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110. For the reaction:
NO₂(g) + CO (g) → CO₂(g) + NO(g)
the experimentally determined rate expression between 440 K is rate = k[NO₂]². What mechanism can be proposed for the above reaction?

NO₂(g) + CO(g) → CO₂(g) + NO(g)
The mechanism proposed for the above reaction involves two steps:

Step. 1.

{NO}_{2} (g) + {NO}_{2} (g) \overset{slow}{\to} NO (g) + {NO}_{3} (g)

Step. 2.
${NO}_{3} (g) + CO (g) \overset{fast}{\to} {CO}_{2} (g) + {NO}_{2} (g)$

Overall reaction:
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${NO}_{2} (g) + CO (g) \to {CO}_{2} (g) + NO (g)$

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As we have given that rate = k[NO₂]²

Since concentration of CO(g) is not involved in the rate expression, so the overall rate of reaction is determined by the intermediate formation of NO₃(g) i.e., Step 1.

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