Dados de potencial de eletrodo padrão
Os valores de potencial de eletrodo padrão são dados na tabela abaixo em volts relativos ao eletrodo de hidrogênio padrão e sob as seguintes condições:
A uma temperatura de 298.15 K (25 °C);
A uma concentração efetiva de 1 mol/L em solução aquosa para cada espécie ou uma espécie em amálgama de mercúrio;
A uma pressão parcial de 101.325 kPa (absoluta) (1 atm, 1.01325 bar) para cada reagente gasoso. Esta pressão é usada porque a maior parte dos dados da literatura são ainda fornecidos neste valor que para o padrão atual de 100 kPa.
Uma atividade de unidade para cada sólido puro, líquido puro, ou para água (solvente).
Legenda: (s) – sólido; (l) – líquido; (g) – gás; (aq) – aquoso (padrão para todas as espécies carregadas); (Hg) – amalgama.
Semi-reação
Sr+ + e− ⇄ Sr+
Ca+ + e− ⇄ Ca
Pr3+ + e− ⇄ Pr2+
3⁄2 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)
Ca(OH)2 + 2 e− ⇄ Ca + 2 OH-
Er3+ + e− ⇄ Er2+
Ba(OH)2 + 2 e− ⇄ Ba + 2 OH-
Rb+ + e− ⇄ Rb(s)
K+ + e− ⇄ K(s)
Ba2+ + 2 e− ⇄ Ba(s)
La(OH)3(s) + 3 e− ⇄ La(s) + 3 OH−
Fr+ + e− ⇄ Fr
Sr2+ + 2 e− ⇄ Sr(s)
Sr(OH)2 + 2 e− ⇄ Sr + 2 OH-
Ca2+ + 2 e− ⇄ Ca(s)
Eu2+ + 2 e− ⇄ Eu(s)
Ra2+ + 2 e− ⇄ Ra(s)
Ho3+ + e− ⇄ Ho2+
Bk3+ + e− ⇄ Bk2+
Yb2+ + 2 e− ⇄ Yb
Na+ + e− ⇄ Na(s)
Mg+ + e− ⇄ Mg
Nd3+ + e− ⇄ Nd2+
Mg(OH)2 + 2 e− ⇄ Mg + 2 OH-
Sm2+ + 2 e− ⇄ Sm
Be2O32- + 3 H2O + 4 e− ⇄ 2 Be + 6 OH-
Pm3+ + e− ⇄ Pm2+
Dy3+ + e− ⇄ Dy2+
No2+ + 2 e− ⇄ No
HfO(OH)2 + H2O + 4 e− ⇄ Hf + 4 OH-
Th(OH)4 + 4 e− ⇄ Th + 4 OH-
Md2+ + 2 e− ⇄ Md
Tm2+ + 2 e− ⇄ Tm
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−
Pr3+ + 3 e− ⇄ Pr
Ce3+ + 3 e− ⇄ Ce
Er3+ + 3 e− ⇄ Er
Ho3+ + 3 e− ⇄ Ho
H2AlO3- + H2O + 3 e− ⇄ Al + 4 OH-
Nd3+ + 3 e− ⇄ Nd
Tm3+ + 3 e− ⇄ Tm
Al(OH)4− + 3 e− ⇄ Al(s) + 4 OH−
Al(OH)3(s) + 3 e− ⇄ Al(s) + 3 OH−
Sm3+ + 3 e− ⇄ Sm
Fm2+ + 2 e− ⇄ Fm
Am3+ + e− ⇄ Am2+
Dy3+ + 3 e− ⇄ Dy
Lu3+ + 3 e− ⇄ Lu
Tb3+ + 3 e− ⇄ Tb
Gd3+ + 3 e− ⇄ Gd
H2(g) + 2 e− ⇄ 2 H−
Es2+ + 2 e− ⇄ Es
Pm2+ + 2 e− ⇄ Pm
