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Standard electrode potential (data page)



The standard electrode potentials are used to determine the electrochemical potential or the electrode potential of an electrochemical cell or Galvanic cell.

These electrode potentials are given in volts relative to the standard hydrogen electrode. The values below are standard electrode potentials taken at 298 K, 1 bar pressure and in aqueous solution, of concentration 1 molar.[1][2][3][4]


Half-reaction Eo (V)
Li+(aq) + e− → Li(s) −3.05
Rb+(aq) + e− → Rb(s) −2.98
K+(aq) + e− → K(s) −2.93
Cs+(aq) + e− → Cs(s) −2.92
Ba2+(aq) + 2e− → Ba(s) −2.91
Sr2+(aq) + 2e− → Sr(s) −2.89
Ra2+(aq) + 2e− → Ra(s) −2.80
Ca2+(aq) + 2e− → Ca(s) −2.76
Na+(aq) + e− → Na(s) −2.71
Mg2+(aq) + 2e− → Mg(s) −2.38
H2 + 2e− → 2H− −2.25
Ac3+(aq) + 3e− → Ac(s) −2.20
Be2+(aq) + 2e− → Be(s) −1.85
Al3+(aq) + 3e− → Al(s) −1.68
Ti2+(aq) + 2e− → Ti(s) −1.63
TiO(s) + 2H+ + 2e− → Ti(s) + H2O −1.31
Ti2O3(s) + 2H+ + 2e− → 2TiO(s) + H2O −1.23
Ti3+(aq) + 3e− → Ti(s) −1.21
Mn2+(aq) + 2e− → Mn(s) −1.18
V2+(aq) + 2e− → V(s) −1.13
Nb3+(aq) + 3e− → Nb(s) −1.099
Sn(s) + 4H+ + 4e− → SnH4(g) −1.07
SiO2(s) + 4H+ + 4e− → Si(s) + 2H2O −0.91
B(OH)3(aq) + 3H+ + 3e− → B(s) + 3H2O −0.89
TiO2+(aq) + 2H+ + 4e− → Ti(s) + H2O −0.86
2 H2O(l) + 2e– → H2(g) + 2 OH–(aq) −0.83
Zn2+(aq) + 2e− → Zn(s) −0.76
Cr3+(aq) + 3e− → Cr(s) −0.74
Au(CN)2–(aq) + e– → Au(s) +2 CN–(aq) −0.60
PbO(s) + H2O + 2e− → Pb(s) + 2OH- −0.58
2TiO2(s) + 2H+ + 2e− → Ti2O3(s) + H2O −0.56
Ga3+(aq) + 3e− → Ga(s) −0.53
H3PO2(aq) + H+ + e− → P(s) + 2H2O −0.51
H3PO3(aq) + 3H+ + 3e− → P(s) + 3H2O −0.50
H3PO3(aq) + 2H+ + 2e− → H3PO2(aq) + H2O −0.50
Fe2+(aq) + 2e− → Fe(s) −0.44
2CO2(g) + 2H+(aq) + 2e– → HOOCCOOH(aq) −0.43
Cr3+(aq) + e− → Cr2+(aq) −0.42
Cd2+(aq) + 2e− → Cd(s) −0.40
PbSO4(s) + 2e– → Pb(s) +SO42-(aq) −0.36
GeO2(s) + 2H+ + 2e− → GeO(s) + H2O −0.37
In3+(aq) + 3e− → In(s) −0.34
Tl+(aq) + e− → Tl(s) −0.34
Ge(s) + 4H+ + 4e− → GeH4(g) −0.29
Co2+(aq) + 2e → Co(s) −0.28
H3PO4(aq) + 2H+ + 2e− → H3PO3(aq) + H2O −0.28
V3+(aq) + e− → V2+(aq) −0.26
Ni2+(aq) + 2e− → Ni(s) −0.25
As(s) + 3H+ + 3e− → AsH3(g) −0.23
MoO2(s) + 4H+ + 4e− → Mo(s) + 2H2O −0.15
Si(s) + 4H+ + 4e− → SiH4(g) −0.14
