21. For the decomposition of N₂Os(g), 2 N₂Os(g) →4 NO₂(g) + O2(g), the following data were obtained for the reaction at 32°C: Time (s) [N₂O5](M) 0.600 0.500 0.416 0.346 0.289 0.240 0.200 0.167 A. Use the data to graphically determine the rate law for the reaction. 0 2000 4000 6000 8000 10000 12000 14000 B. What is the rate constant at 32°C.
21. For the decomposition of N₂Os(g), 2 N₂Os(g) →4 NO₂(g) + O2(g), the following data were obtained for the reaction at 32°C: Time (s) [N₂O5](M) 0.600 0.500 0.416 0.346 0.289 0.240 0.200 0.167 A. Use the data to graphically determine the rate law for the reaction. 0 2000 4000 6000 8000 10000 12000 14000 B. What is the rate constant at 32°C.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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21
0.600
0.500
0.416
0.346
0.289
0.240
0.200
0.167
A. Use the data to graphically determine the rate law for the reaction.
B. What is the rate constant at 32°C.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0d520b33-7440-45bc-bf50-9535ed2d03bc%2F5b0db143-3fe6-4841-89b1-5f5f3a279df4%2F7qwxbp8_processed.jpeg&w=3840&q=75)
Transcribed Image Text:21. For the decomposition of N₂Os(g), 2 N₂Os(g) → 4
NO2(g) + O₂(g), the following data were obtained for
the reaction at 32°C:
Time
(s)
0
2000
4000
6000
8000
10000
12000
14000
[N₂O5](M)
0.600
0.500
0.416
0.346
0.289
0.240
0.200
0.167
A. Use the data to graphically determine the rate law for the reaction.
B. What is the rate constant at 32°C.
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