The experimental rate law for the decomposition of nitrous oxide (N₂O) to N₂ and O₂ is Rate = k[N₂O]². Two mechanisms are proposed: I. N₂O $\rightarrow$ N₂ + O N₂O + O $\rightarrow$ N₂ + O₂ II) 2N₂O N₄O₂ N₄O₂$\rightarrow$2N₂ + O₂ Which of the following could be a correct mechanism?

Question

Quizplus · Accepted Answer

The rate law shows that the rate of the reaction depends on the concentration of N₂O raised to some power ². In mechanism I, the proposed rate-determining step involves the collision between N₂O and O. However, the concentration of O is not included in the rate law. Therefore, mechanism I cannot be correct. In mechanism II, the proposed rate-determining step involves the collision between two molecules of N₂O. This step is consistent with the rate law since it involves the concentration of N₂O raised to a power of 2. Therefore, mechanism II could be correct.

The Experimental Rate Law for the Decomposition of Nitrous Oxide →\rightarrow→

The Experimental Rate Law for the Decomposition of Nitrous Oxide $\rightarrow$