Decomposition of ozone follows the given mechanism. From the mechanism select the option which is not correct
step 1: $O_{3} (g) \underset{K_{2}}{\overset{K_{1}}{⇌}} O_{2} (g) + O (g)$ [fast]
step 2: $O_{3} (g) + O (g) \overset{K_{3}}{⟶} 2 O_{2} (g)$ [slow]

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Rate of formation of ozone will decrease with increase in concentration of oxygen gas

Overall rate will be dependent on rate of (ii) step.

Molecularity of step (ii) will be 2.

Order of the reaction is equal to 2.

answer is B.

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Detailed Solution

slow step is rate determining step.

Hence rate of reaction is given as:

$rate = k_{2} [O] [O_{3}]$

by chemical eqⁿ

$\begin{array}{l} k_{1} = \frac{[0_{3}] [0]}{O_{3}} \\ [O] = \frac{k_{1} [O_{3}]}{[O_{2}]} \end{array}$

$r = K_{3} \times \frac{K_{1}}{K_{2}} \times {[O_{3}]}^{2} {[O_{2}]}^{- 1}$

So, rate $= k_{1} k_{2} {[O_{3}]}^{2} {[O_{2}]}^{- 1}$

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

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