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

The rate law indicates that the reaction rate is proportional to the concentrations of both NOS and OS. In mechanism A and D, there is no step that involves the reaction between NOS and OS; therefore, these mechanisms cannot explain the rate law. In mechanism B, the slow step involves the formation of NS from the reaction of two NOS molecules. This step does not depend on the concentration of OS, so the rate law cannot be explained by this mechanism. Only mechanism C has a slow step that involves the reaction between NOS and OS, leading to the formation of NS and OS. The rate-determining step depends on the concentration of both NOS and OS, which is consistent with the rate law given.

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]