25. The reaction 2 NO2(g) + O3(g) N2O5(g) + O2(g) was studied at a certain temperature with the following results: Experiment [NO2(g)] (M) [O3(g)] (M) Rate (M/s) 1 0.502 0.502 21600
25. The reaction 2 NO2(g) + O3(g) N2O5(g) + O2(g) was studied at a certain temperature with the following results: Experiment [NO2(g)] (M) [O3(g)] (M) Rate (M/s) 1 0.502 0.502 21600
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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25. The reaction 2 NO2(g) + O3(g) N2O5(g) + O2(g) was studied at a certain temperature with the following results:
| Experiment | [NO2(g)] (M) | [O3(g)] (M) | Rate (M/s) |
|---|---|---|---|
| 1 | 0.502 | 0.502 | 21600 |
| 2 | 0.502 | 1.00 | 43100 |
| 3 | 1.00 | 0.502 | 43100 |
| 4 | 1.00 | 1.00 | 85800 |
(a) What is the rate law for this reaction?
Rate = k [NO2(g)] [O3(g)]
Rate = k [NO2(g)]2 [O3(g)]
Rate = k [NO2(g)] [O3(g)]2
Rate = k [NO2(g)]2 [O3(g)]2
Rate = k [NO2(g)] [O3(g)]3
Rate = k [NO2(g)]4 [O3(g)]
(b) What is the value of the rate constant?
(c) What is the reaction rate when the concentration of NO2(g) is 0.505 M and that of O3(g) is 1.37 M if the temperature is the same as that used to obtain the data shown above?
______ M/s
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