In the experiment, below gas-phase homogenous oxidation, k 2 NO + O2 -------> 2NO2 was confirmed to have the third-order kinetics, showing an elementary reaction, at least for low partial pressures of nitrogen oxides. However, the rate constant k actually decreases with increasing absolute temperature, indicating an apparently negative activation energy. It is
In the experiment, below gas-phase homogenous oxidation, k
2 NO + O2 -------> 2NO2
was confirmed to have the third-order kinetics, showing an elementary reaction, at least for low partial pressures of nitrogen oxides. However, the rate constant k actually decreases with increasing absolute temperature, indicating an apparently negative activation energy. It is known that any elementary reaction must have a positive energy.
Provide an explanation, starting from the fact that an active intermediate species, NO3, is a participant in some other know reactions that involve oxides of nitrogen. Other active intermediates could be NO* and O2* and O* (oxygen atom). Using
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