Table 1.

Hydrogen peroxide-based oxidation reactions.

H2O2 activation and related reactions.
H2O2 + Fe2+ → Fe3+ + OH− + •OH	R 1
H2O2 + Fe3+ → Fe2+ + $•{\text{O}}_2^{-}$ + 2H+	R 2
$•{\text{O}}_2^{-}$ + Fe3+ → Fe2+ + O2	R 3
•OH + RhB → products k4 = 2.5 × 1010 1/M × s (Buxton et al., 1988)	R 4
•OH + ${\text{Σ}}_{\text{i}=1}^{\text{n}}$ [Si] → products	R 5
•OH + H2O2 → HO2•− + H2O k6 = 2.7 × 107 1/M × s (Buxton et al., 1988)	R 6
•OH + ≡Si → products	R 7
2H2O2 $\stackrel{\text{Mn- and some Fe-oxides}}{\to }$ O2 + H2O	R 8
2H2O2 $\stackrel{\text{Fe-oxide}}{\to }$ • OH2 + HO2•− + H2O	R 9
H2O2 $\stackrel{\text{UV}}{\to }$ 2 •OH	R 10

Note: ${\text{Σ}}_{\text{i}=1}^{\text{n}}$ [S_i] is the pseudo-first-order rate constant (k_s 1/s) for •OH scavenging by all constituents in solution except the target compound.