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Main article: standard electrode potential

The values of standard electrode potentials are given in the table below in volts relative to the standard hydrogen electrode and are assembled from references [1] [2] [3] [4] [5] [6]

The values are for the following conditions:

  • the temperature of 298.15 K (25 °C);
  • the effective concentration of 1 mol/L for each aqueous species or a species in a mercury amalgam;
  • the partial pressure of 101.325 kPa (absolute) (1 atm, 1.01325 bar) for each gaseous reagent. This pressure is used because most literature data are still given for this value rather than for the current standard of 100 kPa.
  • the activity of unity for each pure solid, pure liquid, or for water (solvent).

The table can be sorted alphabetically by clicking on the sort icon in the column heading. Click on the other column to re-sort by potential. This doesn’t work in the Safari web browser (as of v. 4.0.3; in v. 3.1 or 3.2 it worked but sorted incorrectly); reload the page to restore the original order.

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

Half-reaction E° (V) Ref.
& -9
Zz 9
\tfrac{3}{2} N2(g) + H+ + e− ⇄ HN3(aq)  −3.09 [3]
Li+ + e− ⇄ Li(s)  −3.0401 [2]
N2(g) + 4 H2O + 2 e− ⇄ 2 NH2OH(aq) + 2 OH−  −3.04 [3]
Cs+ + e− ⇄ Cs(s)  −3.026 [2]
Rb+ + e− ⇄ Rb(s)  −2.98 [2]
K+ + e− ⇄ K(s)  −2.931 [2]
Ba2+ + 2 e− ⇄ Ba(s)  −2.912 [2]
La(OH)3(s) + 3 e− ⇄ La(s) + 3OH−  −2.90 [2]
Sr2+ + 2 e− ⇄ Sr(s)  −2.899 [2]
Ca2+ + 2 e− ⇄ Ca(s)  −2.868 [2]
Eu2+ + 2 e− ⇄ Eu(s)  −2.812 [2]
Ra2+ + 2 e− ⇄ Ra(s)  −2.8 [2]
Na+ + e− ⇄ Na(s)  −2.71 [2][6]
La3+ + 3 e− ⇄ La(s)  −2.379 [2]
Y3+ + 3 e− ⇄ Y(s)  −2.372 [2]
Mg2+ + 2 e− ⇄ Mg(s)  −2.372 [2]
ZrO(OH)2(s) + H2O + 4 e− ⇄ Zr(s) + 4OH−  −2.36 [2]
Al(OH)4− + 3 e− ⇄ Al(s) + 4 OH−  −2.33
Al(OH)3(s) + 3 e− ⇄ Al(s) + 3OH−  −2.31
H2(g) + 2 e− ⇄ 2 H−  −2.25
Ac3+ + 3 e− ⇄ Ac(s)  −2.20
Be2+ + 2 e− ⇄ Be(s)  −1.85
U3+ + 3 e− ⇄ U(s)  −1.66 [4]
Al3+ + 3 e− ⇄ Al(s)  −1.66 [6]
Ti2+ + 2 e− ⇄ Ti(s)  −1.63 [6]
ZrO2(s) + 4 H+ + 4 e− ⇄ Zr(s) + 2 H2O  −1.553 [2]
Zr4+ + 4 e− ⇄ Zr(s)  −1.45 [2]
TiO(s) + 2 H+ + 2 e− ⇄ Ti(s) + H2O  −1.31
Zn(OH)42− + 2 e− ⇄ Zn(s) + 4OH-  −1.199 [2]
