Volume 63, 1967
From the journal:

Transactions of the Faraday Society

Mechanism of chemiluminescent reaction between nitric oxide and ozone

P. N. Clough  and  B. A. Thrush  

Abstract

The absolute intensity and quenching constants of the NO2 emission in the chemiluminescent reaction between nitric oxide and ozone have been determined using a large capacity-flow reactor at low pressures. These studies have confirmed the mechanism previously proposed: NO+O3= NO*2(2B1)+O2(1a) NO+O3= NO2(2A1)+O2(1b) NO*2= NO2+hv(2) M+NO2= NO2+M (3) The rate constants of the primary steps are k1a=(7.6 ± 1.5)× 1011 exp (–4180 ± 300/RT) and k1b=(4.3 ± 1.0)× 1011 exp (–2330 ± 150/RT) cm3 mole–1 sec–1. The half-quenching pressures (k2/k3m) of electronically excited NO2 produced are: Ar = 13.0 ± 1.0 µ, O2= 8.3 ± 0.5 µ, NO = 5.2 ± 0.3 µ, NO2= 3.7 ± 0.1 µ. The detailed mechanism of reactions (1a) and (1b) is discussed.

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Article information

DOI
https://doi.org/10.1039/TF9676300915
Article type
Paper

Trans. Faraday Soc., 1967,63, 915-925

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Mechanism of chemiluminescent reaction between nitric oxide and ozone

P. N. Clough and B. A. Thrush, Trans. Faraday Soc., 1967, 63, 915 DOI: 10.1039/TF9676300915

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