If a system has 20.5 J of heat added to it, and the system does 75.5 J of work on its surroundings, what is the change in the internal energy of the system, in J?
If a system has 20.5 J of heat added to it, and the system does 75.5 J of work on its surroundings, what is the change in the internal energy of the system, in J?
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter6: Thermochemisty
Section: Chapter Questions
Problem 6.132QP
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Question
![### Thermodynamics and Internal Energy
#### Problem Statement:
If a system has 20.5 J of heat added to it, and the system does 75.5 J of work on its surroundings, what is the change in the internal energy of the system, in J?
#### Explanation:
In thermodynamics, the change in the internal energy of a system can be determined using the First Law of Thermodynamics, which is stated as:
\[
\Delta U = Q - W
\]
where:
- \(\Delta U\) is the change in internal energy
- \(Q\) is the heat added to the system
- \(W\) is the work done by the system on its surroundings
Given:
- Heat added (\(Q\)) = 20.5 J
- Work done by the system (\(W\)) = 75.5 J
#### Solution:
Substitute the given values into the equation:
\[
\Delta U = 20.5 \, \text{J} - 75.5 \, \text{J} = -55 \, \text{J}
\]
#### Conclusion:
The change in the internal energy of the system is \(-55 \, \text{J}\). This means that the internal energy of the system decreases by 55 Joules.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fdd588ef3-9b5a-418e-afb9-a9c936bcb253%2Fd20980fc-b465-417c-99af-25e8d23c7da9%2Fpnrh4v6_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Thermodynamics and Internal Energy
#### Problem Statement:
If a system has 20.5 J of heat added to it, and the system does 75.5 J of work on its surroundings, what is the change in the internal energy of the system, in J?
#### Explanation:
In thermodynamics, the change in the internal energy of a system can be determined using the First Law of Thermodynamics, which is stated as:
\[
\Delta U = Q - W
\]
where:
- \(\Delta U\) is the change in internal energy
- \(Q\) is the heat added to the system
- \(W\) is the work done by the system on its surroundings
Given:
- Heat added (\(Q\)) = 20.5 J
- Work done by the system (\(W\)) = 75.5 J
#### Solution:
Substitute the given values into the equation:
\[
\Delta U = 20.5 \, \text{J} - 75.5 \, \text{J} = -55 \, \text{J}
\]
#### Conclusion:
The change in the internal energy of the system is \(-55 \, \text{J}\). This means that the internal energy of the system decreases by 55 Joules.
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