The quantity of electricity required for the complete electrolysis of $2 \ mol$ of $Na^{+}$ is = ....... Coulombs.

$A$ metal plate of dimension $(1 \times 2 \ cm^2)$ has to be coated on both sides by $Cu$ metal. How long does it take to deposit $Cu$ of $0.01 \ cm$ thickness,if $1.5 \ A$ current is used (in $s$)? [Electrochemical equivalence of $Cu$ is $0.0003 \ g/C$ and the density of $Cu$ is $9 \ g/cm^3$]

Faraday's laws of electrolysis state that the mass deposited on an electrode is proportional to:

The chemical equivalent of silver is $108$. If the current in a silver voltameter is $2 \ A$,the time required to deposit $27 \ g$ of silver will be ............ $hrs$.

When a current of $0.6 \ A$ is passed through an aqueous solution of $CuSO_4$ for $7 \ minutes$,what is the total quantity of electricity passed in Faradays?

What is the number of moles of electrons passed when a current of $2 \text{ A}$ flows through a solution of an electrolyte for $10 \text{ minutes}$?