41.083 atm is the difference between the ideal pressure (as predicted by the ideal gas law) and the real pressure (as predicted by the van der Waals equation.
Explanation:
Data given for argon gas:
number of moles = 1 mole
volume = 0.5 L
Temperature = 19 degrees or 292.15 K
a= 1.345 (L2⋅atm)/mol2
b= 0.03219L/mol.
R = 0.0821
The real pressure equation given by Van der Waals equation:
P =( RT ÷ Vm-b) - a ÷ Vm^2
Putting the values in the equation:
P = (0.0821 x 292.15) ÷(0.5 - 0.03219) - 1.345÷ (0.5)^2
= 23.98÷0.4678 - 1.345 ÷0 .25
= 51.26 - 5.38
= 45.88 atm is the real pressure.
The pressure from the ideal gas law
PV =nRT
P =( 1 x 0.0821 x 292.15) ÷ 0.5
= 4.797 atm
the difference between the ideal pressure and real pressure is
Pressure by vander waal equation- Pressure by ideal gas law
45.88 - 4.797
= 41.083 atm.is the difference between the two.
