In which of the following scenarios is no change in the internal energy of the system possible? O q<0, w=0 O q<0, w > 0 O q = 0, w > 0 O q<0, w < 0 O q> 0, w > 0
In which of the following scenarios is no change in the internal energy of the system possible? O q<0, w=0 O q<0, w > 0 O q = 0, w > 0 O q<0, w < 0 O q> 0, w > 0
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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![### Understanding Changes in Internal Energy
**Question:** In which of the following scenarios is **no change** in the internal energy of the system possible?
1. \( q < 0, w = 0 \)
2. \( q < 0, w > 0 \)
3. \( q = 0, w > 0 \)
4. \( q < 0, w < 0 \)
5. \( q > 0, w > 0 \)
**Explanation:**
To identify the scenario where there is no change in the internal energy (\(\Delta U = 0\)) of the system, we can use the First Law of Thermodynamics, which is expressed as:
\[ \Delta U = q + w \]
Where
- \(\Delta U\) is the change in internal energy,
- \(q\) is the heat exchanged (with \(q > 0\) indicating heat absorbed by the system and \(q < 0\) indicating heat released by the system),
- \(w\) is the work done on the system (with \(w > 0\) indicating work done on the system and \(w < 0\) indicating work done by the system).
For the internal energy to remain unchanged (\(\Delta U = 0\)), the sum of \(q\) and \(w\) must be zero:
\[ q + w = 0 \]
Among the given options:
1. \( q < 0, w = 0 \): The system releases heat, but no work is done, so \(\Delta U \neq 0\).
2. \( q < 0, w > 0 \): The system releases heat (\( q < 0 \)), and work is done on the system (\( w > 0 \)). If the magnitudes of \(q\) and \(w\) are such that \( |q| = w \), then \( q + w = 0 \).
This is the correct scenario where no change in internal energy is possible.
3. \( q = 0, w > 0 \): No heat exchange, and work is done on the system, so \(\Delta U \neq 0\).
4. \( q < 0, w < 0 \): The system releases heat, and work is done by the system, so \(\Delta U \neq 0](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb99220ad-d702-4943-b904-ec3abe399c73%2Fe6d6c6ae-5aee-40eb-bb2e-601b9bbb63c5%2Fmvsqxbp_processed.png&w=3840&q=75)
Transcribed Image Text:### Understanding Changes in Internal Energy
**Question:** In which of the following scenarios is **no change** in the internal energy of the system possible?
1. \( q < 0, w = 0 \)
2. \( q < 0, w > 0 \)
3. \( q = 0, w > 0 \)
4. \( q < 0, w < 0 \)
5. \( q > 0, w > 0 \)
**Explanation:**
To identify the scenario where there is no change in the internal energy (\(\Delta U = 0\)) of the system, we can use the First Law of Thermodynamics, which is expressed as:
\[ \Delta U = q + w \]
Where
- \(\Delta U\) is the change in internal energy,
- \(q\) is the heat exchanged (with \(q > 0\) indicating heat absorbed by the system and \(q < 0\) indicating heat released by the system),
- \(w\) is the work done on the system (with \(w > 0\) indicating work done on the system and \(w < 0\) indicating work done by the system).
For the internal energy to remain unchanged (\(\Delta U = 0\)), the sum of \(q\) and \(w\) must be zero:
\[ q + w = 0 \]
Among the given options:
1. \( q < 0, w = 0 \): The system releases heat, but no work is done, so \(\Delta U \neq 0\).
2. \( q < 0, w > 0 \): The system releases heat (\( q < 0 \)), and work is done on the system (\( w > 0 \)). If the magnitudes of \(q\) and \(w\) are such that \( |q| = w \), then \( q + w = 0 \).
This is the correct scenario where no change in internal energy is possible.
3. \( q = 0, w > 0 \): No heat exchange, and work is done on the system, so \(\Delta U \neq 0\).
4. \( q < 0, w < 0 \): The system releases heat, and work is done by the system, so \(\Delta U \neq 0
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