The rate of the reaction NO2(g) + CO(g) → NO(g) + CO2(g) depends only on the concentration of nitrogen dioxide below 225°C. At a temperature below 225°C, the following data were collected: Time (s) [NO2] (mol/L) 0 0.500 1.20 x 10³ 0.444 3.00 x 10³ 0.381 4.50 × 103 0.340 9.00 x 103 0.250 1.80 x 104 0.174 a Determine the rate law. (Use k for the rate constant.) Rate = =[ Determine the integrated rate law. 1 [NO2] Submit
The rate of the reaction NO2(g) + CO(g) → NO(g) + CO2(g) depends only on the concentration of nitrogen dioxide below 225°C. At a temperature below 225°C, the following data were collected: Time (s) [NO2] (mol/L) 0 0.500 1.20 x 10³ 0.444 3.00 x 10³ 0.381 4.50 × 103 0.340 9.00 x 103 0.250 1.80 x 104 0.174 a Determine the rate law. (Use k for the rate constant.) Rate = =[ Determine the integrated rate law. 1 [NO2] Submit
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 78GQ
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![The rate of the reaction
NO2(g) + CO(g) → NO(g) + CO2(g)
depends only on the concentration of nitrogen dioxide below 225°C. At a temperature below 225°C, the following data were collected:
Time (s) [NO2] (mol/L)
0
0.500
1.20 x 10³
0.444
3.00 x 10³
0.381
4.50 × 103
0.340
9.00 x 103
0.250
1.80 x 104
0.174
a Determine the rate law.
(Use k for the rate constant.)
Rate =
=[
Determine the integrated rate law.
1
[NO2]
Submit](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fcb973547-96c1-4d9f-a718-a177ed24e455%2Fd10d8df2-dd44-4988-b90a-66febb7a5f37%2Fw37it6u_processed.jpeg&w=3840&q=75)
Transcribed Image Text:The rate of the reaction
NO2(g) + CO(g) → NO(g) + CO2(g)
depends only on the concentration of nitrogen dioxide below 225°C. At a temperature below 225°C, the following data were collected:
Time (s) [NO2] (mol/L)
0
0.500
1.20 x 10³
0.444
3.00 x 10³
0.381
4.50 × 103
0.340
9.00 x 103
0.250
1.80 x 104
0.174
a Determine the rate law.
(Use k for the rate constant.)
Rate =
=[
Determine the integrated rate law.
1
[NO2]
Submit
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