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 (L^{2} ⋅ atm)/mol^{2} 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.

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Van der Waals Equation concept. You can view video lessons to learn Van der Waals Equation. Or if you need more Van der Waals Equation practice, you can also practice Van der Waals Equation practice problems.