Electrolysis

About Electrolysis

Electrolysis uses electrical energy to drive non-spontaneous chemical reactions. An external power source forces electrons to flow in the opposite direction to a galvanic cell. Cations migrate to the cathode where they are reduced, and anions migrate to the anode where they are oxidised.

The products of electrolysis depend on the electrolyte and electrode material. With inert electrodes, the ions in solution are discharged. With reactive electrodes (like copper), the anode itself may dissolve. The amount of substance deposited or liberated is governed by Faraday's laws of electrolysis: m = MIt/nF, where M is molar mass, I is current, t is time, n is electron transfer, and F is Faraday's constant (96485 C/mol).