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The phase diagrams of binary fluid mixtures are classified with regard to the topology of their critical curves and three-phase curves. A new nomenclature for the phase diagram classes is proposed, which can be applied to the previously known as well as to recently discovered phase diagram classes. The class names of the new nomenclature are systematic and descriptive; the (P,T) projection of a binary fluid phase diagram can always be constructed qualitatively from the class name. INTRODUCTION Phase equilibria in binary systems are usually depicted graphically in pressure, temperature, composition (P,T,x) space, in (P,T) and (T,x) projections or in isothermal (PJ) sections, isobaric (TJ ) sections and in constant composition (P,T) sections, so called isopleths. In these diagrams the different types of phase equilibria are represented by areas, curves or points. Some of these equilibrium states are characterized by special values of thermodynamic variables and will be referred to as special states. In the scope of this work a special state or point is defined as a state or point where 1. Either a phase is added or disappears. 2. Where the composition of two phases become identical. The composition of two phases can become identical in three different ways (Rowlinson & Swinton, 1982). The curves representing the composition of two coexisting phases can intersect at x = 0 or x = 1. This is shown in Fig. la, which shows a vapour-liquid equilibrium gl where the curve that represents the composition of the liquid phase 1 intersects the curve for the vapour phase g in the boiling points of both pure components. Also these curves can merge in a horizontal tangent point (dT/dx), = 0 or ( d P / d ~ ) ~ = 0. This type of special point is a critical point, where not only the composition but all thermodynamic properties of the two phases become identical. A diagram with a critical point is shown in Fig. lb. The third possibility is that the two curves have a common horizontal tangent. In this case only the compositions of the two phases are equal, but not the other thermodynamic properties. An example is an azeotropic point (Fig. lc).

Nomenclature for phase diagrams with particular reference to vapour–liquid and liquid–liquid equilibria (Technical report)