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 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).

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

Half-reaction	E° (V)	Ref.
&	-9
Zz	9
N $\tfrac{3}{2}$ N₂(g) + H⁺ + e⁻ ⇄ HN₃(aq)	-3.09 −3.09	^[3]
Li⁺ + e⁻ ⇄ Li(s)	-3.0401 −3.0401	^[2]
N₂(g) + 4 H₂O + 2 e⁻ ⇄ 2 NH₂OH(aq) + 2 OH⁻	-3.04 −3.04	^[3]
Cs⁺ + e⁻ ⇄ Cs(s)	-3.026 −3.026	^[2]
Rb⁺ + e⁻ ⇄ Rb(s)	-2.98 −2.98	^[2]
K⁺ + e⁻ ⇄ K(s)	-2.931 −2.931	^[2]
Ba²⁺ + 2 e⁻ ⇄ Ba(s)	-2.912 −2.912	^[2]
La(OH)₃(s) + 3 e⁻ ⇄ La(s) + 3OH⁻	-2.90 −2.90	^[2]
Sr²⁺ + 2 e⁻ ⇄ Sr(s)	-2.899 −2.899	^[2]
Ca²⁺ + 2 e⁻ ⇄ Ca(s)	-2.868 −2.868	^[2]
Eu²⁺ + 2 e⁻ ⇄ Eu(s)	-2.812 −2.812	^[2]
Ra²⁺ + 2 e⁻ ⇄ Ra(s)	-2.8 −2.8	^[2]
Na⁺ + e⁻ ⇄ Na(s)	-2.71 −2.71	^[2]^[6]
La³⁺ + 3 e⁻ ⇄ La(s)	-2.379 −2.379	^[2]
Y³⁺ + 3 e⁻ ⇄ Y(s)	-2.372 −2.372	^[2]
Mg²⁺ + 2 e⁻ ⇄ Mg(s)	-2.372 −2.372	^[2]
ZrO(OH)₂(s) + H₂O + 4 e⁻ ⇄ Zr(s) + 4OH⁻	-2.36 −2.36	^[2]
Al(OH)₄⁻ + 3 e⁻ ⇄ Al(s) + 4 OH⁻	-2.33 −2.33
Al(OH)₃(s) + 3 e⁻ ⇄ Al(s) + 3OH⁻	-2.31 −2.31
H₂(g) + 2 e⁻ ⇄ 2 H⁻	-2.25 −2.25
Ac³⁺ + 3 e⁻ ⇄ Ac(s)	-2.20 −2.20
Be²⁺ + 2 e⁻ ⇄ Be(s)	-1.85 −1.85
U³⁺ + 3 e⁻ ⇄ U(s)	-1.66 −1.66	^[4]
Al³⁺ + 3 e⁻ ⇄ Al(s)	-1.66 −1.66	^[6]
Ti²⁺ + 2 e⁻ ⇄ Ti(s)	-1.63 −1.63	^[6]
ZrO₂(s) + 4 H⁺ + 4 e⁻ ⇄ Zr(s) + 2 H₂O	-1.553 −1.553	^[2]
Zr⁴⁺ + 4 e⁻ ⇄ Zr(s)	-1.45 −1.45	^[2]
TiO(s) + 2 H⁺ + 2 e⁻ ⇄ Ti(s) + H₂O	-1.31 −1.31
Ti₂O₃(s) + 2 H⁺ + 2 e⁻ ⇄ 2 TiO(s) + H₂O	-1.23 −1.23
Ti³⁺ + 3 e⁻ ⇄ Ti(s)	-1.21 −1.21
Mn²⁺ + 2 e⁻ ⇄ Mn(s)	-1.185 −1.185	^[2]
Te(s) + 2 e⁻ ⇄ Te²⁻	-1.143 −1.143	^[1]
V²⁺ + 2 e⁻ ⇄ V(s)	-1.13 −1.13	^[1]
Nb³⁺ + 3 e⁻ ⇄ Nb(s)	-1.099 −1.099
Sn(s) + 4 H⁺ + 4 e⁻ ⇄ SnH₄(g)	-1.07 −1.07
SiO₂(s) + 4 H⁺ + 4 e⁻ ⇄ Si(s) + 2 H₂O	-0.91 −0.91
B(OH)₃(aq) + 3 H⁺ + 3 e⁻ ⇄ B(s) + 3 H₂O	-0.89 −0.89
TiO²⁺ + 2 H⁺ + 4 e⁻ ⇄ Ti(s) + H₂O	-0.86 −0.86
Bi(s) + 3 H⁺ + 3 e⁻ ⇄ BiH₃	-0.8 −0.8
H2 H₂O + 2 e⁻ ⇄ H₂(g) + 2 OH⁻	-0.8277 −0.8277	^[2]
Zn²⁺ + 2 e⁻ ⇄ Zn(Hg)	-0.7628 −0.7628	^[2]
Zn²⁺ + 2 e⁻ ⇄ Zn(s)	-0.7618 −0.7618	^[2]
Ta₂O₅(s) + 10 H⁺ + 10 e⁻ ⇄ 2 Ta(s) + 5 H₂O	-0.75 −0.75
Cr³⁺ + 3 e⁻ ⇄ Cr(s)	-0.74 −0.74
Au[Au(CN)₂]⁻ + e⁻ ⇄ Au(s) + 2 CN⁻	-0.60 −0.60
Ta³⁺ + 3 e⁻ ⇄ Ta(s)	-0.6 −0.6
PbO(s) + H₂O + 2 e⁻ ⇄ Pb(s) + 2 OH⁻	-0.58 −0.58
