Elementary Steps What is the rate law for the overall reaction below based on the proposed mechanism? You'll need to find an expression for the intermediate as part of your answer. Step 1.02(g) ← 20(g) Step 2. N2(g) + O(g) → NO(g) + N(g) Step 3. N(g) + O(g) → NO(g) Fast, equilibrium Slow Fast Overall. N2(g) + O2(g) → 2NO(g) 8 1 point What is the overall rate law? O O O O O O O rate=k[N2] rate=k[N2]² rate=k[02] rate=k[02]² rate=k[N2][02] rate=k[N2][02]² O rate = k[N2][02]1/2

Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter11: Rate Of Reaction
Section: Chapter Questions
Problem 35QAP: Azomethane decomposes into nitrogen and ethane at high temperatures according to the following...
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Elementary Steps
What is the rate law for the overall reaction below based on the
proposed mechanism? You'll need to find an expression for the
intermediate as part of your answer.
Step 1.02(g) ← 20(g)
Step 2. N2(g) + O(g) → NO(g) + N(g)
Step 3. N(g) + O(g) → NO(g)
Fast, equilibrium
Slow
Fast
Overall. N2(g) + O2(g) → 2NO(g)
8
1 point
What is the overall rate law?
O O O O O O O
rate=k[N2]
rate=k[N2]²
rate=k[02]
rate=k[02]²
rate=k[N2][02]
rate=k[N2][02]²
O rate = k[N2][02]1/2
Transcribed Image Text:Elementary Steps What is the rate law for the overall reaction below based on the proposed mechanism? You'll need to find an expression for the intermediate as part of your answer. Step 1.02(g) ← 20(g) Step 2. N2(g) + O(g) → NO(g) + N(g) Step 3. N(g) + O(g) → NO(g) Fast, equilibrium Slow Fast Overall. N2(g) + O2(g) → 2NO(g) 8 1 point What is the overall rate law? O O O O O O O rate=k[N2] rate=k[N2]² rate=k[02] rate=k[02]² rate=k[N2][02] rate=k[N2][02]² O rate = k[N2][02]1/2
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