We’re being asked to calculate the pressure exerted by a chlorine gas using the Van der Waal’s equation.
The Van der Waals equation is shown below:
▪ P = pressure, atm
▪ V = volume, L
▪ n = # of moles, mol
▪ R = gas constant = 0.08206 (L∙atm)/(mol∙K)
▪ T = temperature, K
▪ a = polarity coefficient
▪ b = size coefficient
Let’s first isolate the pressure in the Van der Waals Equation:
Assuming that the van der Waals equation predictions are accurate, account for why the pressure of He is higher than that predicted for an ideal 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.