Ti2 TiO₂(s) + 2 H⁺ + 2 e⁻ ⇄ Ti₂O₃(s) + H₂O	-0.56 −0.56
Ga³⁺ + 3 e⁻ ⇄ Ga(s)	-0.53 −0.53
AgI(s) + e⁻ ⇄ Ag(s) + I⁻	-0.15224 −0.15224	^[2]
U⁴⁺ + e⁻ ⇄ U³⁺	-0.52 −0.52	^[4]
P H₃PO₂(aq) + H⁺ + e⁻ ⇄ P(white^{[note 1]}) + 2 H₂O	-0.508 −0.508	^[2]
P H₃PO₃(aq) + 2 H⁺ + 2 e⁻ ⇄ H₃PO₂(aq) + H₂O	-0.499 −0.499	^[2]
P H₃PO₃(aq) + 3 H⁺ + 3 e⁻ ⇄ P(red)^{[note 1]} + 3H₂O	-0.454 −0.454	^[2]
Fe²⁺ + 2 e⁻ ⇄ Fe(s)	-0.44 −0.44	^[6]
C2 CO₂(g) + 2 H⁺ + 2 e⁻ ⇄ HOOCCOOH(aq)	-0.43 −0.43
Cr³⁺ + e⁻ ⇄ Cr²⁺	-0.42 −0.42
Cd²⁺ + 2 e⁻ ⇄ Cd(s)	-0.40 −0.40	^[6]
GeO₂(s) + 2 H⁺ + 2 e⁻ ⇄ GeO(s) + H₂O	-0.37 −0.37
Cu₂O(s) + H₂O + 2 e⁻ ⇄ 2 Cu(s) + 2 OH⁻	-0.360 −0.360	^[2]
PbSO₄(s) + 2 e⁻ ⇄ Pb(s) + SO₄²⁻	-0.3588 −0.3588	^[2]
PbSO₄(s) + 2 e⁻ ⇄ Pb(Hg) + SO₄²⁻	-0.3505 −0.3505	^[2]
Eu³⁺ + e⁻ ⇄ Eu²⁺	-0.35 −0.35	^[4]
In³⁺ + 3 e⁻ ⇄ In(s)	-0.34 −0.34	^[1]
Tl⁺ + e⁻ ⇄ Tl(s)	-0.34 −0.34	^[1]
Ge(s) + 4 H⁺ + 4 e⁻ ⇄ GeH₄(g)	-0.29 −0.29
Co²⁺ + 2 e⁻ ⇄ Co(s)	-0.28 −0.28	^[2]
P H₃PO₄(aq) + 2 H⁺ + 2 e⁻ ⇄ H₃PO₃(aq) + H₂O	-0.276 −0.276	^[2]
V³⁺ + e⁻ ⇄ V²⁺	-0.26 −0.26	^[6]
Ni²⁺ + 2 e⁻ ⇄ Ni(s)	-0.25 −0.25
As(s) + 3 H⁺ + 3 e⁻ ⇄ AsH₃(g)	-0.23 −0.23	^[1]
MoO₂(s) + 4 H⁺ + 4 e⁻ ⇄ Mo(s) + 2 H₂O	-0.15 −0.15
Si(s) + 4 H⁺ + 4 e⁻ ⇄ SiH₄(g)	-0.14 −0.14
Sn²⁺ + 2 e⁻ ⇄ Sn(s)	-0.13 −0.13
O₂(g) + H⁺ + e⁻ ⇄ HO₂•(aq)	-0.13 −0.13
Pb²⁺ + 2 e⁻ ⇄ Pb(s)	-0.13 −0.13	^[6]
WO₂(s) + 4 H⁺ + 4 e⁻ ⇄ W(s) + 2 H₂O	-0.12 −0.12
P(red) + 3 H⁺ + 3 e⁻ ⇄ PH₃(g)	-0.111 −0.111	^[2]
C CO₂(g) + 2 H⁺ + 2 e⁻ ⇄ HCOOH(aq)	-0.11 −0.11
Se(s) + 2 H⁺ + 2 e⁻ ⇄ H₂Se(g)	-0.11 −0.11
C CO₂(g) + 2 H⁺ + 2 e⁻ ⇄ CO(g) + H₂O	-0.11 −0.11
SnO(s) + 2 H⁺ + 2 e⁻ ⇄ Sn(s) + H₂O	-0.10 −0.10
SnO₂(s) + 2 H⁺ + 2 e⁻ ⇄ SnO(s) + H₂O	-0.09 −0.09
WO₃(aq) + 6 H⁺ + 6 e⁻ ⇄ W(s) + 3 H₂O	-0.09 −0.09	^[1]
P(white) + 3 H⁺ + 3 e⁻ ⇄ PH₃(g)	-0.063 −0.063	^[2]
C HCOOH(aq) + 2 H⁺ + 2 e⁻ ⇄ HCHO(aq) + H₂O	-0.03 −0.03
H 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]
Mo 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]
C 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]
S HSO₄⁻ + 3 H⁺ + 2 e⁻ ⇄ SO₂(aq) + 2 H₂O	+0.16
UO₂²⁺ + e⁻ ⇄ UO₂⁺	+0.163	^[4]
S SO₄²⁻ + 4 H⁺ + 2 e⁻ ⇄ SO₂(aq) + 2 H₂O	+0.17
TiO²⁺ + 2 H⁺ + e⁻ ⇄ Ti³⁺ + H₂O	+0.19
Bi³⁺ + 2e⁻ ⇄ Bi⁺	+0.2
SbO⁺ + 2 H⁺ + 3 e⁻ ⇄ Sb(s) + H₂O	+0.20
