Latimer diagram

In a Latimer diagram, because by convention redox reactions are shown in the direction of reduction (gain of electrons), the most highly oxidized form of the element is on the left side, with successively lower oxidation states to the right side.

For example, for oxygen, the species would be in the order O2 (0), H2O2 (–1), H2O (-2): The arrow between O2 and H2O2 has a value +0.68 V over it, it indicates that the standard electrode potential for the reaction: is 0.68 volts.

The easiest way to proceed is simply to use energies (nE) directly expressed in electron-volt (eV), because the Faraday constant F and the sign minus simplifies on both side of the equation.

So, the values of E in volt must be simply multiplied by the number (n) of electron transferred in the considered half-reaction.

Since the Faraday constant can disappear from the equation, no need to calculate ΔrGo expressed in joule.