Question

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

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

Answer 1

The correct option is C $9650C$

The oxidation reaction is as shown below.
$Mn{O}_4^{2-}+e^{-}\to Mn{O}_4^{-}$

Oxidation of one mole of $Mn{O}_4^{2-}$ requires 1 mole of electrons.

Hence, the oxidation of 0.1 mole of electrons will require 0.1 mole of electrons.
This corresponds to $96500\times 0.1=9650C$.