Thermodynamic question?

PV=nRT is for ideal gas. Not all gases are ideal. There are other factors that you need to consider, which are the attraction between gas molecules and impact volume (or pressure -- I don't remember exactly, but it has to do with the gas molecule striking the container wall).

My answer to your question will be the temperature is very much the same as the temperature from the outside. Since you didn't specify what kind of container is or what condition the container in, the air with the same temperature and pressure just flows inside the container by following the principle of "flow down the gradient". That means the air moving from place with more air to place with little or no air.

3rd is wrong: "it does work" means you are taking energy OUT of the gas, not putting it in. So it has to get colder.

1st is not important: if the initial pressure were just lower but not 0, you would still get a similar answer.

Your idea that when gas expands, it absorbs heat and cools down is misleading and wrong. It can not absorb any heat if it is isolated, so this depends on the conditions of your experiment.

The temperature of an ideal gas is a function of the average magnitude of the velocity of its molecules or atoms.

Lets say you remove one (or all) wall(s) of a container with a gas in it. What are the molecules of an ideal gas going to do which would have collided with the wall(s)?

They are going to keep going in the same direction. What will the average magnitude of the velocity of those molecules be?

The same as if they had collided with the wall. The wall(s) do not change the magnitude of the velocity in a collision, just the direction.

Now... what happens in a non-ideal gas? What does the total energy depend on in a non-ideal gas? Velocity and... ? How does that modify the temperature?

OK? I have given you all the clues you need (I think). But you will have to think this one through for yourself.

Good luck!

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