Reduction Potentials

O₂/O₂•^–

E = –330(mV)
Recommended value.

Berdnikov, V.M.; Zhuravleva, O.S.
Russ. J. Phys. Chem. 46(10): 1521-3 (1972)

E = –330(mV)

Calcn.

Chevalet, J.; Rouelle, F.; Gierst, L.; Lambert, J.P.
J. Electroanal. Chem. Interfacial Electrochem. 39(1): 201-16 (1972)

E = –288(mV)

Pol.; –532 mV vs SCE

Wood, P.M.
FEBS Lett. 44(1): 22-4 (1974)

E = –330(mV)

Reference compound: DQ
Reference E: –250 mV

Calcn.

Ilan, Y.A.; Meisel, D.; Czapski, G.
Isr. J. Chem. 12(4): 891-5 (1974)

E = –330(mV), ionic strength = 0.1, pH = 7.2

Reference compound: 1.1.4
Reference E: –67 mV
Co-solute: HCO₂^–

Concentrations used to estimate equilibrium constant(+Kinetics used to estimate equilibrium constant).

Ilan, Y.A.; Meisel, D.; Czapski, G.
Isr. J. Chem. 12(4): 891-5 (1974)

E = –310(mV)

Reference compound: DQ

Calc. from data in 730125.

Meisel, D.; Czapski, G.
J. Phys. Chem. 79(15): 1503-9 (1975)

E = –325(mV), pH = 7

Reference compound: DQ
Reference E: –235 mV
Co-solute: HCO₂^–

Concentrations used to estimate equilibrium constant; –155 mV for 1 mol dm^–3 O₂.

Sawada, Y.; Iyanagi, T.; Yamazaki, I.
Biochemistry 14(17): 3761-4 (1975)

E = –330(mV), pH = 7

Reference compound: 1.1.1
Reference E: 100 mV

Kin. reaction QH₂ + H₂O₂ cat. peroxidase.