What are the \"correction terms\" in the van der Waals\' equation that account f

Question

What are the "correction terms" in the van der Waals' equation that account for the non-ideal behavior of real gases? 6. For the van der Waals' equation, why has the volume been modified from that of an ideal gas? 7. For the van der Waals' equation, why has the pressure been modified from that of an ideal gas? 8. The volume of a sample of ideal gas at 25degreeC is 372 mL. What will be the volume of the gas if it is heated at constant pressure to 50degreeC? What will be the volume of the gas if it is cooled to -272degreeC?

Explanation / Answer

In the Vanderwaal eqution, t he equation is (P+a/V2) *(V-b)= RT

a and b represents the magnitude of intermolecular forces and volume that is excluded.

when the molecules come closer, the force of attraction gives higher pressure and lesser volume than ideal gas. So there in an increase in pressure and as a result decrease in volume.

b) At constant pressure V1/T1= V2/T2

V1= 372ml T1= 25 deg.c =25+273.15 =298.15K V2= ? T2= 50 deg.c =50+273.15=323.15K

V2= V1*T2/T1= 372*323.15/298.15=403.19 ml

b) when cooled to -272 deg.c =-272+273.15= 1.5K

V2= 372*1.5/298.15=1.87ml

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