Ozone can be decomposed by the following two elementary reactions NO + O_3 right
ID: 534273 • Letter: O
Question
Ozone can be decomposed by the following two elementary reactions NO + O_3 rightarrow NO_2 + O_2 NO_2 + O rightarrow NO + O_2 a.) Determine the overall b) obtain d[O_2]/dt, c) obtain d[Intermediate]/dt for each intermediate, d) apply the steady-state approximation to the rates for the intermediates and obtain a simplified rate law for the formation of diatomic oxygen that depends upon the concentration of O_3 and NO only. Note this is an usual rate law as it still depends on the concentration of one of the intermediate (NO).Explanation / Answer
The rate of ozone decomposition is d(O2)/dt= K1[NO] [O3]+K2[NO2][O]
The intermediates is NO2 and hence the net rate is zero. Hence d(NO2)/dt= K1[NO][O3]- K2[NO2][O]= 0
And d(NO)/dt= K1[NO][O2]-K2[NO2][O]=0
Hence [O]= (K1/K2) [NO] [O3]/[NO2]
Hence d(O2)/dt= K1[NO][O3] + K2[NO2] (K1/K2) [NO] [O3]/[NO2]
=2 K1[NO] [O3]
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