标准氧化还原电位表

Standard electrode potential (data page)

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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 for the following conditions:

A temperature of 298.15 K (25 °C);

? An of 1 mol/L for each aqueous species or a species in a mercury amalgam;

? A of 101.325 (absolute) (1 , 1.01325 ) 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.

? An of unity for each pure solid, pure liquid, or for water (solvent).

?

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

Half-reaction

3

E° (V)[note 1] Ref. ?3.09 ?3.0401 ?3.04 ?3.026 ?2.98

[1][2]

?2?N2(g) + ?H+ + ?e?

HN3(aq)

Li+ + ?e?

Li(s)

N2(g) + 4?H2O + 2?e?

2?NH2OH(aq) + 2?OH? Cs+ + ?e?

Cs(s) Rb+ + ?e?

Rb(s)

[2]

[1]

[2]

[2]

Half-reaction

K+ + ?e?

K(s) Ba2+ + 2?e?

Ba(s)

La(OH)3(s) + 3?e?

La(s) + 3?OH? Sr2+ + 2?e?

Sr(s) Ca2+ + 2?e?

Ca(s) Eu2+ + 2?e?

Eu(s) Ra2+ + 2?e?

Ra(s) Na+ + ?e?

Na(s) Sc3+ + 3?e?

Sc(s) La3+ + 3?e?

La(s) Y3+ + 3?e?

Y(s) Mg2+ + 2?e?

Mg(s)

ZrO(OH)2(s) + ?H2O + 4?e?

Zr(s) + 4?OH? Al(OH)?4 + 3?e?

Al(s) + 4?OH? Al(OH)3(s) + 3?e?

Al(s) + 3?OH? H2(g) + 2?e?

2?H? Ac3+ + 3?e?

Ac(s) Be2+ + 2?e?

Be(s) U3+ + 3?e?

U(s) Al3+

+ 3?e?

Al(s)

E° (V)[note 1] ?2.931 ?2.912 ?2.90 ?2.899 ?2.868 ?2.812 ?2.8 ?2.71 ?2.077 ?2.379 ?2.372 ?2.372 ?2.36 ?2.33 ?2.31 ?2.25 ?2.20 ?1.85 ?1.66 ?1.66

Ref. [2]

[2]

[2]

[2]

[2]

[2]

[2]

[2][3]

[4]

[2]

[2]

[2]

[2]

[5]

[3]

Half-reaction

Ti2+ + 2?e?

Ti(s)

ZrO2(s) + 4?H+ + 4?e?

Zr(s) + 2?H2O Zr4+ + 4?e?

Zr(s) Ti3+ + 3?e?

Ti(s)

TiO(s) + 2?H+ + 2?e?

Ti(s) + ?H2O Ti+2O3(s) + 2?H + 2?e?

2?TiO(s) + ?H2O Zn(OH)2?4 + 2?e?

Zn(s) + 4?OH? Mn2+ + 2?e?

Mn(s)

Fe(CN)4?6 + 6?H+ + 2 ?e?

Fe(s) + 6HCN(aq) Te(s) + 2?e?

Te2? V2+ + 2?e?

V(s) Nb3+ + 3?e?

Nb(s)

Sn(s) + 4?H+ + 4?e?

SnH4(g) SiO2(s) + 4?H+ + 4?e?

Si(s) + 2?H2O B(OH)+

3(aq) + 3?H + 3?e?

B(s) + 3?H2O Fe(OH)2(s) + 2?e?

Fe(s) + 2?OH?

Fe2O3(s) + 3?H2O + 2?e?

2Fe(OH)2(s) + 2?OH? TiO2+ + 2?H+ + 4?e?

Ti(s) + ?H2O 2??H2O + 2?e?

H2(g) + 2?OH? Bi(s) + 3?H+

+ 3?e?

