Nitrogen dioxide, NO2\text{NO}_2NO2, reacts with carbon monoxide, CO\text{CO}CO, to form nitrogen monoxide, NO\text{NO}NO, and carbon dioxide, CO2\text{CO}_2CO2, as shown by the overall equation below:
NO2+CO→NO+CO2 \text{NO}_2 + \text{CO} \rightarrow \text{NO} + \text{CO}_2 NO2+CO→NO+CO2At temperatures below 500 K500\text{ K}500 K, the mechanism for this reaction is proposed to involve two steps. Step 1 is the slow (rate-determining) step, and Step 2 is the fast step.
The equation for Step 2 is:
NO3+CO→NO2+CO2 \text{NO}_3 + \text{CO} \rightarrow \text{NO}_2 + \text{CO}_2 NO3+CO→NO2+CO2Suggest the equation for Step 1 and write the rate equation for this overall reaction under these conditions.
