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Table Of Standard Reduction Potentials

Written By Monday, October 17, 2022 Add Comment Edit

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The data values of standard electrode potentials (Due east°) are given in the table beneath, in volts relative to the standard hydrogen electrode, and are for the following conditions:

  • A temperature of 298.15 K (25.00 °C; 77.00 °F).
  • An effective concentration of 1 mol/50 for each aqueous species or a species in a mercury constructing (an alloy of mercury with another metal).
  • A partial pressure of 101.325 kPa (accented) (1 atm, i.01325 bar) for each gaseous reagent. This force per unit area is used because most literature data are still given for this value (i atm) rather than for the current standard of 100 kPa (1 bar) presently considered in the standard country.
  • An activity of unity for each pure solid, pure liquid, or for water (solvent). The relation in electrode potential of metals in saltwater (as electrolyte) is given in the galvanic series.
  • Although many of the half cells are written for multiple-electron transfers, the tabulated potentials are for a unmarried-electron transfer. All of the reactions should be divided past the stoichiometric coefficient for the electron to get the corresponding corrected reaction equation. For example, the equation Fe2+ + 2 east − ⇌ Fe(s) (–0.44 5) means that it requires two × 0.44 eV = 0.88 eV of free energy to exist absorbed (hence the minus sign) in guild to create ane neutral cantlet of Fe(s) from one Fetwo+ ion and 2 electrons, or 0.44 eV per electron, which is 0.44 J/C of electrons, which is 0.44 V.
  • Later on dividing by the number of electrons, the standard potential E° is related to the standard Gibbs costless energy of formation ΔGf° by:

    E = ∑ Δ Chiliad left − ∑ Δ G right F {\displaystyle E={\frac {\sum \Delta G_{\text{left}}-\sum \Delta G_{\text{right}}}{F}}}

    where F is the Faraday constant. For example, in the equation Fetwo+ + two e − ⇌ Iron(s) (–0.44 V), the Gibbs free energy required to create one neutral atom of Fe(southward) from 1 Atomic number 262+ ion and two electrons is 2 × 0.44 eV = 0.88 eV, or 84 895 J/mol of electrons, which is just the Gibbs energy of formation of an Fe2+ ion, since the energies of formation of e − and Fe(s) are both nil.
The Nernst equation will and then give potentials at concentrations, pressures, and temperatures other than standard.
  • Note that the table may lack consistency due to information from dissimilar sources. For example:
Cu +
+ east − ⇌ Cu(s) (Eastward
ane = +0.520 Five)
Cuii+ + ii e − ⇌ Cu(s) (Eastward
2 = +0.337 Five)
Cu2+ + due east − ⇌ Cu +
(East
iii = +0.159 V)
Calculating the potential using Gibbs free energy (E
3 = 2Due east
ii – East
1 ) gives the potential for East
iii as 0.154 V, not the experimental value of 0.159 V.

Table of standard electrode potentials [edit]

Legend: (s) – solid; (l) – liquid; (chiliad) – gas; (aq) – aqueous (default for all charged species); (Hg) – amalgam; assuming – water electrolysis equations.

