In a study of the decomposition of nitrous oxide at 565 °C N2O(g)N2(g) + ½ O2(g) the following data were obtained: [N2O], M 2.10 1.05 0.525 0.263 seconds 0 602 1.81×103 4.21×103 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 2.10 M is s and when the starting concentration is 1.05 M is s. (2) The average (1/[N2O]) / t from t = 0 s to t = 602 s is M-1 s-1. The average (1/[N2O]) / t from t = 602 s to t = 1.81×103 s is M-1 s-1. (3) Based on these data, the rate constant for this order reaction is M-1 s-1
In a study of the decomposition of nitrous oxide at 565 °C N2O(g)N2(g) + ½ O2(g) the following data were obtained: [N2O], M 2.10 1.05 0.525 0.263 seconds 0 602 1.81×103 4.21×103 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 2.10 M is s and when the starting concentration is 1.05 M is s. (2) The average (1/[N2O]) / t from t = 0 s to t = 602 s is M-1 s-1. The average (1/[N2O]) / t from t = 602 s to t = 1.81×103 s is M-1 s-1. (3) Based on these data, the rate constant for this order reaction is M-1 s-1
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter18: Chemical Kinetics
Section: Chapter Questions
Problem 7P
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In a study of the decomposition of nitrous oxide at 565 °C
N2O(g)N2(g) + ½ O2(g)
the following data were obtained:
| [N2O], M | 2.10 | 1.05 | 0.525 | 0.263 |
| seconds | 0 | 602 | 1.81×103 | 4.21×103 |
Hint: It is not necessary to graph these data.
(1)
The observed half life for this reaction when the starting concentration is 2.10 M is s and when the starting concentration is 1.05 M is s.
(2)
The average (1/[N2O]) / t from t = 0 s to t = 602 s is M-1 s-1.
The average (1/[N2O]) / t from t = 602 s to t = 1.81×103 s is M-1 s-1.
(3)
Based on these data, the rate constant for this order reaction is M-1 s-1.
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