I read on 27 chapter from Blundell's Thermal Physics 2nd edition.

For ideal gases, Joule expansion doesn't cool gases. But for real gases, Joule expansion makes cooling effects. And this book(page 314) says that when gases expand, their potential energy of molecular interactions increases(since V is proprtional to 1/r). And this energy is exactly from kinetic energy of gas.(So makes kinetic energy of gas decrease)

What does the last sentence mean? Why does temperature decrease when kinetic energy of gas decrease?

I understand that low temperature makes average kinetic energy decrease(because of boltzmann distribution, low temperature makes low average kinetic energy)..

Or... Is temperature defined by boltzmann distribution? If a system has energy distribution of a temperature T, then does it said that the temperature of that system T?

I am sorry for this absurd question.

DrClaude
Mentor
But for real gases, Joule expansion makes cooling effects.
Not always. It depends on the sign of the Joule-Thomson coefficient.

Or... Is temperature defined by boltzmann distribution? If a system has energy distribution of a temperature T, then does it said that the temperature of that system T?
It is not defined from the Boltzmann distribution, but at equilibrium, they are equivalent information. Fit a Boltzmann curve to the distribution of velocities and you will get the temperature.

Philip Wood
Gold Member
Not always. It depends on the sign of the Joule-Thomson coefficient.
Dr Claude: Are you sure of this? Joule expansion is expansion into a vacuum as opposed to Joule Thomson isenthalpic expansion.

DrClaude
Mentor
Dr Claude: Are you sure of this? Joule expansion is expansion into a vacuum as opposed to Joule Thomson isenthalpic expansion.
Right. I misread that as Joule-Thomson. At least the rest of my post is still correct rude man
Homework Helper
Gold Member
I read on 27 chapter from Blundell's Thermal Physics 2nd edition.

For ideal gases, Joule expansion doesn't cool gases. But for real gases, Joule expansion makes cooling effects. And this book(page 314) says that when gases expand, their potential energy of molecular interactions increases(since V is proprtional to 1/r). And this energy is exactly from kinetic energy of gas.(So makes kinetic energy of gas decrease)

What does the last sentence mean? Why does temperature decrease when kinetic energy of gas decrease?

I understand that low temperature makes average kinetic energy decrease(because of boltzmann distribution, low temperature makes low average kinetic energy)..

Or... Is temperature defined by boltzmann distribution? If a system has energy distribution of a temperature T, then does it said that the temperature of that system T?

I am sorry for this absurd question.

Temperature is average kinetic energy of the molecules.

Joule (free) expansion produces a very small change in temperature. Masuring the Joule coefficient is very difficult. As you say, for an ideal gas the Joule coefficient = 0.