The quantity of electricity required to liberate $5600 \ mL$ of $H_2$ at $STP$ is the same as that required to liberate how many grams of silver (equivalent weight = $108$)?

How many coulombs are required for the oxidation of $2 \, mol$ of $H_2O_2$ to $O_2$?

The number of moles of electrons passed when a current of $2 \ A$ is passed through a solution of electrolyte for $20 \ minutes$ is

Three faradays of electricity are passed through molten $Al_2O_3$,aqueous solution of $CuSO_4$ and molten $NaCl$ taken in different electrolytic cells. The amount of $Al$,$Cu$ and $Na$ deposited at the cathodes will be in the ratio of

The electrochemical equivalent of magnesium is $0.126 \ mg/C$. $A$ current of $5 \ A$ is passed in a suitable solution for $1 \ hour$. The mass of magnesium deposited will be ........... $gm$.

When $1 \ F$ (Faraday) of electricity is passed through an aqueous solution of $CuSO_4$,the amount of $Cu$ deposited is: