The rate law for the reaction 2NO₂ + O₃ $\rarr$N₂O₅ + O₂ is rate = k[NO₂][O₃]. Which one of the following mechanisms is consistent with this rate law

Question

Quizplus · Accepted Answer

- Option A has a fast step involving N₂O₄, which is not in the rate law. - Option B has a fast step involving NO₅, which is not in the rate law, and also has a slow step involving a bimolecular collision between two NO₅ molecules, which is unlikely. - Option C has a slow step involving a bimolecular collision between NO₃ and O₂, which is consistent with the rate law, and a fast step involving the formation of the product. This mechanism fits the rate law, and the steps are reasonable. - Option D has a slow step involving a bimolecular collision between two NO₂ molecules, which is unlikely. The product of this step is not part of the rate law, so this mechanism cannot explain the observed rate law.

The Rate Law for the Reaction 2NO2 + O3 →\rarr→ N2O5 + O2 Is Rate = K[NO2][O3]

The Rate Law for the Reaction 2NO₂ + O₃ $\rarr$ N₂O₅ + O₂ Is Rate = K[NO₂][O₃]