Faraday's law for electrolysis discovered by Michael Faraday 1834:

• The mass of a substance produced at an electrode during electrolysis is proportional to the number of moles of electrons (the quantity of electricity) transferred at that electrode
• The number of Faradays of electric charge required to discharge one mole of substance at an electrode is equal to the number of "excess" elementary charges on that ion

n = amount of substance (mols)

m = mass (grams)

M = molecular weight (grams per mol)

z = number of "excess" elementary charges

I = current (ampere)

t = time (seconds)

F = Faraday constant (96500 C/mol)