Faraday's law of electrolysis
|
|
Faraday's law of electrolyses 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
- <math>n = \frac{m}{M} = \frac{It}{zF}<math>
- <math>n =<math> amount of substance (mols)
- <math>m =<math> mass (grams)
- <math>M =<math> molecular weight (grams per mol)
- <math>z =<math> number of "excess" elementary charges
- <math>I =<math> current (ampere)
- <math>t =<math> time (seconds)
- <math>F =<math> Faraday constant (96500 C/mol)