Oxygen atoms reaction with

Fehlner and Strong produced oxygen atoms at 25 and 100 °C from the mercury-sensitized photolysis of N2O. The oxygen atoms reacted with B2H6 to produce H2, B4H10, B5H9, and a white solid of empirical formula HBO. The proposed reaction steps included 

Fontijn and Vree ° examined the reaction of O atoms and electronically excited O2 [principally 02( Ag)] with B2H6. They prepared their active species in a 2450 me microwave discharge in O2 or Ar-02 mixtures. In the presence of O, but not in its absence, chemiluminescence was observed which could be attributed mainly to The emission was enhanced by the presence of elec- 

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Ozone can be destroyed thermally, by electron impact, by reaction with oxygen atoms, and by reaction with electronically and vibrationaHy excited oxygen molecules (90). Rate constants for these reactions are given ia References 11 and 93. Processes involving ions such as 0/, 0/, 0 , 0 , and 0/ are of minor importance. The reaction O3 + 0( P) — 2 O2, is exothermic and can contribute significantly to heat evolution. Efftcientiy cooled ozone generators with typical short residence times (seconds) can operate near ambient temperature where thermal decomposition is small. 

Such results strongly indicate that the S02 is converted into S03 in a termo-lecular reaction with oxygen atoms ... 

This equation accounts for all steps of A conversion in the reaction with oxygen atoms. 

Sato and Cvetanovi6 (88) studied in some detail the photooxidation of 1-butene and isobutene at 3660 A. The 1-butene exhibited all the features of the olefin reactions with oxygen atoms produced by the N2O technique. The addition products, a-butene oxide, n-butyraldehyde, and... 

This ion is not reactive with H2 but can react with a number of other heavy atoms assumed to be present in initial stages of the cloud. In particular, reaction with oxygen atoms leads eventually to the production of the molecular ion H30+ by a chain of exothermic ion-molecule reactions studied in the laboratory ... 

Ozone, produced in the stratosphere by the action of ultraviolet light on 02, helps shield the surface of the earth from harmful ultraviolet radiation. Ozone is slowly decomposed by reaction with oxygen atoms according to the following equation ... 

According to eqn. (109a), only CO may be replaced by inert gas without lowering the overall second limit pressure, and this is contrary to experiment. The situation can be modified by inclusion of further reactions, so that some semblance of agreement is obtained. However, there is a stronger objection. There is no evidence that CO reacts directly with O3 at 350 °C, the formation of CO2 in these conditions being due to reaction with oxygen atoms which arise from the thermal decomposition of the ozone[379, 380]. 

We now use the mass balance discrepancy to subtract the contribution of any "accumulation-reaction" processes present from the measured responses. For example, the corrected response curve for CO, shown in Fig. 12, was obtained at each instant in time by adding to the measured outlet CO concentration the amount of CO that was converted to CO2 by reaction with oxygen atoms stored in the catalyst, as determined from the oxygen balance. The fact that the corrected CO response and the corrected CO2 response, shown in Fig. 13, do not match the instantaneous response demonstrates the action of an "activity change" type of transient chemical process. The process resulted in lower-than-expected CO conversion, since the activity change process included in the simulation was partial deactivation of the catalyst in lean exhaust (e.g., by oxidation of the precious metal). 

The formation of the stratospheric ozone layer can be understood most simply on the basis of a reaction model composed of a minimum set of four elementary processes (a) the dissociation of oxygen molecules by solar radiation in the wavelength region 180-240 nm (b) the attachment of oxygen atoms to molecular oxygen, leading to the formation of ozone (c) the photodissociation of ozone in the Hartley band between 200 and 300 nm and (d) the destruction of ozone by its reaction with oxygen atoms. The reactions may be written... 

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