- #1
sgstudent
- 739
- 3
the equation (P+a(n/V)^2)(V-nb)=nRT was derived in this manner:
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 Pmeasured+a(n/V)^2=Pideal
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 Videal-nb=Vreal
So this seems pretty weird to me.. For the P+a(n/V)^2 term we are substituting values to get Pideal while for the V-nb term we are substituting values to get Vreal
Is there a reason for this?
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 Pmeasured+a(n/V)^2=Pideal
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 Videal-nb=Vreal
So this seems pretty weird to me.. For the P+a(n/V)^2 term we are substituting values to get Pideal while for the V-nb term we are substituting values to get Vreal
Is there a reason for this?