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.
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.
How long does this problem take to solve?
Our expert Chemistry tutor, Leo took 5 minutes and 42 seconds to solve this problem. You can follow their steps in the video explanation above.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Bryant's class at USF.