The number of $Faradays$ needed to reduce $4 \ g$ equivalents of $Cu^{++}$ to $Cu$ metal will be:

$A$ current $I$ is passed for a time $t$ through a number of voltameters. If $m$ is the mass of a substance deposited on an electrode and $z$ is its electrochemical equivalent,then

If $1$ mole of electrons is passed through the solutions of $AlCl_3$,$AgNO_3$,and $MgSO_4$,in what ratio will $Al$,$Ag$,and $Mg$ be deposited at the electrodes?

The amount of silver deposited on passing $2 \ F$ of electricity through an aqueous solution of $AgNO_3$ is: (in $g$)

The amount of substance liberated on electrodes during electrolysis when $1 \ C$ of electricity is passed,is

What is the nature of the Faraday constant?