Chemistry
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
Bartleby Related Questions Icon

Related questions

Question
100%
### 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
expand button
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
Expert Solution
Check Mark
Knowledge Booster
Background pattern image
Chemistry
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
Recommended textbooks for you
Text book image
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Text book image
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Text book image
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Text book image
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Text book image
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Text book image
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY