The decomposition of dinitrogen monoxide gas occurs in two steps- Step 1- N2Og- N2g - Og slow Step 2- N2Og - Og- N2g - O2g fastBased on these elementary steps- which of the following is the rate law-

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Byju's Answer

Standard XII

Chemistry

Rate of Reaction

The decomposi...

Question

The decomposition of dinitrogen monoxide gas occurs in two steps:
$S t e p 1 : N_{2} O_{(g)} \to N_{2 (g)} + O_{(g)}$ (slow)
$S t e p 2 : N_{2} O_{(g)} + O_{(g)} \to N_{2 (g)} + O_{2 (g)}$ (fast)
Based on these elementary steps, which of the following is the rate law?

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

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

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

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

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Solution

The correct option is C $R a t e = k [N_{2} O]$
Rate of reaction depends on the slow step in a reaction.
So based on the elementary steps D is the correct answer.

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Similar questions

Q. The decomposition of dinitrogen monoxide gas occurs in two steps:

S t e p 1 : N_{2} O_{(g)} \to N_{2 (g)} + O_{(g)}

(slow)

S t e p 2 : N_{2} O_{(g)} + O_{(g)} \to N_{2 (g)} + O_{2 (g)}

(fast)
What is the overall reaction?

Q. Consider the reaction :

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

The rate law for this reaction is :

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

Under what conditions could these steps represent the mechanism?
Step 1 :

2 N O (g) ⇌ N_{2} O_{2} (g)

Step 2 :

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

Step 3 :

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

The chemical reaction $2 O_{3} \to 3 O_{2}$ involves two elementary steps :
$O_{3} f a s t - - \to O_{2} + O; O + O_{3} S l o w - -- \to 2 O_{2}$
The differential rate law expression will be :

Q. The rate law for the reaction;

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

\frac{d [N_{2}]}{d t} = k [H_{2}] [N O]^{2}

. Which of the following mechanisms is consistent with the rate law?

Q. The gaseous decomposition of ozone,

2 O_{3} ⟶ 3 O_{2}

, obeys the rate law

r = - \frac{d [O_{3}]}{d t} = \frac{k {[O_{3}]}^{2}}{[O_{2}]}

.
Show that the following mechanism is consistent with the above rate law:

O_{3} K_{e q} ⇌ O_{2} + O

(fast)

O + O_{3} k_{t} - ---- \to 2 O_{2}

(slow)

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The decomposition of dinitrogen monoxide gas occurs in two steps:Step1:N2O(g)→N2(g)+O(g) (slow)Step2:N2O(g)+O(g)→N2(g)+O2(g) (fast)Based on these elementary steps, which of the following is the rate law?

The correct option is C Rate=k[N2O]Rate of reaction depends on the slow step in a reaction.So based on the elementary steps D is the correct answer.

The decomposition of dinitrogen monoxide gas occurs in two steps:
$S t e p 1 : N_{2} O_{(g)} \to N_{2 (g)} + O_{(g)}$ (slow)
$S t e p 2 : N_{2} O_{(g)} + O_{(g)} \to N_{2 (g)} + O_{2 (g)}$ (fast)
Based on these elementary steps, which of the following is the rate law?

The correct option is C $R a t e = k [N_{2} O]$
Rate of reaction depends on the slow step in a reaction.
So based on the elementary steps D is the correct answer.