The quantity of electricity in Faraday needed to reduce $1 \ mol$ of $Cr_{2}O_{7}^{2-}$ to $Cr^{3+}$ is ....

The mass deposited at an electrode during electrolysis is directly proportional to which of the following?

What volume of chlorine gas (molar mass $71 \ g \ mol^{-1}$) is evolved at $STP$ during electrolysis of fused $NaCl$ by passage of $1 \ A$ current for $965 \ s$ (in $L$)? (At $STP$,$V_m = 22.4 \ dm^3 \ mol^{-1}$)

$A$ solution of copper sulphate $(CuSO_4)$ is electrolysed for $10 \, \text{minutes}$ with a current of $1.5 \, \text{amperes}$. The mass of copper deposited at the cathode (atomic mass of $Cu = 63 \, u$) is ............ $g$.

$CuSO_4$ solution is electrolysed for $15 \ minutes$ to deposit $0.4725 \ g$ of copper at the cathode. The current in amperes required is (Faraday $= 96,500 \ C \ mol^{-1}$,atomic weight of copper $= 63$)

Faraday's laws of electrolysis are related to