The decomposition of ozone proceeds as O 3- O 2- O fast O - O 3- 2 O 2 slow The rate expression should beA- r - k - O 3- O 2-1B- r - k - O 3- O 2-C- r - k - O 3-2- O 2-1D- r - k - O 3-2

The chemical reaction $2 O_{3} \to 3 O_{2}$ involves two elementary steps :
$O_{3} f a s t - - \to O_{2} + O; O + O_{3} S l o w - -- \to 2 O_{2}$
The differential rate law expression will be :

Q. The gaseous decomposition of ozone,

2 O_{3} ⟶ 3 O_{2}

, obeys the rate law

r = - \frac{d [O_{3}]}{d t} = \frac{k {[O_{3}]}^{2}}{[O_{2}]}

.
Show that the following mechanism is consistent with the above rate law:

O_{3} K_{e q} ⇌ O_{2} + O

(fast)

O + O_{3} k_{t} - ---- \to 2 O_{2}

(slow)

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The decomposition of ozone proceeds as O3⇔O2+O(fast)O+O3→2O2(slow) The rate expression should be

The correct option is B r=k[O3]2[O2]−1K=[O][O2][O3]or, [O]=K[O3]O2∴r=K[O3][O3][O2]=[O3]2[O2]−1

The decomposition of ozone proceeds as $O_{3} \Leftrightarrow O_{2} + O (f a s t) O + O_{3} \to 2 O_{2} (s l o w)$
The rate expression should be

The correct option is B $r = k [O_{3}]^{2} [O_{2}]^{- 1}$
$K = \frac{[O] [O_{2}]}{[O_{3}]} o r, [O] = \frac{K [O_{3}]}{O_{2}} ∴ r = \frac{K [O_{3}] [O_{3}]}{[O_{2}]} = [O_{3}]^{2} [O_{2}]^{- 1}$