Abstract
Rate constants for the reaction N + O
2
(
1
∆
g
) →
k
1
NO + O (1) have been measured at four temperatures, and fitted to an Arrhenius expression,
k
1
=
A
exp ( ─
E
a
/
RT
). The results indicate that
A
≤ 2 x 10
-14
molecule
-1
cm
3
s
-1
and < 1.2 kcal (5.0 kJ ) mol
-1
: at room temperature (300 K ),
k
1
= 2.7 ± 1.0 x 10
-15
molecule
-1
cm
3
s
-1
. Reaction (1) cannot, therefore, proceed fast enough at 200 K for it to be an important source of nitric oxide in the atmospheric D-region. The rate constant for the reaction N + O
2
(
3
∑
─
g
) →
k
2
NO + O (2) has been measured at 302 K to be 1.08 ± 0.10 x 10
-16
molecule
-1
cm
3
s
-1
. This value, taken together with the data of earlier workers, suggests that
k
2
= 1.5 x 10
-11
exp (—7.1/
RT
) molecule
-1
cm
2
s
-1
. A possible explanation for the difference in pre-exponential factors for reactions (1) and (2) is presented.
Reference12 articles.
1. Clark I. D . & W ayn e R . P . 1969a Proc. Boy. Soc. Lond. A 3 1 4 111.
2. 6 Chem;Clark I. D .;Phys. Lett.,1969
3. Clark I. D . & W ayn e R . P . 1970 Molec. Phys. (in th e Press).
4. Kinetics of the reactions of active nitrogen with oxygen and with nitric oxide
5. J . geophys;Elroy M. B .;Res.,1968
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