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Derivation of Kp and Kc

Consider this...

Question

Consider this reaction. $2 N O_{2 (g)} + O_{3 (g)} \to N_{2} O_{5 (g)} + O_{2 (g)}$
The reaction of nitrogen dioxide and ozone represented in first order in $N O_{2 (g)}$ and $O_{3 (g)}$ . Which of these possible reaction mechanisms is consistent with the rate law?
Mechanism I. $N O_{2} + O_{3} \to N O_{3} + O_{2}$ slow
$N O_{3} + N O_{2} \to N_{2} O_{5}$ fast
Mechanism II. $O_{3} ⇌ O_{2} + O$ fast
$N O_{2} + O \to N O_{3}$ slow
$N O_{3} + N O_{2} \to N_{2} O_{5}$ fast

I only

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II only

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both I and II

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neither I nor II

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Solution

The correct option is A I only
only I is valid as its slowest step shows that
$N O_{2} + O_{3} \to N O_{3} + O_{2}$
it is first order w.r.t. to both reactants.

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Similar questions

2 N O_{2} (g) + O_{3} (g) ⟶ N_{2} O_{5} (g) + O_{2} (g)

N O_{2} (g)

O_{3} (g)

N O_{2} (g) + O_{3} (g) ⟶ N O_{3} (g) + O_{2} (g)

N O_{3} (g) + N O_{2} (g) ⟶ N_{2} O_{5} (g)

O_{3} (g) ⇌ O_{2} (g) + [O]

N O_{2} (g) + [O] (g) ⟶ N O_{3} (g)

N O_{3} (g) + N O_{2} (g) ⟶ N_{2} O_{5} (g)

2 N_{2} O_{5} ⟶ 4 N O_{2} + O_{2}

N_{2} O_{5} ⇌ N O_{2} + N O_{3}

N O_{2} + N O_{3} ⟶ N O + N O_{2} + O_{2}

N O + N O_{3} ⟶ 2 N O_{2}

2 N_{2} O_{5} (g) \to 4 N O_{2} (g) + O_{2} (g)

N_{2} O_{5}_{a} N O_{2} + N O_{3}

N O_{3} + N O_{2}_{- a} N_{2} O_{5}

N O_{2} + N O_{3}_{b} N O_{2} + O_{2} + N O

N O + N O_{3}_{c} 2 N O_{2}

N - O

N O_{2}^{+}

N O_{2}^{-}

N O_{3}^{-}

N O_{2}^{+}, N O_{2}^{-}

N O_{3}^{-}

N - O

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