The quantity of electricity required to deposit $1$ gram-equivalent of a substance at an electrode is equal to .......

What is achieved by Faraday using the principles of electrolysis?

The electrochemical equivalent of a metal is $3.3 \times 10^{-7} \ kg/C$. The mass of the metal liberated at the cathode when a $3 \ A$ current is passed for $2 \ s$ will be:

$Al_2O_3$ is reduced by electrolysis at low potentials and high currents. If $4.0 \times 10^4$ amperes of current is passed through molten $Al_2O_3$ for $6$ hours,what mass of aluminium is produced? (Assume $100\%$ current efficiency,at. mass of $Al = 27 \ g \ mol^{-1}$).

One gram of metal ion $M^{3+}$ is discharged by the passage of $1.81 \times 10^{23}$ electrons. What is the atomic weight of the metal?

How many coulombs are required for the oxidation of $1 \, mol$ of $H_2O_2$ to $O_2$?