How much charge should be supplied to a cell for the electrolytic production of $245 \mathrm{~gm}$…
How much charge should be supplied to a cell for the electrolytic production of $245 \mathrm{~gm}$ $\mathrm{NaClO}_{4}$ from $\mathrm{NaClO}_{3}$ if the anode efficiency for the required reaction is $60 \%$ ?
$6.43 \times 10^{5} \mathrm{C}$
$5.67 \mathrm{~F}$
$6.43 \times 10^{6} \mathrm{C}$
$66.67 \mathrm{~F}$
Solution
$\mathrm{ClO}_{4}^{-}+2 \mathrm{H}^{+}+2 \mathrm{e}^{-} ightarrow \mathrm{ClO}_{3}^{-}+\mathrm{H}_{2} \mathrm{O}$
Number of equivalents of
$\mathrm{NaClO}_{4}=\frac{245}{61.25}=4=4 \mathrm{~F}$
No. of Faradays $=\frac{4 \times 100}{60}=6.67 \mathrm{~F}$
$=6.43 \times 10^{5} \mathrm{C}$