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Chemical Kinetics

Question
CBSEENCH12011488
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For the chemical reaction,

2O3 ⇌ 3O2

The reaction proceeds as follows

O3 ⇌ O2 + O

O + O3 → 2O2 (slow)

The rate law expression will be

  • r = k' [O3]2

  • r = k' [O3]2[O2]-1

  • r = k'[O3][O2]

  • unpredictable

Solution

B.

r = k' [O3]2[O2]-1

As slowest step is the rate determining step. Hence, from slow reaction r = K[O][O3] ... (i)

From the fast reaction, 

Kc = [O2][O][O3][O] = Kc. [O3][O2]. i.er = Kc[O3][O2][O3]⇒ Kc.[O3]2 [O2]-1Therefore rate (r) = K'[O3]2.[O2]-1  (K'  = Kc.K)

Some More Questions From Chemical Kinetics Chapter

A reaction is 50% complete in 2 hours and 75% complete in 4 hours. What is the order of the reaction.

The rate law for the decomposition of N2O5 is rate = k[N2O5]. What is the significance of k in this equation?

Define activation energy of a reaction.

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