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

One litre solution of $MgCl_2$ is electrolyzed completely by passing a current of $1 \ A$ for $16 \ min \ 5 \ sec$. The original concentration of $MgCl_2$ solution was (Atomic mass of $Mg = 24$)

When $0.1 \ mol$ of $MnO_4^{2-}$ is oxidized,the quantity of electricity required to completely oxidize $MnO_4^{2-}$ to $MnO_4^-$ is $........ \ C$.

On passing a current through molten $KCl$,$19.5 \ g$ of potassium is deposited. If the same quantity of electricity is passed through molten aluminium chloride,then the amount of aluminium deposited will be ............. $g$.

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

What is the total charge of one mole of electrons?