Element Half-reaction E° / V Electrons Ref.
Oxidant ⇌ Reductant
& -9
Zz 9
Sr Sr +
+ e − 		⇌ Sr(south) -iv.101 1 [1]
Ca Ca +
+ e − 		⇌ Ca(s) -3.8 i [ane]
Th Th iv+
+ e − 		⇌ Th three+
-3.half-dozen 1 [2]
Pr Pr iii+
+ e − 		⇌ Pr 2+
-3.1 ane [i]
Due north threeN
2 (one thousand) + 2H+ + 2 e − 		⇌ 2HN
iii (aq) 		-3.09 2 [3] [iv]
Li Li +
+ e − 		⇌ Li(s) -3.0401 i [4] [5]
Due north North
2 (g) + fourHtwoO + 2 e − 		⇌ twoNH
ii OH(aq) + twoOH− 		-3.04 2 [three]
Cs Cs +
+ e − 		⇌ Cs(s) -3.026 1 [four]
Ca Ca(OH)
2 + ii due east − 		⇌ Ca(s) + 2OH− -3.02 ii [one]
Er Er 3+
+ e − 		⇌ Er 2+
-iii i [i]
Ba Ba(OH)
2 + ii e − 		⇌ Ba(south) + 2OH− -two.99 2 [1]
Rb Rb +
+ e − 		⇌ Rb(s) -ii.98 one [four]
Chiliad 1000 +
+ east − 		⇌ K(s) -ii.931 ane [4]
Ba Ba two+
+ 2 east − 		⇌ Ba(s) -2.912 ii [4]
La La(OH)
iii (south) + 3 east − 		⇌ La(s) + 3OH− -two.ix three [4]
Fr Fr +
+ e − 		⇌ Fr(s) -2.9 ane [1]
Sr Sr 2+
+ two e − 		⇌ Sr(south) -2.899 2 [four]
Sr Sr(OH)
2 + 2 e − 		⇌ Sr(south) + iiOH− -two.88 ii [1]
Ca Ca two+
+ ii e − 		⇌ Ca(south) -2.868 2 [4] [5]
Li Li +
+ C
6 (s) + eastward − 		⇌ LiC
6 (due south) 		-2.84 1 [iv]
Eu Eu ii+
+ 2 eastward − 		⇌ Eu(s) -2.812 2 [4]
Ra Ra 2+
+ 2 e − 		⇌ Ra(s) -2.8 two [four]
Ho Ho iii+
+ e − 		⇌ Ho2+ -2.8 i [1]
Bk Bk three+
+ e − 		⇌ Bk 2+
-2.8 1 [1]
Yb Yb 2+
+ 2 e − 		⇌ Yb(s) -2.76 2 [1]
Na Na +
+ e − 		⇌ Na(s) -2.71 1 [four] [six]
Mg Mg +
+ due east − 		⇌ Mg(southward) -two.7 i [1]
Nd Nd 3+
+ e − 		⇌ Nd 2+
-2.seven 1 [1]
Mg Mg(OH)
2 + two e − 		⇌ Mg(s) + iiOH− -ii.69 2 [i]
Sm Sm 2+
+ 2 e − 		⇌ Sm(south) -2.68 2 [1]
Be Be
2 O ii−
3 + iiiH2O + 4 eastward − 		⇌ 2Be(south) + sixOH− -2.63 4 [1]
Pm Pm three+
+ e − 		⇌ Pm ii+
-ii.half dozen i [1]
Dy Dy 3+
+ e − 		⇌ Dy 2+
-ii.half dozen ane [1]
No No 2+
+ 2 due east − 		⇌ No -two.5 2 [1]
Hf HfO(OH)
ii + HtwoO + 4 e − 		⇌ Hf(s) + 4OH− -2.5 4 [i]
Thursday Thursday(OH)
4 + 4 e − 		⇌ Th(s) + fourOH− -2.48 iv [1]
Md Md 2+
+ 2 eastward − 		⇌ Doctor -2.4 2 [i]
Tm Tm ii+
+ 2 e − 		⇌ Tm(s) -2.iv 2 [1]
La La iii+
+ 3 e − 		⇌ La(s) -2.379 3 [4]
Y Y 3+
+ three e − 		⇌ Y(s) -2.372 3 [4]
Mg Mg two+
+ 2 e − 		⇌ Mg(s) -2.372 2 [4]
Zr ZrO(OH)
ii (s) + HtwoO + 4 eastward − 		⇌ Zr(s) + fourOH− -2.36 4 [four]
Pr Pr three+
+ 3 eastward − 		⇌ Pr(southward) -two.353 3 [ane]
Ce Ce three+
+ 3 due east − 		⇌ Ce(southward) -2.336 3 [1]
Er Er three+
+ 3 e − 		⇌ Er(s) -2.331 three [1]
Ho Ho iii+
+ three e − 		⇌ Ho(s) -ii.33 3 [1]
Al H
two AlO −
three + H2O + three eastward − 		⇌ Al(s) + 4OH− -2.33 3 [1]
Nd Nd 3+
+ iii east − 		⇌ Nd(s) -ii.323 iii [ane]
Tm Tm 3+
+ iii e − 		⇌ Tm(s) -2.319 3 [1]
Al Al(OH)
3 (southward) + iii e − 		⇌ Al(s) + threeOH− -ii.31 3
Sm Sm 3+
+ 3 e − 		⇌ Sm(due south) -2.304 3 [1]
Fm Fmii+ + 2 due east − ⇌ Fm -2.3 2 [1]
Am Am 3+
+ e − 		⇌ Am two+
-2.three 1 [1]
Dy Dy 3+
+ iii e − 		⇌ Dy(s) -two.295 3 [ane]
Lu Lu iii+
+ 3 e − 		⇌ Lu(s) -ii.28 3 [1]
