Nernstova jednačina

Nernstova jednačina je jednačina za elektrodni potencijal i koristi se u elektrohemiji. Do ovog izraza prvi je došao nemački nobelovac, Valter Nernst, po kome je i dobila ime. Za opšti slučaj polureakcije oksido-redukcije:

${\ce {Ox + ze- -> Red}}$

Nernstova jednačina ima oblik:

${\ E=E^{o}+{\frac {RT}{zF}}ln{\frac {a_{ox}}{a_{red}}}}$

gde je

E – elektrodni potencijal

E° – standardni elektrodni potencijal

R – univerzalna gasna konstanta (8,314 J K⁻¹ mol⁻¹)

T – termodinamička temperatura (izražena u Kelvinima)

z – broj razmenjenih elektrona u gorenavedenoj reakciji oksido-redukcije

F – Faradejeva konstanta (96 485 C mol^-1)

a_ox, a_red – aktiviteti oksidansa i reduktora u rastvoru

Nernstova jednačina pri normalnim uslovima

Prebacivanjem iz prirodnog (ln) u dekadni logaritam (log), razlomak se množi sa 2,303, što dalje se formuliše kao:

$\ln 10=\log _{e}10=2,303$

${\ E=E^{o}+{\frac {2,303RT}{zF}}log{\frac {a_{ox}}{a_{red}}}}$

Pri normalnim uslovima od 25 °C (298 K) i atmosferskom pritisku od 1 atm, Nernstova jednačina uzima skraćen, vrlo često korišćen oblik:

${\ E=E^{o}+{\frac {0,059}{z}}log{\frac {a_{ox}}{a_{red}}}}$

gde je z broj razmenjenih elektrona u reakciji oksido-redukcije.

Izvođenje Nernstove jednačine

Nemački fizikohemičar, nobelovac, Valter Nernst.

Do Nernstove jednačine se uobičajeno dolazi na dva načina. Izvođenjem na osnovu Nernstove osmotske teorije preko osmotskih pritisaka i termodinamičkim izvođenjem preko hemijskih i elektrohemijskih potencijala, što je i prikazano u nastavku.

Za reverzibilnu i izotermsku hemijsku reakciju u kojoj se razmenjuju zF kulona naelektrisanja opšteg oblika:

${\ce {aA\,+bB\,+...<=>[{\pm zF}]cC\,+dD\,+...}}$

slobodna Gibsova energija pri konstantnoj temperaturi i pritisku iznosi:

$-\Delta G_{T,P}=zFE_{T,P}$

pri čemu je elektromotorna sila elektrohemijskog sistema pri istim uslovima:

$E_{T,P}=-{\frac {\Delta G_{T,P}}{zF}}$

Izraz koji povezuje slobodnu Gibsovu energiju i hemijski potencijal $-\Delta G=\sum n_{i}\mu _{i},\mu _{i}=\mu _{i}^{o}+RT\ln a$

$\Delta G=\sum n_{i}\mu _{i}^{o}+RT\ln {\frac {a_{C}^{c}\cdot a_{D}^{d}}{a_{A}^{a}\cdot a_{B}^{b}}}$

$\Delta G=-RT\ln K+RT\ln \prod a_{i}^{n_{i}}$

$E={\frac {RT}{zF}}\ln K-{\frac {RT}{zF}}\ln {\frac {a_{C}^{c}\cdot a_{D}^{d}}{a_{A}^{a}\cdot a_{B}^{b}}}$

$\Delta G^{o}=\sum n_{i}\mu _{i}^{o}=RT\ln K$

Odakle sledi da standardna elektromotorna sila elektrohemijskog sistema iznosi:

$E^{o}=-{\frac {\Delta G^{o}}{zF}}={\frac {RT}{zF}}\ln K$

dok elektromotorna sila ravnotežnog elektrohemijskog sistema iznosi:

$E=E^{o}-{\frac {RT}{zF}}\ln {\frac {a_{C}^{c}\cdot a_{D}^{d}}{a_{A}^{a}\cdot a_{B}^{b}}}$

Znajući matematička logaritamska pravila, znak ispred prirodnog logaritma može se zameniti recipročnom vrednošću razlomka, pri čemu se dobija klasični oblik Nernstove jednačine:

${\ E=E^{o}+{\frac {RT}{zF}}ln{\frac {a_{A}^{a}\cdot a_{B}^{b}}{a_{C}^{c}\cdot a_{D}^{d}}}=E^{o}+{\frac {RT}{zF}}ln{\frac {a_{ox}}{a_{red}}}}$

Standardni elektrodni potencijal

Budući da je nemoguće odrediti apsolutnu vrednost elektrodnog potencijala, koriste se referentne elektrode u odnosu na koje se meri i upoređuje potencijal drugih elektroda.

Postoje dve skale koje se najviše koriste u hemiji, relativna vodonična skala potencijala (prikazana u tabeli) koju je postavio Valter Nernst i skala apsolutnih potencijala. Njen kreator je Ostvald i ona je nešto manje u upotrebi. Nernstova relativna vodonična skala potencijala je, posle Periodnog sistema elemenata, najbolja klasifikacija elemenata. Početna premisa je da je elektrodni potencijal vodonične elektrode, gde atomski vodonik nastaje disocijacijom molekulskog vodonika, iznosi nula. U odnosu na tu elektrodu, meri se razlika potencijala svih ostalih elemenata. Igrom slučaja, vodonik se na toj skali nalazi približno na sredini.

Pomoću relativne vodonične skale potencijala se može:

predvideti smer slobodnog toka hemijske reakcije pri standardnim uslovima
odrediti vrednosti standardne elektromotorne sile i drugih termodinamičkih veličina koji iz nje proizilaze (slobodna energija, entropija, entalpija...)
odrediti standardni elektrodni potencijal u nestandardnim uslovima
predvideti redosled elektrolitičkog razlaganja komponenti u rastvoru.

Standardni elektrodni potencijal je konstanta karakteristična za posmatrani redoks-par, koja predstavlja elektrodni potencijal E kada su aktiviteti oksidansa i reduktora jednaki jedinici.

