When a current of $2 \ A$ is passed through a molten tin salt for $5 \ hours$,$22.2 \ g$ of tin is deposited. What is the oxidation state of tin in the salt? (Atomic weight of $Sn = 118.69$)

Potassium chlorate is prepared by electrolysis of $KCl$ in basic solution as shown by the following equation:
$6 OH^{-} + Cl^{-} \rightarrow ClO_{3}^{-} + 3 H_{2}O + 6 e^{-}$
$A$ current of $x \ A$ has to be passed for $10 \ h$ to produce $10.0 \ g$ of potassium chlorate. The value of $x$ is $.......$ (Nearest integer).
(Molar mass of $KClO_{3} = 122.6 \ g \ mol^{-1}, F = 96500 \ C \ mol^{-1}$)

The atomic weight of $Al$ is $27$. When a current of $5$ Faradays is passed through a solution of $Al^{3+}$ ions,the weight of $Al$ deposited is ............ $g$.

When an electric current is passed through a silver nitrate solution using silver electrodes,$10.79 \ g$ of silver is deposited. If the same amount of electric current is passed through a copper sulfate solution using copper electrodes,how many grams of copper will be deposited at the cathode (in $g$)?

$18.4 \, A$ current is passed for $1$ hour and $42$ minutes through $CuSO_4$ solution using graphite electrodes at $298 \, K$ temperature and $1 \, bar$ pressure. If the cell efficiency is $75 \%$,calculate the mass of $Cu$ deposited and the volume of $O_2$ gas evolved at $STP$. $[Cu = 63.5 \, u, O = 16 \, u, R = 0.08314 \, L \, bar \, K^{-1} \, mol^{-1}]$

How much time is required for the complete decomposition of $2 \ mol$ of $H_2O$ using a current of $4 \ A$?