Faraday:

The quantity of electricity carried by one mole of electrons is called Faraday and is given by the symbol, F.  A charge of an electron is l.6022 × l0^-19. Therefore the charge on one mole of electrons would be

1.6022 × l0^-19 × 6.022 × l0²³ C or   96485C

Therefore one Faraday = 96485 C or approximately 96,500C.

Now consider a reaction,

Mn⁺ + ne ? M

The quantity of electricity required for the deposition of 1 mole of a component will be equal to nF, here n is the number of moles of electrons required for the reaction. Now let M_r be the relative atomic mass of one mole atom of an element. Therefore, for the deposition of M_r g (or 1 mole) of the element, we require nF or n × 96,500 C of electricity.

m =     (M_r Q /96500 n) g

While m = mass of an element deposited through the passage of Q coulomb of current or

m = (M_r × I × t)/95600 n

This equation is meaningful in calculating the mass of an element deposited through the passage of known quantity of current.