Element	Polu-reakcija			E° (V)	Ref.
Element	Oksidans	⇌	Reduktor	E° (V)	Ref.
&	-9
Zz	9
Sr	Sr+ + e^-	⇌	Sr(s)	−4.101	^[1]
Ca	Ca+ + e^-	⇌	Ca(s)	−3.8	^[1]
Pr	Pr3+ + e^-	⇌	Pr2+	−3.1	^[1]
N	N3 N 2(g) + 2 H⁺ + 2e^-	⇌	2 HN 3(aq)	−3.09	^[2]^[3]
Li	Li+ + e^-	⇌	Li(s)	−3.0401	^[3]^[4]
N	N 2(g) + 4 H₂O + 2e^-	⇌	2 NH 2OH(aq) + 2 OH⁻	−3.04	^[2]
Cs	Cs+ + e^-	⇌	Cs(s)	−3.026	^[3]
Ca	Ca(OH) 2 + 2e^-	⇌	Ca(s) + 2 OH⁻	−3.02	^[1]
Er	Er3+ + e^-	⇌	Er2+	−3.0	^[1]
Ba	Ba(OH) 2 + 2e^-	⇌	Ba(s) + 2 OH⁻	−2.99	^[1]
Rb	Rb+ + e^-	⇌	Rb(s)	−2.98	^[3]
K	K+ + e^-	⇌	K(s)	−2.931	^[3]
Ba	Ba2+ + 2e^-	⇌	Ba(s)	−2.912	^[3]
La	La(OH) 3(s) + 3e^-	⇌	La(s) + 3 OH⁻	−2.90	^[3]
Fr	Fr+ + e^-	⇌	Fr(s)	−2.9	^[1]
Sr	Sr2+ + 2e^-	⇌	Sr(s)	−2.899	^[3]
Sr	Sr(OH) 2 + 2e^-	⇌	Sr(s) + 2 OH⁻	−2.88	^[1]
Ca	Ca2+ + 2e^-	⇌	Ca(s)	−2.868	^[3]^[4]
Li	Li+ + C 6(s) + e^-	⇌	LiC 6(s)	−2.84	^[3]
Eu	Eu2+ + 2e^-	⇌	Eu(s)	−2.812	^[3]
Ra	Ra2+ + 2e^-	⇌	Ra(s)	−2.8	^[3]
Ho	Ho3+ + e^-	⇌	Ho²⁺	−2.8	^[1]
Bk	Bk3+ + e^-	⇌	Bk2+	−2.8	^[1]
Yb	Yb2+ + 2e^-	⇌	Yb(s)	−2.76	^[1]
Na	Na+ + e^-	⇌	Na(s)	−2.71	^[3]^[5]
Mg	Mg+ + e^-	⇌	Mg(s)	−2.70	^[1]
Nd	Nd3+ + e^-	⇌	Nd2+	−2.7	^[1]
Mg	Mg(OH) 2 + 2e^-	⇌	Mg(s) + 2 OH⁻	−2.690	^[1]
Sm	Sm2+ + 2e^-	⇌	Sm(s)	−2.68	^[1]
Be	Be 2O2− 3 + 3 H₂O + 4e^-	⇌	2 Be(s) + 6 OH⁻	−2.63	^[1]
Pm	Pm3+ + e^-	⇌	Pm2+	−2.6	^[1]
Dy	Dy3+ + e^-	⇌	Dy2+	−2.6	^[1]
No	No2+ + 2e^-	⇌	No	−2.50	^[1]
Hf	HfO(OH) 2 + H₂O + 4e^-	⇌	Hf(s) + 4 OH⁻	−2.50	^[1]
Th	Th(OH) 4 + 4e^-	⇌	Th(s) + 4 OH⁻	−2.48	^[1]
Md	Md2+ + 2e^-	⇌	Md	−2.40	^[1]
Tm	Tm2+ + 2e^-	⇌	Tm(s)	−2.4	^[1]
La	La3+ + 3e^-	⇌	La(s)	−2.379	^[3]
Y	Y3+ + 3e^-	⇌	Y(s)	−2.372	^[3]
Mg	Mg2+ + 2e^-	⇌	Mg(s)	−2.372	^[3]
Zr	ZrO(OH) 2(s) + H₂O + 4e^-	⇌	Zr(s) + 4 OH⁻	−2.36	^[3]
Pr	Pr3+ + 3e^-	⇌	Pr(s)	−2.353	^[1]
Ce	Ce3+ + 3e^-	⇌	Ce(s)	−2.336	^[1]
Er	Er3+ + 3e^-	⇌	Er(s)	−2.331	^[1]
Ho	Ho3+ + 3e^-	⇌	Ho(s)	−2.33	^[1]
Al	H 2AlO− 3 + H₂O + 3e^-	⇌	Al(s) + 4 OH⁻	−2.33	^[1]
Nd	Nd3+ + 3e^-	⇌	Nd(s)	−2.323	^[1]
Tm	Tm3+ + 3e^-	⇌	Tm(s)	−2.319	^[1]
Al	Al(OH) 3(s) + 3e^-	⇌	Al(s) + 3 OH⁻	−2.31
Sm	Sm3+ + 3e^-	⇌	Sm(s)	−2.304	^[1]
Fm	Fm²⁺ + 2e^-	⇌	Fm	−2.30	^[1]
Am	Am3+ + e^-	⇌	Am2+	−2.3	^[1]
Dy	Dy3+ + 3e^-	⇌	Dy(s)	−2.295	^[1]
Lu	Lu3+ + 3e^-	⇌	Lu(s)	−2.28	^[1]
Tb	Tb3+ + 3e^-	⇌	Tb(s)	−2.28	^[1]
Gd	Gd3+ + 3e^-	⇌	Gd(s)	−2.279	^[1]
H	H 2(g) + 2e^-	⇌	2 H−	−2.23	^[1]
Es	Es2+ + 2e^-	⇌	Es(s)	−2.23	^[1]
Pm	Pm2+ + 2e^-	⇌	Pm(s)	−2.2	^[1]
Tm	Tm3+ + e^-	⇌	Tm²⁺	−2.2	^[1]
Dy	Dy2+ + 2e^-	⇌	Dy(s)	−2.2	^[1]
Ac	Ac3+ + 3e^-	⇌	Ac(s)	−2.20	^[1]
Yb	Yb3+ + 3e^-	⇌	Yb(s)	−2.19	^[1]
Cf	Cf2+ + 2e^-	⇌	Cf(s)	−2.12	^[1]
Nd	Nd2+ + 2e^-	⇌	Nd(s)	−2.1	^[1]
