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Question

The chemical reaction, 2O33O2 proceeds as follows;
O3O2+O ....(Fast)
O+O32O2 ....(Slow)
The rate law expression should 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 B r=K[O3]2[O2]1
For slow step, rate=K[O][O3] .....(i)

Also for equilibrium Kc=[O][O2][O3] ....(ii)

[O]=Kc[O3][O2] ....(iii)

By Eqs. (iii) and (i), the intermediate [O] is eliminated as:

rate=KKc[O3][O3][O2]=K[O3]2[O2].

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