Question

The volume of gases evolved when dil. $H_{2}S{O}_4$ is electrolysed when 2F of charge is passed at STP is:

• A. 22.4 L
• B. 11.2 L
• C. 33.6 L
• D. 44.8 L

Answer 1

The correct option is C 33.6 L

Chemical reactions occur during electrolysis of $H_{2}S{O}_4$
At cathode:
$2H^{+}+2e^{-}\to H_2\left(g\right)$
At Anode:
$H_{2}O\to \frac{1}{2}{O}_2+2e^{-}+2H^{+}$
From the reactions, it is clearly states that 2 moles of electrons give half mole of $O_2$ and one mole of $H_2$ .
1 mole of gas occupied volume is 22.4 L at STP
Total moles $=1.5$
volume $=1.5\times 22.4=33.6L$