In a study of the gas phase decomposition of hydrogen iodide at 700 K HI(g) →→→ H₂(g) + 2 I₂(g) the following data were obtained: [HI], M seconds 1.57 0 0.785 731 S. Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 1.57 M is s and when the starting concentration is 0.785 M is 0.393 0.197 2.19x103 5.10x10³ (2) The average A(1/[HI]) / At from t = 0 s to t = 731 s is 15-1. The average A(1/[HI]) / At from t = 731 s to t = 2.19x10³ s is M-¹ S-¹. (3) Based on these data, the rate constant for this M-1 S-1. M™ order reaction is Previous Next
In a study of the gas phase decomposition of hydrogen iodide at 700 K HI(g) →→→ H₂(g) + 2 I₂(g) the following data were obtained: [HI], M seconds 1.57 0 0.785 731 S. Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 1.57 M is s and when the starting concentration is 0.785 M is 0.393 0.197 2.19x103 5.10x10³ (2) The average A(1/[HI]) / At from t = 0 s to t = 731 s is 15-1. The average A(1/[HI]) / At from t = 731 s to t = 2.19x10³ s is M-¹ S-¹. (3) Based on these data, the rate constant for this M-1 S-1. M™ order reaction is Previous Next
Chemistry
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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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![In a study of the gas phase decomposition of hydrogen iodide at 700 K:
\[ \text{HI(g)} \rightarrow \frac{1}{2} \text{H}_2\text{(g)} + \frac{1}{2} \text{I}_2\text{(g)} \]
The following data were obtained:
| [HI], M | 1.57 | 0.785 | 0.393 | 0.197 |
|---------|------|-------|-------|-------|
| seconds | 0 | 731 | 2.19×10³ | 5.10×10³ |
**Hint:** It is not necessary to graph these data.
**(1)**
The observed half-life for this reaction when the starting concentration is 1.57 M is \[ \_\_\_\_\_\_\_ \] s and when the starting concentration is 0.785 M is \[ \_\_\_\_\_\_\_ \] s.
**(2)**
The average \[ \Delta (1/[HI]) / \Delta t \] from \[ t = 0 \text{ s} \] to \[ t = 731 \text{ s} \] is \[ \_\_\_\_\_\_\_ \] M⁻¹ s⁻¹.
The average \[ \Delta (1/[HI]) / \Delta t \] from \[ t = 731 \text{ s} \] to \[ t = 2.19 \times 10³ \text{ s} \] is \[ \_\_\_\_\_\_\_ \] M⁻¹ s⁻¹.
**(3)**
Based on these data, the rate constant for this \[ \_\_\_\_\_\_\_ \] order reaction is \[ \_\_\_\_\_\_\_ \] M⁻¹ s⁻¹.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb8d8ce1c-d1ae-4fbf-bbe3-121c6915374e%2F2f55e1a9-d064-415b-99b4-c8cbe67b13ca%2F9qaplte_processed.jpeg&w=3840&q=75)
Transcribed Image Text:In a study of the gas phase decomposition of hydrogen iodide at 700 K:
\[ \text{HI(g)} \rightarrow \frac{1}{2} \text{H}_2\text{(g)} + \frac{1}{2} \text{I}_2\text{(g)} \]
The following data were obtained:
| [HI], M | 1.57 | 0.785 | 0.393 | 0.197 |
|---------|------|-------|-------|-------|
| seconds | 0 | 731 | 2.19×10³ | 5.10×10³ |
**Hint:** It is not necessary to graph these data.
**(1)**
The observed half-life for this reaction when the starting concentration is 1.57 M is \[ \_\_\_\_\_\_\_ \] s and when the starting concentration is 0.785 M is \[ \_\_\_\_\_\_\_ \] s.
**(2)**
The average \[ \Delta (1/[HI]) / \Delta t \] from \[ t = 0 \text{ s} \] to \[ t = 731 \text{ s} \] is \[ \_\_\_\_\_\_\_ \] M⁻¹ s⁻¹.
The average \[ \Delta (1/[HI]) / \Delta t \] from \[ t = 731 \text{ s} \] to \[ t = 2.19 \times 10³ \text{ s} \] is \[ \_\_\_\_\_\_\_ \] M⁻¹ s⁻¹.
**(3)**
Based on these data, the rate constant for this \[ \_\_\_\_\_\_\_ \] order reaction is \[ \_\_\_\_\_\_\_ \] M⁻¹ s⁻¹.
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