Question

A certain amount of charge is passed through acidulated water. A total of $504$ mL of hydrogen and oxygen were collected at STP. Find the magnitude of charge that is passed during electrolysis in coulombs.

Answer 1

Since upon electrolysis 168 ml of $O_2$ and 336 ml $H_2$ was produced because volume of $H_2$ is double of $O_2$ in electrolysis.

$H_{2}O⟶H_2+\frac{1}{2}{O}_2$ $(n_f=2)$

So 2 faraday is required for 22.4 litre of $H_2$ liberation

hence for $(168\times 2)$ ml $⟶$ $\left(\frac{2\times 336}{22400}\right)$=0.03 Faraday