Consider the reaction 2 N O 2 ( g ) + O 3 ( g ) → N 2 O 5 ( g ) + O 2 ( g ) The reaction of nitrogen dioxide and ozone represents is first order in N O 2 ( g ) and in O 3 ( g ) . Which of these possib

Question

Consider the reaction 2 N O 2 ( g ) + O 3 ( g ) → N 2 O 5 ( g ) + O 2 ( g ) The reaction of nitrogen dioxide and ozone represents is first order in N O 2 ( g ) and in O 3 ( g ) . Which of these possible reaction mechanism is consistent with the rate law? Mechanism I: 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) Mechanism II: O 3 (g) → O 2 (g) + [O] (fast) NO 2 (g) + [O] → NO 3 (slow) NO 3 (g) + NO 2 (g) → N 2 O 5 (fast)

TestHub · Accepted Answer

Mechanism I: R a t e = k [ N O 2 ] [ O 3 ] Slow step is rate determining Mechanism II: Rate = k ′ [ N O 2 ] [ O ] …(i) From 1st step K = [ O 2 ] [ O ] [ O 3 ] (k = eq. constant) [O] = k O 3 O 2 ...(ii) From equation (i) & (ii) Rate = k ′ [ N O 2 ] [ O 3 ] [ O 2 ] − 1 So both mechanism show that reaction is first order with respect to N O 2 and O 3 .

Mechanism I:	${NO}_{2} {(g) + O}_{3} (g) \to {NO}_{3} (g) + O_{2} (g) (slow)$
	${NO}_{3} {(g) + NO}_{2} (g) \to N_{2} O_{5} (g) (fast)$
Mechanism II:	$O_{3} (g) \to O_{2} (g) + [O] (fast)$
	${NO}_{2} (g) + [O] \to {NO}_{3} (slow)$
	${NO}_{3} {(g) + NO}_{2} (g) \to N_{2} O_{5} (fast)$

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