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Factors Affecting the Rate of a Chemical Reaction

2NO↔ N2O2 fas...

Question

$2 N O \leftrightarrow N_{2} O_{2}$ (fast)
$N_{2} O_{2} + H_{2} \to H_{2} O_{2} + N_{2}$ (slow)
$H_{2} + H_{2} O_{2} \to 2 H_{2} O$ (fast)
For the preceding multi-step reaction mechanism, which of the following is the correct rate law?

R a t e = k [H_{2} O_{2}] [N_{2}]

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R a t e = k [N_{2} O_{2}] [H_{2}]

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R a t e = k [N O]^{2}

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R a t e = k [N O]^{2} [H_{2}]^{2}

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Solution

The correct option is D $R a t e = k [N O]^{2} [H_{2}]^{2}$
$2 N O ⟶ N_{2} O_{2}$ (Fast)
$N_{2} O_{2} + H_{2} ⟶ H_{2} O_{2} + N_{2}$
+ $H_{2} + H_{2} O_{2} ⟶ 2 H_{2} O$
Overall $⟶$ $2 N O + 2 H_{2} ⟶ N_{2} + 2 H_{2} O$
Reaction

Rate Law= $K [N O]^{2} [H_{2}]^{2}$

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Similar questions

2 H_{2} (g) + 2 N O (g) \to N_{2} (g) + 2 H_{2} O (g)

= k [H_{2}] [N O]^{2}

2 N O ⇌ N_{2} O_{2}

N_{2} O_{2} + H_{2} \to N_{2} O + H_{2} O

N_{2} O + H_{2} \to N_{2} + H_{2} O

2 H_{2} + 2 N O \to N_{2} + 2 H_{2} O

2 N O ⇌ N_{2} O_{2}

K_{1} (f a s t)

N_{2} O_{2} + H_{2}_{2} N_{2} O + H_{2} O (s l o w)

N_{2} O + H_{2} \to N_{2} + H_{2} O (f a s t)

2 N O \to N_{2} O_{2} (s l o w)

N_{2} O_{2} + O_{2} \to 2 N O_{2} (f a s t)

2 N O + O_{2} \to 2 N O_{2}

N O + N O_{1} N_{2} O_{2}

N_{2} O_{2} + O_{2}_{2} 2 N O_{2}

2 H_{2} + 2 N O \to 2 H_{2} O + N_{2}

r a t e = k [H_{2}] [N O]^{2}

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