$A$ current of $2.0 \ A$ is passed for $5 \ hours$ through a molten metal salt,which deposits $22.2 \ g$ of metal (At. wt. $= 177$). The oxidation state of the metal in the metal salt is:

On passing $0.1 \ F$ of electricity through aluminium chloride,the amount of aluminium metal deposited on the cathode is $(Al = 27)$ ............ $g$.

$A$ $4 \ A$ current is passed through a solution of zinc sulphate for $50 \ min$. Find the amount of zinc deposited at the cathode in $g$.

When electric current is passed through acidified water for $1930 \,s$, $1120 \,mL$ of $H_2$ gas is collected (at $STP$) at the cathode. What is the current passed in amperes?

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 $mL$)

How much electricity in terms of Faraday is required to reduce $2 \ mol$ of $MnO_4^{-}$ into $Mn^{2+}$?