Tm3+ + e− ⇄ Tm2+
Dy2+ + 2 e− ⇄ Dy
Ac3+ + 3 e− ⇄ Ac(s)
Yb3+ + 3 e− ⇄ Yb
Cf2+ + 2 e− ⇄ Cf
Nd2+ + 2 e− ⇄ Nd
Ho2+ + 2 e− ⇄ Ho
Sc3+ + 3 e− ⇄ Sc(s)
AlF63- + 3 e− ⇄ Al + 6 F-
Am3+ + 3 e− ⇄ Am
Cm3+ + 3 e− ⇄ Cm
Pu3+ + 3 e− ⇄ Pu
Pr2+ + 2 e− ⇄ Pr
Er2+ + 2 e− ⇄ Er
Eu3+ + 3 e− ⇄ Eu
Lr3+ + 3 e− ⇄ Lr
Cf3+ + 3 e− ⇄ Cf
Es3+ + 3 e− ⇄ Es
Pa4+ + e− ⇄ Pa3+
Am2+ + 2 e− ⇄ Am
Th4+ + 4 e− ⇄ Th
Fm3+ + 3 e− ⇄ Fm
Np3+ + 3 e− ⇄ Np
Be2+ + 2 e− ⇄ Be(s)
H2PO2- + e− ⇄ P + 2 OH-
U3+ + 3 e− ⇄ U(s)
Sr2+ + 2 e− ⇄ Sr/Hg[nota 4]
H2BO3- + H2O + 3 e− ⇄ B + 4 OH-
ThO2 + 4H+ + 4 e− ⇄ Th + 2 H2O
HfO2+ + 2 H+ + 4 e− ⇄ Hf + H2O
HPO32- + 2 H2O + 3 e− ⇄ P + 5 OH-
SiO32- + H2O + 4 e− ⇄ Si + 6 OH-
Al3+ + 3 e− ⇄ Al(s)
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
Ti2O3(s) + 2 H+ + 2 e− ⇄ 2 TiO(s) + H2O
Zn(OH)42− + 2 e− ⇄ Zn(s) + 4 OH−
Mn2+ + 2 e− ⇄ Mn(s)
Fe(CN)64− + 6 H+ + 2 e− ⇄ Fe(s) + 4HCN(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
Zn2+ + 2 e− ⇄ Zn(Hg)[nota 4]
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) + H2O + 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(branco)[nota 2] + 2 H2O
H3PO3(aq) + 2 H+ + 2 e− ⇄ H3PO2(aq) + H2O
H3PO3(aq) + 3 H+ + 3 e− ⇄ P(vermelho)[nota 2] + 3 H2O
Fe2+ + 2 e− ⇄ Fe(s)
2 CO2(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−
PbSO4(s) + 2 e− ⇄ Pb(s) + SO42−
PbSO4(s) + 2 e− ⇄ Pb(Hg) + SO42−
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) + H2O
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)
O2(g) + H+ + e− ⇄ HO2•(aq)
Pb2+ + 2 e− ⇄ Pb(s)
WO2(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)
CO2(g) + 2 H+ + 2 e− ⇄ CO(g) + H2O
SnO(s) + 2 H+ + 2 e− ⇄ Sn(s) + H2O
SnO2(s) + 2 H+ + 2 e− ⇄ SnO(s) + H2O
WO3(aq) + 6 H+ + 6 e− ⇄ W(s) + 3 H2O
P(branco) + 3 H+ + 3 e− ⇄ PH3(g)
Fe3+ + 3 e− ⇄ Fe(s)
HCOOH(aq) + 2 H+ + 2 e− ⇄ HCHO(aq) + H2O
2 H+ + 2 e− ⇄ H2(g)
AgBr(s) + e− ⇄ Ag(s) + Br−
S4O62− + 2 e− ⇄ 2 S2O32−
Fe3O4(s) + 8 H+ + 8 e− ⇄ 3 Fe(s) + 4 H2O
N2(g) + 2 H2O + 6 H+ + 6 e− ⇄ 2 NH4OH(aq)
