Question

The following is a proposed mechanism for the reaction NO₂ (g) + CO (g) --> NO (g) + CO₂ (g). The rate law for the reaction is rate = k [NO₂]² a) is this a plausible mechanism? Explain. B) identify the reactants, intermediates, and products. NO₂ (g) + NO₂ (g)--> NO₃ (g) + NO (g) (slow) and NO₃ (g) + CO (g) --> NO₂ (g) + CO₂ (g) (fast)

Answer 1

Ans :

a) yes this is a plausible mechanism.

This is because the rate law of the reaction depend on the rate determining step of the reaction which is the slowest step. Here the slow step is step 1 , so the rate law is given as : rate = k[NO2]².

The overall reaction can also be obtained by adidng the two steps of the mechanism and simplifying it. So this is the correct mechanism for the reaction.

b)

The reactants in the reaction are : NO2 and CO

intermediate is NO3

products are : NO and CO2