- #1

sgstudent

- 739

- 3

The pressure of a real gas is affected by intermolecular forces and so the a(n/V)^2 term must be added to the measured pressure to obtain the ideal pressure where P

_{measured}+a(n/V)^2=P

_{ideal}

On the other hand when they explained the volume, they stated that the molecule had a finite size so we had to subtract the measured volume with the nb term to get the actual volume of the gas. So essentially V

_{ideal}-nb=V

_{real}

So this seems pretty weird to me.. For the P+a(n/V)^2 term we are substituting values to get P

_{ideal}while for the V-nb term we are substituting values to get V

_{real}

Is there a reason for this?