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. Use the data to predict the reaction rate for Experiment 4. NO2 (g) + O3 (g) → NO3 (g) + O2 (g) 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 ? Order with respect to NO2: _______ Order with respect to O3: ___________ Rate Law: What is the overall order of the reaction? What is k? Initial Rate for Experiment 4: _______
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. Use the data to predict the reaction rate for Experiment 4. NO2 (g) + O3 (g) → NO3 (g) + O2 (g) 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 ? Order with respect to NO2: _______ Order with respect to O3: ___________ Rate Law: What is the overall order of the reaction? What is k? Initial Rate for Experiment 4: _______
Chapter12: Chemical Kinetics
Section: Chapter Questions
Problem 3RQ: One experimental procedure that can be used to determine the rate law of a reaction is the method of...
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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. Use the data to predict the reaction rate for Experiment 4.
NO2 (g) + O3 (g) → NO3 (g) + O2 (g)
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 |
? |
- Order with respect to NO2: _______
- Order with respect to O3: ___________
- Rate Law:
- What is the overall order of the reaction?
- What is k?
- Initial Rate for Experiment 4: _______
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