An electric current is passed through a silver voltameter connected to a water voltameter. The cathode of the silver voltameter weighed $0.108 \ g$ more at the end of the electrolysis. The volume of oxygen evolved at $STP$ is ............... $cm^{3}$.

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

The quantity of electricity needed to separately electrolyze $1 \ M$ solution of $ZnSO_{4}$, $AlCl_{3}$ and $AgNO_{3}$ completely is in the ratio of

Two electrolytic cells,one containing acidified ferrous chloride $(FeCl_2)$ and the other containing acidic ferric chloride $(FeCl_3)$,are connected in series. When an electric current is passed through the cells,what is the ratio of iron deposited at the cathodes in the two cells?

Charge required to liberate $11.5 \ g$ of sodium is:

During the electrolysis of a solution of $AgNO_3$,$9650 \ C$ of charge passes through the electroplating bath. The mass of silver deposited at the cathode will be .............. $g$.