Why Does the Van Der Waals Equation Predict Lower Pressure Than Ideal Gas Law?

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The Van der Waals (VDW) equation predicts lower pressure than the Ideal Gas Law due to the presence of electrostatic interactions between gas particles. These interactions cause the particles to behave less freely compared to an ideal gas, which assumes no such forces. As a result, the VDW model accounts for the volume occupied by gas particles and their intermolecular attractions, leading to a reduced pressure prediction. This contrasts with the Ideal Gas Law, which does not consider these factors. Understanding these differences is crucial for accurately modeling real gas behavior.
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Why does the Van Der Walls equation give a less value for pressure than the Ideal Gas equation does?
 
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The main point is a VDW model gas has electrostatic interactions between particles. Thus, the particles are not flowing as free as in an ideal model gas. Therefore the pressure is smaller than the pressure predicted by VDW.
 

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