Ho	Ho2+ + 2e^-	⇌	Ho(s)	−2.1	^[1]
Sc	Sc3+ + 3e^-	⇌	Sc(s)	−2.077	^[6]
Al	AlF3− 6 + 3e^-	⇌	Al(s) + 6 F−	−2.069	^[1]
Am	Am3+ + 3e^-	⇌	Am(s)	−2.048	^[1]
Cm	Cm3+ + 3e^-	⇌	Cm(s)	−2.04	^[1]
Pu	Pu3+ + 3e^-	⇌	Pu(s)	−2.031	^[1]
Pr	Pr2+ + 2e^-	⇌	Pr(s)	−2.0	^[1]
Er	Er2+ + 2e^-	⇌	Er(s)	−2.0	^[1]
Eu	Eu3+ + 3e^-	⇌	Eu(s)	−1.991	^[1]
Lr	Lr3+ + 3e^-	⇌	Lr	−1.96	^[1]
Cf	Cf3+ + 3e^-	⇌	Cf(s)	−1.94	^[1]
Es	Es3+ + 3e^-	⇌	Es(s)	−1.91	^[1]
Pa	Pa4+ + e^-	⇌	Pa3+	−1.9	^[1]
Am	Am2+ + 2e^-	⇌	Am(s)	−1.9	^[1]
Th	Th4+ + 4e^-	⇌	Th(s)	−1.899	^[1]
Fm	Fm3+ + 3e^-	⇌	Fm	−1.89	^[1]
Np	Np3+ + 3e^-	⇌	Np(s)	−1.856	^[1]
Be	Be2+ + 2e^-	⇌	Be(s)	−1.847	^[1]
P	H 2PO− 2 + e^-	⇌	P(s) + 2 OH⁻	−1.82	^[1]
U	U3+ + 3e^-	⇌	U(s)	−1.798	^[1]
Sr	Sr2+ + 2e^-	⇌	Sr(Hg)	−1.793	^[1]
B	H 2BO− 3 + H₂O + 3e^-	⇌	B(s) + 4 OH⁻	−1.79	^[1]
Th	ThO 2 + 4 H⁺ + 4e^-	⇌	Th(s) + 2 H₂O	−1.789	^[1]
Hf	HfO2+ + 2 H⁺ + 4e^-	⇌	Hf(s) + H₂O	−1.724	^[1]
P	HPO2− 3 + 2 H₂O + 3e^-	⇌	P(s) + 5 OH⁻	−1.71	^[1]
Si	SiO2− 3 + H₂O + 4e^-	⇌	Si(s) + 6 OH⁻	−1.697	^[1]
Al	Al3+ + 3e^-	⇌	Al(s)	−1.662	^[1]
Ti	Ti2+ + 2e^-	⇌	Ti(s)	−1.63	^[5]
Zr	ZrO 2(s) + 4 H⁺ + 4e^-	⇌	Zr(s) + 2 H₂O	−1.553	^[7]
Zr	Zr4+ + 4e^-	⇌	Zr(s)	−1.45	^[7]
Ti	Ti3+ + 3e^-	⇌	Ti(s)	−1.37	^[8]
Ti	TiO(s) + 2 H⁺ + 2e^-	⇌	Ti(s) + H₂O	−1.31
Ti	Ti 2O 3(s) + 2 H⁺ + 2e^-	⇌	2 TiO(s) + H₂O	−1.23
Zn	Zn(OH)2− 4 + 2e^-	⇌	Zn(s) + 4 OH⁻	−1.199	^[7]
Mn	Mn2+ + 2e^-	⇌	Mn(s)	−1.185	^[7]
Fe	Fe(CN)4− 6 + 6 H⁺ + 2e^-	⇌	Fe(s) + 6 HCN(aq)	−1.16	^[9]
Te	Te(s) + 2e^-	⇌	Te2−	−1.143	^[10]
V	V2+ + 2e^-	⇌	V(s)	−1.13	^[10]
Nb	Nb3+ + 3e^-	⇌	Nb(s)	−1.099
Sn	Sn(s) + 4 H⁺ + 4e^-	⇌	SnH 4(g)	−1.07
Ti	TiO2+ + 2 H⁺ + 4e^-	⇌	Ti(s) + H₂O	−0.93
Si	SiO 2(s) + 4 H⁺ + 4e^-	⇌	Si(s) + 2 H₂O	−0.91
B	B(OH) 3(aq) + 3 H⁺ + 3e^-	⇌	B(s) + 3 H₂O	−0.89
Fe	Fe(OH) 2(s) + 2e^-	⇌	Fe(s) + 2 OH⁻	−0.89	^[9]
Fe	Fe 2O 3(s) + 3 H₂O + 2e^-	⇌	2 Fe(OH) 2(s) + 2 OH⁻	−0.86	^[9]
H	2 H₂O + 2e^-	⇌	H 2(g) + 2 OH⁻	−0.8277	^[7]
Bi	Bi(s) + 3 H⁺ + 3e^-	⇌	BiH 3	−0.8	^[7]
Zn	Zn2+ + 2e^-	⇌	Zn(Hg)	−0.7628	^[7]
Zn	Zn2+ + 2e^-	⇌	Zn(s)	−0.7618	^[7]
Ta	Ta 2O 5(s) + 10 H⁺ + 10e^-	⇌	2 Ta(s) + 5 H₂O	−0.75
Cr	Cr3+ + 3e^-	⇌	Cr(s)	−0.74
Ni	Ni(OH) 2(s) + 2e^-	⇌	Ni(s) + 2 OH⁻	–0.72	^[1]
Ag	Ag 2S(s) + 2e^-	⇌	2 Ag(s) + S2− (aq)	−0.69
Au	[Au(CN) 2]− + e^-	⇌	Au(s) + 2 CN−	−0.60
Ta	Ta3+ + 3e^-	⇌	Ta(s)	−0.6
Pb	PbO(s) + H₂O + 2e^-	⇌	Pb(s) + 2 OH⁻	−0.58
Ti	2 TiO 2(s) + 2 H⁺ + 2e^-	⇌	Ti 2O 3(s) + H₂O	−0.56
Ga	Ga3+ + 3e^-	⇌	Ga(s)	−0.53
U	U4+ + e^-	⇌	U3+	−0.52	^[11]
P	H 3PO 2(aq) + H⁺ + e^-	⇌	P(white)^{[note 1]} + 2 H₂O	−0.508	^[7]
P	H 3PO 3(aq) + 2 H⁺ + 2e^-	⇌	H 3PO 2(aq) + H₂O	−0.499	^[7]
