**Michael Faraday **was the first scientist who described the quantitative aspects of electrolysis. Faraday published his results during 1833-34 in the form of the following well known Faraday’s **two laws of electrolysis.**

## Laws Of Electrolysis

**First Law:**The amount of chemical reaction which occurs at any electrode during electrolysis by a current is proportional to the quantity of electricity passed through the electrolyte (solution or melt).**Second Law:**The amounts of different substances liberated by the same quantity of electricity passing through the electrolytic solution are proportional to their chemical equivalent weights (Atomic Mass of Metal ÷ Number of electrons required to reduce the cation).

- There were no constant current sources available during Faraday’s times.
- The general practice was to put a coulometer (a standard electrolytic cell) for determining the quantity of electricity passed from the amount of metal (generally silver or copper) deposited or consumed.
- Coulometers are now obsolete and we now have constant current (
*I*) sources available and the quantity of electricity*Q*, passed is given by

Q = It

Q is in coulombs when I is in ampere and t is in second

- The amount of electricity (or charge) required for oxidation or reduction depends on the stoichiometry of the electrode reaction.
- We know that charge on one electron is equal to 1.6021 x 10
^{-19 }C. - Therefore, the charge on one mole of electrons is equal to N
_{A}x 1.6021 x 10^{-19}

C = 6.02 x 10^{23} mol^{-1} x 1.6021 x 10^{-19} = 96487 C mol^{-1}

- This quantity of electricity is called Faraday and is represented by the symbol F.