On passing $0.1 \ F$ of electricity through aluminium chloride,the amount of aluminium metal deposited on the cathode is $(Al = 27)$ ............ $g$.

The relation between Faraday constant $(F)$,chemical equivalent $(E)$,and electrochemical equivalent $(Z)$ is

Calculate the current (in $mA$) required to deposit $0.195 \ g$ of platinum metal in $5.0 \ hours$ from a solution of $[PtCl_6]^{2-}$ : (atomic weight : $Pt = 195$)

Three faradays of electricity are passed through molten $Al_2O_3$,aqueous solution of $CuSO_4$ and molten $NaCl$ taken in different electrolytic cells. The amount of $Al$,$Cu$ and $Na$ deposited at the cathodes will be in the ratio of

When $10 \,A$ current is passed for $80 \,min$, the volume of hydrogen gas liberated at $STP$ is: (in $\,L$)

When a current of $10800 \ C$ is passed through an electrolyte,$2.977 \ g$ of a metal is deposited. If the molar mass of the metal is $106.4 \ g \ mol^{-1}$,what is the charge on the metal cation?