Ni	NiO 2(s) + 2 H 2O + 2e^-	⇌	Ni(OH) 2(s) + 2 OH⁻	–0.49	^[1]
P	H 3PO 3(aq) + 3 H⁺ + 3e^-	⇌	P(red) + 3 H₂O	−0.454	^[7]
Cu	Cu(CN)− 2 + e^-	⇌	Cu(s) + 2 CN−	–0.44	^[10]
Fe	Fe2+ + 2e^-	⇌	Fe(s)	−0.44	^[5]
C	2 CO 2(g) + 2 H⁺ + 2e^-	⇌	HOOCCOOH(aq)	−0.43
Cr	Cr3+ + e^-	⇌	Cr2+	−0.42
Cd	Cd2+ + 2e^-	⇌	Cd(s)	−0.40	^[5]
Ge	GeO 2(s) + 2 H⁺ + 2e^-	⇌	GeO(s) + H₂O	−0.37
Cu	Cu 2O(s) + H₂O + 2e^-	⇌	2 Cu(s) + 2 OH⁻	−0.360	^[7]
Pb	PbSO 4(s) + 2e^-	⇌	Pb(s) + SO2− 4	−0.3588	^[7]
Pb	PbSO 4(s) + 2e^-	⇌	Pb(Hg) + SO2− 4	−0.3505	^[7]
Eu	Eu3+ + e^-	⇌	Eu2+	−0.35	^[11]
In	In3+ + 3e^-	⇌	In(s)	−0.34	^[10]
Tl	Tl+ + e^-	⇌	Tl(s)	−0.34	^[10]
Ge	Ge(s) + 4 H⁺ + 4e^-	⇌	GeH 4(g)	−0.29
Co	Co2+ + 2e^-	⇌	Co(s)	−0.28	^[7]
P	H 3PO 4(aq) + 2 H⁺ + 2e^-	⇌	H 3PO 3(aq) + H₂O	−0.276	^[7]
V	V3+ + e^-	⇌	V2+	−0.26	^[5]
Ni	Ni2+ + 2e^-	⇌	Ni(s)	−0.25
As	As(s) + 3 H⁺ + 3e^-	⇌	AsH 3(g)	−0.23	^[10]
Ag	AgI(s) + e^-	⇌	Ag(s) + I−	−0.15224	^[7]
Mo	MoO 2(s) + 4 H⁺ + 4e^-	⇌	Mo(s) + 2 H₂O	−0.15
Si	Si(s) + 4 H⁺ + 4e^-	⇌	SiH 4(g)	−0.14
Sn	Sn2+ + 2e^-	⇌	Sn(s)	−0.13
O	O 2(g) + H⁺ + e^-	⇌	HO• 2(aq)	−0.13
Pb	Pb2+ + 2e^-	⇌	Pb(s)	−0.126	^[5]
W	WO 2(s) + 4 H⁺ + 4e^-	⇌	W(s) + 2 H₂O	−0.12
P	P(red) + 3 H⁺ + 3e^-	⇌	PH 3(g)	−0.111	^[7]
C	CO 2(g) + 2 H⁺ + 2e^-	⇌	HCOOH(aq)	−0.11
Se	Se(s) + 2 H⁺ + 2e^-	⇌	H 2Se(g)	−0.11
C	CO 2(g) + 2 H⁺ + 2e^-	⇌	CO(g) + H₂O	−0.11
Cu	Cu(NH 3)+ 2 + e^-	⇌	Cu(s) + 2 NH 3(aq)	–0.10	^[10]
Sn	SnO(s) + 2 H⁺ + 2e^-	⇌	Sn(s) + H₂O	−0.10
Sn	SnO 2(s) + 2 H⁺ + 2e^-	⇌	SnO(s) + H₂O	−0.09
W	WO 3(aq) + 6 H⁺ + 6e^-	⇌	W(s) + 3 H₂O	−0.09	^[10]
Fe	Fe 3O 4(s) + 8 H⁺ + 8e^-	⇌	3 Fe(s) + 4 H₂O	−0.085	^[12]
P	P(white) + 3 H⁺ + 3e^-	⇌	PH 3(g)	−0.063	^[7]
Fe	Fe3+ + 3e^-	⇌	Fe(s)	−0.04	^[9]
C	HCOOH(aq) + 2 H⁺ + 2e^-	⇌	HCHO(aq) + H₂O	−0.03
H	2 H⁺ + 2e^-	⇌	H 2(g)	0.0000	= 0
Ag	AgBr(s) + e^-	⇌	Ag(s) + Br−	+0.07133	^[7]
S	S 4O2− 6 + 2e^-	⇌	2 S 2O2− 3	+0.08
N	N 2(g) + 2 H₂O + 6 H⁺ + 6e^-	⇌	2 NH 4OH(aq)	+0.092
Hg	HgO(s) + H₂O + 2e^-	⇌	Hg(l) + 2 OH⁻	+0.0977
Cu	Cu(NH 3)2+ 4 + e^-	⇌	Cu(NH 3)+ 2 + 2 NH 3(aq)	+0.10	^[10]
Ru	Ru(NH 3)3+ 6 + e^-	⇌	Ru(NH 3)2+ 6	+0.10	^[11]
N	N 2H 4(aq) + 4 H₂O + 2e^-	⇌	2 NH+ 4 + 4 OH⁻	+0.11	^[2]
Mo	H 2MoO 4(aq) + 6 H⁺ + 6e^-	⇌	Mo(s) + 4 H₂O	+0.11
Ge	Ge4+ + 4e^-	⇌	Ge(s)	+0.12
C	C(s) + 4 H⁺ + 4e^-	⇌	CH 4(g)	+0.13	^[10]
C	HCHO(aq) + 2 H⁺ + 2e^-	⇌	CH 3OH(aq)	+0.13
S	S(s) + 2 H⁺ + 2e^-	⇌	H 2S(g)	+0.14
Sn	Sn4+ + 2e^-	⇌	Sn2+	+0.15
Cu	Cu2+ + e^-	⇌	Cu+	+0.159	^[10]
S	HSO− 4 + 3 H⁺ + 2e^-	⇌	SO 2(aq) + 2 H₂O	+0.16
U	UO2+ 2 + e^-	⇌	UO+ 2	+0.163	^[11]
S	SO2− 4 + 4 H⁺ + 2e^-	⇌	SO 2(aq) + 2 H₂O	+0.17
