The data below tabulates standard electrode potentials (E°), in volts relative to the standard hydrogen electrode (SHE), at:
Temperature 298.15 K (25.00 °C; 77.00 °F); Effective concentration (activity) 1 mol/dm3 for each aqueous or amalgamated (mercury-alloyed) species; Unit activity for each solvent and pure solid or liquid species; and Absolute partial pressure 101.325 kPa (1.00000 atm; 1.01325 bar) for each gaseous reagent — the convention in most literature data but not the current standard state (100 kPa (0.99 atm; 1.0 bar)). Variations from these ideal conditions affect measured voltage via the Nernst equation.
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.
See also Galvanic series lists electrode potentials in saltwater Standard apparent reduction potentials in biochemistry at pH 7 Reactivity series#Comparison with standard electrode potentials
Notes
References
External links Chemistry LibreTexts (2021-04-26). "P1: Standard Reduction Potentials by Element". Chemistry LibreTexts. Retrieved 2021-11-30. California State University, Northridge (CSUN). "Standard Reduction Potentials" (PDF). csun.edu. Archived (PDF) from the original on 2017-12-15. Retrieved 2021-11-30. Wardman, Peter (1989). "Reduction potentials of one-electron couples involving free radicals in aqueous solution" (PDF). srd.nist.gov. p. 1637. Bibcode:1989JPCRD..18.1637W. doi:10.1063/1.555843. Archived (PDF) from the original on 2022-10-09. Retrieved 2021-11-30. http://www.jesuitnola.org/upload/clark/Refs/red_pot.htm Archived 2008-07-20 at the Wayback Machine https://web.archive.org/web/20150924015049/http://www.fptl.ru/biblioteka/spravo4niki/handbook-of-Chemistry-and-Physics.pdf http://hyperphysics.phy-astr.gsu.edu/Hbase/tables/electpot.html#c1