One Faraday of electricity when passed through a solution of copper sulphate deposits:

When electricity is passed through the solution of $AlCl_3$,$13.5 \ g$ of $Al$ are deposited. The number of Faraday required is:

If nearly $10^5 \ C$ liberate $1 \ gm$ equivalent of aluminium,then the amount of aluminium (equivalent weight $9$) deposited through electrolysis in $20 \ minutes$ by a current of $50 \ A$ will be .............. $gm$.

Which equation represents Faraday's first law of electrolysis? ($m \rightarrow$ mass,$c \rightarrow$ current,$t \rightarrow$ time,$z \rightarrow$ electrochemical equivalent)

On passing a current of $1.2 \ A$ through a solution of salt of copper for $40 \ min$,$0.96 \ g$ of copper was deposited. The equivalent weight of copper in $g$ is

Calculate the quantity of electricity required to produce $0.42 \ g$ of $Ag$ at the cathode during the electrolysis of an $AgNO_3$ solution. (Molar mass of $Ag = 108 \ g \ mol^{-1}$) (in $C$)