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...
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![**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)
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