Question

Nitrogen dioxide reacts with carbon monoxide to produce nitrogen monoxide and carbon dioxide. NO2(g) + CO(g) ⟶ NO(g) + CO2(g) A proposed mechanism for this reaction is 2NO2(g) ⟶ NO3(g) + NO(g) (fast, equilibrium) NO3(g) + CO(g) ⟶ NO2(g) + CO2(g) (slow) What is a rate law that is consistent with the proposed mechanism?

Answer 1

The rate law for the proposed mechanism is rate = k[NO2][CO], indicating a first-order reaction with respect to both NO2 and CO.

Step-by-step explanation:

The rate law for the proposed mechanism is rate = k[NO2][CO]. This means that the rate of the reaction is directly proportional to the concentrations of NO2 and CO. The reaction is first order with respect to both NO2 and CO.