The reaction described by the equation O₂(g) + NO(g) →→→ O₂(g) + NO₂(g) mas, at 310 K, the rate law rate of reaction = k[03][NO] k = 3.0 x 106 M-1.s-1 Given that [0₂] 4.0 x 10-4 M and [NO] = 2.0 x 10-5 M at t = 0, calculate the rate of the reaction at t = 0. rate: What is the overall order of this reaction? 2 1 20 M
The reaction described by the equation O₂(g) + NO(g) →→→ O₂(g) + NO₂(g) mas, at 310 K, the rate law rate of reaction = k[03][NO] k = 3.0 x 106 M-1.s-1 Given that [0₂] 4.0 x 10-4 M and [NO] = 2.0 x 10-5 M at t = 0, calculate the rate of the reaction at t = 0. rate: What is the overall order of this reaction? 2 1 20 M
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 31QRT
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![The reaction described by the equation
O₂(g) + NO(g)
has, at 310 K, the rate law
rate of reaction = k[O3 ][NO] k = 3.0 x 106 M-¹.s-1
Given that [0₂] = 4.0 × 10-4 M and [NO] = 2.0 × 10-5 M at t = 0, calculate the rate of the reaction at t = 0.
rate:
What is the overall order of this reaction?
ö808
3
O₂(g) + NO₂ (g)
2
1
M/s](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F21d5b8d8-205d-4590-8ec0-d96e151b6c0d%2F840f3990-e2ea-4459-b1a7-f4703da40a68%2Fx50znb6_processed.png&w=3840&q=75)
Transcribed Image Text:The reaction described by the equation
O₂(g) + NO(g)
has, at 310 K, the rate law
rate of reaction = k[O3 ][NO] k = 3.0 x 106 M-¹.s-1
Given that [0₂] = 4.0 × 10-4 M and [NO] = 2.0 × 10-5 M at t = 0, calculate the rate of the reaction at t = 0.
rate:
What is the overall order of this reaction?
ö808
3
O₂(g) + NO₂ (g)
2
1
M/s
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