Ti2O3(s) + 2 H+ + 2 e− ⇄ 2 TiO(s) + H2O  −1.23
Ti3+ + 3 e− ⇄ Ti(s)  −1.21
Mn2+ + 2 e− ⇄ Mn(s)  −1.185 [2]
Te(s) + 2 e− ⇄ Te2−  −1.143 [1]
V2+ + 2 e− ⇄ V(s)  −1.13 [1]
Nb3+ + 3 e− ⇄ Nb(s)  −1.099
Sn(s) + 4 H+ + 4 e− ⇄ SnH4(g)  −1.07
SiO2(s) + 4 H+ + 4 e− ⇄ Si(s) + 2 H2O  −0.91
B(OH)3(aq) + 3 H+ + 3 e− ⇄ B(s) + 3 H2O  −0.89
TiO2+ + 2 H+ + 4 e− ⇄ Ti(s) + H2O  −0.86
Bi(s) + 3 H+ + 3 e− ⇄ BiH3  −0.8 [2]
2 H2O + 2 e− ⇄ H2(g) + 2 OH−  −0.8277 [2]
Zn2+ + 2 e− ⇄ Zn(Hg)  −0.7628 [2]
Zn2+ + 2 e− ⇄ Zn(s)  −0.7618 [2]
Ta2O5(s) + 10 H+ + 10 e− ⇄ 2 Ta(s) + 5 H2O  −0.75
Cr3+ + 3 e− ⇄ Cr(s)  −0.74
[Au(CN)2]− + e− ⇄ Au(s) + 2 CN−  −0.60
Ta3+ + 3 e− ⇄ Ta(s)  −0.6
PbO(s) + H2O + 2 e− ⇄ Pb(s) + 2 OH−  −0.58
2 TiO2(s) + 2 H+ + 2 e− ⇄ Ti2O3(s) + H2O  −0.56
Ga3+ + 3 e− ⇄ Ga(s)  −0.53
AgI(s) + e− ⇄ Ag(s) + I−  −0.15224 [2]
U4+ + e− ⇄ U3+  −0.52 [4]
H3PO2(aq) + H+ + e− ⇄ P(white[note 1]) + 2 H2O  −0.508 [2]
H3PO3(aq) + 2 H+ + 2 e− ⇄ H3PO2(aq) + H2O  −0.499 [2]
H3PO3(aq) + 3 H+ + 3 e− ⇄ P(red)[note 1] + 3H2O  −0.454 [2]
Fe2+ + 2 e− ⇄ Fe(s)  −0.44 [6]
2 CO2(g) + 2 H+ + 2 e− ⇄ HOOCCOOH(aq)  −0.43
Cr3+ + e− ⇄ Cr2+  −0.42
Cd2+ + 2 e− ⇄ Cd(s)  −0.40 [6]
GeO2(s) + 2 H+ + 2 e− ⇄ GeO(s) + H2O  −0.37
Cu2O(s) + H2O + 2 e− ⇄ 2 Cu(s) + 2 OH−  −0.360 [2]
PbSO4(s) + 2 e− ⇄ Pb(s) + SO42−  −0.3588 [2]
PbSO4(s) + 2 e− ⇄ Pb(Hg) + SO42−  −0.3505 [2]
Eu3+ + e− ⇄ Eu2+  −0.35 [4]
In3+ + 3 e− ⇄ In(s)  −0.34 [1]
Tl+ + e− ⇄ Tl(s)  −0.34 [1]
Ge(s) + 4 H+ + 4 e− ⇄ GeH4(g)  −0.29
Co2+ + 2 e− ⇄ Co(s)  −0.28 [2]
H3PO4(aq) + 2 H+ + 2 e− ⇄ H3PO3(aq) + H2O  −0.276 [2]
V3+ + e− ⇄ V2+  −0.26 [6]
Ni2+ + 2 e− ⇄ Ni(s)  −0.25
As(s) + 3 H+ + 3 e− ⇄ AsH3(g)  −0.23 [1]
MoO2(s) + 4 H+ + 4 e− ⇄ Mo(s) + 2 H2O  −0.15
Si(s) + 4 H+ + 4 e− ⇄ SiH4(g)  −0.14
Sn2+ + 2 e− ⇄ Sn(s)  −0.13
O2(g) + H+ + e− ⇄ HO2•(aq)  −0.13
Pb2+ + 2 e− ⇄ Pb(s)  −0.13 [6]
WO2(s) + 4 H+ + 4 e− ⇄ W(s) + 2 H2O  −0.12
P(red) + 3 H+ + 3 e− ⇄ PH3(g)  −0.111 [2]
CO2(g) + 2 H+ + 2 e− ⇄ HCOOH(aq)  −0.11
Se(s) + 2 H+ + 2 e− ⇄ H2Se(g)  −0.11
CO2(g) + 2 H+ + 2 e− ⇄ CO(g) + H2O  −0.11
SnO(s) + 2 H+ + 2 e− ⇄ Sn(s) + H2O  −0.10
SnO2(s) + 2 H+ + 2 e− ⇄ SnO(s) + H2O  −0.09
WO3(aq) + 6 H+ + 6 e− ⇄ W(s) + 3 H2O  −0.09 [1]
P(white) + 3 H+ + 3 e− ⇄ PH3(g)  −0.063 [2]
