Derive the rate law for the following reaction given the mechanistic steps below: 2NO(g) + O₂(g) 2NO₂(g), rate= k [NO] [0₂] The mechanism proposed for this reaction consists of two steps. The first step is a fast equilibrium. k₁ 2NO(g) N₂O₂ (8) k_1 k₂ N₂O₂(g) + O₂(g) →→→→2 NO₂ (g) What is the rate law in terms of k₁, k₂, and k_₁? Be sure to simplify the rate law before inputting your answer.

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Derive the rate law for the following reaction given the mechanistic steps below:
2NO(g) + O₂(g) 2NO₂(g), rate=k [NO]²[0₂]
The mechanism proposed for this reaction consists of two steps. The first step is a fast equilibrium.
k₁
1
2 NO(g) ⇒ N₂O₂(g)
k_1
k₂
N₂O₂(g) + O₂ (g) → 2 NO₂ (g)
What is the rate law in terms of k₁, k₁, and k_₁? Be sure to simplify the rate law before inputting your answer.
rate=
[NO]²[0₂]
00
X
Ś
0|0
Transcribed Image Text:Derive the rate law for the following reaction given the mechanistic steps below: 2NO(g) + O₂(g) 2NO₂(g), rate=k [NO]²[0₂] The mechanism proposed for this reaction consists of two steps. The first step is a fast equilibrium. k₁ 1 2 NO(g) ⇒ N₂O₂(g) k_1 k₂ N₂O₂(g) + O₂ (g) → 2 NO₂ (g) What is the rate law in terms of k₁, k₁, and k_₁? Be sure to simplify the rate law before inputting your answer. rate= [NO]²[0₂] 00 X Ś 0|0
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