Table 1. Standard electrode and Nernst electrode potentials vs. SHE of the involved half-cell reactions.

Half cell	E 0 [V]	E NERNST [V]	Source E0
e– + [AuCl2]– ⇌ Au0 + 2Cl–	1.15	0.97 ± 0.03	36
e– + H2O ⇌ eaq–	–2.79	–2.28 ± 0.36	26
e– + H+ ⇌ H˙	–2.23	–2.09 ± 0.15	26
O2 + H+ + e– ⇌ HO2˙	–0.04	–0.27 ± 0.12	27
2H2O + 2e– ⇌ H2 + 2OH–	–0.83	–0.26 ± 0.42	37
2H+ + 2e– ⇌ H2	0.00	–0.09 ± 0.05	37
O2 + e– ⇌ O2˙–	–0.33	0.05 ± 0.14	27
O2 + 2H+ + 2e– ⇌ H2O2	0.70	0.49 ± 0.12	37
O2– + H+ + e– ⇌ HO2–	1.02	0.65 ± 0.16	27
O2 + 2H2O + 4e– ⇌ 4OH–	0.40	0.78 ± 0.28	37
HO2˙ + e– ⇌ HO2–	0.73	0.88 ± 0.24	27
O2˙– + 2H+ + e– ⇌ H2O2	1.73	0.92 ± 0.28	27
O2 + 2H+ + 4e– ⇌ 2H2O	1.27	0.98 ± 0.12	37
H2O2 + 2H+ + e– ⇌ 2H2O	1.76	1.05 ± 0.25	37
HO2˙ + H+ + e– ⇌ H2O2	1.46	1.18 ± 0.13	38
OH˙ + e– ⇌ OH–	1.83	1.95 ± 0.12	27