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)