Ti	TiO2+ + 2 H⁺ + e^-	⇌	Ti3+ + H₂O	+0.19
Sb	SbO+ + 2 H⁺ + 3e^-	⇌	Sb(s) + H₂O	+0.20
Fe	3 Fe 2O 3(s) + 2 H⁺ + 2e^-	⇌	2 Fe 3O 4(s) + H₂O	+0.22	^[13]^‍:p.100
Ag	AgCl(s) + e^-	⇌	Ag(s) + Cl−	+0.22233	^[7]
As	H 3AsO 3(aq) + 3 H⁺ + 3e^-	⇌	As(s) + 3 H₂O	+0.24
Ge	GeO(s) + 2 H⁺ + 2e^-	⇌	Ge(s) + H₂O	+0.26
U	UO+ 2 + 4 H⁺ + e^-	⇌	U4+ + 2 H₂O	+0.273	^[11]
Re	Re3+ + 3e^-	⇌	Re(s)	+0.300
Bi	Bi3+ + 3e^-	⇌	Bi(s)	+0.308	^[7]
Cu	Cu2+ + 2e^-	⇌	Cu(s)	+0.337	^[10]
V	[VO]2+ + 2 H⁺ + e^-	⇌	V3+ + H₂O	+0.34
Fe	[Fe(CN) 6]3− + e^-	⇌	[Fe(CN) 6]4−	+0.3704	^[14]
Fe	Fc+ + e^-	⇌	Fc(s)	+0.4	^[15]
O	O 2(g) + 2 H₂O + 4e^-	⇌	4 OH⁻(aq)	+0.401	^[5]
Mo	H 2MoO 4 + 6 H⁺ + 3e^-	⇌	Mo3+ + 4 H₂O	+0.43
C	CH 3OH(aq) + 2 H⁺ + 2e^-	⇌	CH 4(g) + H₂O	+0.50
S	SO 2(aq) + 4 H⁺ + 4e^-	⇌	S(s) + 2 H₂O	+0.50
Cu	Cu+ + e^-	⇌	Cu(s)	+0.520	^[10]
C	CO(g) + 2 H⁺ + 2e^-	⇌	C(s) + H₂O	+0.52
I	I− 3	⇌	3 I−	+0.53	^[5]
I	I 2(s) + 2e^-	⇌	2 I−	+0.54	^[5]
Au	[AuI 4]− + 3e^-	⇌	Au(s) + 4 I−	+0.56
As	H 3AsO 4(aq) + 2 H⁺ + 2e^-	⇌	H 3AsO 3(aq) + H₂O	+0.56
Au	[AuI 2]− + e^-	⇌	Au(s) + 2 I−	+0.58
Mn	MnO− 4 + 2 H₂O + 3e^-	⇌	MnO 2(s) + 4 OH⁻	+0.595	^[1]
S	S 2O2− 3 + 6 H⁺ + 4e^-	⇌	2 S(s) + 3 H₂O	+0.60
Mo	H 2MoO 4(aq) + 2 H⁺ + 2e^-	⇌	MoO 2(s) + 2 H₂O	+0.65
C	+ 2 H⁺ + 2e^-	⇌		+0.6992	^[7]
O	O 2(g) + 2 H⁺ + 2e^-	⇌	H 2O 2(aq)	+0.70
Tl	Tl3+ + 3e^-	⇌	Tl(s)	+0.72
Pt	PtCl2− 6 + 2e^-	⇌	PtCl2− 4 + 2 Cl−	+0.726	^[11]
Fe	Fe 2O 3(s) + 6 H⁺ + 2e^-	⇌	2 Fe2+ + 3 H₂O	+0.728	^[13]^‍:p.100
Se	H 2SeO 3(aq) + 4 H⁺ + 4e^-	⇌	Se(s) + 3 H₂O	+0.74
Pt	PtCl2− 4 + 2e^-	⇌	Pt(s) + 4 Cl−	+0.758	^[11]
Fe	Fe3+ + e^-	⇌	Fe2+	+0.77
Ag	Ag+ + e^-	⇌	Ag(s)	+0.7996	^[7]
Hg	Hg2+ 2 + 2e^-	⇌	2 Hg(l)	+0.80
N	NO− 3(aq) + 2 H⁺ + e^-	⇌	NO 2(g) + H₂O	+0.80
Fe	2 FeO2− 4 + 5 H₂O + 6e^-	⇌	Fe 2O 3(s) + 10 OH⁻	+0.81	^[9]
Au	[AuBr 4]− + 3e^-	⇌	Au(s) + 4 Br−	+0.85
Hg	Hg2+ + 2e^-	⇌	Hg(l)	+0.85
Ir	[IrCl 6]2− + e^-	⇌	[IrCl 6]3−	+0.87	^[4]
Mn	MnO− 4 + H⁺ + e^-	⇌	HMnO− 4	+0.90
Hg	2 Hg2+ + 2e^-	⇌	Hg2+ 2	+0.91	^[10]
Pd	Pd2+ + 2e^-	⇌	Pd(s)	+0.915	^[11]
Au	[AuCl 4]− + 3e^-	⇌	Au(s) + 4 Cl−	+0.93
Mn	MnO 2(s) + 4 H⁺ + e^-	⇌	Mn3+ + 2 H₂O	+0.95
N	NO− 3(aq) + 4 H⁺ + 3e^-	⇌	NO(g) + 2 H₂O(l)	+0.958	^[5]
Au	[AuBr 2]− + e^-	⇌	Au(s) + 2 Br−	+0.96
Fe	Fe 3O 4(s) + 8 H⁺ + 2e^-	⇌	3Fe2+ + 4 H₂O	+0.98	^[13]^‍:p.100
Xe	[HXeO 6]3− + 2 H₂O + 2e^-	⇌	[HXeO 4]− + 4 OH⁻	+0.99	^[16]
V	[VO 2]+ (aq) + 2 H⁺ + e^-	⇌	[VO]2+ (aq) + H₂O	+1.0	^[17]
Te	H 6TeO 6(aq) + 2 H⁺ + 2e^-	⇌	TeO 2(s) + 4 H₂O	+1.02	^[17]
Br	Br 2(l) + 2e^-	⇌	2 Br−	+1.066	^[7]
Br	Br 2(aq) + 2e^-	⇌	2 Br−	+1.0873	^[7]
Cu	Cu2+ + 2 CN− + e^-	⇌	Cu(CN)− 2	+1.12	^[10]
I	IO− 3 + 5 H⁺ + 4e^-	⇌	HIO(aq) + 2 H₂O	+1.13
Au	[AuCl 2]− + e^-	⇌	Au(s) + 2 Cl−	+1.15
Se	HSeO− 4 + 3 H⁺ + 2e^-	⇌	H 2SeO 3(aq) + H₂O	+1.15
Ag	Ag 2O(s) + 2 H⁺ + 2e^-	⇌	2 Ag(s) + H₂O	+1.17
Cl	ClO− 3 + 2 H⁺ + e^-	⇌	ClO 2(g) + H₂O	+1.18
Xe	[HXeO 6]3− + 5 H₂O + 8e^-	⇌	Xe(g) + 11 OH⁻	+1.18	^[16]
Pt	Pt2+ + 2e^-	⇌	Pt(s)	+1.188	^[11]
Cl	ClO 2(g) + H⁺ + e^-	⇌	HClO 2(aq)	+1.19
I	2 IO− 3 + 12 H⁺ + 10e^-	⇌	I 2(s) + 6 H₂O	+1.20
Cl	ClO− 4 + 2 H⁺ + 2e^-	⇌	ClO− 3 + H₂O	+1.20
Mn	MnO 2(s) + 4 H⁺ + 2e^-	⇌	Mn2+ + 2 H₂O	+1.224	^[7]
O	O 2(g) + 4 H⁺ + 4e^-	⇌	2 H₂O	+1.229	^[5]
Ru	[Ru(bipy) 3]3+ + e^-	⇌	[Ru(bipy) 3]2+	+1.24	^[1]
Xe	[HXeO 4]− + 3 H₂O + 6e^-	⇌	Xe(g) + 7 OH⁻	+1.24	^[16]
Tl	Tl3+ + 2e^-	⇌	Tl+	+1.25
Cr	Cr 2O2− 7 + 14 H⁺ + 6e^-	⇌	2 Cr3+ + 7 H₂O	+1.33
Cl	Cl 2(g) + 2e^-	⇌	2 Cl−	+1.36	^[5]
Co	CoO 2(s) + 4 H⁺ + e^-	⇌	Co3+ + 2 H₂O	+1.42
N	2 NH 3OH+ + H⁺ + 2e^-	⇌	N 2H+ 5 + 2 H₂O	+1.42	^[2]
I	2 HIO(aq) + 2 H⁺ + 2e^-	⇌	I 2(s) + 2 H₂O	+1.44
Br	BrO− 3 + 5 H⁺ + 4e^-	⇌	HBrO(aq) + 2 H₂O	+1.45
Pb	β-PbO 2(s) + 4 H⁺ + 2e^-	⇌	Pb2+ + 2 H₂O	+1.460	^[10]
Pb	α-PbO 2(s) + 4 H⁺ + 2e^-	⇌	Pb2+ + 2 H₂O	+1.468	^[10]
Br	2 BrO− 3 + 12 H⁺ + 10e^-	⇌	Br 2(l) + 6 H₂O	+1.48
Cl	2 ClO− 3 + 12 H⁺ + 10e^-	⇌	Cl 2(g) + 6 H₂O	+1.49
Cl	HClO(aq) + H⁺ + 2e^-	⇌	Cl− (aq) + H₂O	+1.49	^[1]
Mn	MnO− 4 + 8 H⁺ + 5e^-	⇌	Mn2+ + 4 H₂O	+1.51
O	HO• 2 + H⁺ + e^-	⇌	H 2O 2(aq)	+1.51
Au	Au3+ + 3e^-	⇌	Au(s)	+1.52
Ni	NiO 2(s) + 2 H⁺ + 2e^-	⇌	Ni2+ + 2 OH⁻	+1.59
Ce	Ce4+ + e^-	⇌	Ce3+	+1.61
Cl	2 HClO(aq) + 2 H⁺ + 2e^-	⇌	Cl 2(g) + 2 H₂O	+1.63
Ag	Ag 2O 3(s) + 6 H⁺ + 4e^-	⇌	2 Ag+ + 3 H₂O	+1.67
Cl	HClO 2(aq) + 2 H⁺ + 2e^-	⇌	HClO(aq) + H₂O	+1.67
Pb	Pb4+ + 2e^-	⇌	Pb2+	+1.69	^[10]
Mn	MnO− 4 + 4 H⁺ + 3e^-	⇌	MnO 2(s) + 2 H₂O	+1.70
Ag	AgO(s) + 2 H⁺ + e^-	⇌	Ag+ + H₂O	+1.77
O	H 2O 2(aq) + 2 H⁺ + 2e^-	⇌	2 H₂O	+1.78
Co	Co3+ + e^-	⇌	Co2+	+1.82
Au	Au+ + e^-	⇌	Au(s)	+1.83	^[10]
Br	BrO− 4 + 2 H⁺ + 2e^-	⇌	BrO− 3 + H₂O	+1.85
Ag	Ag2+ + e^-	⇌	Ag+	+1.98	^[10]
O	S 2O2− 8 + 2e^-	⇌	2 SO2− 4	+2.010	^[7]
O	O 3(g) + 2 H⁺ + 2e^-	⇌	O 2(g) + H₂O	+2.075	^[11]
Mn	HMnO− 4 + 3 H⁺ + 2e^-	⇌	MnO 2(s) + 2 H₂O	+2.09
Xe	XeO 3(aq) + 6 H⁺ + 6e^-	⇌	Xe(g) + 3 H₂O	+2.12	^[16]
Xe	H 4XeO 6(aq) + 8 H⁺ + 8e^-	⇌	Xe(g) + 6 H₂O	+2.18	^[16]
Fe	FeO2− 4 + 8 H⁺ + 3e^-	⇌	Fe3+ + 4 H₂O	+2.20	^[18]
Xe	XeF 2(aq) + 2 H⁺ + 2e^-	⇌	Xe(g) + 2 HF(aq)	+2.32	^[16]
Xe	H 4XeO 6(aq) + 2 H⁺ + 2e^-	⇌	XeO 3(aq) + 3 H₂O	+2.42	^[16]
F	F 2(g) + 2e^-	⇌	2 F−	+2.87	^[4]^[5]^[10]
F	F 2(g) + 2 H⁺ + 2e^-	⇌	2 HF(aq)	+3.05	^[10]
Kr	KrF 2(aq) + 2e^-	⇌	Kr(g) + 2 F− (aq)	+3.27	^[19]

