When an electric current is passed through acidified water,$112 \ mL$ of hydrogen gas at $N.T.P.$ was collected at the cathode in $965 \ seconds$. The current passed,in ampere,is

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

The quantity of electricity required for the complete electrolysis of $2 \ mol$ of $Na^{+}$ is = ....... Coulombs.

On passing $1 \ F$ of electricity through electrolytic cells containing $Ag^{+}$,$Ni^{2+}$,and $Cr^{3+}$ ions,the mass of $Ag$ $(At. wt. = 108)$,$Ni$ $(At. wt. = 59)$,and $Cr$ $(At. wt. = 52)$ deposited is:

Calculate the volume of $O_2$ gas liberated at the anode when a current of $2.5 \ A$ is passed for $1 \ hour$ through an aqueous solution of $Na_2SO_4$ using inert electrodes at $1 \ bar$ pressure and $300 \ K$ temperature. (Assume $1 \ mole$ of gas occupies $24.6 \ L$ at $1 \ bar$ and $300 \ K$) (in $mL$)

In the electrolysis of $AgNO_3$,the mass of $Ag$ deposited is plotted against the charge. Slope of the line gives