Questions: C. The reaction of NO2(g) and CO(g) is thought to occur in two steps: Step 1 slow NO2(g)+NO2(g) → NO(g)+NO3(g) Step 2 Fast NO3(g)+CO(g)+NO2(g)+CO2(g) What is the molecularity of Step 2? bimolecular termolecular unimolecular (d) The reaction of NO2(g) and CO(g) is thought to occur in two steps: Step 1 Slow NO2(g)+NO2(g) → NO(g)+NO3(g) Step 2 Fast NO3(g)+CO(g) → NO2(g)+CO2(g) For this mechanism to be consistent with kinetic data, what must be the experimental rate equation? rate =k[NO2] rate =k[NO2]^2 rate =k[NO2][CO]

Transcript text: C. The reaction of $\mathrm{NO}_{2}(g)$ and $\mathrm{CO}(g)$ is thought to occur in two steps: Step 1 slow \[ \mathrm{NO}_{2}(g)+\mathrm{NO}_{2}(g) \rightarrow \mathrm{NO}(g)+\mathrm{NO}_{3}(g) \] Step 2 Fast \[ \mathrm{NO}_{3}(g)+\mathrm{CO}(g)+\mathrm{NO}_{2}(g)+\mathrm{CO}_{2}(g) \] What is the molecularity of Step 2? bimolecular termolecular unimolecular (d) The reaction of $\mathrm{NO}_{2}(g)$ and $\mathrm{CO}(g)$ is thought to occur in two steps: Step 1 Slow \[ \mathrm{NO}_{2}(g)+\mathrm{NO}_{2}(g) \rightarrow \mathrm{NO}(g)+\mathrm{NO}_{3}(g) \] Step 2 Fast \[ \mathrm{NO}_{3}(g)+\mathrm{CO}(g) \rightarrow \mathrm{NO}_{2}(g)+\mathrm{CO}_{2}(g) \] For this mechanism to be consistent with kinetic data, what must be the experimental rate equation? rate $=\mathrm{k}\left[\mathrm{NO}_{2}\right]$ rate $=k\left[\mathrm{NO}_{2}\right]^{2}$ rate $=k\left[\mathrm{NO}_{2}\right][\mathrm{CO}]$