AgCl(s) + e⁻ ⇄ Ag(s) + Cl⁻	+0.22233	^[2]
As 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)	+0.32
VO²⁺ + 2 H⁺ + e⁻ ⇄ V³⁺ + H₂O	+0.34
Cu²⁺ + 2 e⁻ ⇄ Cu(s)	+0.340	^[1]
Fe [Fe(CN)₆]³⁻ + e⁻ ⇄ [Fe(CN)₆]⁴⁻	+0.36
O₂(g) + 2 H₂O + 4 e⁻ ⇄ 4 OH⁻(aq)	+0.40	^[6]
Mo H₂MoO₄ + 6 H⁺ + 3 e⁻ ⇄ Mo³⁺ + 2 H₂O	+0.43
Bi⁺ + e⁻ ⇄ Bi(s)	+0.50
C CH₃OH(aq) + 2 H⁺ + 2 e⁻ ⇄ CH₄(g) + H₂O	+0.50
S SO₂(aq) + 4 H⁺ + 4 e⁻ ⇄ S(s) + 2 H₂O	+0.50
Cu⁺ + e⁻ ⇄ Cu(s)	+0.520	^[1]
C 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]
Au [AuI₄]⁻ + 3 e⁻ ⇄ Au(s) + 4 I⁻	+0.56
As H₃AsO₄(aq) + 2 H⁺ + 2 e⁻ ⇄ H₃AsO₃(aq) + H₂O	+0.56
Au [AuI₂]⁻ + e⁻ ⇄ Au(s) + 2 I⁻	+0.58
MnO₄⁻ + 2 H₂O + 3 e⁻ ⇄ MnO₂(s) + 4 OH⁻	+0.59
S₂O₃^2 − + 6 H⁺ + 4 e⁻ ⇄ 2 S(s) + 3 H₂O	+0.60
Mo H₂MoO₄(aq) + 2 H⁺ + 2 e⁻ ⇄ MoO₂(s) + 2 H₂O	+0.65
C + 2 H⁺ + 2 e⁻ ⇄	+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]
Se 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
N NO₃⁻(aq) + 2 H⁺ + e⁻ ⇄ NO₂(g) + H₂O	+0.80
Au [AuBr₄]⁻ + 3 e⁻ ⇄ Au(s) + 4 Br⁻	+0.85
Hg²⁺ + 2 e⁻ ⇄ Hg(l)	+0.85
MnO₄⁻ + H⁺ + e⁻ ⇄ HMnO₄⁻	+0.90
Hg 2 Hg²⁺ + 2 e⁻ ⇄ Hg₂²⁺	+0.91	^[1]
Pd²⁺ + 2 e⁻ ⇄ Pd(s)	+0.915	^[4]
Au [AuCl₄]⁻ + 3 e⁻ ⇄ Au(s) + 4 Cl⁻	+0.93
MnO₂(s) + 4 H⁺ + e⁻ ⇄ Mn³⁺ + 2 H₂O	+0.95
Au [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]
I IO₃⁻ + 5 H⁺ + 4 e⁻ ⇄ HIO(aq) + 2 H₂O	+1.13
Au [AuCl₂]⁻ + e⁻ ⇄ Au(s) + 2 Cl⁻	+1.15
Se 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
I 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]
Cr₂O₇^− − + 14 H⁺ + 6 e⁻ ⇄ 2 Cr³⁺ + 7 H₂O	+1.33
CoO₂(s) + 4 H⁺ + e⁻ ⇄ Co³⁺ + 2 H₂O	+1.42
N 2 NH₃OH⁺ + H⁺ + 2 e⁻ ⇄ N₂H₅⁺ + 2 H₂O	+1.42	^[3]
I 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
PbO β-PbO₂(s) + 4 H⁺ + 2 e⁻ ⇄ Pb²⁺ + 2 H₂O	+1.460	^[1]
PbO α-PbO₂(s) + 4 H⁺ + 2 e⁻ ⇄ Pb²⁺ + 2 H₂O	+1.468	^[1]
Br 2 BrO₃⁻ + 12 H⁺ + 10 e⁻ ⇄ Br₂(l) + 6 H₂O	+1.48
Cl 2ClO₃⁻ + 12 H⁺ + 10 e⁻ ⇄ Cl₂(g) + 6 H₂O	+1.49
MnO₄⁻ + 8 H⁺ + 5 e⁻ ⇄ Mn²⁺ + 4 H₂O	+1.51
O 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
Cl 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
Cl 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
O 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]
Mn 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]