Sn2+(aq) + 2e− → Sn(s) −0.13
O2(g) + H+ + e− → HO2•(aq) −0.13
Pb2+(aq) + 2e− → Pb(s) −0.13
WO2(s) + 4H+ + 4e− → W(s) + 2H2O −0.12
CO2(g) + 2H+ + 2e− → HCOOH(aq) −0.11
Se(s) + 2H+ + 2e− → H2Se(g) −0.11
CO2(g) + 2H+ + 2e− → CO(g) + H2O −0.11
SnO(s) + 2H+ + 2e− → Sn(s) + H2O −0.10
SnO2(s) + 2H+ + 2e− → SnO(s) + H2O −0.09
WO3(aq) + 6H+ + 6e− → W(s) −0.09
P(s) + 3H+ + 3e− → PH3(g) −0.06
HCOOH(aq) + 2H+ + 2e− → HCHO(aq) + H2O −0.03
2H+(aq) + 2e− → H2(g)   0.00
H2MoO4(aq) + 6H+ + 6e− → Mo(s) + 4H2O +0.11
Ge4+(aq) + 4e− → Ge(s) +0.12
C(s) + 4H+ + 4e− → CH4(g) +0.13
HCHO(aq) + 2H+ + 2e− → CH3OH(aq) +0.13
S(s) + 2H+ + 2e− → H2S(g) +0.14
Sn4+(aq) + 2e− → Sn2+(aq) +0.15
Cu2+(aq) + e− → Cu+(aq) +0.16
HSO4−(aq) + 3H+ + 2e− → 2H2O(l) + SO2(aq) +0.16
SO42−(aq) + 4H+ + 2e− → 2H2O(l) + SO2(aq) +0.17
SbO+ + 2H+ + 3e− → Sb(s) + H2O +0.20
H3AsO3(aq) + 3H+ + 3e− → As(s) + 3H2O +0.24
GeO(s) + 2H+ + 2e− → Ge(s) + H2O +0.26
Re3+(aq) + 3e− → Re(s) +0.300
Bi3+(aq) + 3e− → Bi(s) +0.32
VO2+(aq) + 2H+ + e− → V3+(aq) +0.34
Cu2+(aq) + 2e− → Cu(s) +0.34
[Fe(CN)6]3−(aq) + e− → [Fe(CN)6]4−(aq) +0.36
O2(g) + 2H2O(l) + 4e– → 4OH–(aq) +0.40
H2MoO4 + 6H+ + 3e− → Mo3+(aq) +0.43
CH3OH(aq) + 2H+ + 2e− → CH4(g) + H2O +0.50
SO2(aq) + 4H+ + 4e− → S(s) + 2H2O +0.50
Cu+(aq) + e− → Cu(s) +0.52
CO(g) + 2H+ + 2e− → C(s) + H2O +0.52
I2(s) + 2e− → 2I−(aq) +0.54
I3−(aq) + 2e− → 3I−(aq) +0.54
[AuI4]−(aq) + 3e− → Au(s) + 4I−(aq) +0.56
H3AsO4(aq) + 2H+ + 2e− → H3AsO3(aq) + H2O +0.56
[AuI2]−(aq) + e− → Au(s) + 2I−(aq) +0.58
MnO4–(aq) + 2H2O(l) + 3e– → MnO2(s) + 4OH–(aq) +0.59
S2O32− + 6H+ + 4e− → 2S(s) + 3H2O +0.60
H2MoO4(aq) + 2H+ + 2e− → MoO2(s) + 2H2O +0.65
O2(g) + 2H+ + 2e− → H2O2(aq) +0.70
Tl3+(aq) + 3e− → Tl(s) +0.72
H2SeO3(aq) + 4H+ + 4e− → Se(s) + 3H2O +0.74
Fe3+(aq) + e− → Fe2+(aq) +0.77
Hg22+(aq) + 2e− → 2Hg(l) +0.80
Ag+(aq) + e− → Ag(s) +0.80
NO3–(aq) + 2H+ + e− → NO2(g) + H2O +0.80
[AuBr4]−(aq) + 3e− → Au(s) + 4Br−(aq) +0.85
Hg2+(aq) + 2e− → Hg(l) +0.85
MnO4−(aq) + H+ + e− → HMnO4−(aq) +0.90
2Hg2+(aq) + 2e− → Hg22+(aq) +0.91
[AuCl4]−(aq) + 3e− → Au(s) + 4Cl−(aq) +0.93
MnO2(s) + 4H+ + e− → Mn3+(aq) + 2H2O +0.95
[AuBr2]−(aq) + e− → Au(s) + 2Br−(aq) +0.96
Br2(l) + 2e− → 2Br−(aq) +1.07
Br2(aq) + 2e− → 2Br−(aq) +1.09
