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Question If 1.00mol of argon is placed in a 0.500-L container at 21.0∘C, what 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)? For argon, a=1.345(L2⋅atm)/mol2 and b=0.03219L/mol.

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Question

If 1.00mol of argon is placed in a 0.500-L container at 21.0∘C, what 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)?

For argon, a=1.345(L2⋅atm)/mol2 and b=0.03219L/mol.

 
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