By H. C. Van Ness (Auth.)

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**Extra info for Classical Thermodynamics of Non-Electrolyte Solutions**

**Sample text**

Dp ^ (*, d In/,) = 27 (*, d lnfc) + - p - . Substitution in Eq. (2-75) gives άΡ+^-άΤ^ΣίΧιάΙηφο. \RT P) RT2 But RT 1 P 1 / F _ RT RT\ P I RT' where <% is the residual volume as defined by Eq. (2-52). Therefore -^-dP+^-dr=i;(xidln^). (2-78) t One of the d JC/S can be eliminated from this equation through the relation Σάχ{ = 0. All the remaining variables are then independent. This procedure is illustrated on p. 80 for another equation of similar form. In Eq. (2-76) as it stands the variables are not all independent; hence certain mathematical operations on it are excluded.

L. Kang, L. J. Hirth, K. A. Kobe, and J. J. McKetta, /. Chem. and Eng. Data, 6, 220 (1961). 50 THERMODYNAMICS OF NON-ELECTROLYTE SOLUTIONS is well above the critical. The virial coefficients determined by means of this graph were used with the virial equation to calculate compressibility factors for the purpose of comparison with experimental values. This com parison is shown in Fig. 3-5. For the 50°C isotherm no deviations between H 3000 - 2 8 0 \- FIG. 3-3. Second and third virial coefficients for the nitrogen-n-butane system at 370°F.

We now have values of ln