When a current of $10 \ A$ is passed through molten $AlCl_{3}$ for $1.608 \ minutes$,the mass of $Al$ deposited will be [Atomic mass of $Al = 27 \ g/mol$]:- (in $g$)

Calculate the quantity of electricity required to liberate $0.224 \ dm^3$ of chlorine at $STP$ during the electrolysis of fused sodium chloride (in $C$)?

$A$ solution of $CuSO_4$ is electrolysed using a current of $1.5 \ A$ for $10 \ minutes$. What mass of $Cu$ is deposited at the cathode (in $g$)? (Atomic mass of $Cu = 63.7$)

The number of moles of electrons passed when a current of $2 \ A$ is passed through a solution of electrolyte for $20 \ minutes$ is

Charge required to liberate $11.5 \ g$ of sodium is:

The electrolytic cells,one containing acidified ferrous chloride and another acidified ferric chloride,are connected in series. The ratio of iron deposited at the cathodes in the two cells when electricity is passed through the cells will be: