Gibbs energy attraction

The mutual solubility of two liquids A and B depends, in general, on how much the molecules of each liquid tend to attract those of its own kind, relative to their tendency to attract those of the other. This tendency is measured by the excess Gibbs energy of mixing of the two liquids (see section 2.4), Am gL, which is related to the partial vapor pressures p/ and of the two liquids A and B in the mixture. If the composition of the system is given by and Wb moles of the respective components in a given phase, their mole fractions in this phase are... 

Figure 3.6. Gibbs energy vs composition diagrams of A-B systems showing the effect of (a) attractive and (b) repulsive interactions.

The nature of the various attractive and repulsive forces that can act is discussed in the rest of this chapter. Because entropic contributions often are involved, we need to consider free energy (more precisely Gibbs energy) rather than internal energy. Especially the repulsive forces tend to depend greatly on the substances adsorbed onto particles or film surfaces, i.e., on surfactant properties and concentration. 

Attractive Potential Energy See Gibbs Energy of Attraction. 

Potential Energy of Attraction—Interaction—Repulsion See Gibbs Energy of... 

Attraction, Gibbs Energy of Interaction, Gibbs Energy of Repulsion. 

Close proximity between atoms leads to synchronization of their orbiting electrons. This causes the induction of dipoles that attract each other (London-van der Waals interaction). At closer approach, the electron clouds overlap, giving rise to repulsion (Born repulsion). The variation of the Gibbs energy of dispersion interactions Gji p between two atoms with their separation distance r is given by... 

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