The atomic weight of $Al$ is $27$. When a current of $5$ Faradays is passed through a solution of $Al^{3+}$ ions,the weight of $Al$ deposited is ............ $g$.

What is the quantity of electricity in Faradays required to produce $8 \text{ g}$ of $Mg$ (molar mass = $24 \text{ g mol}^{-1}$) from $MgCl_2$ solution (in $\text{ F}$)?

$A$ certain quantity of electricity is passed through an aqueous solution of $AgNO_3$ and a cupric salt solution connected in series. The amount of $Ag$ deposited is $1.08 \ g$. The amount of copper deposited is ............. $g$ (atomic weight of $Cu = 63.5$; $Ag = 108$).

In a certain electrolysis experiment,$0.650 \ g$ of zinc is deposited in a cell having $ZnSO_4$ solution. Calculate the mass of $Cu$ deposited in another cell having $CuSO_4$ solution arranged in series with the first cell (in $g$)? (Molar mass of $Zn = 65 \ g \ mol^{-1}$,$Cu = 63.5 \ g \ mol^{-1}$)

The time required to remove electrolytically one fourth of $Ag^+$ from $0.2 \ L$ of $0.1 \ M \ AgCl$ solution by a current of $0.1 \ A$ is approximately $.......... \ min$.

Oxidation of succinate ion produces ethylene and carbon dioxide gases. On passing $0.2 \ F$ electricity through an aqueous solution of potassium succinate,the total volume of gases (at both cathode and anode) at $STP$ ($1 \ atm$ and $273 \ K$) is .............. $L$