The determinations of rate constants for the reactions de Cl atoms with organic compounds could show discrepancies when they are carried out in N2 or air as the diluent gas. Kaiser and Wallington [1] discovered that the apparent rate constant of the reaction “Cl + C2H4 ® Products” increased when the amount of O2 in the diluent gas was raised. They observed that O2 affected the measured rate constant indicating that reactions of C2H4 with radicals other than Cl may occur at low pressures in their relative rate determinations, leading to erroneous results in the presence of O2. In agreement with Michael et al. [2] and Tyndall et al. [3], Kaiser and Wallington indicated that the potential interference is the OH radical formed via secondary reactions involving O2 and that the magnitude of this interference may depend on the total pressure and on the initial reactant concentrations.
The aims of this study have been:
* Extending the existing scant data base of rate constants for the reactions of chlorine atoms with hydrochloroethers as part of ongoing work in our laboratory regarding the atmospheric impact of these compounds as acceptable candidates to replace the harmful CFCs and their derivatives in industrial uses.
* Testing the potential systematic errors that could affect the rate coefficients for the reactions studied due to interference by OH radicals.
A relative rate technique was used to study the kinetics of the reactions of Cl atoms with CH3OCHCl2 and CH3OCH2CH2Cl at (298 ± 2)K and atmospheric pressure (~ 750 Torr), using synthetic air as diluent gas. All the experiments were carried out in a
To the best of our knowledge, this kinetic study constitutes the first experimental determination of the rate coefficient for the reaction of Cl atoms with CH3OCHCl2.
The results obtained will be presented and compared with those obtained previously for the same and related reactions of Cl atoms. The atmospheric implications for the studied hydrochloroethers are considered briefly.
[1] Kaiser, E.W., Wallington, T.J., 1996. Journal of Physical Chemistry 100, 4111.
[2] Michael, J.V., Keil, D.G., Klemm, R.B., 1985. Journal of Chemical Physics 83, 1630.
[3] Tyndall, G.S., Staffelbach, T.A., Orlando, J.J., Calvert, J.G., 1995. International Journal of Chemical Kinetics 27, 1009.