The following initial rate data are for the reaction of nitrogen monoxide with ozone at 25 °C: NO+O3 → NO₂ + O2 Experiment [NO]o, M [03]0, M 0.171 0.0160 0.171 0.0320 0.342 0.0160 0.342 0.0320 1 2 3 4 Rate = Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. k = Initial Rate, M s 0.279 0.558 0.558 1.12 M-¹.s-¹ S 1
The following initial rate data are for the reaction of nitrogen monoxide with ozone at 25 °C: NO+O3 → NO₂ + O2 Experiment [NO]o, M [03]0, M 0.171 0.0160 0.171 0.0320 0.342 0.0160 0.342 0.0320 1 2 3 4 Rate = Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. k = Initial Rate, M s 0.279 0.558 0.558 1.12 M-¹.s-¹ S 1
Chemistry for Engineering Students
3rd Edition
ISBN:9781285199023
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter11: Chemical Kinetics
Section: Chapter Questions
Problem 11.52PAE
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Question
![The following initial rate data are for the reaction of nitrogen monoxide with
ozone at 25 °C:
NO+O3 → NO2 + O2
Experiment [NO]o, M [03]0, M Initial Rate, M-s¯¹
0.171
0.0160
0.279
0.171
0.0320
0.558
0.342
0.0160
0.558
0.342
0.0320 1.12
1
2
3
4
Complete the rate law for this reaction in the box below.
m
Use the form k[A] [B]", where '1' is understood for m or n and concentrations
taken to the zero power do not appear. Don't enter 1 for m or n.
Rate =
k =
M-¹ s -1](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F410de4e1-4314-42c8-8492-083aa9a0c480%2F33ea1cfb-0393-42b3-94ae-c518fd2ab244%2F21frwaj_processed.png&w=3840&q=75)
Transcribed Image Text:The following initial rate data are for the reaction of nitrogen monoxide with
ozone at 25 °C:
NO+O3 → NO2 + O2
Experiment [NO]o, M [03]0, M Initial Rate, M-s¯¹
0.171
0.0160
0.279
0.171
0.0320
0.558
0.342
0.0160
0.558
0.342
0.0320 1.12
1
2
3
4
Complete the rate law for this reaction in the box below.
m
Use the form k[A] [B]", where '1' is understood for m or n and concentrations
taken to the zero power do not appear. Don't enter 1 for m or n.
Rate =
k =
M-¹ s -1
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