HCOOH(aq) + 2 H+ + 2 e− ⇄ HCHO(aq) + H2O  −0.03
2 H+ + 2 e− ⇄ H2(g)    0.0000 ≡ 0
AgBr(s) + e− ⇄ Ag(s) + Br−  +0.07133 [2]
S4O62− + 2 e− ⇄ 2 S2O32−  +0.08
Fe3O4(s) + 8 H+ + 8 e− ⇄ 3 Fe(s) + 4 H2O  +0.085 [5]
N2(g) + 2 H2O + 6H+ + 6 e− ⇄ 2 NH4OH(aq)  +0.092
HgO(s) + H2O + 2 e− ⇄ Hg(l) + 2 OH−  +0.0977
Cu(NH3)42+ + e− ⇄ Cu(NH3)2+ + 2 NH3  +0.10 [1]
Ru(NH3)63+ + e− ⇄ Ru(NH3)62+  +0.10 [4]
N2H4(aq) + 4 H2O + 2 e− ⇄ 2 NH4+ + 4 OH−  +0.11 [3]
H2MoO4(aq) + 6 H+ + 6 e− ⇄ Mo(s) + 4 H2O  +0.11
Ge4+ + 4 e− ⇄ Ge(s)  +0.12
C(s) + 4 H+ + 4 e− ⇄ CH4(g)  +0.13 [1]
HCHO(aq) + 2 H+ + 2 e− ⇄ CH3OH(aq)  +0.13
S(s) + 2 H+ + 2 e− ⇄ H2S(g)  +0.14
Sn4+ + 2 e− ⇄ Sn2+  +0.15
Cu2+ + e− ⇄ Cu+  +0.159 [1]
HSO4− + 3 H+ + 2 e− ⇄ SO2(aq) + 2 H2O  +0.16
UO22+ + e− ⇄ UO2+  +0.163 [4]
SO42− + 4 H+ + 2 e− ⇄ SO2(aq) + 2 H2O  +0.17
TiO2+ + 2 H+ + e− ⇄ Ti3+ + H2O  +0.19
SbO+ + 2 H+ + 3 e− ⇄ Sb(s) + H2O  +0.20
AgCl(s) + e− ⇄ Ag(s) + Cl−  +0.22233 [2]
H3AsO3(aq) + 3 H+ + 3 e− ⇄ As(s) + 3 H2O  +0.24
GeO(s) + 2 H+ + 2 e− ⇄ Ge(s) + H2O  +0.26
UO2+ + 4 H+ + e− ⇄ U4+ + 2 H2O  +0.273 [4]
Re3+ + 3 e− ⇄ Re(s)  +0.300
Bi3+ + 3 e− ⇄ Bi(s)  +0.308 [2]
VO2+ + 2 H+ + e− ⇄ V3+ + H2O  +0.34
Cu2+ + 2 e− ⇄ Cu(s)  +0.340 [1]
[Fe(CN)6]3− + e− ⇄ [Fe(CN)6]4−  +0.36
O2(g) + 2 H2O + 4 e− ⇄ 4 OH−(aq)  +0.40 [6]
H2MoO4 + 6 H+ + 3 e− ⇄ Mo3+ + 2 H2O  +0.43
CH3OH(aq) + 2 H+ + 2 e− ⇄ CH4(g) + H2O  +0.50
SO2(aq) + 4 H+ + 4 e− ⇄ S(s) + 2 H2O  +0.50
Cu+ + e− ⇄ Cu(s)  +0.520 [1]
CO(g) + 2 H+ + 2 e− ⇄ C(s) + H2O  +0.52
I2(s) + 2 e− ⇄ 2 I−  +0.54 [6]
I3− + 2 e− ⇄ 3 I−  +0.53 [6]
[AuI4]− + 3 e− ⇄ Au(s) + 4 I−  +0.56
H3AsO4(aq) + 2 H+ + 2 e− ⇄ H3AsO3(aq) + H2O  +0.56
[AuI2]− + e− ⇄ Au(s) + 2 I−  +0.58
MnO4− + 2 H2O + 3 e− ⇄ MnO2(s) + 4 OH−  +0.59
S2O32 − + 6 H+ + 4 e− ⇄ 2 S(s) + 3 H2O  +0.60
H2MoO4(aq) + 2 H+ + 2 e− ⇄ MoO2(s) + 2 H2O  +0.65
1,4-Benzochinon.svg + 2 H+ + 2 e− ⇄ Hydrochinon2.svg  +0.6992 [2]
O2(g) + 2 H+ + 2 e− ⇄ H2O2(aq)  +0.70
Tl3+ + 3 e− ⇄ Tl(s)  +0.72
PtCl62− + 2 e− ⇄ PtCl42− + 2 Cl−  +0.726 [4]
H2SeO3(aq) + 4 H+ + 4 e− ⇄ Se(s) + 3 H2O  +0.74
PtCl42− + 2 e− ⇄ Pt(s) + 4 Cl−  +0.758 [4]
Fe3+ + e− ⇄ Fe2+  +0.77
Ag+ + e− ⇄ Ag(s)  +0.7996 [2]
Hg22+ + 2 e− ⇄ 2 Hg(l)  +0.80
NO3−(aq) + 2 H+ + e− ⇄ NO2(g) + H2O  +0.80
