By L. Lue [n.b. text has advertisements]
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Extra resources for Chemical Thermodynamics
Below the critical temperature, the system can split into two coexisting liquid phases, depending on the overall composition. The basic reason why liquid-liquid phase separation occurs is that the attractive interactions between different molecules are weaker than the attractive interactions beween similar molecules. As a result, similar molecules prefer to be near to each other and than to dissimilar molecules. The consequence of this at a macroscopic level is the formation of two liquid phases.
At a given temperature and pressure, only the composition of a ternary system needs to specified to fix its state. 10. The corners of the triangles represent the pure components. The upper corner is pure 1; the lower left corner is pure 2; and the lower right corner is pure 3. For a general point within the triangle, the mole fraction of a species is equal to the ratio of the distance of the point from the corresponding corner to the height of the triangle. Therefore, the sides of the triangle represent binary mixtures.
Chem. Soc. 63, 998 (1893). , ΔGα (T, p) = ◦,(s) ◦,(l) μα (T, p) − μα (T, p)). , xα ), γα , and the function ΔGα , then we could use Eq. 1) to predict the freezing temperature T of the mixture. One method to approximate the function ΔGα is by using a Taylor series expansion around the temperature Tm , the melting temperature of pure α at pressure p. com 63 Solid-liquid equilibrium Chemical Thermodynamics molar Gibbs free energy of the pure liquid phase. 3) Therefore, the first term of the Taylor series expansion in Eq.
Chemical Thermodynamics by L. Lue [n.b. text has advertisements]