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Faraday's 1^st Law of Electrolysis:

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.

Faraday's 2^nd Law of Electrolysis:

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.

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$m\; =\; cdot\; =\; cdot\; =\; cdot$

m is the mass of the substance produced at the electrode (in grams),

Q is the total electric charge that passed through the solution (in coulombs),

q is the electron charge = 1.602 x 10^-19 coulombs per electron,

n is the valence number of the substance as an ion in solution (electrons per ion),

$F\; =\; qN\_A\; =\; 96,485\; mathrm\; cdot\; mathrm$ is Faraday's constant,

M is the molar mass of the substance (in grams per mole), and

N_A is Avogadro's number = 6.022 x 10²³ ions per mole.

$Q\; =\; int\_0^T\; I(t)\; cdot\; dt$

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Electrolysis

Michael Faraday

Faraday constant