G-Chem question about gasses

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At high pressures, the intermolecular forces are more significant and molecular size is more significant between molecules. Therefore, the actual volume will be less than the ideal gas model.
 
At very high pressure volume of real gasses is larger than ideal, due to the size of the gas molecules starting to play a significant role in the total volume.
 
At high pressures, the intermolecular forces are more significant and molecular size is more significant between molecules. Therefore, the actual volume will be less than the ideal gas model.

That's true at moderately high pressure and low temperature, but at extreme pressures the actual volume of the molecules comes into play and the volume ends up being larger than ideal.
 
That's true at moderately high pressure and low temperature, but at extreme pressures the actual volume of the molecules comes into play and the volume ends up being larger than ideal.

Thanks for the clarification. I was thinking a few hundred atms, but your absolutely correct at a few thousand atms.🙂
 
Exactly what they said, larger. here is a good analogy I heard somewhere.

Think of it like 10 marbles in your bedroom. This is at stp and have no affect on the overall volume (this is an assumption we make with the ideal gases). now as you increase the pressure of the room, you are forcing all of those marbles into a glass. So, if we were to use the pv=nrt at this high pressure, we would only be masuring the spaces between the marbles, not the actual marbles themselves. But, these marbles are significant compared to the sapce between them, giving it a larger volume.
 
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