When a current of $2 \ A$ is passed through a molten salt of a metal for $5 \ hours$,$22.2 \ g$ of the metal (atomic mass $= 177$) is deposited at the cathode. What is the oxidation state of the metal in the molten salt?

Aluminium oxide may be electrolysed at $1000 \, ^\circ C$ to furnish aluminium metal (At. Mass $= 27 \, amu$; $1 \, F = 96,500 \, C$). The cathode reaction is $Al^{3+} + 3e^- \to Al^0$. To prepare $5.12 \, kg$ of aluminium metal by this method would require:

Silver is removed electrically from $200 \ mL$ of a $0.1 \ N$ solution of $AgNO_3$ by a current of $0.1 \ A$. How long will it take to remove half of the silver from the solution? $(F = 96500 \ C \ mol^{-1})$

Silver plating is done on a silver cup by passing a current of $965 \ A$ for $1 \ s$. How many grams of $Ag$ are deposited? $(Ag = 107.87 \ g/mol)$

The amount of copper metal deposited at cathode on passing electric current of $500 \ mA$ for $20 \ min$ in cupric chloride solution is ............ $g$

Clarify the stoichiometry of the reactions occurring on the electrodes of an electrolytic cell and its relationship with the quantity of electricity.