Problem: Part B If 1.00 mol of argon is placed in a 0.500-L container at 30.0°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 = 0.03219 L/mol.Express your answer to two significant figures and include the appropriate units. 

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Part B

 If 1.00 mol of argon is placed in a 0.500-L container at 30.0°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 = 0.03219 L/mol.

Express your answer to two significant figures and include the appropriate units. 


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