For a 0.300 mol sample of helium gas in a 0.200 L container at 248K, will the pressure be greater if calculated with the ideal gas law or the van der Waals equation, and by roughly how much? (For He, a=0.0342L2atmmol2,b=0.0237 Lmol)

It changes by roughly 1 atm.

Explanation:

Hello!

In this case, since the ideal gas equation differs from the van der Waals' one by the presence of the a and b parameters which correct the assumption of no interactions into the container, they are written as:

Thus, the pressure via the ideal gas equation is:

And the pressure via the van der Waals equation, considering the molar volume (vm=0.200L/0.300L=0.667L/mol) is:

It means that the pressure change by 1 atm, which is not a significant difference for helium.

a

explanation:

in the analysis of systems that involve fluid flow, we frequently encounter the combination of properties u and pv.