Abstract
The kinetics of oxidation of iodine by chlorite is much more complicated than previously found. The rate exhibits a minimum as a function of hydrogen ion concentration, the reaction being characteristically autocatalytic, mainly due to the fact that oxidation of iodine is even faster by hypochlorous acid and chlorine. An important feature of the reaction is the acceleration of the disproportionation of chlorite by the intermediates of the title reaction, leading to the formation of a significant amount of chlorine dioxide. The rate cannot be described by an overall equation, but all the findings can be quantitatively explained by a mechanism consisting of 13 elementary or quasi-elementary steps. The stoichiometry of the reaction is kinetically controlled. Formation and reactions of Cl2O2 seem to play a crucial role in the reaction and in other reactions involving chlorite.
| Original language | English |
|---|---|
| Pages (from-to) | 1195-1199 |
| Number of pages | 5 |
| Journal | Inorganic Chemistry |
| Volume | 26 |
| Issue number | 8 |
| Publication status | Published - 1987 |
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- Inorganic Chemistry
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Kinetics and mechanism of the autocatalytic reaction between iodine and chlorite ion. / Rábai, G.; Beck, Mihály T.
In: Inorganic Chemistry, Vol. 26, No. 8, 1987, p. 1195-1199.Research output: Contribution to journal › Article
}
TY - JOUR
T1 - Kinetics and mechanism of the autocatalytic reaction between iodine and chlorite ion
AU - Rábai, G.
AU - Beck, Mihály T.
PY - 1987
Y1 - 1987
N2 - The kinetics of oxidation of iodine by chlorite is much more complicated than previously found. The rate exhibits a minimum as a function of hydrogen ion concentration, the reaction being characteristically autocatalytic, mainly due to the fact that oxidation of iodine is even faster by hypochlorous acid and chlorine. An important feature of the reaction is the acceleration of the disproportionation of chlorite by the intermediates of the title reaction, leading to the formation of a significant amount of chlorine dioxide. The rate cannot be described by an overall equation, but all the findings can be quantitatively explained by a mechanism consisting of 13 elementary or quasi-elementary steps. The stoichiometry of the reaction is kinetically controlled. Formation and reactions of Cl2O2 seem to play a crucial role in the reaction and in other reactions involving chlorite.
AB - The kinetics of oxidation of iodine by chlorite is much more complicated than previously found. The rate exhibits a minimum as a function of hydrogen ion concentration, the reaction being characteristically autocatalytic, mainly due to the fact that oxidation of iodine is even faster by hypochlorous acid and chlorine. An important feature of the reaction is the acceleration of the disproportionation of chlorite by the intermediates of the title reaction, leading to the formation of a significant amount of chlorine dioxide. The rate cannot be described by an overall equation, but all the findings can be quantitatively explained by a mechanism consisting of 13 elementary or quasi-elementary steps. The stoichiometry of the reaction is kinetically controlled. Formation and reactions of Cl2O2 seem to play a crucial role in the reaction and in other reactions involving chlorite.
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UR - http://www.scopus.com/inward/citedby.url?scp=0001420174&partnerID=8YFLogxK
M3 - Article
AN - SCOPUS:0001420174
VL - 26
SP - 1195
EP - 1199
JO - Inorganic Chemistry
JF - Inorganic Chemistry
SN - 0020-1669
IS - 8
ER -