IO3−(aq) + 5H+ + 4e− → HIO(aq) + 2H2O +1.13
[AuCl2]−(aq) + e− → Au(s) + 2Cl−(aq) +1.15
HSeO4−(aq) + 3H+ + 2e− → H2SeO3(aq) + H2O +1.15
Ag2O(s) + 2H+ + 2e− → 2Ag(s) +1.17
ClO3−(aq) + 2H+ + e− → ClO2(g) + H2O +1.18
ClO2(g) + H+ + e− → HClO2(aq) +1.19
2IO3−(aq) + 12H+ + 10e− → I2(s) + 6H2O +1.20
ClO4−(aq) + 2H+ + 2e− → ClO3−(aq) + H2O +1.20
O2(g) + 4H+ + 4e− → 2H2O +1.23
MnO2(s) + 4H+ + 2e− → Mn2+(aq) + 2H2O +1.23
Tl3+(aq) + 2e− → Tl+(aq) +1.25
Cl2(g) + 2e− → 2Cl−(aq) +1.36
Cr2O72−(aq) + 14H+ + 6e− → 2Cr3+(aq) + 7H2O +1.36
CoO2(s) + 4H+ + e− → Co3+(aq) + 2H2O +1.42
2HIO(aq) + 2H+ + 2e− → I2(s) + 2H2O +1.44
BrO3−(aq) + 5H+ + 4e− → HBrO(aq) + 2H2O +1.45
2BrO3− + 12H+ + 10e− → Br2(l) + 6H2O +1.48
2ClO3− + 12H+ + 10e− → Cl2(g) + 6H2O +1.49
MnO4−(aq) + 8H+ + 5e− → Mn2+(aq) + 4H2O +1.51
HO2• + H+ + e− → H2O2(aq) +1.51
Au3+(aq) + 3e− → Au(s) +1.52
NiO2(s) + 4H+ + 2e− → Ni2+(aq) +1.59
2HClO(aq) + 2H+ + 2e− → Cl2(g) + 2H2O +1.63
Ag2O3(s) + 6H+ + 4e− → 2Ag+(aq) + 3H2O +1.67
HClO2(aq) + 2H+ + 2e− → HClO(aq) + H2O +1.67
Pb4+(aq) + 2e− → Pb2+(aq) +1.69
MnO4−(aq) + 4H+ + 3e− → MnO2(s) + 2H2O +1.70
H2O2(aq) + 2H+ + 2e− → 2H2O +1.76
AgO(s) + 2H+ + e− → Ag+(aq) + H2O +1.77
Au+(aq) + e− → Au(s) +1.83
BrO4−(aq) + 2H+ + 2e− → BrO3−(aq) + H2O +1.85
Co3+(aq) + e− → Co2+(aq) +1.92
Ag2+(aq) + e− → Ag+(aq) +1.98
S2O82− + 2e– → 2SO42− +2.07
HMnO4−(aq) + 3H+ + 2e− → MnO2(s) + 2H2O +2.09
F2(g) + 2e− → 2F−(aq) +2.87
F2(g) + 2H+ + 2e− → 2HF(aq) +3.05

References

  1. ^ Milazzo, G., Caroli, S., and Sharma, V. K. (1978). Tables of Standard Electrode Potentials (Wiley, Chichester).
  2. ^ Bard, A. J., Parsons, R., and Jordan, J. (1985). Standard Potentials in Aqueous Solutions (Marcel Dekker, New York).
  3. ^ Bratsch, S. G. (1989). Journal of Physical Chemistry Reference Data Vol. 18, pp. 1–21.
  4. ^ Vanysek, Petr (2006). "Electrochemical Series," in Handbook of Chemistry and Physics: 87th Edition (Chemical Rubber Company).

See also

 
This article is licensed under the GNU Free Documentation License. It uses material from the Wikipedia article "Standard_electrode_potential_(data_page)". A list of authors is available in Wikipedia.
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