The mass of zinc produced by the electrolysis of zinc sulphate solution with a steady current of $0.015 \ A$ for $15$ minutes is . . . . . . $ \times 10^{-4} \ g$. (Atomic mass of zinc $= 65.4 \ amu$)

$18.4 \, A$ current is passed for $1$ hour and $42$ minutes through $CuSO_4$ solution using graphite electrodes at $298 \, K$ temperature and $1 \, bar$ pressure. If the cell efficiency is $75 \%$,calculate the mass of $Cu$ deposited and the volume of $O_2$ gas evolved at $STP$. $[Cu = 63.5 \, u, O = 16 \, u, R = 0.08314 \, L \, bar \, K^{-1} \, mol^{-1}]$

What is the number of faraday required to form $1 \ mol \ H_2$ by reduction of $H^{+}$ ions?

If $5 \ A$ of current is passed for $193 \ s$ through a solution containing $Cu$ salt,$0.32 \ g$ of copper is deposited. What is the oxidation state of the $Cu$ in the salt?

To complete the precipitation of $Ag$ from $400 \ mL$ of $0.04 \ M$ $AgNO_3$ solution,how long should a $4.8 \ A$ current be passed?

The $E.C.E.$ of $Cu$ and $Ag$ are $7 \times 10^{-6} \ g/C$ and $1.2 \times 10^{-6} \ g/C$ respectively. If a certain current deposits $14 \ g$ of $Cu$,the amount of $Ag$ deposited is .............. $g$.