HgO(s) + H2O + 2 e− ⇄ Hg(l) + 2 OH−
Cu(NH3)42+ + e− ⇄ Cu(NH3)2+ + 2 NH3
Ru(NH3)63+ + e− ⇄ Ru(NH3)62+
N2H4(aq) + 4 H2O + 2 e− ⇄ 2 NH4+ + 4 OH−
H2MoO4(aq) + 6 H+ + 6 e− ⇄ Mo(s) + 4 H2O
Ge4+ + 4 e− ⇄ Ge(s)
C(s) + 4 H+ + 4 e− ⇄ CH4(g)
HCHO(aq) + 2 H+ + 2 e− ⇄ CH3OH(aq)
S(s) + 2 H+ + 2 e− ⇄ H2S(g)
Sn4+ + 2 e− ⇄ Sn2+
Cu2+ + e− ⇄ Cu+
HSO4− + 3 H+ + 2 e− ⇄ SO2(aq) + 2 H2O
UO22+ + e− ⇄ UO2+
SO42− + 4 H+ + 2 e− ⇄ SO2(aq) + 2 H2O
TiO2+ + 2 H+ + e− ⇄ Ti3+ + H2O
SbO+ + 2 H+ + 3 e− ⇄ Sb(s) + H2O
AgCl(s) + e− ⇄ Ag(s) + Cl−
H3AsO3(aq) + 3 H+ + 3 e− ⇄ As(s) + 3 H2O
GeO(s) + 2 H+ + 2 e− ⇄ Ge(s) + H2O
UO2+ + 4 H+ + e− ⇄ U4+ + 2 H2O
Re3+ + 3 e− ⇄ Re(s)
Bi3+ + 3 e− ⇄ Bi(s)
VO2+ + 2 H+ + e− ⇄ V3+ + H2O
Cu2+ + 2 e− ⇄ Cu(s)
[Fe(CN)6]3− + e− ⇄ [Fe(CN)6]4−
O2(g) + 2 H2O + 4 e− ⇄ 4 OH−(aq)
H2MoO4 + 6 H+ + 3 e− ⇄ Mo3+ + 2 H2O
CH3OH(aq) + 2 H+ + 2 e− ⇄ CH4(g) + H2O
SO2(aq) + 4 H+ + 4 e− ⇄ S(s) + 2 H2O
Cu+ + e− ⇄ Cu(s)
CO(g) + 2 H+ + 2 e− ⇄ C(s) + H2O
I3− + 2 e− ⇄ 3 I−
I2(s) + 2 e− ⇄ 2 I−
[AuI4]− + 3 e− ⇄ Au(s) + 4 I−
H3AsO4(aq) + 2 H+ + 2 e− ⇄ H3AsO3(aq) + H2O
[AuI2]− + e− ⇄ Au(s) + 2 I−
MnO4− + 2 H2O + 3 e− ⇄ MnO2(s) + 4 OH−
S2O32 − + 6 H+ + 4 e− ⇄ 2 S(s) + 3 H2O
Fc+[nota 3] + e− ⇄ Fc(s)
H2MoO4(aq) + 2 H+ + 2 e− ⇄ MoO2(s) + 2 H2O
E° (V)[nota 1]
−3.80
−3.80
−3.1
−3.09
−3.0401
−3.04
−3.026
−3.02
−3.0
−2.99
−2.98
−2.931
−2.912
−2.90
−2.9
−2.899
−2.88
−2.868
−2.812
−2.8
−2.8
−2.8
−2.76
−2.71
−2.70
−2.7
−2.690
−2.68
−2.63
−2.6
−2.6
−2.50
−2.50
−2.48
−2.40
−2.4
−2.379
−2.372
−2.372
−2.36
−2.353
−2.336
−2.331
−2.33
−2.33
−2.323
−2.319
−2.33
−2.31
−2.304
−2.30
−2.3
−2.295
−2.28
−2.28
−2.279
−2.23
−2.23
−2.2
−2.2
−2.2
−2.20
−2.19
−2.12
−2.1
−2.1
−2.077
−2.069
−2.048
−2.04
−2.031
−2.0
−2.0
−1.991
−1.96
−1.94
−1.91
−1.9
−1.9
−1.899
−1.89
−1.856
−1.847
−1.82
−1.798
−1.793
−1.79
−1.789
−1.724
−1.71
−1.697
−1.662
−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
−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
−0.3505
−0.35
−0.34