Tb Tb 3+
+ 3 e − 		⇌ Tb(s) -two.28 3 [1]
Gd Gd iii+
+ 3 e − 		⇌ Gd(s) -2.279 3 [1]
H H
2 (yard) + 2 eastward − 		⇌ 2H −
-2.23 two [ane]
Es Es 2+
+ 2 due east − 		⇌ Es(s) -ii.23 2 [i]
Pm Pm ii+
+ ii e − 		⇌ Pm(s) -two.2 two [1]
Tm Tm iii+
+ e − 		⇌ Tm2+ -two.2 1 [i]
Dy Dy 2+
+ 2 eastward − 		⇌ Dy(s) -ii.2 2 [1]
Ac Ac 3+
+ iii e − 		⇌ Ac(s) -2.2 3 [1]
Yb Yb 3+
+ iii due east − 		⇌ Yb(s) -2.19 iii [1]
Cf Cf 2+
+ 2 e − 		⇌ Cf(southward) -ii.12 2 [1]
Nd Nd 2+
+ 2 e − 		⇌ Nd(s) -2.1 2 [1]
Ho Ho 2+
+ ii e − 		⇌ Ho(s) -two.one 2 [1]
Sc Sc 3+
+ 3 due east − 		⇌ Sc(s) -2.077 iii [7]
Al AlF 3−
6 + three e − 		⇌ Al(southward) + 6F −
-2.069 3 [ane]
Am Am 3+
+ iii e − 		⇌ Am(s) -2.048 3 [1]
Cm Cm 3+
+ iii e − 		⇌ Cm(s) -two.04 3 [ane]
Pu Pu 3+
+ 3 east − 		⇌ Pu(s) -ii.031 3 [1]
Pr Pr 2+
+ 2 east − 		⇌ Pr(s) -ii 2 [1]
Er Er 2+
+ 2 eastward − 		⇌ Er(s) -2 2 [1]
Eu Eu 3+
+ 3 e − 		⇌ European union(due south) -1.991 three [i]
Lr Lr 3+
+ three e − 		⇌ Lr -1.96 three [i]
Cf Cf 3+
+ iii e − 		⇌ Cf(due south) -1.94 3 [1]
Es Es 3+
+ 3 eastward − 		⇌ Es(s) -ane.91 3 [1]
Pa Pa 4+
+ e − 		⇌ Pa 3+
-1.9 1 [1]
Am Am 2+
+ 2 e − 		⇌ Am(southward) -1.9 2 [1]
Th Thursday 4+
+ four due east − 		⇌ Th(s) -ane.899 iv [1]
Fm Fm 3+
+ 3 e − 		⇌ Fm -1.89 3 [i]
Np Np 3+
+ iii e − 		⇌ Np(s) -1.856 three [1]
Exist Be 2+
+ 2 e − 		⇌ Exist(southward) -1.847 two [i]
P H
2 PO −
ii + e − 		⇌ P(s) + iiOH− -1.82 ane [1]
U U 3+
+ 3 e − 		⇌ U(s) -1.798 iii [1]
Sr Sr two+
+ ii eastward − 		⇌ Sr(Hg) -ane.793 two [1]
B H
2 BO −
iii + HtwoO + iii e − 		⇌ B(s) + ivOH− -1.79 3 [1]
Th ThO
2 + ivH+ + 4 e − 		⇌ Th(south) + iiH2O -ane.789 4 [1]
Hf HfO 2+
+ 2H+ + iv eastward − 		⇌ Hf(s) + HiiO -1.724 4 [one]
P HPO ii−
3 + iiH2O + 3 e − 		⇌ P(s) + 5OH− -one.71 iii [1]
Si SiO 2−
iii + iiiH2O + four eastward − 		⇌ Si(s) + 6OH− -1.697 4 [1]
Al Al 3+
+ 3 e − 		⇌ Al(due south) -1.662 3 [ane]
Ti Ti 2+
+ two e − 		⇌ Ti(southward) -i.63 2 [six]
Zr ZrO
ii (s) + ivH+ + 4 e − 		⇌ Zr(s) + 2H2O -ane.553 4 [8]
Zr Zr 4+
+ 4 eastward − 		⇌ Zr(southward) -1.45 iv [8]
Ti Ti 3+
+ 3 e − 		⇌ Ti(south) -1.37 3 [9]
Ti TiO(s) + twoH+ + ii east − ⇌ Ti(s) + HiiO -1.31 2
Ti Ti
two O
3 (due south) + 2H+ + two e − 		⇌ 2TiO(south) + H2O -1.23 2
Zn Zn(OH) 2−
4 + 2 east − 		⇌ Zn(s) + 4OH− -ane.199 ii [8]
Mn Mn 2+
+ 2 e − 		⇌ Mn(southward) -i.185 ii [8]
Atomic number 26 Fe(CN) 4−
6 + 6H+ + two e − 		⇌ Fe(s) + 6HCN(aq) -1.16 2 [10]
Te Te(s) + 2 east − ⇌ Te two−
-i.143 2 [11]
V V 2+
+ 2 east − 		⇌ V(s) -1.13 two [11]
Nb Nb 3+
+ 3 e − 		⇌ Nb(s) -1.099 iii
Sn Sn(s) + ivH+ + 4 east − ⇌ SnH
4 (g) 		-1.07 4
Ti TiO two+
+ 2H+ + four eastward − 		⇌ Ti(s) + HiiO -0.93 iv
Si SiO
2 (s) + fourH+ + 4 e − 		⇌ Si(s) + 2H2O -0.91 4
B B(OH)
iii (aq) + threeH+ + 3 e − 		⇌ B(due south) + threeH2O -0.89 3
Atomic number 26 Fe(OH)
2 (southward) + two e − 		⇌ Fe(s) + iiOH− -0.89 two [x]
Fe Fe
ii O
