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Section: 5 | Electrochemical Series |
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John R. Rumble, ed., CRC Handbook of Chemistry and Physics, 103rd Edition (Internet Version 2022), CRC Press/Taylor & Francis, Boca Raton, FL.
If a specific table is cited, use the format: "Physical Constants of Organic Compounds," in CRC Handbook of Chemistry and Physics, 103rd Edition (Internet Version 2022), John R. Rumble, ed., CRC Press/Taylor & Francis, Boca Raton, FL.

ELECTROCHEMICAL SERIES

Petr Vanýsek

There are three tables for the electrochemical series. Each table lists standard reduction potentials, E° values, at 298.15 K (25 °C), and at a pressure of 101.325 kPa (1 atm) (not the standard pressure of 1 bar). The activity of all soluble species is assumed to be 1.000 mol/L. This is particularly important when pH (H+ or OH-) takes part in the equilibrium. Table 1 is an alphabetical listing of the elements and compounds, according to the symbol of the elements. Thus, data for silver (Ag) precede those for aluminum (Al). Table 2 lists only those reduction reactions that have E° values positive with respect to the standard hydrogen electrode. In Table 2, the reactions are listed in the order of increasing positive potential, and they range from 0.0000 V to +3.4 V. Table 3 lists only those reduction potentials that have E° negative with respect to the standard hydrogen electrode. In Table 3, the reactions are listed in the order of decreasing potential and range from 0.0000 V to –4.10 V. The reliability of the potentials is not the same for all the data. Typically, the values with fewer significant figures have lower reliability. The values of reduction potentials, in particular those of less common reactions, are not definite; they are subject to occasional revisions.

Abbreviations: ac = acetate; bipy = 2,2'-dipyridine, or bipyridine; en = ethylenediamine; phen = 1,10-phenanthroline.

References

  1. Milazzo, G., Caroli, S., and Sharma, V. K., Tables of Standard Electrode Potentials, Fourth Edition, Wiley, Chichester, 1978. [https://doi.org/10.1149/1.2131790]
  2. Bard, A. J., Parsons, R., and Jordan, J., Standard Potentials in Aqueous Solutions, Marcel Dekker, New York, 1985.
  3. Bratsch, S. G., J. Phys. Chem. Ref. Data, 18, 1–21, 1989. [https://doi.org/10.1063/1.555839]
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TABLE 1. Electrochemical Series - Alphabetical Listing



ReactionE°/V
Continued on next page...
Ac3+ + 3 e ⇌ Ac-2.20
Ag+ + e ⇌ Ag0.7996
Ag2+ + e ⇌ Ag+1.980
Ag(ac) + e ⇌ Ag + (ac)–0.643
AgBr + e ⇌ Ag + Br–0.07133
AgBrO3 + e ⇌ Ag + BrO3–0.546
Ag2C2O4 + 2 e ⇌ 2 Ag + C2O42–0.4647
AgCl + e ⇌ Ag + Cl–0.22233
AgCN + e ⇌ Ag + CN–-0.017
Ag2CO3 + 2 e ⇌ 2 Ag + CO32–0.47
Ag2CrO4 + 2 e ⇌ 2 Ag + CrO42–0.4470
AgF + e ⇌ Ag + F–0.779
Ag4[Fe(CN)6] + 4 e ⇌ 4 Ag + [Fe(CN)6]4–0.1478
AgI + e ⇌ Ag + I–-0.15224
AgIO3 + e ⇌ Ag + IO3–0.354
Ag2MoO4 + 2 e ⇌ 2 Ag + MoO42–0.4573
AgNO2 + e ⇌ Ag + 2 NO2–0.564
Ag2O + H2O + 2 e ⇌ 2 Ag + 2 OH–0.342
Ag2O3 + H2O + 2 e ⇌ 2 AgO + 2 OH–0.739


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