A study of the gas-phase oxidation of nitrogen monoxide at 25°C and 1.00 atm pressure gave the following results: 2NO(g) + O2(9) → NO2(g) Conc. NO, moVL Сonc. Oz, тol/ Initial Rate Exp. 1 1.5 x 1о-2 3.2 x 10-2 1.3 x 10-8 mol/(L - s) Exp. 2 1.5 x 1о-2 6.4 x 10-2 2.6 x 10-8 mol/(L .s) Exp. 3 3.0 x 1о-2 0.13 2.1 x 10-2 mol/(L.s) Еxp. 4 0.64 4.4 x 10-3 ? a What is the experimental rate law for the reaction above? (Use k for the rate constant.) Rate law = k[NO]°[0,] b What is the initial rate of the reaction in Experiment 4? Initial rate = | mol/(L s)
A study of the gas-phase oxidation of nitrogen monoxide at 25°C and 1.00 atm pressure gave the following results: 2NO(g) + O2(9) → NO2(g) Conc. NO, moVL Сonc. Oz, тol/ Initial Rate Exp. 1 1.5 x 1о-2 3.2 x 10-2 1.3 x 10-8 mol/(L - s) Exp. 2 1.5 x 1о-2 6.4 x 10-2 2.6 x 10-8 mol/(L .s) Exp. 3 3.0 x 1о-2 0.13 2.1 x 10-2 mol/(L.s) Еxp. 4 0.64 4.4 x 10-3 ? a What is the experimental rate law for the reaction above? (Use k for the rate constant.) Rate law = k[NO]°[0,] b What is the initial rate of the reaction in Experiment 4? Initial rate = | mol/(L s)
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...
Related questions
Question
![**A study of the gas-phase oxidation of nitrogen monoxide at 25°C and 1.00 atm pressure gave the following results:**
\[ 2NO(g) + O_2(g) \rightarrow NO_2(g) \]
| Experiment | Conc. NO, mol/L | Conc. O₂, mol/L | Initial Rate mol/(L·s) |
|------------|----------------|----------------|------------------------|
| Exp. 1 | 1.5 × 10⁻² | 3.2 × 10⁻² | 1.3 × 10⁻³ |
| Exp. 2 | 1.5 × 10⁻² | 6.4 × 10⁻² | 2.6 × 10⁻³ |
| Exp. 3 | 3.0 × 10⁻² | 0.13 | 2.1 × 10⁻² |
| Exp. 4 | 0.64 | 4.4 × 10⁻³ | ? |
---
**(a) What is the experimental rate law for the reaction above?**
*(Use \( k \) for the rate constant.)*
Rate law = \[ k[NO]^2[O_2] \] ✔
---
**(b) What is the initial rate of the reaction in Experiment 4?**
Initial rate = \_\_\_\_\_\_ mol/(L·s)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc0168238-e244-4a34-84ac-e572ee66fc4c%2F33f1f80b-96f6-47de-92db-6586f353dfcd%2Fe0vt6k8f_processed.png&w=3840&q=75)
Transcribed Image Text:**A study of the gas-phase oxidation of nitrogen monoxide at 25°C and 1.00 atm pressure gave the following results:**
\[ 2NO(g) + O_2(g) \rightarrow NO_2(g) \]
| Experiment | Conc. NO, mol/L | Conc. O₂, mol/L | Initial Rate mol/(L·s) |
|------------|----------------|----------------|------------------------|
| Exp. 1 | 1.5 × 10⁻² | 3.2 × 10⁻² | 1.3 × 10⁻³ |
| Exp. 2 | 1.5 × 10⁻² | 6.4 × 10⁻² | 2.6 × 10⁻³ |
| Exp. 3 | 3.0 × 10⁻² | 0.13 | 2.1 × 10⁻² |
| Exp. 4 | 0.64 | 4.4 × 10⁻³ | ? |
---
**(a) What is the experimental rate law for the reaction above?**
*(Use \( k \) for the rate constant.)*
Rate law = \[ k[NO]^2[O_2] \] ✔
---
**(b) What is the initial rate of the reaction in Experiment 4?**
Initial rate = \_\_\_\_\_\_ mol/(L·s)
Expert Solution
![](/static/compass_v2/shared-icons/check-mark.png)
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 2 steps with 2 images
![Blurred answer](/static/compass_v2/solution-images/blurred-answer.jpg)
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781259911156/9781259911156_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
![Principles of Instrumental Analysis](https://www.bartleby.com/isbn_cover_images/9781305577213/9781305577213_smallCoverImage.gif)
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781259911156/9781259911156_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
![Principles of Instrumental Analysis](https://www.bartleby.com/isbn_cover_images/9781305577213/9781305577213_smallCoverImage.gif)
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
![Organic Chemistry](https://www.bartleby.com/isbn_cover_images/9780078021558/9780078021558_smallCoverImage.gif)
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
![Chemistry: Principles and Reactions](https://www.bartleby.com/isbn_cover_images/9781305079373/9781305079373_smallCoverImage.gif)
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
![Elementary Principles of Chemical Processes, Bind…](https://www.bartleby.com/isbn_cover_images/9781118431221/9781118431221_smallCoverImage.gif)
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY