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Volume 63, 1967
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Mechanism of chemiluminescent reaction between nitric oxide and ozone

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 type: Paper
DOI: 10.1039/TF9676300915
Citation: 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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