Work out electrolysis (faraday law) instantly with clear inputs, formula shown and shareable results.
Faraday's law ties deposited mass to charge: one mole of electrons is 96,485 C, and each ion needs n of them. So mass = ItM/(nF). Two amps for an hour is 7200 C, which plates 2.37 g of copper from Cu2+ because the divalent ion consumes two electrons per atom.
Faraday's law
mass = (I x t x M) / (n x F)
Charge passed
Q = I x t
Multiply the mass by the current efficiency. Side reactions such as hydrogen evolution consume charge without depositing metal.
Aluminium at n = 3 needs half again as much charge per mole as a divalent metal, which is why aluminium smelting is so energy hungry.