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Flash photolysis resonance fluorescence investigation of the reaction of Cl(2P) atoms with ClONO2

โœ Scribed by Michael J. Kurylo; Ronald G. Manning


Publisher
Elsevier Science
Year
1977
Tongue
English
Weight
426 KB
Volume
48
Category
Article
ISSN
0009-2614

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Flash photolysis resonance fluorescence
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The flash photolysis resonance fluorescencc technique has been used to measure the rrtte constant for the rcaction of O(3P) atoms with CION at 10 torr total pressure over the temperature range 225-273 K. The values obtained can be fit to the Arrhenius equation kr = (1.87 f 1.29) X 10-12 exp[ -(692 i

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The reaction of Cl atoms with chlorine nitrate has been reinvestigated by flash photolysis resonance fluorcsccnce over the temperature range 220-296 I;. The new results can be tit to the Arrhenius expression kr = 7.3 X 10-r\* esp(165/7I cm3 molecule-' s-l, in good agreement with another recent study

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Rate constants for the reaction of OH radicals with CCS and CS, have been determined at 296 K using the flash photolysis resonance fh~orescen~ technique. The values derived from this study are kOH +mS = (5.66 \* 1.21) X lo-l4 cm3 mokcuk-' s-l a& \_+OH + CS2 = (1 .I35 2 0.34) X lOmu cm3 molecu!e-' s-

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Rate constants for the reaction of OH radicals in a homogeneous gas phase reaction with dhnethyl sulfide have been determined using the flash photolysis resonance fluorescence technique over the temperature range 273400 K. The data (combined with the results of another recent study) can be fit to th

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## Abstract The flash photolysis resonance fluorescence technique has been used to measure the rate constant for the reaction equation image over the temperature range of 250โ€“370 K. The present results are in excellent agreement with three very recent studies, and the combined data set can been u

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Using the technique of flash photolysis-resonance fluorescence, absolute rate constants have been measured for the reaction H + 0 2 + M 4 HOz + M over a temperature range of 220-360ยฐK. Over this temperature range, the data could be fit to an Arrhenius expression of the following form: The units for