ElectrochemistryHard

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%.

Options

A.1.344 L
B.2.688 L
C.4.032 L
D.1.792 L

Solution

$n_{eq}CH_{3}COO^{-}\text{ oxidised = }\frac{Q}{F}$

Or, $n \times 1 = \frac{0.5 \times 482.5 \times 60 \times 0.8}{96500} \Rightarrow n = 0.12$

∴ Moles of (C2H6 + CO2) produced = $\frac{3}{2} \times 0.12 = 0.18$

and total volume = 0.18 × 22.4 = 4.032 L

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