The quantity of electricity needed to liberate $0.5 \ g$ equivalent of an element is

$A$ metal plate of dimension $(1 \times 2 \ cm^2)$ has to be coated on both sides by $Cu$ metal. How long does it take to deposit $Cu$ of $0.01 \ cm$ thickness,if $1.5 \ A$ current is used (in $s$)? [Electrochemical equivalence of $Cu$ is $0.0003 \ g/C$ and the density of $Cu$ is $9 \ g/cm^3$]

The required charge for one equivalent weight of silver deposited on cathode is

The amount of $Ag$ (atomic mass $= 108$) deposited at the cathode when a current of $0.5 \, A$ is passed through a solution of $AgNO_3$ for $1 \, h$ is closest to $... \, g$.

On passing electric current through molten aluminium chloride,$11.2 \ L$ of $Cl_2$ is liberated at $NTP$ at the anode. The quantity of aluminium deposited at the cathode is .............. $g$ (atomic weight of $Al = 27$).

Two electrolytic cells containing molten solutions of nickel chloride and aluminium chloride are connected in series. If the same amount of electric current is passed through them,what will be the weight of nickel obtained when $18 \ g$ of aluminium is obtained (in $g$)? $[Al = 27 \ g/mol, Ni = 58.5 \ g/mol]$