three (due south) + 3HiiO + two e − 		⇌ iiFe(OH)
2 (s) + 2OH− 		-0.86 2 [10]
H 2H2O + 2 e − ⇌ H
2 (chiliad) + 2OH− 		-0.8277 two [viii]
Bi Bi(s) + threeH+ + 3 e − ⇌ BiH
iii 		-0.8 3 [eight]
Zn Zn two+
+ two eastward − 		⇌ Zn(Hg) -0.7628 2 [8]
Zn Zn 2+
+ 2 east − 		⇌ Zn(due south) -0.7618 2 [8]
Ta Ta
2 O
5 (s) + 10H+ + x eastward − 		⇌ 2Ta(s) + 5HiiO -0.75 10
Cr Cr 3+
+ iii eastward − 		⇌ Cr(s) -0.74 three
Ni Ni(OH)
ii (southward) + two e − 		⇌ Ni(south) + twoOH− -0.72 2 [1]
Ag Ag
2 S(s) + 2 e − 		⇌ 2Ag(s) + S 2−
(aq) 		-0.69 ii
Au [Au(CN)
2 ] −
+ e − 		⇌ Au(due south) + 2CN −
-0.half dozen 1
Ta Ta three+
+ iii e − 		⇌ Ta(s) -0.6 3
Lead PbO(southward) + HtwoO + 2 due east − ⇌ Pb(s) + 2OH− -0.58 2
Ti twoTiO
2 (s) + 2H+ + 2 east − 		⇌ Ti
2 O
three (s) + HiiO 		-0.56 ii
Ga Ga 3+
+ 3 e − 		⇌ Ga(s) -0.53 3
U U 4+
+ e − 		⇌ U iii+
-0.52 one [12]
P H
3 PO
2 (aq) + H+ + due east − 		⇌ P(white)[note i] + twoH2O -0.508 ane [eight]
P H
iii PO
iii (aq) + twoH+ + ii e − 		⇌ H
iii PO
2 (aq) + H2O 		-0.499 ii [eight]
Ni NiO
2 (s) + 2HiiO + two e − 		⇌ Ni(OH)
two (southward) + 2OH− 		-0.49 two [i]
P H
3 PO
3 (aq) + 3H+ + three e − 		⇌ P(red)[note one] + threeHiiO -0.454 3 [eight]
Cu Cu(CN) −
2 + e − 		⇌ Cu(s) + twoCN −
-0.44 1 [11]
Fe Iron 2+
+ 2 e − 		⇌ Fe(southward) -0.44 2 [6]
C 2CO
two (chiliad) + 2H+ + two e − 		⇌ HOOCCOOH(aq) -0.43 2
Cr Cr 3+
+ e − 		⇌ Cr 2+
-0.42 1
Cd Cd 2+
+ 2 e − 		⇌ Cd(s) -0.iv two [6]
Ge GeO
2 (s) + 2H+ + two east − 		⇌ GeO(south) + H2O -0.37 2
Cu Cu
2 O(south) + HiiO + 2 e − 		⇌ 2Cu(s) + 2OH− -0.36 ii [8]
Pb PbSO
4 (south) + 2 e − 		⇌ Pb(s) + And so 2−
4 		-0.3588 two [8]
Lead PbSO
4 (s) + two e − 		⇌ Pb(Hg) + So 2−
iv 		-0.3505 2 [8]
European union Eu 3+
+ due east − 		⇌ Eu 2+
-0.35 1 [12]
In In 3+
+ 3 e − 		⇌ In(southward) -0.34 iii [11]
Tl Tl +
+ e − 		⇌ Tl(s) -0.34 one [xi]
Ge Ge(s) + 4H+ + four e − ⇌ GeH
4 (g) 		-0.29 four
Co Co 2+
+ 2 e − 		⇌ Co(s) -0.28 2 [8]
P H
3 PO
4 (aq) + 2H+ + two due east − 		⇌ H
3 PO
iii (aq) + HiiO 		-0.276 2 [8]
Five V iii+
+ e − 		⇌ V ii+
-0.26 1 [6]
Ni Ni 2+
+ 2 due east − 		⇌ Ni(south) -0.25 2
As As(south) + 3H+ + 3 eastward − ⇌ AsH
iii (g) 		-0.23 three [11]
Ag AgI(south) + e − ⇌ Ag(southward) + I −
-0.15224 ane [viii]
Mo MoO
2 (s) + 4H+ + 4 e − 		⇌ Mo(s) + twoHiiO -0.fifteen 4
Si Si(s) + 4H+ + four due east − ⇌ SiH
iv (one thousand) 		-0.14 4
Sn Sn ii+
+ ii eastward − 		⇌ Sn(s) -0.xiii ii
O O
2 (g) + H+ + eastward − 		⇌ HO •
two (aq) 		-0.13 i
Lead Pb 2+
+ ii e − 		⇌ Atomic number 82(s) -0.126 two [6]
West WO
2 (southward) + 4H+ + 4 e − 		⇌ W(due south) + 2H2O -0.12 4
P P(red) + 3H+ + 3 due east − ⇌ PH
3 (g) 		-0.111 three [viii]
C CO
2 (g) + twoH+ + 2 east − 		⇌ HCOOH(aq) -0.11 2
Se Se(southward) + 2H+ + ii due east − ⇌ H
2 Se(g) 		-0.11 2
C CO
2 (g) + 2H+ + 2 e − 		⇌ CO(one thousand) + H2O -0.11 2
Cu Cu(NH
iii ) +
2 + due east − 		⇌ Cu(south) + iiNH
