Thermodynamics | real gas question.
re: the compression factor.

So Z = Vm / Vm* (perfect), and then this relationship can be rearanged to pVm = ZRT and Z is 1 for the ideal gas.

Gases at low pressure appear in states quite close to that of an ideal gas.

Then it says, at high pressure, Z 1 and molar volume is large. I imagine that at high pressure, all the molecules would be closer together, and hence the volume would decrease... Isn't volume supposed to be inversely proportional to pressure?

Can anyone explain why, at high pressure, the compression factor for a real gas is Z1?

Question

Thermodynamics | real gas question.
re: the compression factor.

So Z = Vm / Vm* (perfect), and then this relationship can be rearanged to pVm = ZRT and Z is 1 for the ideal gas.

Gases at low pressure appear in states quite close to that of an ideal gas.

Then it says, at high pressure, Z > 1 and molar volume is large. I imagine that at high pressure, all the molecules would be closer together, and hence the volume would decrease... Isn't volume supposed to be inversely proportional to pressure?

Can anyone explain why, at high pressure, the compression factor for a real gas is Z>1?