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The plots of ln([OXC]/[OXC]0) vs ∫[Cl2]dt, ∫[ClO2]dt and ∫[O3]dt shown in Figure S1 (available with the online version of this paper) exhibit straight lines with slopes of kapp. All the reactions strictly followed the second-order kinetic model with the coefficient of determination (R2) > 0.99. In addition, the plots of ln([OXC]/[OXC]0) vs reaction time (t) show satisfactory linear form (R2 > 0.99), which mean pseudo-first-order kinetics with respect to OXC concentration during all processes (Figure S2, available with the online version of this paper). The calculated kapp, kobs and t1/2 (half-life of OXC oxidation) are compiled in Table 1. Ozonation was most effective with regard to OXC degradation with a kapp value of 3.02 × 103 M−1 s−1, while ClO2 oxidation and chlorination were of much lower efficiency with kapp values of 3.42 × 102 M−1 s−1 and 1.46 × 102 M−1 s−1, respectively. The values of t1/2 calculated from Figure S2 also demonstrated that ozonation was fastest in OXC degradation with the value of 239 s.

Table 1

Rate constants and t1/2 for OXC oxidation by Cl2, ClO2 and O3

OXCa degradationkapp (M−1 s−1)R2kobs (s−1)R2t1/2 (s)
By Cl2 1.46 × 102 0.990 1.19 × 10−4 0.994 6,766 
By ClO2 3.42 × 102 0.994 1.29 × 10−4 0.997 5,218 
By O3 3.02 × 103 0.995 2.72 × 10−3 0.993 239 
OXCa degradationkapp (M−1 s−1)R2kobs (s−1)R2t1/2 (s)
By Cl2 1.46 × 102 0.990 1.19 × 10−4 0.994 6,766 
By ClO2 3.42 × 102 0.994 1.29 × 10−4 0.997 5,218 
By O3 3.02 × 103 0.995 2.72 × 10−3 0.993 239 

a[OXC]0: 0.40 μmol L−1.

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