Abstract
The reaction between active nitrogen and acetylene was studied in a low-pressure flow reactor using a leak to a mass spectrometer as the analytical device and varying reaction time from a few to 45 ms. In mixtures in which the initial ratio of acetylene to atomic nitrogen is larger than unity a comparatively slow reaction takes place whose main products are cyanogen, hydrogen and cyanoacetylene. The reaction is accelerated by rising pressure and temperature. The proposed rate determining steps are C
2
H
2
+ N
K1
⇆
K-1
C
2
H
2
N*, C
2
H
2
N*+ N
2
→
K2
C
2
H
2
N+ N
2
with
K
1
= 1·1X 10
-12(+-0·12)
exp (-2000(±400)/
RT
) cm
3
molecule
-1
s
-1
and
k
-1
= 4x10
-s
T
e
s
-1
, if
k
2
is taken to be the collisional frequency. The radical C
2
H
2
N is found to react competitively with nitrogen atoms and with acetylene to form the end products. At low (≤ 0·5) initial acetylene to atomio nitrogen ratios a much faster reaction occurs which is accompanied by chemiluminescence of CH and CN radicals and whose main products are hydrogen cyanide, cyanogen and hydrogen. Simultaneously, a rapid recombination of nitrogen atoms takes place, as many as 20 atoms reacting per molecule of acetylene consumed. This rapid reaction has a negative temperature coefficient. It is suggested that this is a chain reaction started by metastable nitrogen molecules (
A
3
Σ
+
u
) nitrogen atoms which react with acetylene to form hydrogen cyanide and cyanide radicals. The latter cause the recombination of nitrogen atoms by the chain reactions CN + N + N
2
→ NCN + N
2
NCN+N → N*
2
+ CN, with 3 x 10-30 <k
6
< 2 x 10
-29
cm
6
molecule
-2
s
-1
. These chains are broken by recombination of cyanide radicals and by the reactions of CN and NCN radicals with acetylene. Cyanogen also causes a catalytic recombination of nitrogen atoms. Ammonia added to acetylene-active nitrogen mixtures suppresses the rapid reaction but has no effect on the slow reaction in richer mixtures.
Reference26 articles.
1. Arrington C. A. 1965 Harvard University Ph.D. Thesis.
2. Bayes K. D. 1961 Can.J .Ghem. 39 1074.
3. chem;Berkowitz J.;Phys.,1956
4. Bernardini O. O. 1967 Harvard University Ph.D. Thesis.
5. Campbell I. M. & Thrush B. A. 1964 Proc. Ghem. Soc. p. 410.
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