Electrode potential,\xa0E, in chemistry or\xa0electrochemistry, according to a\xa0IUPAC\xa0definition,[1]\xa0is the\xa0electromotive force\xa0of acell\xa0built of two\xa0electrodes:\ton the left-hand side is the\xa0standard hydrogen electrode, and\ton the right-hand side is the electrode the potential of which is being defined.By\xa0convention:

\t

ECell\xa0=\xa0ECathode\xa0−\xa0EAnode

From the above, for the cell with the\xa0standard hydrogen electrode\xa0(potential of 0 by convention), one obtains:

\t

ECell\xa0=\xa0ERight\xa0− 0 =\xa0EElectrode

The left-right convention is consistent with the international agreement that redox potentials be given for reactions written in the form of reduction half-reactions.Electrode potential is measured in\xa0volts\xa0(V).
Electrode potential is defined as the potential of a cell consisting of the electrode in question acting as a cathode and the standard hydrogen electrode acting as an anode. Reduction always takes place at the cathode, and oxidation at the anode.