What is Faraday's Law in Electrochemistry?

Faraday's law:


'The amount of any substance deposited or dissolved during electrolysis is proportional to the quantity of electric charge passed through and to the equivalent weight of the substance to be deposited or dissolved'


  Where m=mass of substance deposited or dissolved
                                    Q = total electric charge passed through
                                    F = Faraday's constant = 96485 C mol⁻¹
                                                            M = Molar mass of the substance
                                    Z = Valency number  

Further, Q=It; where I= Electric Current, t=total time of electrolysis



Note that The equivalent weight of a substance is actually equal to its molar mass (M) divided by the change in oxidation state it undergoes upon electrolysis process. It is usually equal to its charge or valence.