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Hey guys...had a quick question regarding Ideal Gases that wasn't tackled to my liking in similar posts. I understand that ideal gases behave at high T and low P....due to the increased kinetic energy and low pressure resulting in less intermolecular attraction of gas molecules...I also understand that at moderately high pressure and low temperature...the expected volume from the ideal gas law..is greater than the real gas due to the intermolecular forces present at the increased pressure and low temperature. All of this makes sense...my question pertains to extremely high pressure and extremely low temperature. I'm using Kap...and what I've gotten is this...
Moderately high P and low T = gas is smaller than predicted by ideal gas law due to increased intermolecular attractions
Extreme high P and extremely low T = gas is larger than predicted by ideal gas law...due to the fact at such extremes...the volume of the gas particles themselves is bigger than the distance between particles.
So now to my question.....how can we differentiate between the two? Is there a number we should memorize that is considered moderately high vs extreme? And have I understood the above material correctly? Or am I confusing concepts?
Thanks!
Moderately high P and low T = gas is smaller than predicted by ideal gas law due to increased intermolecular attractions
Extreme high P and extremely low T = gas is larger than predicted by ideal gas law...due to the fact at such extremes...the volume of the gas particles themselves is bigger than the distance between particles.
So now to my question.....how can we differentiate between the two? Is there a number we should memorize that is considered moderately high vs extreme? And have I understood the above material correctly? Or am I confusing concepts?
Thanks!