Do gasses ever truly reach a state of internal thermodynamic equilibrium?

[am77494]

@Max_S

I believe you are mistaken

Maybe, but please check out the links. This is also why I tried to get our definitions consistent.

@Max_S

Temperature is said to be intensive at equilibrium, but specific internal energy is extensive and proportional to size

Wikipedia includes “Specific Internal Energy” as an example of an intensive property. I am including a screenshot but you can check for yourself at (cite) : Intensive and extensive properties - Wikipedia

Screenshot of cite with red underline of relevant part :

@Max_S

It is also measured in joules, not joules per kg which is effectively a measure of acceleration.

Specific Internal Energy is measured in J/kg or J/mol as mentioned above in my post. I have a feeling that you are not reading the cites, so I am citing and attaching a screenshot with red underline : Internal energy - Wikipedia

[Max_S]

Ack, I had confused specific internal energy with internal energy.

@am77494

This is where you confused me because this is not Classical Thermodynamics. A gas in Classical Thermodynamics is a continuum and not discrete particles in motion. In my opinion, you are mixing Classical TD and Statistical Mechanics in the question but want the answer purely from the Classical TD

I suppose I have in mind a combination of pre-Boltzmann classical thermodynamics and kinetic theory. It should all date to around the 1870s, and in my experience, this was all that was taught in public school.

~Max