The quantity of charge required to obtain $2$ moles of aluminium from $Al_2O_3$ is: (in $F$)

The anodic half-cell of a lead-acid battery is recharged using electricity of $0.05 \ F$. The amount of $PbSO_4$ electrolyzed in $g$ during the process is (Molar mass of $PbSO_4 = 303 \ g \ mol^{-1}$)

How many atoms of calcium will be deposited from molten $CaCl_2$ by a current of $25 \, mA$ flowing for $60 \, s$?

Calculate the quantity of electricity required to liberate $0.1 \ mole$ of chlorine gas during electrolysis of molten sodium chloride. (in $C$)

Copper sulphate solution is electrolysed between two platinum electrodes. $A$ current is passed until $1.6 \ g$ of oxygen is liberated at the anode. The amount of copper deposited at the cathode during the same period is .............. $g$ [At. mass of $Cu = 63.6$]

How many seconds of current at $241.25 \ A$ must be passed to deposit all the silver present in $125 \ mL$ of $1 \ M \ AgNO_3$ solution? $(1 \ F = 96500 \ C)$