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: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter11: Chemical Kinetics: Rates Of Reactions
Section: Chapter Questions
Problem 77QRT
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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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