Chemical Kinetics and Nuclear ChemistryHard
Question
The reaction of NO2 (g) and O3 (g) is first-order in NO2 (g) and O3 (g)
2NO2 (g) + O3 (g) → N2O5 (g) + O2 (g)
The reaction can take place by mechanism :
I : NO2 + O3
NO3 + O2
NO3 + NO2
N2O5
II : O3
O2 + [O]
NO2 + O
NO3
NO3 + NO2
N2O5
Select correct mechanism.
2NO2 (g) + O3 (g) → N2O5 (g) + O2 (g)
The reaction can take place by mechanism :
I : NO2 + O3
NO3 + O2NO3 + NO2
N2O5II : O3
O2 + [O]NO2 + O
NO3NO3 + NO2
N2O5Select correct mechanism.
Options
A.I only
B.II only
C.both I and II
D.None of I and II
Solution
For Rxn rate determining step is slowest step
Then in 1st Rxn
Rate = k [NO2] [O3] .....(i)
But 2nd Rxn
O3
O2 + [O] ....(a)
NO2 + O
NO3 ....(b)
NO3 + NO2
N2O5 ....(c)
Then for Rxn (a)
= keq ....(d)
by Rxn (b)
Rate = k [NO2] [O] ....(ii)
put value of [O] from (d) to (ii)
Rate = k
× [NO2]
Rate =
Then in 1st Rxn
Rate = k [NO2] [O3] .....(i)
But 2nd Rxn
O3
O2 + [O] ....(a)NO2 + O
NO3 ....(b)NO3 + NO2
N2O5 ....(c)Then for Rxn (a)
= keq ....(d)by Rxn (b)
Rate = k [NO2] [O] ....(ii)
put value of [O] from (d) to (ii)
Rate = k
× [NO2]Rate =
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