Van der Waals Equation Video Lessons

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Problem: 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.

FREE Expert Solution

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+an2V2V-nb=nRT

P = pressure, atm
V = volume, L
n = # of moles, mol
R = gas constant = 0.08206 (Latm)/(molK)
T = temperature, K
a = polarity coefficient
= size coefficient


Let’s first isolate the pressure in the Van der Waals Equation:

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Problem Details

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.

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