Question

When 0.1 mol $Mn{O}_4^{2-}$ is oxidised, quantity of electricity required to completely oxidise $Mn{O}_4^{2-}$ to $Mn{O}_4^{-}$ is

• A. 96500 C
• B. 2 $\times$ 96500 C
• C. 9650 C
• D. 96.50 C

Answer 1

The correct option is C 9650 C

The oxidation reaction is
$\underset{0.1mol}{\stackrel{+6}{Mn{O}_4^{2-}}}\to \stackrel{+7}{Mn{O}_4^{-}}+\stackrel{e^{-}}{0.1mol}$
$Q=0.1\times F=0.1\times 96500C=9650C$