One Faraday of electricity when passed through a solution of copper sulphate deposits:

How much electricity is required to deposit $108 \ g$ of silver from a silver nitrate solution?

$10 \, A$ current is passed through $CuSO_4$ solution for $193 \, \text{minutes}$ at $1 \, \text{bar}$ pressure and $300 \, K$ temperature. If the cell has $80 \%$ efficiency,find the weight of $Cu$ deposited and the volume of $O_2$ evolved. $[Cu = 63.5 \, u, R = 0.08314 \, \text{L bar K}^{-1} \text{mol}^{-1}]$

One litre solution of $MgCl_2$ is electrolyzed completely by passing a current of $1 \ A$ for $16 \ min \ 5 \ sec$. The original concentration of $MgCl_2$ solution was (Atomic mass of $Mg = 24$)

The quantity of electricity required to liberate $112 \, cm^3$ of hydrogen at $STP$ from acidified water is

When $9.65 \ A$ current was passed for $1.0 \ h$ into nitrobenzene in an acidic medium,the amount of $p$-aminophenol produced is .............. $g$.