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Chemistry Question on Chemical Kinetics

For the chemical reaction, 2O3⇌3O22\text{O}_3\rightleftharpoons 3\text{O}_2, the reaction proceeds as follows:
O3⇌O2+O (fast)\text{O}_3\rightleftharpoons \text{O}_2 + \text{O} \, \text{(fast)}
O+O3→2O2 (slow)\text{O} + \text{O}_3 \rightarrow 2\text{O}_2 \, \text{(slow)}
The rate law expression will be:

A

r=k′[O3]2r = k'[\text{O}_3]^2

B

r=k′[O3]2[O2]−1r = k'[\text{O}_3]^2[\text{O}_2]^{-1}

C

r=k′[O3][O2]r = k'[\text{O}_3][\text{O}_2]

D

Unpredictable

Answer

r=k′[O3]2[O2]−1r = k'[\text{O}_3]^2[\text{O}_2]^{-1}

Explanation

Solution

The correct option is (B): r=k′[O3]2[O2]−1r = k'[\text{O}_3]^2[\text{O}_2]^{-1}