In a study of the gas phase decomposition of hydrogen iodide at 700 K HI(g) 12 H₂(g) + 2 I₂(g) the following data were obtained: [HI], M seconds 1.57 0 0.785 731 0.393 2.19x10³ 0.197 5.10x10³ 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 concentration is 0.785 M is S. (2) The average A(1/[HI]) / At from t = 0 s to t = 731 s is 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 zero Border reaction is M-1 S-1. M-1 S-¹. s and when the starting
In a study of the gas phase decomposition of hydrogen iodide at 700 K HI(g) 12 H₂(g) + 2 I₂(g) the following data were obtained: [HI], M seconds 1.57 0 0.785 731 0.393 2.19x10³ 0.197 5.10x10³ 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 concentration is 0.785 M is S. (2) The average A(1/[HI]) / At from t = 0 s to t = 731 s is 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 zero Border reaction is M-1 S-1. M-1 S-¹. s and when the starting
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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![**Study of the Gas Phase Decomposition of Hydrogen Iodide at 700 K**
**Reaction:**
\[ \text{HI(g)} \rightarrow \frac{1}{2} \text{H}_2\text{(g)} + \frac{1}{2} \text{I}_2\text{(g)} \]
The following data were obtained:
| \([HI], M\) | 1.57 | 0.785 | 0.393 | 0.197 |
|---|---|---|---|---|
| Seconds | 0 | 731 | \(2.19 \times 10^3\) | \(5.10 \times 10^3\) |
**Hint:** It is not necessary to graph these data.
1. **Half-Life Observation:**
- The observed half-life for this reaction when the starting concentration is 1.57 M is ______ seconds and when the starting concentration is 0.785 M is ______ seconds.
2. **Average Rate Calculation:**
- The average \(\Delta(1/[HI]) / \Delta t\) from \(t = 0\) s to \(t = 731\) s is ______ \(M^{-1} s^{-1}\).
- The average \(\Delta(1/[HI]) / \Delta t\) from \(t = 731\) s to \(t = 2.19 \times 10^3\) s is ______ \(M^{-1} s^{-1}\).
3. **Rate Constant:**
- Based on these data, the rate constant for this zero-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%2F1fa4f0ae-f5cf-4899-8e3d-9ffab5720d19%2Fy3243js_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Study of the Gas Phase Decomposition of Hydrogen Iodide at 700 K**
**Reaction:**
\[ \text{HI(g)} \rightarrow \frac{1}{2} \text{H}_2\text{(g)} + \frac{1}{2} \text{I}_2\text{(g)} \]
The following data were obtained:
| \([HI], M\) | 1.57 | 0.785 | 0.393 | 0.197 |
|---|---|---|---|---|
| Seconds | 0 | 731 | \(2.19 \times 10^3\) | \(5.10 \times 10^3\) |
**Hint:** It is not necessary to graph these data.
1. **Half-Life Observation:**
- The observed half-life for this reaction when the starting concentration is 1.57 M is ______ seconds and when the starting concentration is 0.785 M is ______ seconds.
2. **Average Rate Calculation:**
- The average \(\Delta(1/[HI]) / \Delta t\) from \(t = 0\) s to \(t = 731\) s is ______ \(M^{-1} s^{-1}\).
- The average \(\Delta(1/[HI]) / \Delta t\) from \(t = 731\) s to \(t = 2.19 \times 10^3\) s is ______ \(M^{-1} s^{-1}\).
3. **Rate Constant:**
- Based on these data, the rate constant for this zero-order reaction is ______ \(M^{-1} s^{-1}\).
Expert Solution
Step 1
Given ->
Reaction is ->
HI(g) ------> 1/2H2(g) + 1/2I2(g)
-> Half life is time at which concentration left just half the initial concentration.
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