For the chemical reaction, 2O3→3O2 proceed as follows O3⇌O2+O.....(fast) O+O2→2O2.....(slow) The rate law expression will be:
A
r=k′[O3]2
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B
r=k′[O3]2[O2]−1
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C
r=k′[O3][O2]
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D
Unpredictable
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Solution
The correct option is Ar=k′[O3]2[O2]−1 As slowest step is the rate determining step. Hence, from slow reaction, r=K[O][O3].....(i) From fast reaction, KC=[O2][O][O3] [O]=KC.[O3][O2], i.e. r=KC[O3][O2].[O3] ⇒KC.[O3]2[O2]−1 ∴Rate(r)=K′[O3]2⋅[O2]−1(K′=KC⋅K).