Abstract
Ammonia is oxidized by nitrous oxide
smoothly and homogeneously at temperatures between 658 and 730� and total
pressures up to 250 mm. The products of reaction, nitrogen, water, and
hydrazine are accounted for by a free-radical mechanism initiated by oxygen
atoms which result from the thermal decomposition of nitrous oxide. Ammonia
labelled with the 15N-isotope was used to distinguish between the nitrogen
formed from the nitrous oxide and that from the ammonia.
The kinetics follow an empirical rate
equation, ������������� Rate = k'[N2O]1.56
+ k"[N2O]0.61[NH3]. This is of a form which
shows the importance of the ammonia molecule participating in the activation of
nitrous oxide through bimolecular collision. Assigning a collisional efficiency
of unity for like N2O-N2O collisions, the efficiency of
ammonia in the process ������������ NH3 + N2O →
NH3 + N2O* is determined as 0.85.
Cited by
2 articles.
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1. Examples of Reactions Catalysed by Acids and Bases;The Proton in Chemistry;1973
2. Bibliography;Guide to Gas Chromatography Literature;1967