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At 225oC, nitrogen dioxide, NO2, reacts with carbon monoxide, CO, to produce carbon dioxide, CO2, and...

At 225oC, nitrogen dioxide, NO2, reacts with carbon monoxide, CO, to produce carbon dioxide, CO2, and nitrogen monoxide, NO, according to the following equation.

NO2(g) + CO(g)  CO2(g) + NO(g)

The experimentally determined rate law for the reaction is,

Rate = kobs[NO2]2

and NO3(g) has been experimentally identified as an intermediate in the reaction.

a. Explain why the mechanism for this reaction cannot consist of a single step; that is, based on the experimental data provided above, why must the reaction mechanism involve more than one step?

b. Assuming that the reaction mechanism does not involve a fast, pre-equilibrium step, propose a two-step mechanism for this reaction that satisfies the two tests discussed in lecture and explain your reasoning.

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