When 0.1 mol ${MnO}_4^{2-}$ is oxidised the quantity of electricity required to completely oxidise ${MnO}_4^{2-}$ is

Question

When 0.1 mol ${MnO}_4^{2-}$ is oxidised the quantity of electricity required to completely oxidize ${MnO}_4^{2-}$ is

(a) $69500 {C}$

(b) $2 \times 96500 {C}$

(c) $9650 {C}$

(d) $96.50 {C}$

Answer 1

Correct Option : (C)

Explanation—

The oxidation reaction is

$+6$                  $+7 $

${MnO}_4^{2-} \longrightarrow  {MnO}_4^{-}+e^{-}$

$0.1 {mol}$.            ${0.1 {mol}}$

${Q}=0.1 \times {F}=  0.1 \times 96500 {C}=9650 {C}$