Abstract
The single temperature pulse technique, developed at the Cornell Aeronautical Laboratory, has been used to study the kinetics of the formation of nitric oxide in the temperature range from 2000° to 3000°K. It has been found that the kinetics of the reaction are consistent with the chain mechanism proposed by Zeldovich. The rate-determining step in the chain is: O+N2→NO+N, with ΔH25000=75.8 kcal/mole. The activation energy for this step is found to be 74±5 kcal/mole. The collision cross-section, as calculated from classical reaction rate theory, is 10—16 cm2, which corresponds to a steric factor of about 0.05, assuming σN2,O=5 A.
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