When $0.1 \ mol$ of $MnO_4^{2-}$ is oxidized,the quantity of electricity required to completely oxidize $MnO_4^{2-}$ to $MnO_4^-$ is $........ \ C$.

$A$ current of $0.01 \ A$ is passed through a solution of a metal bromide $(MBr_x)$. The only reaction at the cathode is the deposition of metal $(M)$. After $3 \ hours$,$0.072 \ g$ of metal $(M)$ is deposited. The value of '$x$' is approximately (Given: Atomic weight of $M = 192$)

If a current of $5 \ A$ is passed through a zinc sulfate solution for $40 \ \text{minutes}$,what is the mass of zinc deposited at the cathode (in $g$)?

$A$ current of $0.25 \, A$ is passed through $CuSO_4$ solution placed in a voltameter for $45 \, minutes$. The amount of $Cu$ deposited on the cathode is ............. $g$ $(At. \, weight \, of \, Cu = 63.6)$.

On passing $C$ ampere of electricity through an electrolyte solution for $t$ seconds,$m$ grams of metal are deposited on the cathode. The equivalent weight $E$ of the metal is:

Which of the following aqueous solutions will result in the maximum number of moles of metal deposited on passing the same amount of charge?