Use the information in Table 5.1 to determine the rate equation for this reaction. Give an explanation for your deduction.
Use your rate equation from (a)(i) together with the data from experiment 1 to work out the rate constant, $k$, for this reaction. Give the units of $k$ too.
$\text{NO}_2\text{Cl}$ is another compound that contains nitrogen, oxygen and chlorine. In sunlight, $\text{NO}_2\text{Cl}$ can undergo homolytic fission to produce chlorine radicals that catalyse the conversion of ozone, $\text{O}_3$, into oxygen. Complete the mechanism for this process. Initiation (homolytic fission): $\text{NO}_2\text{Cl} \rightarrow \dots + \dots$ Propagation step 1: $\dots + \text{O}_3 \rightarrow \dots + \dots$ Propagation step 2: $\dots + \dots \rightarrow \dots + \dots$
Ozone reacts with nitrogen dioxide, as shown: $\text{O}_3 + 2\text{NO}_2 \rightarrow \text{N}_2\text{O}_5 + \text{O}_2$. The reaction is first order with respect to $\text{O}_3$ and first order with respect to $\text{NO}_2$. Suggest equations for a two-step mechanism for this reaction. Step 1: Step 2: