Which is the weight of $Al$ deposited at cathode when $1 \ A$ current is passed through molten $AlCl_3$ for $9650 \ s$ (in $g$)?
(Atomic mass of $Al = 27$)

The amount of metal deposited at the cathode on passing an electric current of $0.75 \ A$ in an aqueous ferric sulphate solution for $30 \ min$ will be - ........... $g$ (atomic weight of $Fe = 56$).

The electric charge required for the electrolytic decomposition of one gram equivalent of a substance is

$A$ metal surface of $100 \, cm^2$ area has to be coated with a nickel layer of thickness $0.001 \, mm$. $A$ current of $2 \, A$ was passed through a solution of $Ni(NO_3)_2$ for '$x$' seconds to coat the desired layer. The value of $x$ is $.........$. (Nearest integer)
($\rho_{Ni}$ (density of Nickel) is $10 \, g \cdot cm^{-3}$,Molar mass of Nickel is $60 \, g \cdot mol^{-1}$,$F = 96500 \, C \cdot mol^{-1}$)

$A$ current of $0.4 \ A$ is passed through excess of molten $MgCl_2$ for $9.65 \times 10^4 \ sec$. The mass of $Mg$ deposited at the cathode is .............. $gm$

According to Faraday's laws of electrolysis,the amount of decomposition is proportional to