𝔖 Bobbio Scriptorium
✦   LIBER   ✦

Temperature and third-body dependence of the rate constant for the reaction O + O2 + M → O3 + M

✍ Scribed by C. L. Lin; M. T. Leu

Publisher
John Wiley and Sons
Year
1982
Tongue
English
Weight
730 KB
Volume
14
Category
Article
ISSN
0538-8066

No coin nor oath required. For personal study only.

✦ Synopsis

The flash photolysis resonance fluorescence technique was used to measure the rate constants of the reaction 0 + 0 2 + M -0 3 + M (M = N2,02. Ar, and He) as a function of temperature. The results for the rate constants are given by knf(218

The activation energies with N2,02, and Ar as third bodies are equal within the experimental error, (-1370 f 340 cal/mol), and the relative third-body efficiencies at 298 K for Nz. 02, Ar, and He are 1.00,0.99,0.69, and 0.60, respectively.

📜 SIMILAR VOLUMES

A reinvestigation of the temperature dep
A reinvestigation of the temperature dependence of the rate constant for the reaction O + O2 + M → O3 + M (for M = O2, N2, and Ar) by the flash photolysis resonance fluorescence technique
✍ Odo Klais; Philip C. Anderson; Michael J. Kurylo 📂 Article 📅 1980 🏛 John Wiley and Sons 🌐 English ⚖ 915 KB

## Abstract The flash photolysis resonance fluorescence technique has been used to reinvestigate the kinetics of the oxygen atom–oxygen molecule combination reaction. Third‐order rate constants for O~2~, N~2~, and Ar as deactivant molecules were determined over the temperature range of 219–368 K. T

Temperature dependence of the rate const
Temperature dependence of the rate constant for the reaction OH + H2S in He, N2, and O2
✍ Yu-Lin Lin; Niann-Shiah Wang; Yuan-Pern Lee 📂 Article 📅 1985 🏛 John Wiley and Sons 🌐 English ⚖ 699 KB

The rate constants of the reaction between OH and H2S in He, N,, and O2 over the temperature range 245-450 K have been determined using the discharge flow-resonance fluorescence technique. At 299 K, kl = (4.4 ? 0.7) x lo-'' cm3 molecule-' S K I . T h e t e m p e r a t u r e dependence of t h e r a

Determination of the rate coefficients o
Determination of the rate coefficients of the SO2 + O + M → SO3 + M reaction
✍ S. M. Hwang; J. A. Cooke; K. J. De Witt; M. J. Rabinowitz 📂 Article 📅 2010 🏛 John Wiley and Sons 🌐 English ⚖ 360 KB 👁 1 views

Rate coefficients of the title reaction R 31 (SO 2 + O + M → SO 3 + M) and R 56 (SO 2 + HO 2 → SO 3 + OH), important in the conversion of S(IV) to S(VI), were obtained at T = 970-1150 K and ρ ave = 16.2 μmol cm -3 behind reflected shock waves by a perturbation method. Shockheated H 2 /O 2 /Ar mixtur

The decomposition of dimethyl peroxide a
The decomposition of dimethyl peroxide and the rate constant for CH3O + O2 → CH2O + HO2
✍ John R. Barker; Sidney W. Benson; David M. Golden 📂 Article 📅 1977 🏛 John Wiley and Sons 🌐 English ⚖ 951 KB

The decomposition of dimethyl peroxide (DMP) was studied in the presence and absence of added NO, to determine rate constants k l and k z in the temperature range of 391-432OK: The results reconcile the studies by Takezaki and Takeuchi, Hanst and Calvert, and Batt and McCulloch, giving log kl(sec-1

A study of the reaction NO3 + NO2 + M →
A study of the reaction NO3 + NO2 + M → N2O5 + M(M = N2, O2)
✍ Timothy J. Wallington; Roger Atkinson; Arthur M. Winer; James N. Pitts Jr. 📂 Article 📅 1987 🏛 John Wiley and Sons 🌐 English ⚖ 359 KB

The gas-phase reaction of the NOa radical with NO, was investigated, using a flash photolysis-visible absorption technique, over the total pressure range 25-400 Torr of nitrogen or oxygen diluent a t 298 2 2 K. The absolute rate constants determined (in units of em3 molecule-' s-') a t 25, 100, and

The rate constant of NO + O3 → NO2 + O2
The rate constant of NO + O3 → NO2 + O2 in the temperature range of 283–443 K
✍ H. H. Lippmann; Barbara Jesser; Ulrich Schurath 📂 Article 📅 1980 🏛 John Wiley and Sons 🌐 English ⚖ 398 KB

## Abstract The reaction NO + O~3~ → NO~2~ + O~2~ has been studied in a 220‐m^3^ spherical stainless steel reactor under stopped‐flow conditions below 0.1 mtorr total pressure. Under the conditions used, the mixing time of the reactants was negligible compared with the chemical reaction time. The p