−0.34
−0.29
−0.28
−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
−0.11
−0.10
−0.09
−0.09
-0.063
−0.04
−0.03
0.0000
+0.07133
+0.08
+0.085
+0.092
+0.0977
+0.10
+0.10
+0.11
+0.11
+0.12
+0.12
+0.13
+0.14
+0.15
+0.159
+0.16
+0.163
+0.17
+0.19
+0.20
+0.22233
+0.24
+0.26
+0.273
+0.300
+0.308
+0.34
+0.340
+0.36
+0.40
+0.43
+0.50
+0.50
+0.520
+0.52
+0.53
+0.54
+0.56
+0.56
+0.58
+0.59
+0.60
+0.641
+0.65
+0.6992
+0.70
+0.72
+0.726
+0.74
+0.758
+0.77
+0.7996
+0.80
+0.80
+0.81
+0.85
+0.85
+0.87
+0.90
+0.91
+0.915
+0.93
+0.95
+0.96
+0.99
+1.02
+1.066
+1.0873
+1.13
+1.15
+1.15
+1.17
+1.18
+1.18
+1.188
+1.19
+1.20
+1.20
+1.229
+1.23
+1.24
+1.25
+1.33
+1.36
+1.42
+1.42
+1.44
+1.44
+1.45
+1.460
+1.468
+1.48
+1.49
+1.51
+1.51
+1.52
+1.59
+1.63
+1.67
+1.67
+1.69
+1.70
+1.77
+1.78
+1.82
+1.83
+1.85
+1.98
+2.010
+2.075
+2.09
+2.12
+2.18
+2.20
+2.32
+2.42
+2.87
+3.05
Ref.
[1]
[1]
[1]
[2][3]
[3][4]
[2]
[3]
[1]
[1]
[1]
[3]
[3]
[3]
[3]
[1]
[3]
[1]
[3]
[3]
[3]
[1]
[1]
[1]
[3][5]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[3]
[3]
[3]
[3]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[6]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[1]
[7]
[7]
[7]
[8]
[7]
[7]
[9]
[10]
[10]
[9]
[9]
[7]
[7]
[7]
[7]
[11]
[7]
[7]
[7]
[5]
[5]
[7]
[7]
[7]
[11]
[10]
[10]
[7]
[7]
[5]
[10]
[7]
[5]
[7]
[10]
[7]
[9]
≡ 0
[7]
[12]
[10]
[11]
[2]
[10]
[10]
[5]
[7]
[11]
[7]
[10]
[5]
[10]
[5]
[5]
[13]
[7]
[11]
[11]
[7]
[9]
[4]
[10]
[11]
[14]
[15]
[7]
[7]
[14]
[11]
[5]
[14]
[5]
[2]
[10]
[10]
[10]
[10]
[10]
[7]
[11]
[14]
[14]
[16]
[14]
[14]
[10][5][4]
[10]
* + 2 H+ + 2 e− ⇄
O2(g) + 2 H+ + 2 e− ⇄ H2O2(aq)
Tl3+ + 3 e− ⇄ Tl(s)
PtCl62− + 2 e− ⇄ PtCl42− + 2 Cl−
H2SeO3(aq) + 4 H+ + 4 e− ⇄ Se(s) + 3 H2O
PtCl42− + 2 e− ⇄ Pt(s) + 4 Cl−
Fe3+ + e− ⇄ Fe2+
Ag+ + e− ⇄ Ag(s)
Hg22+ + 2 e− ⇄ 2 Hg(l)
NO3−(aq) + 2 H+ + e− ⇄ NO2(g) + H2O
FeO42− + 5 H2O + 6 e− ⇄ Fe2O3(s) + 10 OH−
[AuBr4]− + 3 e− ⇄ Au(s) + 4 Br−
Hg2+ + 2 e− ⇄ Hg(l)
[IrCl6]2- + e− ⇄ [IrCl6]3-
