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In thermodynamics, the limit of local stability with respect to small fluctuations is clearly defined by the condition that the second derivative of Gibbs free energy is zero. The locus of these points (the inflection point within a G-x or G-c curve, Gibbs free energy as a function of composition) is known as the spinodal curve.^{[1]}^{[2]} For compositions within this curve, infinitesimally small fluctuations in composition and density will lead to phase separation via spinodal decomposition. Outside of the curve, the solution will be at least metastable with respect to fluctuations.^{[2]} In other words, outside of the spinodal curve some careful process may obtain a single phase system.^{[2]} Inside of it, only processes far from thermodynamic equilibrium, such as physical vapor deposition, will allow to prepare single phase compositions.^{[3]} The local points of coexisting compositions, defined by the common tangent construction, are known as binodal (coexistence) curve, which denotes the minimum-energy equilibrium state of the system. Increasing temperature results in a decreasing difference between mixing entropy and mixing enthalpy, thus, the coexisting compositions come closer. The binodal curve forms the bases for the miscibility gap in a phase diagram. Since the free energy of mixture changes with temperature and concentration, the binodal and spinodal meet at the critical or consulate temperature and composition.^{[4]}
For binary solutions, the thermodynamic criterion which defines the spinodal curve is that the second derivative of free energy with respect to density or some composition variable is zero.^{[2]}^{[5]}^{[6]}
Extrema of the spinodal in temperature with respect to the composition variable coincide with ones of the binodal curve and are known as critical points.^{[6]}
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