During the electrolysis of molten sodium chloride,the time required to produce $0.10 \ mol$ of chlorine gas using a current of $3 \ A$ is .......... $\min.$

Three electrolytic cells $A, B, C$ containing solutions of $ZnSO_{4}, AgNO_{3}$ and $CuSO_{4}$ respectively are connected in series. $A$ steady current of $1.5 \ A$ was passed through them until $1.45 \ g$ of silver deposited at the cathode of cell $B$. How long did the current flow? What mass of copper and zinc were deposited?

The quantity of electricity (in $C$) required to oxidize $1 \ mol$ of $H_2O$ to $O_2$ is approximately ..................... $\times 10^5 \ C$.

The number of coulombs required for the deposition of $107.870 \ g$ of silver is

The electrochemical equivalent of a metal is $x \ g \ C^{-1}$. The equivalent weight of the metal is:

If the electrochemical equivalent of a substance is $0.0006735 \ g/C$,what is its equivalent weight?