# The anodic half-cell of lead-acid battery is recharged using electricity of 0.05 Faraday.

Question:

The anodic half-cell of lead-acid battery is recharged using electricity of $0.05$ Faraday. The amount of $\mathrm{PbSO}_{4}$ electrolyzed in $g$ during the process is : (Molar mass of $\mathrm{PbSO}_{4}=303 \mathrm{~g} \mathrm{~mol}^{-1}$ )

1. $22.8$

2. $15.2$

3. $7.6$

4.  $11.4$

Correct Option: , 3

Solution:

Half cell reaction: $\mathrm{PbSO}_{4} \rightarrow \mathrm{Pb}^{4+}+2 \mathrm{e}^{-}$

According to the reaction:

$\mathrm{PbSO}_{4} \rightarrow \mathrm{Pb}^{4+}+2 \mathrm{e}^{-}$

We require $2 \mathrm{~F}$ for the electrolysis of $1 \mathrm{~mol}$ or $303 \mathrm{~g}$ of $\mathrm{PbSO}_{4}$

$\therefore$ Amount of $\mathrm{PbSO}_{4}$ electrolysed by

$0.05 \mathrm{~F}=x .05=7.575 \mathrm{~g} \approx 7.6 \mathrm{~g}$