Using the experimental data provided, determine the order of reaction with respect to each reactant, the rate law equation, the overall order of reaction, and calculate the rate law constant, k. NO2 (g) + O3 (g) → NO3 (g) + O2 (g) Question :What is the overall order of the reaction? Experiment Initial Concentration (mol/L) Initial Rate (mol/L•s) NO2 O3 1 0.21 0.70 6.3 2 0.21 1.39 12.5 3 0.38 0.70 11.4 4 0.66 0.18 ?
Using the experimental data provided, determine the order of reaction with respect to each reactant, the rate law equation, the overall order of reaction, and calculate the rate law constant, k. NO2 (g) + O3 (g) → NO3 (g) + O2 (g) Question :What is the overall order of the reaction? Experiment Initial Concentration (mol/L) Initial Rate (mol/L•s) NO2 O3 1 0.21 0.70 6.3 2 0.21 1.39 12.5 3 0.38 0.70 11.4 4 0.66 0.18 ?
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
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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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Using the experimental data provided, determine the order of reaction with respect to each reactant, the rate law equation, the overall order of reaction, and calculate the rate law constant, k.
NO2 (g) + O3 (g) → NO3 (g) + O2 (g)
Question :What is the overall order of the reaction?
Experiment |
Initial Concentration (mol/L) |
Initial Rate (mol/L•s) |
|
NO2 |
O3 |
||
1 |
0.21 |
0.70 |
6.3 |
2 |
0.21 |
1.39 |
12.5 |
3 |
0.38 |
0.70 |
11.4 |
4 |
0.66 |
0.18 |
? |
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