When a current of $2 \ A$ is passed for $2 \ hours$ through a copper voltameter,$W \ g$ of copper is deposited. If a current of $1 \ A$ is passed for $4 \ hours$ through the same voltameter,how much copper will be deposited?

Calculate the quantity of electricity required to produce $0.42 \ g$ of $Ag$ at the cathode during the electrolysis of an $AgNO_3$ solution. (Molar mass of $Ag = 108 \ g \ mol^{-1}$) (in $C$)

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 the electrolysis of $KCl$ in basic solution:
$6 OH^{-} + Cl^{-} \rightarrow ClO_{3}^{-} + 3 H_{2}O + 6 e^{-}$
If only $60\%$ of the current is utilized in the reaction,the time (rounded to the nearest hour) required to produce $10 \ g$ of $KClO_{3}$ using a current of $2 \ A$ is:
(Given: $F = 96,500 \ C \ mol^{-1}$,molar mass of $KClO_{3} = 122 \ g \ mol^{-1}$)

When a current of $0.1 \, A$ is passed through $200 \, mL$ of a $0.1 \, N$ $AgNO_3$ solution,silver is deposited. How much time in $sec$ is required to remove half of the silver from the solution?

The number of moles of electrons required to deposit $1 \, g$ equivalent of aluminium $(At. \, wt. = 27)$ from a solution of aluminium chloride will be