3 (aq) 		-0.1 ane [eleven]
Sn SnO(due south) + 2H+ + 2 eastward − ⇌ Sn(s) + H2O -0.i ii
Sn SnO
2 (s) + 2H+ + ii e − 		⇌ SnO(s) + H2O -0.09 2
West WO
3 (aq) + half-dozenH+ + 6 e − 		⇌ W(s) + 3H2O -0.09 half dozen [eleven]
Fe Atomic number 26
iii O
four (s) + 8H+ + 8 e − 		⇌ 3Fe(southward) + 4H2O -0.085 8 [xiii]
P P(white) + iiiH+ + 3 due east − ⇌ PH
3 (g) 		-0.063 3 [viii]
Fe Atomic number 26 3+
+ three due east − 		⇌ Fe(s) -0.04 3 [ten]
C HCOOH(aq) + 2H+ + 2 e − ⇌ HCHO(aq) + HtwoO -0.03 ii
H 2H+ + two eastward − ⇌ H
2 (m) 		0 ii
Ag AgBr(s) + east − ⇌ Ag(southward) + Br −
0.07133 one [viii]
South Due south
iv O 2−
half-dozen + 2 e − 		⇌ 2S
2 O 2−
3 		0.08 ii
Northward N
2 (chiliad) + 2H2O + 6H+ + 6 due east − 		⇌ 2NH
four OH(aq) 		0.092 6
Hg HgO(s) + H2O + 2 e − ⇌ Hg(l) + 2OH− 0.0977 two
Cu Cu(NH
3 ) two+
4 + e − 		⇌ Cu(NH
iii ) +
2 + 2NH
iii (aq) 		0.i i [11]
Ru Ru(NH
3 ) iii+
6 + e − 		⇌ Ru(NH
3 ) 2+
6 		0.1 ane [12]
N N
ii H
4 (aq) + 4H2O + 2 east − 		⇌ 2NH +
4 + 4OH− 		0.11 2 [three]
Mo H
2 MoO
4 (aq) + 6H+ + 6 e − 		⇌ Mo(s) + 4H2O 0.11 vi
Ge Ge four+
+ iv e − 		⇌ Ge(s) 0.12 4
C C(s) + 4H+ + 4 e − ⇌ CH
4 (1000) 		0.13 four [11]
C HCHO(aq) + twoH+ + ii e − ⇌ CH
3 OH(aq) 		0.13 2
S S(s) + 2H+ + 2 e − ⇌ H
2 Due south(1000) 		0.14 2
Sn Sn four+
+ 2 e − 		⇌ Sn 2+
0.15 2
Cu Cu ii+
+ e − 		⇌ Cu +
0.159 ane [11]
Southward HSO −
iv + iiiH+ + two e − 		⇌ SO
2 (aq) + iiH2O 		0.16 ii
U UO ii+
2 + e − 		⇌ UO +
2 		0.163 1 [12]
S SO 2−
iv + 4H+ + 2 e − 		⇌ And then
2 (aq) + 2H2O 		0.17 2
Ti TiO two+
+ twoH+ + due east − 		⇌ Ti 3+
+ H2O 		0.xix ane
Sb SbO +
+ iiH+ + 3 e − 		⇌ Sb(s) + H2O 0.2 3
Fe 3Atomic number 26
2 O
3 (s) + 2H+ + 2 e − 		⇌ 2Fe
3 O
4 (s) + HtwoO 		0.22 two [14] : p.100
Ag AgCl(southward) + due east − ⇌ Ag(s) + Cl −
0.22233 1 [8]
As H
3 AsO
3 (aq) + iiiH+ + 3 e − 		⇌ As(s) + 3H2O 0.24 3
Ru Ru 3+
(aq) + eastward − 		⇌ Ru ii+
(aq) 		0.249 ane [15]
Ge GeO(s) + 2H+ + 2 e − ⇌ Ge(s) + HtwoO 0.26 two
U UO +
2 + ivH+ + east − 		⇌ U 4+
+ 2H2O 		0.273 1 [12]
Re Re 3+
+ three e − 		⇌ Re(south) 0.iii three
Bi Bi 3+
+ 3 east − 		⇌ Bi(s) 0.308 3 [8]
Cu Cu 2+
+ 2 east − 		⇌ Cu(s) 0.337 2 [11]
V [VO] 2+
+ twoH+ + east − 		⇌ Five 3+
+ HiiO 		0.34 1
Atomic number 26 [Fe(CN)
half dozen ] 3−
+ e − 		⇌ [Fe(CN)
half-dozen ] four−
0.3704 1 [16]
Fe Fc +
+ e − 		⇌ Fc(southward) 0.4 i [17]
O O
2 (k) + 2HiiO + 4 e − 		⇌ 4OH−(aq) 0.401 four [six]
Mo H
2 MoO
iv + 6H+ + three due east − 		⇌ Mo 3+
+ 4HtwoO 		0.43 3
Ru Ru 2+
(aq) + 2 e − 		⇌ Ru 0.455 2 [15]
C CH
3 OH(aq) + 2H+ + 2 due east − 		⇌ CH
four (thousand) + HiiO 		0.five 2
S And then
2 (aq) + fourH+ + iv e − 		⇌ S(due south) + twoHiiO 0.five 4
Cu Cu +
+ due east − 		⇌ Cu(s) 0.52 1 [eleven]
C CO(thousand) + 2H+ + two eastward − ⇌ C(southward) + H2O 0.52 2
I I −
3 + two eastward − 		⇌ 3I −
0.53 2 [vi]
I I
ii (due south) + ii e − 		⇌ iiI −
