The chemical reaction, proceeds as follows:O3→O2+O (fast)O+O3→2O2 (slow)The rate law expression should be:

r=k'O3O2 r=k'k"O3O3O2 r=kO32O2−1

r=k'O3O2 r=k'k"O3O3O2 r=kO32O2−1

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The chemical reaction, proceeds as follows:
$O_{3} \to O_{2} + O$ (fast)
$O + O_{3} \to 2 O_{2}$ (slow)
The rate law expression should be:

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$r = k {[O_{3}]}^{2} {[O_{2}]}^{- 1}$

$r = k {[O_{3}]}^{2}$

$r = k [O_{3}] [O_{2}]$

$r = k [O_{3}] {[O_{2}]}^{2}$

answer is B.

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$r=k' [O_{3}] [O_{2}] r = \frac{k' k " [O_{3}] [O_{3}]}{[O_{2}]} r = k {[O_{3}]}^{2} {[O_{2}]}^{- 1}$

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