When the same quantity of electricity is passed through electrolytic cells containing different electrolytes connected in series,the amount of products obtained at the various electrodes is proportional to their:

The amount of silver deposited on passing $2 \ F$ of electricity through an aqueous solution of $AgNO_3$ is: (in $g$)

How long would it take to reduce completely $80 \ mL$ of $0.1 \ M$ $Fe_2(SO_4)_3$ to $FeSO_4$ by passing a current of $2 \ A$?

$18.4 \, A$ 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 $STP$. $[Cu = 63.5 \, u, O = 16 \, u, R = 0.08314 \, L \, bar \, K^{-1} \, mol^{-1}]$

Calculate the quantity of electricity required to liberate $0.224 \ dm^3$ of chlorine at $STP$ during the electrolysis of fused sodium chloride (in $C$)?

$A$ steady current of $5 \, A$ is maintained for $45 \, min$. During this time,it deposits $4.572 \, g$ of zinc at the cathode of a voltameter. The $E.C.E.$ of zinc is: