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

$A$ current of $2 \ A$ passing for $5 \ hours$ through molten tin salt deposited $22.2 \ g$ of tin. The oxidation state of tin in the salt is . . . . . . . (Atomic mass of $Sn = 119$)

How much current should be passed through acidified water for $100 \ s$ to liberate $0.224 \ L$ of $H_2$ gas at $STP$ (in $A$)?

Salts of $A$ (atomic weight $8$),$B$ (atomic weight $18$) and $C$ (atomic weight $50$) were electrolysed under identical conditions using the same quantity of electricity. It was found that $2.4 \ g$ of $A$ was deposited,the weight of $B$ and $C$ deposited are $1.8 \ g$ and $7.5 \ g$ respectively. The valences of $A$,$B$ and $C$ are,respectively,

To gain $1 \ mole$ $Mg$ from $Mg^{2+}$ and $1 \ mole$ $Al$ from $Al^{3+}$,how many Coulombs of electricity are required respectively?

$9.65 \ C$ of electric current is passed through fused anhydrous $MgCl_2$. The magnesium metal thus obtained is completely converted into a Grignard reagent. The number of moles of Grignard reagent obtained is