When an electric current is passed through a solution of $KCl$,$19.5 \ g$ of potassium (atomic mass $= 39$) is deposited. If the same amount of electric current is passed through a solution of $AlCl_3$,how many grams of aluminum will be liberated?

How much charge is required for the deposition of $1$ equivalent of a substance?

The quantity of electricity required for the complete electrolysis of $2 \ mol$ of $Na^{+}$ is = ....... Coulombs.

$A$ 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 $.7$)

The density and equivalent weight of a metal are $10.5\, g\, cm^{-3}$ and $100$,respectively. The time required for a current of $3\, A$ to deposit a $0.005\, mm$ thick layer of the same metal on an area of $80\, cm^2$ is closest to $....\, s$

Electrolytic cells containing $Zn$ and $Al$ salt solutions are connected in series. If $6.5 \ g$ of $Zn$ is deposited in one cell,calculate the mass of $Al$ deposited in the second cell (molar mass: $Zn=65 \ g \ mol^{-1}$,$Al=27 \ g \ mol^{-1}$) by passing a definite quantity of electricity. (in $g$)