Thermodynamics concept question

In summary, when an ideal gas expands adiabatically and reversibly, it does work at the expense of its internal energy. This results in a decrease in the average kinetic energy of its molecules, leading to a decrease in temperature. This is because no heat energy is allowed into the gas from outside, which would otherwise increase the internal energy and temperature.
  • #1
itr
43
0
Problem: Why does an ideal gas cool when it expands adiabatically and reversibly?

Is the volume of the container expanding? so the total kinetic energy of the gas is getting smaller as it occupies more space making the temperature cool?
 
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  • #2
The gas does work in order to expand. This work is done at the expense of the internal energy of the gas. (KE of its molecules)
 
  • #3
Is that all? so when the gas is doing work, it will loose energy? is that because the system is loosing energy and the temperature willl decrease??
 
  • #4
still unsure...
 
  • #5
The gas does work.
The energy to do this comes from the internal energy of the gas.
The temperature of the gas depends on the (average) KE of the molecules.
If internal energy is lost, KE is reduced, temperature goes down.
(Because its adiabatic, no heat energy is allowed into the gas from outside.
If it was allowed, this heat energy would appear as internal energy and cause the temperature to rise.)
 

Related to Thermodynamics concept question

1. What is thermodynamics?

Thermodynamics is a branch of physics that deals with the study of heat and its relation to energy and work. It explains how energy is transferred and transformed between different forms, and how it affects the behavior of matter.

2. What are the laws of thermodynamics?

The laws of thermodynamics are fundamental principles that govern the behavior of energy in a system. The first law states that energy cannot be created or destroyed, only transferred or converted. The second law states that the total entropy (measure of disorder) of a closed system always increases over time. The third law states that the entropy of a perfect crystal at absolute zero temperature is zero.

3. How is thermodynamics applied in real life?

Thermodynamics has many practical applications in our daily lives, such as in refrigerators, air conditioners, and car engines. It also plays a crucial role in the fields of chemistry, engineering, and environmental science. Understanding thermodynamics allows us to design more efficient systems and processes.

4. What is the difference between heat and temperature in thermodynamics?

Heat is the transfer of energy between two objects at different temperatures, while temperature is a measure of the average kinetic energy of particles in a system. In thermodynamics, heat is considered a form of energy, while temperature is a measurement of the intensity of heat.

5. How does thermodynamics relate to entropy?

Entropy is a measure of the disorder or randomness of a system. In thermodynamics, the second law states that the total entropy of a closed system will always increase over time. This means that as energy is transferred and transformed, it tends to spread out and become more disorganized, leading to an overall increase in entropy.

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