How many faraday of electricity are required to deposit $10 \ g$ of calcium from molten calcium chloride using inert electrodes (in $F$)? (Molar mass of calcium $= 40 \ g \ mol^{-1}$)

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

An electrolytic cell contains a solution of $Ag_{2}SO_{4}$ and has platinum electrodes. $A$ current is passed until $1.6 \ g$ of $O_{2}$ is liberated at the anode. The amount of silver deposited at the cathode would be ............ $g$.

The mass of copper deposited from a solution of $CuSO_4$ by passage of $5 \ A$ current for $965 \ s$ is ............ $g$ (Mol. wt. of Copper $= 63.5$)

How much electricity in terms of Faraday is required to produce $40.0 \text{ g}$ of $\text{Al}$ from molten $\text{Al}_2\text{O}_3$ (in $\text{ F}$)?

$A$ 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: