We are now ready to compare g. sol (X. \end{equation}\].
Phase Diagrams - Purdue University The choice of the standard state is, in principle, arbitrary, but conventions are often chosen out of mathematical or experimental convenience. \\ \tag{13.9} Notice that the vapor pressure of pure B is higher than that of pure A. Let's focus on one of these liquids - A, for example.
Raoult's Law and Ideal Mixtures of Liquids - Chemistry LibreTexts Liquids boil when their vapor pressure becomes equal to the external pressure. (13.15) above. For a solute that does not dissociate in solution, \(i=1\). Raoults law applied to a system containing only one volatile component describes a line in the \(Px_{\text{B}}\) plot, as in Figure 13.1. Description. This happens because the liquidus and Dew point lines coincide at this point.
Solid solution - Wikipedia 6. &= \underbrace{\mu_{\text{solvent}}^{{-\kern-6pt{\ominus}\kern-6pt-}} + RT \ln P_{\text{solvent}}^*}_{\mu_{\text{solvent}}^*} + RT \ln x_{\text{solution}} \\ P_i=x_i P_i^*. For example, the water phase diagram has a triple point corresponding to the single temperature and pressure at which solid, liquid, and gaseous water can coexist in a stable equilibrium (273.16K and a partial vapor pressure of 611.657Pa). A volume-based measure like molarity would be inadvisable. Since the degrees of freedom inside the area are only 2, for a system at constant temperature, a point inside the coexistence area has fixed mole fractions for both phases. B is the more volatile liquid. Thus, we can study the behavior of the partial pressure of a gasliquid solution in a 2-dimensional plot. \tag{13.19} On the last page, we looked at how the phase diagram for an ideal mixture of two liquids was built up. Similarly to the previous case, the cryoscopic constant can be related to the molar enthalpy of fusion of the solvent using the equivalence of the chemical potential of the solid and the liquid phases at the melting point, and employing the GibbsHelmholtz equation: \[\begin{equation} In addition to the above-mentioned types of phase diagrams, there are many other possible combinations. Once the temperature is fixed, and the vapor pressure is measured, the mole fraction of the volatile component in the liquid phase is determined. If we move from the \(Px_{\text{B}}\) diagram to the \(Tx_{\text{B}}\) diagram, the behaviors observed in Figure 13.7 will correspond to the diagram in Figure 13.8. The liquidus line separates the *all . where x A. and x B are the mole fractions of the two components, and the enthalpy of mixing is zero, . [9], The value of the slope dP/dT is given by the ClausiusClapeyron equation for fusion (melting)[10]. Figure 13.5: The Fractional Distillation Process and Theoretical Plates Calculated on a TemperatureComposition Phase Diagram. Raoults law states that the partial pressure of each component, \(i\), of an ideal mixture of liquids, \(P_i\), is equal to the vapor pressure of the pure component \(P_i^*\) multiplied by its mole fraction in the mixture \(x_i\): Raoults law applied to a system containing only one volatile component describes a line in the \(Px_{\text{B}}\) plot, as in Figure \(\PageIndex{1}\). Some organic materials pass through intermediate states between solid and liquid; these states are called mesophases. That means that an ideal mixture of two liquids will have zero enthalpy change of mixing. B) with g. liq (X. Subtracting eq. The fact that there are two separate curved lines joining the boiling points of the pure components means that the vapor composition is usually not the same as the liquid composition the vapor is in equilibrium with. Have seen that if d2F/dc2 everywhere 0 have a homogeneous solution. The osmotic pressure of a solution is defined as the difference in pressure between the solution and the pure liquid solvent when the two are in equilibrium across a semi-permeable (osmotic) membrane. If the proportion of each escaping stays the same, obviously only half as many will escape in any given time. Colligative properties usually result from the dissolution of a nonvolatile solute in a volatile liquid solvent, and they are properties of the solvent, modified by the presence of the solute. The first type is the positive azeotrope (left plot in Figure 13.8).
