Electrochemical_series

Standard electrode potential (data page)

Standard electrode potential (data page)

Data values of standard electrode potential

The data below tabulates standard electrode potentials (E°), in volts relative to the standard hydrogen electrode, at:

Main article: Standard electrode potential

The Nernst equation adjusts for general concentrations, pressures, or temperatures.

Simultaneous half-reactions do not in general add voltages, but instead add Gibbs free energy change: the product of the voltage and the number of electrons transferred, typically the Faraday constant. For example, from Fe2+ + 2 e− ⇌ Fe(s) (–0.44 V), the energy to create one neutral atom of Fe(s) from one Fe2+ ion and two electrons is 2 × 0.44 eV = 0.88 eV, or 84 895 J/(mol  e−). That value is also the standard formation energy for an Fe2+ ion, since  e− and Fe(s) both have zero formation energy.

Data from different sources may cause table inconsistencies. For example:

Additivity of Gibbs energy implies

not the experimental 0.159 V.

Table of standard electrode potentials

Legend: (s) – solid; (l) – liquid; (g) – gas; (aq) – aqueous (default for all charged species); (Hg) – amalgam; bold – water electrolysis equations.

More information Element, Half-reaction ...

See also

Notes

  1. [N 1]
    Not specified in the indicated reference, but assumed due to the difference between the value −0.454 and that computed by (2×(−0.499) + (−0.508))/3 = −0.502, exactly matching the difference between the values for white (−0.063) and red (−0.111) phosphorus in equilibrium with PH3.

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