MnO4− + H+ + e− ⇄ HMnO4−
2 Hg2+ + 2 e− ⇄ Hg22+
Pd2+ + 2 e− ⇄ Pd(s)
[AuCl4]− + 3 e− ⇄ Au(s) + 4 Cl−
MnO2(s) + 4 H+ + e− ⇄ Mn3+ + 2 H2O
[AuBr2]− + e− ⇄ Au(s) + 2 Br−
[HXeO6]3− + 2 H2O + 2 e− + ⇄ [HXeO4]− + 4 OH−
H6TeO6(aq) + 2 H+ + 2 e− ⇄ TeO2(s) + 4 H2O
Br2(l) + 2 e− ⇄ 2 Br−
Br2(aq) + 2 e− ⇄ 2 Br−
IO3− + 5 H+ + 4 e− ⇄ HIO(aq) + 2 H2O
[AuCl2]− + e− ⇄ Au(s) + 2 Cl−
HSeO4− + 3 H+ + 2 e− ⇄ H2SeO3(aq) + H2O
Ag2O(s) + 2 H+ + 2 e− ⇄ 2 Ag(s) + H2O
ClO3− + 2 H+ + e− ⇄ ClO2(g) + H2O
[HXeO6]3− + 5 H2O + 8 e− ⇄ Xe(g) + 11 OH−
Pt2+ + 2 e− ⇄ Pt(s)
ClO2(g) + H+ + e− ⇄ HClO2(aq)
2 IO3− + 12 H+ + 10 e− ⇄ I2(s) + 6 H2O
ClO4− + 2 H+ + 2 e− ⇄ ClO3− + H2O
O2(g) + 4 H+ + 4 e− ⇄ 2 H2O
MnO2(s) + 4 H+ + 2 e− ⇄ Mn2+ + 2 H2O
[HXeO4]− + 3 H2O + 6 e− ⇄ Xe(g) + 7 OH−
Tl3+ + 2 e− ⇄ Tl+
Cr2O72− + 14 H+ + 6 e− ⇄ 2 Cr3+ + 7 H2O
Cl2(g) + 2 e− ⇄ 2 Cl−
CoO2(s) + 4 H+ + e− ⇄ Co3+ + 2 H2O
2 NH3OH+ + H+ + 2 e− ⇄ N2H5+ + 2 H2O
2 HIO(aq) + 2 H+ + 2 e− ⇄ I2(s) + 2 H2O
Ce4+ + e− ⇄ Ce3+
BrO3− + 5 H+ + 4 e− ⇄ HBrO(aq) + 2 H2O
β-PbO2(s) + 4 H+ + 2 e− ⇄ Pb2+ + 2 H2O
α-PbO2(s) + 4 H+ + 2 e− ⇄ Pb2+ + 2 H2O
2 BrO3− + 12 H+ + 10 e− ⇄ Br2(l) + 6 H2O
2ClO3− + 12 H+ + 10 e− ⇄ Cl2(g) + 6 H2O
MnO4− + 8 H+ + 5 e− ⇄ Mn2+ + 4 H2O
HO2• + H+ + e− ⇄ H2O2(aq)
Au3+ + 3 e− ⇄ Au(s)
NiO2(s) + 4 H+ + 2 e− ⇄ Ni2+ + 2 OH−
2 HClO(aq) + 2 H+ + 2 e− ⇄ Cl2(g) + 2 H2O
Ag2O3(s) + 6 H+ + 4 e− ⇄ 2 Ag+ + 3 H2O
HClO2(aq) + 2 H+ + 2 e− ⇄ HClO(aq) + H2O
Pb4+ + 2 e− ⇄ Pb2+
MnO4− + 4 H+ + 3 e− ⇄ MnO2(s) + 2 H2O
AgO(s) + 2 H+ + e− ⇄ Ag+ + H2O
H2O2(aq) + 2 H+ + 2 e− ⇄ 2 H2O
Co3+ + e− ⇄ Co2+
Au+ + e− ⇄ Au(s)
BrO4− + 2 H+ + 2 e− ⇄ BrO3− + H2O
Ag2+ + e− ⇄ Ag+
S2O82− + 2 e− ⇄ 2 SO42−
O3(g) + 2 H+ + 2 e− ⇄ O2(g) + H2O
HMnO4− + 3 H+ + 2 e− ⇄ MnO2(s) + 2 H2O
XeO3(aq) + 6 H+ + 6 e− ⇄ Xe(g) + 3 H2O
H4XeO6(aq) + 8 H+ + 8 e− ⇄ Xe(g) + 6 H2O
FeO42− + 3 e− + 8 H+ ⇄ Fe3+ + 4 H2O
XeF2(aq) + 2 H+ + 2 e− ⇄ Xe(g) + 2HF(aq)
H4XeO6(aq) + 2 H+ + 2 e− ⇄ XeO3(aq) + H2O
F2(g) + 2 e− ⇄ 2 F−
F2(g) + 2 H+ + 2 e− ⇄ 2 HF(aq)
