A series of experiments was done on the decomposition of NO2 at 573K as shown in to the following equation: 2NO2(g) ? 2NO(g) + O2(g) The following data were collected: Table 1 Table 2 Time, min [NO2], M Initial [NO2] Initial Rate, M/s Temperature, oC 0 0.0835 0.10M 0.152 2.0 15.0 0.0680 0.10M 0.144 2.5 65.0 0.0350 0.10M 0.147 2.3 105 0.0220 0.10M 0.474 26.0 0.10M 0.480 25.0 0.10M 0.485 25.5 Determine the rate law for the reaction and the activation energy of the reaction. Show all your work.
A series of experiments was done on the decomposition of NO2 at 573K as shown in to the following equation: 2NO2(g) ? 2NO(g) + O2(g) The following data were collected: Table 1 Table 2 Time, min [NO2], M Initial [NO2] Initial Rate, M/s Temperature, oC 0 0.0835 0.10M 0.152 2.0 15.0 0.0680 0.10M 0.144 2.5 65.0 0.0350 0.10M 0.147 2.3 105 0.0220 0.10M 0.474 26.0 0.10M 0.480 25.0 0.10M 0.485 25.5 Determine the rate law for the reaction and the activation energy of the reaction. Show all your work.
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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- A series of experiments was done on the decomposition of NO2 at 573K as shown in to the following equation:
2NO2(g) ? 2NO(g) + O2(g)
The following data were collected:
|
Table 1 |
Table 2 |
||||
|
Time, min |
[NO2], M |
Initial [NO2] |
Initial Rate, M/s |
Temperature, oC |
|
|
0 |
0.0835 |
0.10M |
0.152 |
2.0 |
|
|
15.0 |
0.0680 |
0.10M |
0.144 |
2.5 |
|
|
65.0 |
0.0350 |
0.10M |
0.147 |
2.3 |
|
|
105 |
0.0220 |
0.10M |
0.474 |
26.0 |
|
|
0.10M |
0.480 |
25.0 |
|||
|
0.10M |
0.485 |
25.5 |
Determine the rate law for the reaction and the activation energy of the reaction. Show all your work.
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