^ ^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 Q10_ox / Coenzyme Q10_red	+0.06^[7]
Cytochrome bc₁ complex	Cytochrome b_ox / Cytochrome b_red	+0.12^[7]
Complex IV	Cytochrome c_ox / Cytochrome c_red	+0.22^[7]
Complex IV	Cytochrome a_ox / Cytochrome a_red	+0.29^[7]
Complex IV	O₂ / HO^-	+0.82^[7]

[edit] References

^ ^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).
^ ^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 Vanýsek, Petr (2007). “Electrochemical Series”, in Handbook of Chemistry and Physics: 88^th Edition (Chemical Rubber Company).
^ ^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
^ ^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).
^ ^a ^b Marcel Pourbaix (1966). Atlas of Electrochemical Equilibria in Aqueous Solutions (NACE International, Houston, Texas; Cebelcor, Brussels).
^ ^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).
^ ^a ^b ^c ^d ^e ^f ^g Medical CHEMISTRY Compendium. By Anders Overgaard Pedersen and Henning Nielsen. Aarhus University. 2008

[edit] See also

[rwP-6] 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.

[Bar-0] ^ ^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).

[van-1] ^ ^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 Vanýsek, Petr (2007). “Electrochemical Series”, in Handbook of Chemistry and Physics: 88^th Edition (Chemical Rubber Company).

[Gre-2] Greenwood, Norman N.; Earnshaw, A. (1997), Chemistry of the Elements (2nd ed.), Oxford: Butterworth-Heinemann, ISBN 0-7506-3365-4

[Bar2-3] ^ ^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).

[Pou-4] Marcel Pourbaix (1966). Atlas of Electrochemical Equilibria in Aqueous Solutions (NACE International, Houston, Texas; Cebelcor, Brussels).

[Atk-5] ^ ^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).

[Ped-7] ^ ^a ^b ^c ^d ^e ^f ^g Medical CHEMISTRY Compendium. By Anders Overgaard Pedersen and Henning Nielsen. Aarhus University. 2008

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Standard electrode potential (data page)

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