In order to completely oxidize `0.1 mol` of `MnO_(4)^(2-)` to permanganate ion. The quantity of electricity required is

In an electrolytic cell, one litre of a 1 M aqueous solution of MnO_(4)^(-) is reduced at the cathode the quantity of electricity required so that the final solution is 0.1M MnO_(4)^(2-) will be

Number of coulombs of current required to convert completely 1 mole of MnO_(4)^(-) ions in acid medium to one mole of Mn^(2+) ions electrolytically is

Consider the following reaction MnO_4^(-) + 8 H^(+) 5e^(-) to Mn^(2+) + 4H_2 O , E^@ = 1.51 V . The quantity of electricity required in Faraday to reduce five moles of MnO_4^- is _____________ .

In a neutral medium, 1 mol of MnO_(4)^(2-) ion undergoes disproportionation to form -