The quantity of electricity in Faraday needed to reduce $1 \ mol$ of $Cr_{2}O_{7}^{2-}$ to $Cr^{3+}$ is ....

The density of $Cu$ is $8.94 \, g \, cm^{-3}$. The quantity of electricity needed to plate an area $10 \, cm \times 10 \, cm$ to a thickness of $10^{-2} \, cm$ using $CuSO_4$ solution would be,if atomic mass of $Cu$ is $63.5$ .................. $C$

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

From the solution of which of the following will one Faraday of electricity liberate one gram atom of metal?

The number of moles of electrons required to deposit $1 \, g$ equivalent of aluminium $(At. \, wt. = 27)$ from a solution of aluminium chloride will be

$7.5 \ A$ current is passed for $200 \ s$ through $AgNO_3$ solution. If experimentally $1.08 \ g$ of $Ag$ is obtained,then calculate the current efficiency (cell capacity). $[Ag = 108 \ u]$