Calculate the amount of electricity required in coulombs to convert $0.08 \ mol$ of $MnO_4^{-}$ to $Mn^{2+}$. (in $C$)

Two Faraday of electricity is passed through a solution of $CuSO_4$. The mass of copper deposited at the cathode is ......... $g$. (at. mass of $Cu = 63.5 \ amu$)

Calculate the mass of $Ca$ deposited at the cathode by passing $0.8 \ A$ current through molten $CaCl_2$ for $60 \ minutes$. [Molar mass of $Ca = 40 \ g \ mol^{-1}$] (in $g$)

Cells $A$ and $B$ contain aqueous solutions of ferrous chloride $(FeCl_2)$ and ferric chloride $(FeCl_3)$ respectively. If the same quantity of electricity is passed through both cells, what is the ratio of the mass of iron deposited in cell $A$ to that in cell $B$?

One Faraday of electricity liberates $x \times 10^{-1}$ gram atom of copper from copper sulphate,$x$ is . . . . . . .

The amount of ion discharged during electrolysis is not directly proportional to