0.54 2 [6]
Au [AuI
iv ] −
+ 3 e − 		⇌ Au(s) + 4I −
0.56 3
Equally H
iii AsO
4 (aq) + iiH+ + ii east − 		⇌ H
three AsO
three (aq) + HiiO 		0.56 2
Au [AuI
2 ] −
+ due east − 		⇌ Au(s) + 2I −
0.58 ane
Mn MnO −
4 + 2H2O + three eastward − 		⇌ MnO
2 (s) + fourOH− 		0.595 3 [1]
Southward S
2 O 2−
3 + 6H+ + 4 e − 		⇌ 2S(due south) + 3H2O 0.6 4
Mo H
2 MoO
4 (aq) + iiH+ + two e − 		⇌ MoO
2 (s) + twoHtwoO 		0.65 ii
C 1,4-Benzochinon.svg + 2H+ + 2 e − ⇌ Hydrochinon2.svg 0.6992 2 [8]
O O
ii (k) + iiH+ + ii e − 		⇌ H
2 O
ii (aq) 		0.7 two
Tl Tl iii+
+ 3 e − 		⇌ Tl(s) 0.72 3
Pt PtCl 2−
half-dozen + two e − 		⇌ PtCl 2−
4 + 2Cl −
0.726 ii [12]
Fe Fe
2 O
3 (south) + 6H+ + 2 e − 		⇌ twoFe 2+
+ 3H2O 		0.728 2 [xiv] : p.100
Se H
2 SeO
3 (aq) + fourH+ + 4 eastward − 		⇌ Se(s) + iiiHiiO 0.74 4
Pt PtCl 2−
four + ii e − 		⇌ Pt(s) + fourCl −
0.758 ii [12]
Atomic number 26 Atomic number 26 3+
+ e − 		⇌ Fe 2+
0.77 1
Ag Ag +
+ e − 		⇌ Ag(s) 0.7996 1 [8]
Hg Hg 2+
2 + 2 due east − 		⇌ 2Hg(l) 0.eight 2
Northward NO −
3 (aq) + iiH+ + east − 		⇌ NO
two (g) + HtwoO 		0.8 ane
Fe 2FeO 2−
4 + 5HiiO + 6 due east − 		⇌ Iron
2 O
3 (s) + tenOH− 		0.81 6 [10]
Au [AuBr
four ] −
+ 3 e − 		⇌ Au(southward) + 4Br −
0.85 3
Hg Hg ii+
+ ii e − 		⇌ Hg(fifty) 0.85 2
Ir [IrCl
half dozen ] ii−
+ e − 		⇌ [IrCl
six ] 3−
0.87 1 [5]
Mn MnO −
4 + H+ + due east − 		⇌ HMnO −
4 		0.9 1
Hg 2Hg 2+
+ 2 e − 		⇌ Hg ii+
2 		0.91 two [xi]
Pd Pd 2+
+ 2 east − 		⇌ Pd(south) 0.915 2 [12]
Au [AuCl
4 ] −
+ 3 e − 		⇌ Au(south) + 4Cl −
0.93 3
Mn MnO
2 (s) + fourH+ + e − 		⇌ Mn 3+
+ 2H2O 		0.95 1
Due north NO −
3 (aq) + 4H+ + three east − 		⇌ NO(g) + 2H2O(50) 0.958 3 [6]
Au [AuBr
2 ] −
+ due east − 		⇌ Au(s) + twoBr −
0.96 1
Iron Fe
3 O
iv (southward) + viiiH+ + 2 e − 		⇌ iiiAtomic number 26 ii+
+ fourH2O 		0.98 two [14] : p.100
Xe [HXeO
half dozen ] iii−
+ iiH2O + 2 e − 		⇌ [HXeO
4 ] −
+ ivOH− 		0.99 two [eighteen]
V [VO
2 ] +
(aq) + 2H+ + e − 		⇌ [VO] two+
(aq) + H2O 		i 1 [19]
Te H
6 TeO
6 (aq) + iiH+ + ii due east − 		⇌ TeO
2 (s) + fourH2O 		1.02 2 [nineteen]
Br Br
ii (50) + 2 e − 		⇌ 2Br −
1.066 2 [8]
Br Br
2 (aq) + ii east − 		⇌ 2Br −
1.0873 2 [8]
Ru RuO
ii + 4H+ + 2 eastward − 		⇌ Ru ii+
(aq) + 2H2O 		1.120 2 [15]
Cu Cu 2+
+ 2CN −
+ e − 		⇌ Cu(CN) −
2 		1.12 ane [11]
I IO −
3 + 5H+ + 4 e − 		⇌ HIO(aq) + 2HtwoO ane.thirteen four
Au [AuCl
2 ] −
+ e − 		⇌ Au(south) + 2Cl −
1.15 one
Se HSeO −
4 + 3H+ + 2 e − 		⇌ H
2 SeO
three (aq) + H2O 		ane.15 ii
Ag Ag
2 O(south) + iiH+ + 2 e − 		⇌ 2Ag(due south) + H2O 1.17 2
Cl ClO −
3 + 2H+ + e − 		⇌ ClO
2 (g) + H2O 		1.eighteen 1
Xe [HXeO
6 ] iii−
+ 5H2O + eight e − 		⇌ Xe(g) + 11OH− 1.18 eight [18]
Pt Pt 2+
+ ii east − 		⇌ Pt(southward) i.188 2 [12]
Cl ClO
2 (thou) + H+ + e − 		⇌ HClO
2 (aq) 		i.19 ane
I 2IO −
three + 12H+ + 10 e − 		⇌ I
2 (s) + 6H2O 		one.ii 10
Cl ClO −
4 + 2H+ + 2 e − 		⇌ ClO −
iii + H2O 		1.2 2
Mn MnO
