Problem: The reaction of nitrogen dioxide with carbon monoxide NO2(g) + CO(g) => CO2(g) + NO(g) has been studied and the following mechanism has been proposed:NO2(g) + NO2(g) => NO3(g) + NO(g) slowNO3(g) + CO(g) => NO2(g) + CO2(g) fastWhat rate law corresponds to this mechanism?A. rate = k[NO2][CO]/[CO2][NO]B. rate = k[NO2][CO]C. rate = k[NO2]2 D. rate = k[NO2]E. rate = k[CO2][NO]/[NO2][CO]

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Determine the overall order of the reaction by analyzing the provided elementary reactions:

1. NO2(g) + NO2(g) → NO3(g) + NO(g)                (slow)

2. NO3(g) + CO(g) → NO2(g) + CO2(g) fast

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The reaction of nitrogen dioxide with carbon monoxide NO2(g) + CO(g) => CO2(g) + NO(g) has been studied and the following mechanism has been proposed:

NO2(g) + NO2(g) => NO3(g) + NO(g) slow

NO3(g) + CO(g) => NO2(g) + CO2(g) fast

What rate law corresponds to this mechanism?

A. rate = k[NO2][CO]/[CO2][NO]

B. rate = k[NO2][CO]

C. rate = k[NO2]2 

D. rate = k[NO2]

E. rate = k[CO2][NO]/[NO2][CO]

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