The cost of energy required to deposit $1 \ g$ of $Mg$ is $5.00$ rupees. What is the cost to deposit $10 \ g$ of $Al$? (Atomic mass of $Al = 27, Mg = 24$)

If the total electricity required to deposit $1$ mole of a metal $M$ is equal to that of $10.7$ amperes of current for $10$ hours,the equivalent weight of the metal is (atomic weight $= M \ u$):

On passing $3 \ A$ of electricity for $50 \ minutes$,$1.8 \ g$ of metal deposits. The equivalent mass of the metal is:

$10 \, A$ current is passed through $CuSO_4$ solution for $193 \, \text{minutes}$ at $1 \, \text{bar}$ pressure and $300 \, K$ temperature. If the cell has $80 \%$ efficiency,find the weight of $Cu$ deposited and the volume of $O_2$ evolved. $[Cu = 63.5 \, u, R = 0.08314 \, \text{L bar K}^{-1} \text{mol}^{-1}]$

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 $C$)

$A$ current of $15.0 \ A$ is passed through a solution of $CrCl_2$ for $45 \ min$. The volume of $Cl_2$ (in $L$) obtained at the anode at $1 \ atm$ and $273 \ K$ is around ($1 \ F = 96500 \ C \ mol^{-1}$,At. wt. of $Cl=35.5$,$R=0.082 \ L \ atm \ K^{-1} \ mol^{-1}$) (in $.7$)