How much electricity is required in Faraday to produce $40.0 \ g$ of $Al$ from molten $Al_2O_3$? (Atomic mass of $Al = 27 \ g \ mol^{-1}$)

$5 \ A$ current is passed through $AgNO_3$ solution for $193 \ s$. If $0.972 \ g$ of $Ag$ is deposited,calculate the current efficiency (cell capacity) of the electrolytic cell. $[Ag = 108 \ u]$ (in $\%$)

How much time (in $sec$) is required to coat a metal surface of $80 \, cm^2$ with a $0.005 \, mm$ thick layer of silver from a silver nitrate solution using a current of $3 \, A$? (Density of silver $= 10.5 \, g \, cm^{-3}$)

The number of coulombs required for the deposition of $107.870 \ g$ of silver is

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

On passing a current through $KCl$ solution,$19.5 \ g$ of potassium is deposited. If the same quantity of electricity is passed through a solution of aluminium chloride,the amount of aluminium deposited is ............ $g$