The reaction of nitrogen dioxide with carbon monoxide.
${NO}_{2} (g) + CO (g) ⟶ {CO}_{2} (g) + NO (g)$
has been studied and the following mechanism has been proposed :
${NO}_{2} (g) + {NO}_{2} (g) ⟶ {NO}_{3} (g) + NO (g)$ (slow)
${NO}_{3} (g) + CO (g) ⟶ {NO}_{2} (g) + {CO}_{2} (g)$ (fast)
What rate law corresponds to this mechanism?

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$Rate = k {[{NO}_{2}]}^{2} [CO]$

$Rate = k [{NO}_{2}]$

$Rate = k [{NO}_{2}] [CO]$

$Rate = k {[{NO}_{2}]}^{2}$

answer is C.

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Detailed Solution

The reaction's slowest step is used to calculate a reaction's pace. Since the first equation in the previous problem is the one that moves most slowly, the rate should be established to create this step. Nitrogen dioxide, 2 moles, is present in the reactant.

As a result, $Rate = k {[{NO}_{2}]}^{2}$ is the formula for the reaction's rate, where k is the rate constant.

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