When $9.65 \ C$ of electricity is passed through a solution of silver nitrate (atomic weight of $Ag = 108$),the amount of silver deposited is $............ \ mg$.

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

How long will it take to produce $5.4 \ g$ of $Ag$ from molten $AgCl$ by passing $5 \ A$ current (in $s$)? (Molar mass $Ag = 108 \ g \ mol^{-1}$)

Consider the following reaction:
$MnO_4^- + 8H^{+} + 5e^- \rightarrow Mn^{2+} + 4H_2O$,$E^\circ = 1.51 \ V$
The quantity of electricity required in Faraday to reduce five moles of $MnO_4^-$ is ..... .

When $1 \ F$ (Faraday) of electricity is passed through an aqueous solution of $CuSO_4$,the amount of $Cu$ deposited is:

Electrolysis of dilute aqueous $NaCl$ solution was carried out by passing $10 \ mA$ current. The time required to liberate $0.01 \ mol$ of $H_2$ gas at the cathode is $(1 \ F = 96500 \ C \ mol^{-1})$