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+ + 3e− | → | MnO2(s) + 2H2O | +2.09 |
| F2(g) + 2e− | → | 2F−(aq) | +2.87 |
| F2(g) + 2H+ + 2e− | → | 2HF(aq) | +3.05 |
Referencias[editar]
- ↑ 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).