Electrolytic Cell
An electrochemical cell in which an external electrical supply drives a non-spontaneous redox reaction.
Formula / equation
E°cell < 0
Unit
V
In depth
The applied voltage must exceed the decomposition potential of the electrolyte before any sustained current flows. Electrode polarity is reversed relative to a galvanic cell: the anode is positive and the cathode negative, though oxidation and reduction still occur at the same-named electrodes.
Examples in the real world
Electrolysis of water into hydrogen and oxygen; the Hall–Héroult cell producing aluminium.