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The van der Waals equation, named for its originator, the Dutch physicist Johannes Diderik van der Waals, is an equation of state that extends the ideal gas law to include the non-zero size of gas molecules and the interactions between them (both of which depend on the specific substance).
The Van der Waals equation adjusts for deviations from ideal behavior by incorporating correction factors for molecular size (volume) and intermolecular forces (attraction). It allows for a more precise prediction of gas behavior under conditions where these deviations become significant.
The van der Waals Equation of State is an equation relating the density of gases and liquids to the pressure, volume, and temperature conditions (i.e., it is a thermodynamic equation of state). It can be viewed as an adjustment to the ideal gas law that takes into account the non-zero volume of gas molecules and inter-particle attraction using ...
A8: van der Waal's Constants for Real Gases. The van der Waal's equation of state for a non-ideal (real) gas is: (P + an2 V2) (V − nb) = nRT (A8.1) (A8.1) (P + a n 2 V 2) (V − n b) = n R T. Template:HideTOC.
Van der Waals’ equation is \[\left(P+\frac{an^2}{V^2}\right)\left(V-nb\right)=nRT \nonumber \] It fits pressure-volume-temperature data for a real gas better than the ideal gas equation does.
A modification of the ideal gas law was proposed by Johannes D. van der Waals in 1873 to take into account molecular size and molecular interaction forces. It is usually referred to as the van der Waals equation of state.
This lecture deals with a more general form of the equation of state, called van der Waals equation, which gives a better description of reality both under the conceptual and numerical point of view.
