Anexo:Tabla de potenciales de reducción
El potencial estándar de reducción se utiliza para determinar el potencial electroquímico o el potencial de un electrodo de una celda electroquímica o de una celda galvánica.
Estos potenciales de reducción vienen dados en relación de un electrodo estándar de hidrógeno. Los valores de los potenciales estándares de reducción que se presentan en la tabla son en condiciones normales o estándar, es decir: a una temperatura de 25 °C / 298.15 K, una presión de 1 atm / 100 kPa y en una solución acuosa con una concentración de 1 molar. [1] [2] [3] [4]
Media reacción | E | ||
---|---|---|---|
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 |
Be2+(aq) + 2e− | → | Be(s) | −2.76 |
Na+(aq) + e− | → | Na(s) | −2.71 |
Mg2+(aq) + 2e− | → | Mg(s) | −2.38 |
H2 + 2e− | → | 2H− | −2.25 |
Ca2+(aq) + 2e− | → | Ca(s) | −1.85 |
Al3+(aq) + 3e− | → | Al(s) | −1.66 |
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 |
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 |
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) | −0.14 |
O2(g) + H+ + e− | → | HO2•(aq) | −0.13 |
Pb2+(aq) + 2e− | → | Pb(s) | −0.13 |
WO2(s) + 4H+ + 4e− | → | W(s) | −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 |
Hg2Cl2 + 2e− | → | 2Hg + 2Cl− | +0.27 |
Bi3+(aq) + 3e− | → | Bi(s) | +0.32 |
Cu2+(aq) + 2e− | → | Cu(s) | +0.34 |
[Fe(CN)6]3−(aq) + e− | → | [Fe(CN)6]4−(aq) | +0.36 |
VO2+(aq) + 2H+ + e− | → | V3+(aq) + H2O | +0.361 |
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) + 4 OH–(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) | +0.79 |
Ag+(aq) + e− | → | Ag(s) | +0.80 |
NO3–(aq) + 2H+(aq) +e– | → | NO2(g) + H2O(l) | +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+(s) | +1.25 |
Cl2(g) + 2e− | → | 2Cl−(aq) | +1.36 |
Cr2O72−(aq) + 14H+ + 6e− | → | 2Cr3+(aq) + 7H2O | +1.33 |
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 |
O2• + 2H+ + 2e− | → | 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 |
Au+(aq) + 1e− | → | Au(aq) | +1.68 |
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 |
Referencias
- Milazzo, G., Caroli, S., and Sharma, V. K. (1978). Tables of Standard Electrode Potentials (Wiley, Chichester).
- Bard, A. J., Parsons, R., and Jordan, J. (1985). Standard Potentials in Aqueous Solutions (Marcel Dekker, New York).
- Bratsch, S. G. (1989). Journal of Physical Chemistry Reference Data Vuelo. 18, pp. 1-21.
- Vanysek, Petr (2006). "Electrochemical Series," in Handbook of Chemistry and Physics: 87 th Edition (Chemical Rubber Company).
Este artículo ha sido escrito por Wikipedia. El texto está disponible bajo la licencia Creative Commons - Atribución - CompartirIgual. Pueden aplicarse cláusulas adicionales a los archivos multimedia.