Question

Electrolysis of dilute aqueous $NaCl$ solution was carried out by passing $10\text{mA}$ current. The time required ( in seconds) to liberate 0.01 mole of $H_2$ gas at the cathode is $x\times {10}^{4}s$. Find the value of $x$. $(1F=96500{\text{C mol}}^{-1})$.

Answer 1

$0.01\text{mol}$ of $H_2=0.02\text{g equivalent}$
$\Rightarrow$ Columbs required=$0.02\times 96500=1930C$
$\Rightarrow Q=It=1930C$
$\Rightarrow t=\frac{1930}{10\times {10}^{-3}}=19.3\times {10}^{4}s$