Vidi još

Napomene

^ 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 the values for white (−0.063) and red (−0.111) phosphorus in equilibrium with PH₃.

Izvori

^ ^a ^b ^v ^g ^d ^đ ^e ^ž ^z ⁱ ^j ^k ^l ^lj ^m ⁿ ^nj ^o ^p ^r ^s ^t ^ć ^u ^f ^h ^c ^č ^dž ^š ^aa ^ab ^av ^ag ^ad ^ađ ^ae ^až ^az ^ai ^aj ^ak ^al ^alj ^am ^an ^anj ^ao ^ap ^ar ^as ^at ^ać ^au ^af ^ah ^ac ^ač ^adž ^aš ^ba ^bb ^bv ^bg ^bd ^bđ ^be ^bž ^bz ^bi ^bj ^bk ^bl ^blj ^bm ^bn ^bnj Lide David R., ur. (2006). CRC Handbook of Chemistry and Physics (87th izd.). Boca Raton, FL: CRC Press. ISBN 978-0-8493-0487-3.
^ ^a ^b ^v ^g Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (II izd.). Oxford: Butterworth-Heinemann. ISBN 0080379419.
^ ^a ^b ^v ^g ^d ^đ ^e ^ž ^z ⁱ ^j ^k ^l ^lj ^m ⁿ ^nj Vanýsek, Petr (2011). „Electrochemical Series”. Ur.: Haynes, William M. CRC Handbook of Chemistry and Physics (92nd izd.). CRC Press. str. 5—80—9. ISBN 978-1-4398-5512-6.
^ ^a ^b ^v ^g Atkins, Peter (2010). Inorganic Chemistry (5th izd.). W. H. Freeman. str. 153. ISBN 978-1-42-921820-7.
^ ^a ^b ^v ^g ^d ^đ ^e ^ž ^z ⁱ ^j ^k ^l Atkins, Peter W. (1997). Physical Chemistry (6th izd.). W.H. Freeman. ISBN 9780716734659.
^ David R. Lide, ed., CRC Handbook of Chemistry and Physics, Internet Version 2005, http://www.hbcpnetbase.com Arhivirano na sajtu Wayback Machine (24. jul 2017), CRC Press, Boca Raton, FL, 2005.
^ ^a ^b ^v ^g ^d ^đ ^e ^ž ^z ⁱ ^j ^k ^l ^lj ^m ⁿ ^nj ^o ^p ^r ^s ^t ^ć ^u ^f ^h ^c ^č Vanýsek, Petr (2012). „Electrochemical Series”. Ur.: Haynes, William M. Handbook of Chemistry and Physics (93rd izd.). CRC Press. str. 5—80. ISBN 9781439880494.
^ Aylward, Gordon; Findlay, Tristan (2008). SI Chemical Data (6th izd.). Wiley. ISBN 978-0-470-81638-7.
^ ^a ^b ^v ^g ^d „compounds information”. Iron. WebElements Periodic Table of the Elements.
^ ^a ^b ^v ^g ^d ^đ ^e ^ž ^z ⁱ ^j ^k ^l ^lj ^m ⁿ ^nj ^o ^p ^r ^s ^t Bard, Allen J.; Parsons, Roger; Jordan, Joseph (1985). Standard Potentials in Aqueous Solution. CRC Press. ISBN 978-0-8247-7291-8.
^ ^a ^b ^v ^g ^d ^đ ^e ^ž ^z ⁱ Bard, A.J.; Faulkner, L.R. (2001). Electrochemical Methods. Fundamentals and Applications (2nd izd.). Wiley. ISBN 9781118312803.
^ Pourbaix, Marcel (1966). Atlas of Electrochemical Equilibria in Aqueous Solutions. Houston, Texas; Cebelcor, Brussels: NACE International. OCLC 475102548.
^ ^a ^b ^v Pang, Suh Cem; Chin, Suk Fun; Anderson, Marc A. (jul 2007). „Redox equilibria of iron oxides in aqueous-based magnetite dispersions: Effect of pH and redox potential”. J. Colloid Interface Sci. 311 (1): 94—101. Bibcode:2007JCIS..311...94P. PMID 17395194. doi:10.1016/j.jcis.2007.02.058. Pristupljeno 26. 3. 2017.
^ Rock, Peter A. (februar 1966). „The Standard Oxidation Potential of the Ferrocyanide-Ferricyanide Electrode at 25° and the Entropy of Ferrocyanide Ion”. The Journal of Physical Chemistry. 70 (2): 576—580. ISSN 0022-3654. doi:10.1021/j100874a042.
^ Connelly, Neil G.; Geiger, William E. (1. 1. 1996). „Chemical Redox Agents for Organometallic Chemistry”. Chemical Reviews. 96 (2): 877—910. PMID 11848774. doi:10.1021/cr940053x.
^ ^a ^b ^v ^g ^d ^đ ^e „compounds information”. Xenon. WebElements Periodic Table of the Elements.
^ ^a ^b Cotton F. Albert; Wilkinson Geoffrey; Murillo Carlos A; Bochmann, Manfred (1999). Advanced Inorganic Chemistry (6th izd.). New York: Wiley-Interscience. ISBN 0-471-19957-5. .
^ Courtney, Arlene. „Oxidation Reduction Chemistry of the Elements”. Ch 412 Advanced Inorganic Chemistry: Reading Materials. Western Oregon University.
^ Leszczyński, P.J.; Grochala, W. (2013). „Strong Cationic Oxidizers: Thermal Decomposition, Electronic Structure and Magnetism of Their Compounds” (PDF). Acta Chim. Slov. 60 (3): 455—470. Arhivirano iz originala (PDF) 07. 11. 2013. g. Pristupljeno 30. 08. 2020.

