9. Nitric oxide, NO, reacts with hydrogen to give nitrous oxide, N,O, and water. 2NO + H, 2(g) N,0 + H,O (3) (g) In a series of experiments, the following initial rates of disappearance of NO were obtained: Show work! (20 points) Initial Initial Rate Concentrations of Reaction [NO] [H,] 3.2 X 10° M -3 1.1 X 10° M -5 1.3 X 10° M/s Exp. 1 |Exp. 2 Exp. 3 -5 5.2 X 10° M/s -3 6.4 X 10° M 1.1 X 10° M -5 3.2 X 10° M 2.2 X 10° M 1.3 X 10° M/s a. Find the rate law expression. b. Draw the rate law graph with respect to H2. c. Find the value of the rate constant. -3 d. What would the rate be if I initially add 6.4 X 10° M of NO and 4.4 X 10° M of H,?
9. Nitric oxide, NO, reacts with hydrogen to give nitrous oxide, N,O, and water. 2NO + H, 2(g) N,0 + H,O (3) (g) In a series of experiments, the following initial rates of disappearance of NO were obtained: Show work! (20 points) Initial Initial Rate Concentrations of Reaction [NO] [H,] 3.2 X 10° M -3 1.1 X 10° M -5 1.3 X 10° M/s Exp. 1 |Exp. 2 Exp. 3 -5 5.2 X 10° M/s -3 6.4 X 10° M 1.1 X 10° M -5 3.2 X 10° M 2.2 X 10° M 1.3 X 10° M/s a. Find the rate law expression. b. Draw the rate law graph with respect to H2. c. Find the value of the rate constant. -3 d. What would the rate be if I initially add 6.4 X 10° M of NO and 4.4 X 10° M of H,?
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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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Nitric oxide, NO, reacts with hydrogen to give nitrous oxide, N2O, and water.
2NO(g) + H2(g) ---------> N2O(g) + H2O(g)
In a series of experiments, the following initial rates of disappearance of NO were
obtained
![### Educational Content on Reaction Rates
#### 9. Nitric oxide, NO, reacts with hydrogen to give nitrous oxide, N₂O, and water.
**Chemical Equation:**
\[ 2NO_{(g)} + H_2{_{(g)}} \rightarrow N_2O_{(g)} + H_2O_{(g)} \]
In a series of experiments, the following initial rates of disappearance of NO were obtained. Show work! (20 points)
| Experiment | Initial Concentrations | Initial Rate of Reaction |
|------------|------------------------|-------------------------|
| | [NO] (M) | [H₂] (M) | (M/s) |
| Exp. 1 | 3.2 x 10⁻³ | 1.1 x 10⁻³ | 1.3 x 10⁻⁵ |
| Exp. 2 | 6.4 x 10⁻³ | 1.1 x 10⁻³ | 5.2 x 10⁻⁵ |
| Exp. 3 | 3.2 x 10⁻³ | 2.2 x 10⁻³ | 1.3 x 10⁻⁵ |
**Questions:**
a. Find the rate law expression.
b. Draw the rate law graph with respect to H₂.
c. Find the value of the rate constant.
d. What would the rate be if I initially add 6.4 x 10⁻³ M of NO and 4.4 x 10⁻³ M of H₂?
**Explanation of the Table:**
- **Experiment 1:** The initial concentration of NO is \(3.2 \times 10^{-3} \, M\) and H₂ is \(1.1 \times 10^{-3} \, M\). The initial rate of the reaction is \(1.3 \times 10^{-5}\) M/s.
- **Experiment 2:** The initial concentration of NO is \(6.4 \times 10^{-3} \, M\) and H₂ is \(1.1 \times 10^{-3} \, M\). The initial rate of the reaction increases to \(5.2 \times 10^{-5}\) M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2ffb9870-2903-4965-9b25-0c5e2f1ebec2%2F6605ab02-25a4-49df-8d7b-377497dabdec%2Fxbapxid.png&w=3840&q=75)
Transcribed Image Text:### Educational Content on Reaction Rates
#### 9. Nitric oxide, NO, reacts with hydrogen to give nitrous oxide, N₂O, and water.
**Chemical Equation:**
\[ 2NO_{(g)} + H_2{_{(g)}} \rightarrow N_2O_{(g)} + H_2O_{(g)} \]
In a series of experiments, the following initial rates of disappearance of NO were obtained. Show work! (20 points)
| Experiment | Initial Concentrations | Initial Rate of Reaction |
|------------|------------------------|-------------------------|
| | [NO] (M) | [H₂] (M) | (M/s) |
| Exp. 1 | 3.2 x 10⁻³ | 1.1 x 10⁻³ | 1.3 x 10⁻⁵ |
| Exp. 2 | 6.4 x 10⁻³ | 1.1 x 10⁻³ | 5.2 x 10⁻⁵ |
| Exp. 3 | 3.2 x 10⁻³ | 2.2 x 10⁻³ | 1.3 x 10⁻⁵ |
**Questions:**
a. Find the rate law expression.
b. Draw the rate law graph with respect to H₂.
c. Find the value of the rate constant.
d. What would the rate be if I initially add 6.4 x 10⁻³ M of NO and 4.4 x 10⁻³ M of H₂?
**Explanation of the Table:**
- **Experiment 1:** The initial concentration of NO is \(3.2 \times 10^{-3} \, M\) and H₂ is \(1.1 \times 10^{-3} \, M\). The initial rate of the reaction is \(1.3 \times 10^{-5}\) M/s.
- **Experiment 2:** The initial concentration of NO is \(6.4 \times 10^{-3} \, M\) and H₂ is \(1.1 \times 10^{-3} \, M\). The initial rate of the reaction increases to \(5.2 \times 10^{-5}\) M
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