2 (southward) + 4H+ + 2 east − 		⇌ Mn ii+
+ 2H2O 		1.224 2 [eight]
O O
two (yard) + fourH+ + 4 e − 		⇌ 2H2O ane.229 iv [half dozen]
Ru [Ru(bipy)
3 ] iii+
+ e − 		⇌ [Ru(bipy)
iii ] 2+
1.24 1 [1]
Xe [HXeO
4 ] −
+ threeH2O + 6 e − 		⇌ Xe(grand) + 7OH− 1.24 half-dozen [18]
Tl Tl three+
+ 2 e − 		⇌ Tl +
ane.25 ii
Cr Cr
2 O 2−
7 + 14H+ + half dozen e − 		⇌ iiCr 3+
+ 7H2O 		1.33 6
Cl Cl
two (k) + 2 e − 		⇌ 2Cl −
1.36 ii [6]
Ru RuO −
four (aq) + 8H+ + 5 e − 		⇌ Ru ii+
(aq) + 4HtwoO 		ane.368 v [xv]
Ru RuO
4 + 4H+ + 4 east − 		⇌ RuO
2 + iiH2O 		ane.387 4 [fifteen]
Co CoO
2 (due south) + 4H+ + e − 		⇌ Co 3+
+ twoHiiO 		one.42 1
North 2NH
3 OH +
+ H+ + ii east − 		⇌ N
two H +
v + 2H2O 		1.42 2 [3]
I 2HIO(aq) + 2H+ + 2 e − ⇌ I
2 (southward) + 2H2O 		1.44 two
Br BrO −
3 + vH+ + 4 e − 		⇌ HBrO(aq) + 2HtwoO 1.45 4
Atomic number 82 β-PbO
two (south) + fourH+ + 2 e − 		⇌ Pb 2+
+ 2HiiO 		1.46 2 [11]
Lead α-PbO
ii (s) + 4H+ + 2 e − 		⇌ Pb 2+
+ 2H2O 		1.468 2 [xi]
Br 2BrO −
3 + 12H+ + 10 e − 		⇌ Br
2 (fifty) + viH2O 		i.48 10
Cl 2ClO −
3 + 12H+ + 10 e − 		⇌ Cl
2 (g) + 6H2O 		1.49 ten
Cl HClO(aq) + H+ + 2 e − ⇌ Cl −
(aq) + H2O 		i.49 2 [1]
Mn MnO −
four + eightH+ + 5 eastward − 		⇌ Mn 2+
+ 4H2O 		one.51 five
O HO •
2 + H+ + due east − 		⇌ H
2 O
ii (aq) 		1.51 i
Au Au three+
+ 3 e − 		⇌ Au(south) 1.52 3
Ru RuO two−
4 (aq) + 8H+ + 4 e − 		⇌ Ru 2+
(aq) + 4HtwoO 		1.563 four [15]
Ni NiO
2 (southward) + 2H+ + 2 e − 		⇌ Ni 2+
+ iiOH− 		i.59 ii
Ce Ce 4+
+ e − 		⇌ Ce three+
1.61 ane
Cl 2HClO(aq) + twoH+ + ii eastward − ⇌ Cl
two (grand) + 2H2O 		1.63 2
Ag Ag
2 O
3 (s) + viH+ + 4 e − 		⇌ 2Ag +
+ 3H2O 		i.67 4
Cl HClO
2 (aq) + 2H+ + 2 e − 		⇌ HClO(aq) + H2O one.67 2
Pb Lead 4+
+ 2 e − 		⇌ Pb 2+
i.69 2 [11]
Mn MnO −
4 + fourH+ + 3 e − 		⇌ MnO
ii (due south) + 2H2O 		1.7 3
Ag Ago(s) + 2H+ + e − ⇌ Ag +
+ HtwoO 		ane.77 1
O H
2 O
2 (aq) + 2H+ + 2 e − 		⇌ 2H2O 1.78 two
Co Co 3+
+ e − 		⇌ Co 2+
1.82 1
Au Au +
+ e − 		⇌ Au(south) 1.83 1 [xi]
Br BrO −
iv + twoH+ + 2 e − 		⇌ BrO −
3 + H2O 		1.85 2
Ag Ag 2+
+ e − 		⇌ Ag +
1.98 1 [11]
O S
2 O ii−
viii + 2 e − 		⇌ 2SO two−
iv 		2.01 two [8]
O O
three (one thousand) + 2H+ + ii due east − 		⇌ O
two (g) + H2O 		two.075 2 [12]
Mn HMnO −
4 + 3H+ + 2 e − 		⇌ MnO
2 (s) + iiH2O 		2.09 2
Xe XeO
3 (aq) + sixH+ + 6 eastward − 		⇌ Xe(m) + iiiH2O ii.12 6 [18]
Xe H
4 XeO
6 (aq) + 8H+ + 8 e − 		⇌ Xe(yard) + viHtwoO ii.18 8 [18]
Fe FeO ii−
4 + 8H+ + three e − 		⇌ Atomic number 26 3+
+ ivH2O 		two.2 3 [20]
Xe XeF
2 (aq) + 2H+ + 2 e − 		⇌ Xe(grand) + 2HF(aq) 2.32 2 [eighteen]
Xe H
four XeO
6 (aq) + 2H+ + 2 eastward − 		⇌ XeO
3 (aq) + 3H2O 		2.42 2 [18]
F F
two (thousand) + 2 east − 		⇌ 2F −
ii.87 2 [5] [half-dozen] [11]
F F
2 (thou) + 2H+ + ii due east − 		⇌ 2HF(aq) 3.05 two [eleven]
Tb Tb4+ + e– ⇌ Tbthree+ 3.1 1
Pr Pr4+ + e– ⇌ Pr3+ 3.2 i [21]
Kr KrF
2 (aq) + 2 e − 		⇌ Kr(g) + 2F −
(aq) 		3.27 two [22]

