Van der Waals Equation Video Lessons

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Problem: If 1.00 mol of argon is placed in a 0.500-L container at 24.0 °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.Ideal versus real behavior for gasesIn the following part you can see how the behavior of real gases deviates from the ideal behavior. You will calculate the pressure values for a gas using the ideal gas law and also the van der Waals equation. Take note of how they differ.

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If 1.00 mol of argon is placed in a 0.500-L container at 24.0 °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.


Ideal versus real behavior for gases

In the following part you can see how the behavior of real gases deviates from the ideal behavior. You will calculate the pressure values for a gas using the ideal gas law and also the van der Waals equation. Take note of how they differ.

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