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Sander, S. P.

Publications and source records attributed to Sander, S. P..

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NASA NTRS1984

Kinetics and mechanism of HO2 and DO2 disproportionations

A flash photolysis/UV abosrption technique was used to study the HO2 + HO2 and DO2 + DO2 reactions in the gas phase. Rate constants were measured at pressures between 100 and 700 torr of Ar and N2, and at temperatures between 230 and 420 K with up to 10 torr of added water vapor. The overall disproportionation rate constants for the reaction is given as the sum of pressure-independent and pressure-dependent terms. A kinetic analysis shows that both reactions have a zero-pressure bimolecular component and a termolecular component which is linearly dependent on pressure up to 700 torr. A priori estimates of the vibrational frequencies of the product of the HO2 + HO2 reaction suggest binding energies of 12-20 kcal per mol (for the initial association).

Kircher, C. C.↗
NASA NTRS1984

Pressure and temperature dependence of the reaction NO2 + NO3 + M yields N2O5 + M

The pressure and temperature dependences of the reaction NO2 + NO3 + M which yields N2O5 + M are investigated by using the flash photolysis/visible absorption technique in which the pseudo-first-order decay of NO3 is monitored as a function of total pressure (20-700 torr), diluent gas (M = He and N2), and temperature (236-358 K). The reaction is found to be in the falloff region in the 20-700 torr pressure range with collision efficiencies increasing in the order He less than N2. Falloff parameters are obtained by fitting the experimental data to the falloff equation of Troe and co-workers. The expression for k1(N2 concentration, T) is obtained and compared with the evaluations presented in the NASA (DeMore, 1983) and CODATA (Baulch et al., 1982) reviews of kinetic data for atmospheric chemistry. Both evaluations are based on N2O5 thermal decomposition data coupled with estimates of the equilibrium constant. The significance of the reactions for atmospheric chemistry rests not only on their rates but on the extent to which they result in a permanent sink for NOX.

Kircher, C. C.↗
NASA NTRS1984

Low-pressure study of the HO2 + HO2 reaction at 298 K

The rate constant for the reaction HO2 + HO2 yields H2O2 + O2 was measured at 298 K and 1 torr total pressure of helium by using the discharge flow technique. A quadrupole mass spectrometer was used to detect HO2 in conjunction with in situ long-path ultraviolet absorption which was used for calibration. A value of 1.5 + or - 0.4 x 10 to the -12th per molecule/s was obtained for k1 where the rate constant is defined by the relation -d(HO2)/dt = 2K1(HO2)HO2.

Sander, S. P.↗
NASA NTRS1981

Kinetics and mechanism of the disproportionation of BrO radicals

In the reported investigation, measurements were conducted of the rate constant for the reaction BrO + BrO yields products (1), taking into account the temperature range from 223 to 338 K and the pressure range from 50 to 475 torr of He. The flash photolysis-ultraviolet absorption technique was employed in the experiments. Two independent approaches were used to determine the relative rates of the two reaction branches, BrO + BrO yields BrOO + Br (1a), and BrO + BrO yields Br2 + O2 (1b), one dependent and the other independent of the BrO absorption cross section with the results being in excellent agreement. The rate constant, k(1), was found to be independent of pressure.

Sander, S. P.↗
NASA NTRS1981

Temperature dependence of the self-reaction of CH3O2 radicals

The rate constants for the reaction CH3O2 + CH3O2 yields products (1) were measured in the temperature range from 248 to 417 K, taking into consideration pressures in the range from 60 to 700 torr of N2. The experimental investigation was carried out in a Pyrex flash photolysis system employing ultraviolet absorption detection. Methylperoxy radicals (CH3O2) were produced by the photolysis of Cl2-CH4-O2 mixtures. Rate constants were measured by observing the second-order disappearance of CH3O2 radicals. Plots of 1/(CH3O2 optical density) vs. time were observed to be linear over a concentration change of a factor of 10-50. Results of the kinetic runs at each temperature are summarized in a table, and an Arrhenius plot of the data is shown in a graph.

Sander, S. P.↗
NASA NTRS1981

A kinetics study of the reaction of SO2 with CH3O2

The reaction of CH3O2 with SO2 has been studied using the flash photolysis/ultraviolet absorption technique. In contrast to previous measurements, no reaction could be detected over the temperature range 298-423 K. An upper limit of 5 x 10 to the -17th cu cm/molecule/sec has been determined for the reaction rate constant.

Sander, S. P.↗
NASA NTRS1980

Kinetics studies of the reactions of CH3O2 with NO, NO2, and CH3O2 at 298 K

Rate constants for the reactions of CH3O2 with NO, NO2, and CH3O2 at 298 K were measured by using the FP/UV technique. The disappearance of CH3O2 was observed over a wide range of reactant concentrations and total pressure. It is shown that the reaction of CH3O2 with NO2 is still in the falloff region at 700 torr and that the high-pressure limit is attained only at pressures exceeding several atmospheres.

Sander, S. P.↗
NASA NTRS1980

Atmospheric bromine and ozone perturbations in the lower stratosphere

The role of bromine compounds in the photochemistry of the natural and perturbed stratosphere has been reexamined using an expanded reaction scheme and the results of recent laboratory studies of several key reactions. The most important finding is that through the reaction BrO + ClO yielding Br + Cl + O2 there is a synergistic effect between bromine and chlorine which results in an efficient catalytic destruction of ozone in the lower stratosphere. One-dimensional photochemical model results indicate that BrO is the major bromine species throughout the stratosphere, followed by BrONO2, HBr, HOBr and Br. It is shown from the foregoing that bromine is more efficient than chlorine as a catalyst for destroying ozone, and the implications for stratospheric ozone of possible future growth in the industrial and agricultural use of bromine are discussed. Bromine concentrations of 20 pptv (2 x 10 to the -11th power), as suggested by recent observations, can decrease the present-day integrated ozone column density by 2.4%, and can enhance ozone depletion from steady-state chlorofluoromethane release at 1973 rates by a factor of 1.1-1.2.

Yung, Y. L.↗
NASA NTRS1979

Pressure and temperature dependence kinetics study of the NO + BrO yielding NO2 + Br reaction - Implications for stratospheric bromine photochemistry

The reactivity of NO with BrO radicals over a wide range of pressure (100-700 torr) and temperature (224-398 K) is investigated using the flash photolysis-ultraviolet absorption technique. The flash photolysis system consists of a high-pressure xenon arc light source, a reaction cell/gas filter/flash lamp combination, and a 216.5 half-meter monochromator/polychromator/spectrography for wavelength selectivity. The details of the reaction and its corresponding Arrhenius expression are identified. The results are compared with previous measurements, and atmospheric implications of the reaction are discussed. The NO + BrO yielding NO2 + Br reaction is shown to be important in controlling the concentration ratios of BrO/Br and BrO/HBr in the stratosphere, but this reaction does not affect the catalytic efficiency of BrOx in ozone destruction.

Watson, R. T.↗
NASA NTRS1976

Chemical kinetics of homogeneous atmospheric oxidation of sulfur dioxide

A systematic evaluation of known homogeneous SO2 reactions which might be important in air pollution chemistry is carried out. A mechanism is developed to represent the chemistry of NOx/hydrocarbon/SO2 systems, and the mechanism is used to analyze available experimental data appropriate for quantitative analysis of SO2 oxidation kinetics. Detailed comparisons of observed and predicted concentration behavior are presented. In all cases, observed SO2 oxidation rates cannot be explained solely on the basis of those SO2 reactions for which rate constants have been measured. The role of ozone-olefin reactions in SO2 oxidation is elucidated.

Sander, S. P.↗