[AuBr4]− + 3 e− ⇄ Au(s) + 4 Br−  +0.85
Hg2+ + 2 e− ⇄ Hg(l)  +0.85
MnO4− + H+ + e− ⇄ HMnO4−  +0.90
2 Hg2+ + 2 e− ⇄ Hg22+  +0.91 [1]
Pd2+ + 2 e− ⇄ Pd(s)  +0.915 [4]
[AuCl4]− + 3 e− ⇄ Au(s) + 4 Cl−  +0.93
MnO2(s) + 4 H+ + e− ⇄ Mn3+ + 2 H2O  +0.95
[AuBr2]− + e− ⇄ Au(s) + 2 Br−  +0.96
Br2(l) + 2 e− ⇄ 2 Br−  +1.066 [2]
Br2(aq) + 2 e− ⇄ 2 Br−  +1.0873 [2]
IO3− + 5 H+ + 4 e− ⇄ HIO(aq) + 2 H2O  +1.13
[AuCl2]− + e− ⇄ Au(s) + 2 Cl−  +1.15
HSeO4− + 3 H+ + 2 e− ⇄ H2SeO3(aq) + H2O  +1.15
Ag2O(s) + 2 H+ + 2 e− ⇄ 2 Ag(s) + H2O  +1.17
ClO3− + 2 H+ + e− ⇄ ClO2(g) + H2O  +1.18
Pt2+ + 2 e− ⇄ Pt(s)  +1.188 [4]
ClO2(g) + H+ + e− ⇄ HClO2(aq)  +1.19
2 IO3− + 12 H+ + 10 e− ⇄ I2(s) + 6 H2O  +1.20
ClO4− + 2 H+ + 2 e− ⇄ ClO3− + H2O  +1.20
O2(g) + 4 H+ + 4 e− ⇄ 2 H2O  +1.23 [6]
MnO2(s) + 4 H+ + 2 e− ⇄ Mn2+ + 2H2O  +1.23
Tl3+ + 2 e− ⇄ Tl+  +1.25
Cl2(g) + 2 e− ⇄ 2 Cl−  +1.36 [6]
Cr2O72− + 14 H+ + 6 e− ⇄ 2 Cr3+ + 7 H2O  +1.33
CoO2(s) + 4 H+ + e− ⇄ Co3+ + 2 H2O  +1.42
2 NH3OH+ + H+ + 2 e− ⇄ N2H5+ + 2 H2O  +1.42 [3]
2 HIO(aq) + 2 H+ + 2 e− ⇄ I2(s) + 2 H2O  +1.44
Ce4+ + e− ⇄ Ce3+  +1.44
BrO3− + 5 H+ + 4 e− ⇄ HBrO(aq) + 2 H2O  +1.45
β-PbO2(s) + 4 H+ + 2 e− ⇄ Pb2+ + 2 H2O  +1.460 [1]
α-PbO2(s) + 4 H+ + 2 e− ⇄ Pb2+ + 2 H2O  +1.468 [1]
2 BrO3− + 12 H+ + 10 e− ⇄ Br2(l) + 6 H2O  +1.48
2ClO3− + 12 H+ + 10 e− ⇄ Cl2(g) + 6 H2O  +1.49
MnO4− + 8 H+ + 5 e− ⇄ Mn2+ + 4 H2O  +1.51
HO2• + H+ + e− ⇄ H2O2(aq)  +1.51
Au3+ + 3 e− ⇄ Au(s)  +1.52
NiO2(s) + 4 H+ + 2 e− ⇄ Ni2+ + 2 OH−  +1.59
2 HClO(aq) + 2 H+ + 2 e− ⇄ Cl2(g) + 2 H2O  +1.63
Ag2O3(s) + 6 H+ + 4 e− ⇄ 2 Ag+ + 3 H2O  +1.67
HClO2(aq) + 2 H+ + 2 e− ⇄ HClO(aq) + H2O  +1.67
Pb4+ + 2 e− ⇄ Pb2+  +1.69 [1]
MnO4− + 4 H+ + 3 e− ⇄ MnO2(s) + 2 H2O  +1.70
H2O2(aq) + 2 H+ + 2 e− ⇄ 2 H2O  +1.78
AgO(s) + 2 H+ + e− ⇄ Ag+ + H2O  +1.77
Co3+ + e− ⇄ Co2+  +1.82
Au+ + e− ⇄ Au(s)  +1.83 [1]
BrO4− + 2 H+ + 2 e− ⇄ BrO3− + H2O  +1.85
Ag2+ + e− ⇄ Ag+  +1.98 [1]
S2O82− + 2 e− ⇄ 2 SO42−  +2.010 [2]
O3(g) + 2 H+ + 2 e− ⇄ O2(g) + H2O  +2.075 [4]
HMnO4− + 3 H+ + 2 e− ⇄ MnO2(s) + 2 H2O  +2.09
F2(g) + 2 e− ⇄ 2 F−  +2.87 [1][6]
F2(g) + 2 H+ + 2 e− ⇄ 2 HF(aq)  +3.05 [1]
  1. ^ a b 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 white and red phosphorus in equilibrium with phosphine.

