Modified van der Waals equation for liquids
- 1 January 1966
- journal article
- research article
- Published by Royal Society of Chemistry (RSC) in Transactions of the Faraday Society
- Vol. 62, 828-837
- https://doi.org/10.1039/tf9666200828
Abstract
The van der Waals equation is modified for application to the liquid state by (a) using the conventional Hildebrand term for the internal pressure; (b) introducing an interaction constant B to describe external kinetic degrees of freedom; (c) introducing a quantity β0 for the residual compressibility of the molecules themselves. At high volumes β0 can be neglected and the proposed form of the van der Waals equation reduced to βT/α=(V—b0)/BR, where b0 is the molar volume at 0°K. Good linearity is observed when βT/α is plotted against volume for simple liquids; the number of “apparent degrees of freedom” 3B is for argon 4, for nitrogen 5.3, oxygen 5.8 and methane 6.5. Values of b0 are extrapolated from the same plots and reasonable values are obtained. For straight chain hydrocarbons with r carbon atoms, 3B=(r+5) and the above equation predict the internal pressure successfully. At low volumes, and pressures of 0–10,000 atm, polyatomic liquids may be treated successfully if (β0) is taken into account, and values of β0 may be estimated. The moduli 1/β0for methanol, diethyl ether, n-octane and acetone are 1–2 × 1011dynes/cm2.Keywords
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