How does estimate of absolute zero vary with gas?

Question

Can an expert on the subject tell me if this is a correct hypothesis for the question above?

"The faster a gas can increase temperature/pressure, the higher the temperature estimated absolute value can be reached."

If it isn't, please provide me with something that can be written as a correct hypothesis to how estimate of absolute value varies with gas with a sufficient explanation. Thanks in advance! :)

Answer 1

Absolute temperature comes from Charles's law, in which volume change of a gas is proportional to temperature. What is the temperature, if the gas volume vanishes all the way to "zero?" The accepted value is -273degC, with several hundredths of a degree to go. But this is for an ideal gas. There are no ideal gases, only real ones. If you try this out on water vapor, ammonia, or sulfur dioxide, you'll get some weird values for 'absolute zero."

Answer 2

I'm pretty sure that it depends upon the size of the molecule, and the fact that you have packing issues at low temperatures. Therefore a gas made up of a large element like radon, would have a greater volume at very low temperatures than say hydrogen.

This matters because abolute zero is figured out by looking at the relationship between volume/temperature

Now the speed in which a gas can increase temp/pressure may be dependent upon the overall size of the gas molecule, but I'm not sure about that relationship