Mechanism and kinetics of the reaction between hydrogen iodide and ozone

Larin, I. K.; Spasskii, A. I.; Trofimova, E. M.; Turkin, L. E.

doi:10.1134/s0023158407010016

Cited by 10 publications

(14 citation statements)

References 9 publications

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“…The high degree of 131 I localization in the chamber is likely due to high chemical activity of the products of CH 3 131 I photolysis. This agree with formation of reactive atomic iodine upon irradiation of CH 3 I with a mercury lamp, reported in [6].…”

Section: Resultssupporting

confidence: 91%

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Gas-Phase UV Photolysis of CH3 131I

et al. 2005

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Gas-phase UV photolysis of 131 I-labeled CH 3 I was studied. CH 3 131 I (228 mg) is completely photolyzed within 5 min under the static conditions at room temperature in an argon atmosphere. The final radioiodine compound formed under these conditions is 131 I 2 . The chemical composition of the final products of CH 3 I photolysis in air is more complex. Agglomeration corcystallization of the CH 3 I photolysis products with NH 4 Cl in the gas phase was studied. The results of this study suggest that the main final product of CH 3 I photolysis in air is a fine I x O y aerosol. In the presence of NH 4 Cl, formation of NH 4 131 I aerosols is possible.

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Section: Resultssupporting

confidence: 91%

“…This is due to partial radiolysis of CH 3 I to form water-soluble iodine species. In addition, CH 3 I is photolyzed on exposure to UV radiation to form chemically active atomic iodine [6]. Thus, CH 3 I can decompose into various chemical species on exposure to external radiation.…”

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confidence: 99%

Gas-Phase UV Photolysis of CH3 131I

et al. 2005

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“…The only experimental study of the reaction (Larin et al, 1999) gives upper limits for the rate coefficients for the two channels which are substantially higher than the corresponding rate coefficients for the analogous reactions of FO, ClO, and BrO radicals. It is likely that the rate coefficients are substantially smaller but the measured upper limits are provisionally accepted.…”

Section: Comments On Preferred Valuesmentioning

confidence: 86%

Evaluated kinetic and photochemical data for atmospheric chemistry: Volume III – reactions of inorganic halogens

Atkinson¹,

Baulch²,

Cox³

et al. 2006

Preprint

141

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Abstract. This article, the third in the series, presents kinetic and photochemical data evaluated by the IUPAC Subcommittee on Gas Kinetic Data Evaluation for Atmospheric Chemistry. It covers the gas phase and photochemical reactions of inorganic halogen species, which were last published in J. Phys. Chem. Ref. Data in 2000 (Atkinson et al., 2000), and were updated on the IUPAC website in 2003. The article consists of a summary sheet, containing the recommended kinetic parameters for the evaluated reactions, and five appendices containing the data sheets, which provide information upon which the recommendations are made.

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“…The only experimental study of the reaction (R1) was made by Bale et al, 14 who obtained a value of k 1 (295 K) = (6.0 AE 1.3) Â 10 À11 cm 3 molecule À1 s À1 . Reaction (R3) between IO and O 3 was studied by Larin et al 15 who obtained upper limits for the rate coefficients k 3a (323 K) o 2.6 Â 10 À16 cm 3 molecule À1 s À1 and k 3b (292 K) r1.2 Â 10 À15 cm 3 molecule À1 s À1 . 15 The focus of this work was to measure rate coefficients, k, for the reactions: IO + CH 3 O 2products (R1) and the analogous fluorinated reaction IO + CF 3 O 2products (R2), which may play a role in our laboratory experiments on (R1) as CF 3 I was present as IO source.…”

Section: Io þ Homentioning

confidence: 99%

Laser induced fluorescence studies of iodine oxide chemistry : Part II. The reactions of IO with CH3O2, CF3O2 and O3

Dillon

Tucceri

Crowley

2006

Phys. Chem. Chem. Phys.

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The technique of pulsed laser photolysis was coupled to laser induced fluorescence detection of iodine oxide (IO) to measure rate coefficients, k for the reactions IO + CH(3)O(2)--> products (R1, 30-318 Torr N(2)), IO + CF(3)O(2)--> products (R2, 70-80 Torr N(2)), and IO + O(3)--> OIO + O(2) (R3a). Values of k(1) = (2 +/- 1) x 10(-12) cm(3) molecule(-1) s(-1), k(2) = (3.6 +/- 0.8) x 10(-11) cm(3) molecule(-1) s(-1), and k(3a) <5 x 10(-16) cm(3) molecule(-1) s(-1) were obtained at T = 298 K. In the course of this work, the product yield of IO from the reaction of CH(3)O(2) with I was determined to be close to zero, whereas CH(3)OOI was formed efficiently at 70 Torr N(2). Similarly, no evidence was found for IO formation in the CF(3)O(2) + I reaction. An estimate of the rate coefficients k(CH(3)O(2) + I) = 2 x 10(-11) cm(3) molecule(-1) s(-1) and k(CH(3)OOI + I) = 1.5 x 10(-10) cm(3) molecule(-1) s(-1) was also obtained. The results on k(1)-k(3) are compared to the limited number of previous investigations and the implications for the chemistry of the marine boundary layer are briefly discussed.

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Mechanism and kinetics of the reaction between hydrogen iodide and ozone

Cited by 10 publications

References 9 publications

Gas-Phase UV Photolysis of CH3 131I

Gas-Phase UV Photolysis of CH3 131I

Evaluated kinetic and photochemical data for atmospheric chemistry: Volume III – reactions of inorganic halogens

Laser induced fluorescence studies of iodine oxide chemistry : Part II. The reactions of IO with CH3O2, CF3O2 and O3

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