The reaction 2 NO₂(g) + O3(g) → N₂O5(g) + O₂(g) was studied at a certain temperature with the following results: (a) What is the rate law for this reaction? Rate = k [NO₂(g)] [03(9)] O Rate = k [NO₂(g)]² [03(9)] O Rate = k [NO₂(g)] [03(g)]² O Rate = k [NO₂(g)]² [03(g)]² O Rate = k [NO₂(g)] [03(g)]³ O Rate = k [NO₂(g)]* [03(g)] (b) What is the value of the rate constant? x 137268 Experiment ✔ M/s 1 2 3 4 [NO₂(g)] (M) 0.718 0.718 1.44 1.44 [03(g)] (M) 0.718 1.44 0.718 1.44 Rate (M/s) (c) What is the reaction rate when the concentration of NO₂(g) is 1.26 M and that of O3(g) is 2.10 M if the temperature is the same as that used to obtain the data shown above? 26600 53400 53400 1.07e+05
The reaction 2 NO₂(g) + O3(g) → N₂O5(g) + O₂(g) was studied at a certain temperature with the following results: (a) What is the rate law for this reaction? Rate = k [NO₂(g)] [03(9)] O Rate = k [NO₂(g)]² [03(9)] O Rate = k [NO₂(g)] [03(g)]² O Rate = k [NO₂(g)]² [03(g)]² O Rate = k [NO₂(g)] [03(g)]³ O Rate = k [NO₂(g)]* [03(g)] (b) What is the value of the rate constant? x 137268 Experiment ✔ M/s 1 2 3 4 [NO₂(g)] (M) 0.718 0.718 1.44 1.44 [03(g)] (M) 0.718 1.44 0.718 1.44 Rate (M/s) (c) What is the reaction rate when the concentration of NO₂(g) is 1.26 M and that of O3(g) is 2.10 M if the temperature is the same as that used to obtain the data shown above? 26600 53400 53400 1.07e+05
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter14: Chemical Kinetics: The Rates Of Chemical Reactions
Section: Chapter Questions
Problem 12PS: The reaction 2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g) was studied at 904 C, and the data in the table...
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![The reaction 2 NO₂(g) + O₂(g) → N₂O5(g) + O₂(g) was studied at a certain temperature with the following results:
(a) What is the rate law for this reaction?
Rate = k [NO₂(g)] [03(g)]
O Rate = k [NO₂(g)]² [03(g)]
O Rate = k [NO₂(g)] [03(g)]²
O Rate = k [NO₂(g)]² [03(g)]²
O Rate = k [NO₂(g)] [03(g)]³
O Rate = k [NO₂(g)]* [03(g)]
(b) What is the value of the rate constant?
137268
Experiment
M/S
AWNPE
1
2
3
4
[NO₂(g)] (M)
0.718
0.718
1.44
1.44
[03(g)] (M)
0.718
1.44
0.718
1.44
Rate (M/s)
(c) What is the reaction rate when the concentration of NO₂(g) is 1.26 M and that of O3(g) is 2.10 M if the temperature is the same as that used to obtain the data shown above?
26600
53400
53400
1.07e+05](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fddcb5aca-4883-4ca8-afdb-70bc4fab9914%2F41f3a859-aed4-45f9-917c-34d4ed015aec%2Fck9q2_processed.jpeg&w=3840&q=75)
Transcribed Image Text:The reaction 2 NO₂(g) + O₂(g) → N₂O5(g) + O₂(g) was studied at a certain temperature with the following results:
(a) What is the rate law for this reaction?
Rate = k [NO₂(g)] [03(g)]
O Rate = k [NO₂(g)]² [03(g)]
O Rate = k [NO₂(g)] [03(g)]²
O Rate = k [NO₂(g)]² [03(g)]²
O Rate = k [NO₂(g)] [03(g)]³
O Rate = k [NO₂(g)]* [03(g)]
(b) What is the value of the rate constant?
137268
Experiment
M/S
AWNPE
1
2
3
4
[NO₂(g)] (M)
0.718
0.718
1.44
1.44
[03(g)] (M)
0.718
1.44
0.718
1.44
Rate (M/s)
(c) What is the reaction rate when the concentration of NO₂(g) is 1.26 M and that of O3(g) is 2.10 M if the temperature is the same as that used to obtain the data shown above?
26600
53400
53400
1.07e+05
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