When `0.1 mol MnO_(4)^(2-)` is oxidized the quantity of electricity required to completely oxidize `MnO_(4)^(2-)` to `MnO_(4)^(-)` is

Options

A. `96500 C`
B. `2xx96500C `
C. `9650 C`
D. `96.50 C `

Answer

C

Explanation

( c) `underset((+6))(MnO_(4)^(2-))overset([1" mole "e^(-)=1F])iff underset((+7))(MnO_(4)^(-))`
As per the equation, for 1 mole of `MnO_(4)^(2-)`, 1 F of electricity is required. Thus, for 0.1 mole of `MnO_(4)^(2-)`, 0.1 F of electricity is required,
Since , 1 F = 96500 C
`:. " " 0.1F=0.1xx96500C=9650C`
Hence, 9650 C of electricity is require to completely oxidised `MnO_(4)^(2-) " to " MnO_(4)^(-)`