Nitrogen dioxide reacts with carbon monoxide to produce...

Nitrogen dioxide reacts with carbon monoxide to produce nitrogen monoxide and carbon dioxide in the reaction, $\mathrm{NO}_{2}(g)+\mathrm{CO}(g) \longrightarrow \mathrm{NO}(g)+\mathrm{CO}_{2}(g)$ The first step in the reaction is proposed to be two $\mathrm{NO}_{2}$ molecules colliding to form $\mathrm{NO}_{3}$ and NO. The $\mathrm{NO}_{3}$ intermediate then reacts with $\mathrm{CO}$ to form $\mathrm{CO}_{2}$. What is the rate law for this proposed mechanism?

Nitrogen dioxide reacts with carbon monoxide to produce nitrogen monoxide and carbon dioxide in the reaction, $\mathrm{NO}_{2}(g)+\mathrm{CO}(g) \longrightarrow \mathrm{NO}(g)+\mathrm{CO}_{2}(g)$
The first step in the reaction is proposed to be two $\mathrm{NO}_{2}$ molecules colliding to form $\mathrm{NO}_{3}$ and NO. The $\mathrm{NO}_{3}$ intermediate then reacts with $\mathrm{CO}$ to form $\mathrm{CO}_{2}$. What is the rate law for this proposed mechanism?

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Key Concepts

Reaction Mechanism

A reaction mechanism is a detailed, step?by?step description of how reactants transform into products through a series of elementary steps. Understanding the mechanism helps explain the actual pathway molecules follow during the reaction and can reveal which intermediates are formed along the way.

Elementary Steps and Their Rate Laws

Each elementary step in a mechanism has its own rate law that reflects the molecularity of that step. For an elementary process, the rate law is written directly from the stoichiometry of that step, e.g., a bimolecular collision between two identical molecules leads to a rate law that is second order in that species.

Rate-Determining Step

Within a multi-step mechanism, the slowest step is termed the rate?determining step. Because it limits the overall reaction rate, the rate law for the entire reaction is approximated by the rate law of this slow step, despite subsequent fast steps that might involve other species, including intermediates.

Intermediate Species

Intermediates are species that are produced in one step of a reaction mechanism and consumed in a subsequent step. While they play a critical role in the reaction pathway, they typically do not appear in the overall rate law because their steady-state concentrations can be expressed in terms of the reactants.

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