Phase Diagrams and Thermodynamic Modeling of Solutions The Thomas Group - PTCL, Oxford - University of Oxford However, careful differential scanning calorimetry (DSC) of EG + ChCl mixtures surprisingly revealed that the liquidus lines of the phase diagram apparently follow the predictions for an ideal binary non-electrolyte mixture. The axes correspond to the pressure and temperature. The diagram also includes the melting and boiling points of the pure water from the original phase diagram for pure water (black lines). (9.9): \[\begin{equation} (i) mixingH is negative because energy is released due to increase in attractive forces.Therefore, dissolution process is exothermic and heating the solution will decrease solubility. \mu_i^{\text{solution}} = \mu_i^* + RT \ln x_i, Compared to the \(Px_{\text{B}}\) diagram of Figure 13.3, the phases are now in reversed order, with the liquid at the bottom (low temperature), and the vapor on top (high Temperature). \mu_i^{\text{vapor}} = \mu_i^{{-\kern-6pt{\ominus}\kern-6pt-}} + RT \ln \frac{P_i}{P^{{-\kern-6pt{\ominus}\kern-6pt-}}}. \end{equation}\]. Composition is in percent anorthite. Using the phase diagram. The LibreTexts libraries arePowered by NICE CXone Expertand are supported by the Department of Education Open Textbook Pilot Project, the UC Davis Office of the Provost, the UC Davis Library, the California State University Affordable Learning Solutions Program, and Merlot. For non-ideal gases, we introduced in chapter 11 the concept of fugacity as an effective pressure that accounts for non-ideal behavior. For example, if the solubility limit of a phase needs to be known, some physical method such as microscopy would be used to observe the formation of the second phase. mixing as a function of concentration in an ideal bi-nary solution where the atoms are distributed at ran-dom. \tag{13.5} This explanation shows how colligative properties are independent of the nature of the chemical species in a solution only if the solution is ideal. As is clear from the results of Exercise 13.1, the concentration of the components in the gas and vapor phases are different. Any two thermodynamic quantities may be shown on the horizontal and vertical axes of a two-dimensional diagram.
PDF CHEMISTRY 313 PHYSICAL CHEMISTRY I Additional Problems for Exam 3 Exam where \(P_i^{\text{R}}\) is the partial pressure calculated using Raoults law. \end{equation}\]. where \(\mu_i^*\) is the chemical potential of the pure element.
The lowest possible melting point over all of the mixing ratios of the constituents is called the eutectic temperature.On a phase diagram, the eutectic temperature is seen as the eutectic point (see plot on the right). The activity of component \(i\) can be calculated as an effective mole fraction, using: \[\begin{equation} This fact, however, should not surprise us, since the equilibrium constant is also related to \(\Delta_{\text{rxn}} G^{{-\kern-6pt{\ominus}\kern-6pt-}}\) using Gibbs relation. At this pressure, the solution forms a vapor phase with mole fraction given by the corresponding point on the Dew point line, \(y^f_{\text{B}}\). \tag{13.3} That is exactly what it says it is - the fraction of the total number of moles present which is A or B. That means that there are only half as many of each sort of molecule on the surface as in the pure liquids. \tag{13.16} Additional thermodynamic quantities may each be illustrated in increments as a series of lines curved, straight, or a combination of curved and straight. Since the vapors in the gas phase behave ideally, the total pressure can be simply calculated using Daltons law as the sum of the partial pressures of the two components \(P_{\text{TOT}}=P_{\text{A}}+P_{\text{B}}\). Colligative properties are properties of solutions that depend on the number of particles in the solution and not on the nature of the chemical species. For a pure component, this can be empirically calculated using Richard's Rule: Gfusion = - 9.5 ( Tm - T) Tm = melting temperature T = current temperature y_{\text{A}}=? A simple example diagram with hypothetical components 1 and 2 in a non-azeotropic mixture is shown at right. When two phases are present (e.g., gas and liquid), only two variables are independent: pressure