BiH3

E° (V)[note 1] ?1.63 ?1.553 ?1.45 ?1.37 ?1.31 ?1.23 ?1.199 ?1.185 ?1.16 ?1.143 ?1.13 ?1.099 ?1.07 ?0.91 ?0.89 ?0.89 ?0.86 ?0.86 ?0.8277 ?0.8

Ref. [3]

[6]

[6]

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[8]

[9]

[9]

[8]

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Half-reaction

Zn2+ + 2?e?

Zn(Hg) Zn2+ + 2?e?

Zn(s)

Ta2O5(s) + 10?H+ + 10?e?

2?Ta(s) + 5?H2O Cr3+ + 3?e?

Cr(s)

[Au(CN)2]? + ?e?

Au(s) + 2?CN? Ta3+ + 3?e?

Ta(s)

PbO(s) + ?H?

2O + 2?e Pb(s) + 2?OH? 2?TiO2(s) + 2?H+ + 2?e?

Ti2O3(s) + ?H2O Ga3+ + 3?e?

Ga(s) U4+ + ?e?

U3+

H3PO2(aq) + ?H+ + ?e?

P(white)[note 2] + 2?H2O H?

3PO3(aq) + 2?H+ + 2?e H3PO2(aq) + ?H2O

H3PO3(aq) + 3?H+ + 3?e?

P(red)[note 2] + 3?H2O Fe2+ + 2?e?

Fe(s)

2?CO+

2(g) + 2?H + 2?e?

HOOCCOOH(aq) Cr3+ + ?e?

Cr2+ Cd2+ + 2?e?

Cd(s)

GeO2(s) + 2?H+ + 2?e?

GeO(s) + ?H2O Cu2O(s) + ?H2O + 2?e?

2?Cu(s) + 2?OH? PbSO?

4(s) + 2?e Pb(s) + SO2

?4

E° (V)[note 1] ?0.7628 ?0.7618 ?0.75 ?0.74 ?0.60 ?0.6 ?0.58 ?0.56 ?0.53 ?0.52

?0.508 ?0.499

?0.454 ?0.44 ?0.43 ?0.42 ?0.40 ?0.37 ?0.360 ?0.3588

Ref. [6]

[6]

[5]

[6]

[6]

[6]

[3]

[3]

[6]

[6]

Half-reaction

PbSO?

4(s) + 2?e Pb(Hg) + SO2?4 Eu3+ + ?e?

Eu2+ In3+ + 3?e?

In(s) Tl+ + ?e?

Tl(s)

Ge(s) + 4?H+ + 4?e?

GeH4(g) Co2+ + 2?e?

Co(s)

H3PO4(aq) + 2?H+ + 2?e?

H3PO3(aq) + V3+ + ?e?

V2+ Ni2+ + 2?e?

Ni(s)

As(s) + 3?H+ + 3?e?

AsH3(g) AgI(s) + ?e?

Ag(s) + I?

MoO2(s) + 4?H+ + 4?e?

Mo(s) + 2?H2O Si(s) + 4?H+ + 4?e?

SiH4(g) Sn2+ + 2?e?

Sn(s)

O+

2(g) + ?H + ?e?

HO2?(aq) Pb2+ + 2?e?

Pb(s)

WO+2(s) + 4?H + 4?e?

W(s) + 2?H2O P(red) + 3?H+ + 3?e?

PH3(g) CO2(g) + 2?H+ + 2?e?

HCOOH(aq) Se(s) + 2?H+ + 2?e?

H2Se(g)

E° (V)[note 1] ?0.3505 ?0.35 ?0.34 ?0.34 ?0.29 ?0.28 H2O ?0.276 ?0.26 ?0.25 ?0.23 ?0.15224 ?0.15 ?0.14 ?0.13 ?0.13 ?0.13 ?0.12 ?0.111 ?0.11 ?0.11

Ref. [6]

[5]

[9]

[9]

[6]

[6]

[3]

[9]

[6]

[3]

[6]

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