See too [edit]

  • Standard credible reduction potentials in biochemistry at pH seven
  • Standard state

Notes [edit]

  1. ^ a b Not specified in the indicated reference, simply 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 departure between the values for white (−0.063) and red (−0.111) phosphorus in equilibrium with PHiii.

References [edit]

  1. ^ a b c d e f g h i j m 50 chiliad n o p q r s t u v due west ten y z aa ab ac ad ae af ag ah ai aj ak al am an ao ap aq ar as at au av aw ax ay az ba bb bc bd be bf bg bh bi bj bk bl bm bn bo bp bq br bs bt bu bv bw bx past Lide, David R., ed. (2006). CRC Handbook of Chemistry and Physics (87th ed.). Boca Raton, FL: CRC Printing. ISBN0-8493-0487-3.
  2. ^ Greenwood and Earnshaw, p. 1263
  3. ^ a b c d Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN978-0-08-037941-eight.
  4. ^ a b c d e f thousand h i j yard l m n o p q Vanýsek, Petr (2011). "Electrochemical Series". In Haynes, William Thou. (ed.). CRC Handbook of Chemistry and Physics (92nd ed.). CRC Press. pp. 5–lxxx–9. ISBN978-ane-4398-5512-half dozen.
  5. ^ a b c d Atkins, Peter (2010). Inorganic Chemistry (5th ed.). Westward. H. Freeman. p. 153. ISBN978-1-42-921820-7.
  6. ^ a b c d e f g h i j one thousand l m Atkins, Peter West. (1997). Physical Chemical science (6th ed.). Westward.H. Freeman. ISBN9780716734659.
  7. ^ David R. Lide, ed., CRC Handbook of Chemistry and Physics, Internet Version 2005, http://www.hbcpnetbase.com Archived 2017-07-24 at the Wayback Machine, CRC Press, Boca Raton, FL, 2005.
  8. ^ a b c d due east f g h i j thou l g n o p q r s t u v w x y z aa ab Vanýsek, Petr (2012). "Electrochemical Serial". In Haynes, William K. (ed.). Handbook of Chemical science and Physics (93rd ed.). CRC Press. pp. 5–80. ISBN9781439880494.
  9. ^ Aylward, Gordon; Findlay, Tristan (2008). SI Chemical Data (6th ed.). Wiley. ISBN978-0-470-81638-seven.
  10. ^ a b c d eastward "compounds information". Iron. WebElements Periodic Table of the Elements.
  11. ^ a b c d e f g h i j yard l g n o p q r due south t u 5 Bard, Allen J.; Parsons, Roger; Jordan, Joseph (1985). Standard Potentials in Aqueous Solution. CRC Press. ISBN978-0-8247-7291-8.
  12. ^ a b c d due east f k h i j Bard, A.J.; Faulkner, 50.R. (2001). Electrochemical Methods. Fundamentals and Applications (second ed.). Wiley. ISBN9781118312803.
  13. ^ Pourbaix, Marcel (1966). Atlas of Electrochemical Equilibria in Aqueous Solutions. Houston, Texas; Cebelcor, Brussels: NACE International. OCLC 475102548.
  14. ^ a b c Pang, Suh Cem; Chin, Suk Fun; Anderson, Marc A. (July 2007). "Redox equilibria of atomic number 26 oxides in aqueous-based magnetite dispersions: Effect of pH and redox potential". J. Colloid Interface Sci. 311 (1): 94–101. Bibcode:2007JCIS..311...94P. doi:10.1016/j.jcis.2007.02.058. PMID 17395194. Retrieved 2017-03-26 .
  15. ^ a b c d e f Greenwood and Earnshaw, p. 1077
  16. ^ Rock, Peter A. (February 1966). "The Standard Oxidation Potential of the Ferrocyanide-Ferricyanide Electrode at 25° and the Entropy of Ferrocyanide Ion". The Periodical of Physical Chemistry. 70 (two): 576–580. doi:ten.1021/j100874a042. ISSN 0022-3654.
  17. ^ Connelly, Neil G.; Geiger, William Eastward. (1 Jan 1996). "Chemical Redox Agents for Organometallic Chemistry". Chemical Reviews. 96 (two): 877–910. doi:10.1021/cr940053x. PMID 11848774.
  18. ^ a b c d east f g "compounds information". Xenon. WebElements Periodic Table of the Elements.
  19. ^ a b Cotton, F. Albert; Wilkinson, Geoffrey; Murillo, Carlos A.; Bochmann, Manfred (1999), Avant-garde Inorganic Chemistry (sixth ed.), New York: Wiley-Interscience, ISBN0-471-19957-5 .
  20. ^ Courtney, Arlene. "Oxidation Reduction Chemistry of the Elements". Ch 412 Avant-garde Inorganic Chemistry: Reading Materials. Western Oregon Academy.
  21. ^ Petr Vanysek. "Electrochemical series" (PDF). depa.fquim.unam.mx. Archived (PDF) from the original on 2022-10-09.
  22. ^ Leszczyński, P.J.; Grochala, W. (2013). "Strong Cationic Oxidizers: Thermal Decomposition, Electronic Construction and Magnetism of Their Compounds" (PDF). Acta Chim. Slov. 60 (3): 455–470. PMID 24169699. Archived (PDF) from the original on 2022-x-09.

External links [edit]

  • Chemistry LibreTexts (2021-04-26). "P1: Standard Reduction Potentials by Element". Chemical science LibreTexts . Retrieved 2021-11-30 .
  • California State Academy, Northridge (CSUN). "Standard Reduction Potentials" (PDF). csun.edu . Retrieved 2021-eleven-30 .
  • Bratsch, Steven G. (1989). "Standard electrode potentials and temperature coefficients in water at 298.xv K" (PDF). nist.gov . Retrieved 2021-11-30 .
  • Wardman, Peter (1989). "Reduction potentials of one-electron couples involving free radicals in aqueous solution" (PDF). srd.nist.gov. Archived (PDF) from the original on 2022-ten-09. Retrieved 2021-11-30 .
  • http://world wide web.jesuitnola.org/upload/clark/Refs/red_pot.htm Archived 2008-07-twenty at the Wayback Machine
  • https://web.archive.org/spider web/20150924015049/http://world wide web.fptl.ru/biblioteka/spravo4niki/handbook-of-Chemistry-and-Physics.pdf
  • http://hyperphysics.phy-astr.gsu.edu/Hbase/tables/electpot.html#c1

Table Of Standard Reduction Potentials,

Source: https://en.wikipedia.org/wiki/Standard_electrode_potential_(data_page)

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