Notas
1. Para localizar um potencial, use o comando CTRL-F do teclado.
2. Não especificado na referência indicada, mas assumida devido à diferença entre o valor −0.454 e que é calculado por (2×−0.499 + −0.508)/3 = −0.502 exatamente coincidindo com a diferença entre os valores para as variedades alotrópicas de fósforo branca (−0.063) e vermelha (−0.111) em equilíbrio com PH3.
3: Ferroceno Fe(C5H5)2 - Ferroceno - Wikipedia
4. Amálgama de mercúrio.
Referências
1. Lide, David R., ed. (2006). CRC Handbook of Chemistry and Physics (87th ed.). Boca Raton, FL: CRC Press. ISBN 0-8493-0487-3.
2. Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth–Heinemann. ISBN 0080379419.
3. Vanýsek, Petr (2011). “Electrochemical Series”, in Handbook of Chemistry and Physics: 92nd Edition (Chemical Rubber Company).
4. Atkins, Peter (2010). Inorganic Chemistry (5th Edition). New York: W. H. Freeman and Company. p. 153. ISBN 978–1–42–921820–7.
5. Peter Atkins (1997). Physical Chemistry, 6th edition (W.H. Freeman and Company, New York).
6. David R. Lide, ed., CRC Handbook of Chemistry and Physics, Internet Version 2005, www.hbcpnetbase.com , CRC Press, Boca Raton, FL, 2005.
7. Vanýsek, Petr (2012). "Electrochemical Series". In Haynes, William M. Handbook of Chemistry and Physics: 93rd Edition. Chemical Rubber Company. p. 5-80.ISBN 9781439880494..
8. Gordon Aylward & Tristan Findlay (2008). "SI Chemical Data", 6th edition (John Wiley & Sons, Australia), ISBN 978-0-470-81638-7.
9. WebElements Periodic Table of the Elements | Iron | compounds information
10. Bard, A. J., Parsons, R., and Jordan, J. (1985). Standard Potentials in Aqueous Solutions (Marcel Dekker, New York).
11. Bard, A.J., Faulkner, L.R.(2001). Electrochemical Methods. Fundamentals and Applications, 2nd edition (John Wiley and Sons Inc).
12. Marcel Pourbaix (1966). Atlas of Electrochemical Equilibria in Aqueous Solutions (NACE International, Houston, Texas; Cebelcor, Brussels).
13. Connelly, Neil G.; Geiger, William E. (1 January 1996). "Chemical Redox Agents for Organometallic Chemistry". Chemical Reviews 96 (2): 877–910. doi:10.1021/cr940053x. PMID 11848774.
14. WebElements Periodic Table of the Elements | Xenon | compounds information
15. Cotton, F. Albert; Wilkinson, Geoffrey; Murillo, Carlos A.; Bochmann, Manfred (1999), Advanced Inorganic Chemistry (6th ed.), New York: Wiley-Interscience, ISBN 0-471-19957-5
16. Redox Reactions, Western Oregon University website
Sugestões para consulta
Standard Reduction Potentials - www.jesuitnola.org
Standard Electrode Potentials in Aqueous Solution at 25°C - hyperphysics.phy-astr.gsu.edu