The kinetics and mechanism of the chlorine(III)-bromine reaction are studied by the stopped-flow method under acidic conditions in 1.0 M NaClO4 and at 25.0 °C. There are two kinetically well-separated phases in this reaction. A detailed mechanism is proposed for the first phase of the reaction, in which Br2 oxidizes ClO2- to chlorine dioxide. It is confirmed that the oxidation occurs via competing parallel reaction steps. The autoinhibition observed in the reaction is attributed to a backward shift in the reversible initial step as the oxidation proceeds. On the basis of simultaneous evaluations of the kinetic traces, the following forward rate constants are obtained for the kinetically significant reaction steps: Br2 + ClO2- = ClO2 + Br2-, k1 = (1.3 ± 0.2) x 103 M-1 s-1 (k-1 = 1.1 x 109 M-1 s-1); Br2- + ClO2- = ClO2 + 2Br-, k2 = (4.0 ± 0.1) x 106 M-1 s -1; Br + ClO2- = ClO2 + Br-, k8 = (2.3 ± 0.7) x 108 M-1 s-1; HOBr + HClO2 = BrClO2 + H20 (BrClO2 + ClO2- = Br- + 2ClO2, very fast), k9 = (1.9 ± 0.1) x 105 M-1 s-1. The possible kinetic role of the reactive BrClO2 intermediate is discussed in detail.
ASJC Scopus subject areas
- Physical and Theoretical Chemistry
- Inorganic Chemistry