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

Calculate the volume of $O_2$ gas liberated at the anode when a current of $2.5 \ A$ is passed for $1 \ hour$ through an aqueous solution of $Na_2SO_4$ using inert electrodes at $1 \ bar$ pressure and $300 \ K$ temperature. (Assume $1 \ mole$ of gas occupies $24.6 \ L$ at $1 \ bar$ and $300 \ K$) (in $mL$)

When the same quantity of electricity is passed through electrolytic cells containing different electrolytes connected in series,the amount of products obtained at the various electrodes is proportional to their:

How many $Faradays$ are required to generate one gram atom of magnesium from $MgCl_2$?

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 $........ \ C$.

The quantity of electricity required to liberate $5600 \ mL$ of $H_2$ at $STP$ is the same as that required to liberate how many grams of silver (equivalent weight = $108$)?