The Van der Waals' Equation is as follows:
where a is the polarity coefficient, which accounts for the attractive or repulsive interactions of the gas molecules, and b is the size coefficient, which accounts for the size of the individual gas molecules. This equation show how real gases deviate from ideal behavior.
We can rearrange this equation to see how both a and b affect the pressure of the gas.
The graph below shows the change in pressure as the temperature increases for a 1 mol sample of a gas confined to a 1 L container. The four plots correspond to an ideal gas and three real gases: CO2, N2, and Cl2.
At room temperature, all three real gases have a pressure less than the ideal gas. Which van der Waals constant, a or b, accounts for the influence intermolecular forces have in lowering the pressure of a real gas?
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.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Austell's class at UNC.