Consider this reaction :
2 NO 2 (g) + O 3 (g) ⎯→ N 2 O 5 (g) + O 2 (g)
The reaction of NO 2 (g) and O 3 (g) represented is first order in NO 2 (g) and in O 3 (g) Which of the following mechanism is/are consistent with the rate law ?
MechanismI : NO 2 (g) + O 3 (g) ⎯→ NO 3 (g) + O 2 (g) (slow)
NO 3 (g) + NO 2 (g) ⎯→ N 2 O 5 (g) (fast)
MechanismII : O 3 (g) 
O 2 (g) + O (fast)
NO 2 (g) + O ⎯→ NO 3 (g) (slow)
NO 3 (g) + NO 2 (g) ⎯→ N 2 O 5 (g) (fast)
Text Solution
Verified by ExpertsA
As per mechanism (I), rate = k [NO 2 ] [O 2 ]
slowest step is the r.d.s.
As per mechanism (II), rate = k [NO 2 ] [O]
K eq = 
or [O] = K eq 
∴ as per mechanism (II), rate = k K eq [NO 2 ] [O 3 ] [O 2 ] –1
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