An aqueous solution containing 82 grams of sodium acetate is subjected to electrolysis. The volume of gas obtained at anode (at STP) will be

$2{\mathrm{CH}}_3-\mathrm{COONa}+2{\mathrm{H}}_2\mathrm{O}\stackrel{\mathrm{electr}o\mathrm{lysis}}{\to }\underset{\mathrm{Anode}}{{\mathrm{CH}}_3-{\mathrm{CH}}_3\uparrow + 2{\mathrm{CO}}_2}\uparrow +2\mathrm{NaOH}+\underset{\mathrm{Cathode}}{{\mathrm{H}}_2}\uparrow$

At anode

2moles of ${\mathrm{CH}}_3\mathrm{COONa}$ ------- 1mole of Ethane + 2moles of ${\mathrm{CO}}_2$

1mole of ${\mathrm{CH}}_3\mathrm{COONa}\left(82\mathrm{g}\right)$ ----- $\frac{1}{2}$  mole of ethane + 1mole of ${\mathrm{CO}}_2$

$\therefore$ 11.2 lit of ${\mathrm{C}}_2{\mathrm{H}}_6$ + 22.4 lit of ${\mathrm{CO}}_2$ at STP.

$33.6 \mathrm{lit} \mathrm{of} \mathrm{gases} \mathrm{at} \mathrm{STP}$