Chemistry help please
posted by Deborah on .
At pressures greater than 60,000 kPa, how does the volume of a real gas compare with the volume of an ideal gas under the same conditions?
A.)It is much greater.
B.)It is much less.
C.)There is no difference.
D.)It depends on the type of gas.
I think it is A.
Why not pick n(mols) and a convenient T (say 300 K) and a pressure (say 70,000 kPa) and calculate volume using the ideal gas law versus the van der waals equation for some gas (I wouldn't use H2 as but something like CH4 or CO2). Compare.