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Chemical Kinetics

Question
CBSEENCH12011512
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For the chemical reaction, 2O3 ⇌ 3O2. The reaction proceeds as follows

O3 ⇌ O2 + O (fast)

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].[O3]⇒ Kc.[O3]2[O2]-1∴ Rate (r) = K'[O3]2.[O2]-1    (K' = Kc.K)

Some More Questions From Chemical Kinetics Chapter

The conversion of molecules X to Y follows second order kinetics. If concentration of X is increased to three times how will it affect the rate of formation of Y?

What will be the effect of temperature on rate constant?

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

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