[edit] In oxidative phosphorylation

Further information: Oxidative phosphorylation#Eukaryotic electron transport chains

Oxidative phosphorylation is the means by which organism generate energy, and is driven by differences in electrode potential between intermediaries in a chain of reactions.

The following values are calculated for pH 7, which is more biologically realistic, but makes the values incompatible with the values in the table above with standard criteria.

Respiratory enzymes and substrates in eukaryotes.
Respiratory enzyme Redox pair  Midpoint potential 

(Volts)
 NADH dehydrogenase NAD+ / NADH −0.32[7]
 Succinate dehydrogenase FMN or FAD / FMNH2 or FADH2 −0.20[7]
 Cytochrome bc1 complex Coenzyme Q10ox / Coenzyme Q10red +0.06[7]
 Cytochrome bc1 complex Cytochrome box / Cytochrome bred +0.12[7]
 Complex IV Cytochrome cox / Cytochrome cred +0.22[7]
 Complex IV Cytochrome aox / Cytochrome ared +0.29[7]
 Complex IV O2 / HO- +0.82[7]

[edit] References

  1. ^ a b c d e f g h i j k l m n o p q r s t Bard, A. J., Parsons, R., and Jordan, J. (1985). Standard Potentials in Aqueous Solutions (Marcel Dekker, New York).
  2. ^ a b c d e f g h i j k l m n o p q r s t u v w x y z aa ab ac ad ae af ag ah ai aj ak al am an ao ap aq Vanýsek, Petr (2007). “Electrochemical Series”, in Handbook of Chemistry and Physics: 88th Edition (Chemical Rubber Company).
  3. ^ a b c d e Greenwood, Norman N.; Earnshaw, A. (1997), Chemistry of the Elements (2nd ed.), Oxford: Butterworth-Heinemann, ISBN 0-7506-3365-4 
  4. ^ a b c d e f g h i j k l Bard, A.J., Faulkner, L.R.(2001). Electrochemical Methods. Fundamentals and Applications, 2nd edition (John Wiley and Sons Inc).
  5. ^ a b Marcel Pourbaix (1966). Atlas of Electrochemical Equilibria in Aqueous Solutions (NACE International, Houston, Texas; Cebelcor, Brussels).
  6. ^ a b c d e f g h i j k l m n Peter Atkins (1997). Physical Chemistry, 6th edition (W.H. Freeman and Company, New York).
  7. ^ a b c d e f g Medical CHEMISTRY Compendium. By Anders Overgaard Pedersen and Henning Nielsen. Aarhus University. 2008

[edit] See also

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