How much charge is required for the following reduction: 1 mole of $Mn{ O }_{ 4 }^{ - }$ to ${{Mn}^{2+}}$

cbse
electrochemistry

#1

The charge on manganese is + 7 in $Mn{ O }_{ 4 }^{ - }$ to ${{Mn}^{2+}}$ The chemical reaction involved is

${{Mn}^{7+}}$+ ${{5e}^{-}}$ --------> ${{Mn}^{2+}}$

Therefore, to convert 1 mole of $Mn{ O }_{ 4 }^{ - }$ to ${{Mn}^{2+}}$ ions, 5 F electricity is required. The amount of charge is therefore,
5 x 96500 C = 482500 C.