Spoljašnje veze

[rwP-12] 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 the values for white (−0.063) and red (−0.111) phosphorus in equilibrium with PH₃.

[CRC-1] v ^g ^d ^đ ^e ^ž ^z ⁱ ^j ^k ^l ^lj ^m ⁿ ^nj ^o ^p ^r ^s ^t ^ć ^u ^f ^h ^c ^č ^dž ^š ^aa ^ab ^av ^ag ^ad ^ađ ^ae ^až ^az ^ai ^aj ^ak ^al ^alj ^am ^an ^anj ^ao ^ap ^ar ^as ^at ^ać ^au ^af ^ah ^ac ^ač ^adž ^aš ^ba ^bb ^bv ^bg ^bd ^bđ ^be ^bž ^bz ^bi ^bj ^bk ^bl ^blj ^bm ^bn ^bnj Lide David R., ur. (2006). CRC Handbook of Chemistry and Physics (87th izd.). Boca Raton, FL: CRC Press. ISBN 978-0-8493-0487-3.

[Gre-2] v ^g Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (II izd.). Oxford: Butterworth-Heinemann. ISBN 0080379419.

[van92-3] v ^g ^d ^đ ^e ^ž ^z ⁱ ^j ^k ^l ^lj ^m ⁿ ^nj Vanýsek, Petr (2011). „Electrochemical Series”. Ur.: Haynes, William M. CRC Handbook of Chemistry and Physics (92nd izd.). CRC Press. str. 5—80—9. ISBN 978-1-4398-5512-6.

[atkinshriver-4] v ^g Atkins, Peter (2010). Inorganic Chemistry (5th izd.). W. H. Freeman. str. 153. ISBN 978-1-42-921820-7.

[Atk-5] v ^g ^d ^đ ^e ^ž ^z ⁱ ^j ^k ^l Atkins, Peter W. (1997). Physical Chemistry (6th izd.). W.H. Freeman. ISBN 9780716734659.

[6] David R. Lide, ed., CRC Handbook of Chemistry and Physics, Internet Version 2005, http://www.hbcpnetbase.com Arhivirano na sajtu Wayback Machine (24. jul 2017), CRC Press, Boca Raton, FL, 2005.

[van-7] v ^g ^d ^đ ^e ^ž ^z ⁱ ^j ^k ^l ^lj ^m ⁿ ^nj ^o ^p ^r ^s ^t ^ć ^u ^f ^h ^c ^č Vanýsek, Petr (2012). „Electrochemical Series”. Ur.: Haynes, William M. Handbook of Chemistry and Physics (93rd izd.). CRC Press. str. 5—80. ISBN 9781439880494.

[si-8] Aylward, Gordon; Findlay, Tristan (2008). SI Chemical Data (6th izd.). Wiley. ISBN 978-0-470-81638-7.

[webelements_fe-9] v ^g ^d „compounds information”. Iron. WebElements Periodic Table of the Elements.

[Bar-10] v ^g ^d ^đ ^e ^ž ^z ⁱ ^j ^k ^l ^lj ^m ⁿ ^nj ^o ^p ^r ^s ^t Bard, Allen J.; Parsons, Roger; Jordan, Joseph (1985). Standard Potentials in Aqueous Solution. CRC Press. ISBN 978-0-8247-7291-8.

[Bar2-11] v ^g ^d ^đ ^e ^ž ^z ⁱ Bard, A.J.; Faulkner, L.R. (2001). Electrochemical Methods. Fundamentals and Applications (2nd izd.). Wiley. ISBN 9781118312803.

[Pou-13] Pourbaix, Marcel (1966). Atlas of Electrochemical Equilibria in Aqueous Solutions. Houston, Texas; Cebelcor, Brussels: NACE International. OCLC 475102548.

[Pang2007-14] v Pang, Suh Cem; Chin, Suk Fun; Anderson, Marc A. (jul 2007). „Redox equilibria of iron oxides in aqueous-based magnetite dispersions: Effect of pH and redox potential”. J. Colloid Interface Sci. 311 (1): 94—101. Bibcode:2007JCIS..311...94P. PMID 17395194. doi:10.1016/j.jcis.2007.02.058. Pristupljeno 26. 3. 2017.

[15] Rock, Peter A. (februar 1966). „The Standard Oxidation Potential of the Ferrocyanide-Ferricyanide Electrode at 25° and the Entropy of Ferrocyanide Ion”. The Journal of Physical Chemistry. 70 (2): 576—580. ISSN 0022-3654. doi:10.1021/j100874a042.

[16] Connelly, Neil G.; Geiger, William E. (1. 1. 1996). „Chemical Redox Agents for Organometallic Chemistry”. Chemical Reviews. 96 (2): 877—910. PMID 11848774. doi:10.1021/cr940053x.

[webelements_xe-17] v ^g ^d ^đ ^e „compounds information”. Xenon. WebElements Periodic Table of the Elements.

[Cotton-18] Cotton F. Albert; Wilkinson Geoffrey; Murillo Carlos A; Bochmann, Manfred (1999). Advanced Inorganic Chemistry (6th izd.). New York: Wiley-Interscience. ISBN 0-471-19957-5. .

[wou-19] Courtney, Arlene. „Oxidation Reduction Chemistry of the Elements”. Ch 412 Advanced Inorganic Chemistry: Reading Materials. Western Oregon University.

[20] Leszczyński, P.J.; Grochala, W. (2013). „Strong Cationic Oxidizers: Thermal Decomposition, Electronic Structure and Magnetism of Their Compounds” (PDF). Acta Chim. Slov. 60 (3): 455—470. Arhivirano iz originala (PDF) 07. 11. 2013. g. Pristupljeno 30. 08. 2020.

[1]

[2]

[3]

[4]

[5]

[6]

[7]

[8]

[9]

[10]

[11]

[note 1]

[12]

[13]

[14]

[15]

[16]

[17]

[18]

[19]