3n = 3 x 0.024= 0.036Now, according to the gas equationPV = nRTOr V = nRT/PPut n = 0.036, R = 0.0821, T= 300 K, P = 0.97 atmV = [0.036*0.0821*300]/0.97= 0.91LHence, option D is the correct option.