and concentration. where \(R\) is the ideal gas constant, \(M\) is the molar mass of the solvent, and \(\Delta_{\mathrm{vap}} H\) is its molar enthalpy of vaporization. Figure 13.10: Reduction of the Chemical Potential of the Liquid Phase Due to the Addition of a Solute. (13.14) can also be used experimentally to obtain the activity coefficient from the phase diagram of the non-ideal solution. On this Wikipedia the language links are at the top of the page across from the article title. This method has been used to calculate the phase diagram on the right hand side of the diagram below. \end{equation}\]. . P_{\text{A}}^* = 0.03\;\text{bar} \qquad & \qquad P_{\text{B}}^* = 0.10\;\text{bar} \\ "Guideline on the Use of Fundamental Physical Constants and Basic Constants of Water", 3D Phase Diagrams for Water, Carbon Dioxide and Ammonia, "Interactive 3D Phase Diagrams Using Jmol", "The phase diagram of a non-ideal mixture's p v x 2-component gas=liquid representation, including azeotropes", DoITPoMS Teaching and Learning Package "Phase Diagrams and Solidification", Phase Diagrams: The Beginning of Wisdom Open Access Journal Article, Binodal curves, tie-lines, lever rule and invariant points How to read phase diagrams, The Alloy Phase Diagram International Commission (APDIC), List of boiling and freezing information of solvents, https://en.wikipedia.org/w/index.php?title=Phase_diagram&oldid=1142738429, Creative Commons Attribution-ShareAlike License 3.0, This page was last edited on 4 March 2023, at 02:56. Therefore, the number of independent variables along the line is only two. Such a mixture can be either a solid solution, eutectic or peritectic, among others. The phase diagram shows, in pressuretemperature space, the lines of equilibrium or phase boundaries between the three phases of solid, liquid, and gas. You would now be boiling a new liquid which had a composition C2. The diagram is divided into three fields, all liquid, liquid + crystal, all crystal. The diagram just shows what happens if you boil a particular mixture of A and B. The equilibrium conditions are shown as curves on a curved surface in 3D with areas for solid, liquid, and vapor phases and areas where solid and liquid, solid and vapor, or liquid and vapor coexist in equilibrium. (13.1), to rewrite eq. Working fluids are often categorized on the basis of the shape of their phase diagram. As emerges from Figure 13.1, Raoults law divides the diagram into two distinct areas, each with three degrees of freedom.57 Each area contains a phase, with the vapor at the bottom (low pressure), and the liquid at the top (high pressure). We write, dy2 dy1 = dy2 dt dy1 dt = g l siny1 y2, (the phase-plane equation) which can readily be solved by the method of separation of variables . & = \left( 1-x_{\text{solvent}}\right)P_{\text{solvent}}^* =x_{\text{solute}} P_{\text{solvent}}^*, 1) projections on the concentration triangle ABC of the liquidus, solidus, solvus surfaces; Both the Liquidus and Dew Point Line are Emphasized in this Plot. Employing this method, one can provide phase relationships of alloys under different conditions. A 30% anorthite has 30% calcium and 70% sodium. You can easily find the partial vapor pressures using Raoult's Law - assuming that a mixture of methanol and ethanol is ideal. We now move from studying 1-component systems to multi-component ones. \\ y_{\text{A}}=? \end{equation}\]. (11.29) to write the chemical potential in the gas phase as: \[\begin{equation} If the temperature rises or falls when you mix the two liquids, then the mixture is not ideal. \begin{aligned} Typically, a phase diagram includes lines of equilibrium or phase boundaries. This ratio can be measured using any unit of concentration, such as mole fraction, molarity, and normality.
Phase Diagrams - Wisc-Online OER In other words, it measures equilibrium relative to a standard state. As with the other colligative properties, the Morse equation is a consequence of the equality of the chemical potentials of the solvent and the solution at equilibrium.59, Only two degrees of freedom are visible in the \(Px_{\text{B}}\) diagram. You get the total vapor pressure of the liquid mixture by adding these together. For the purposes of this topic, getting close to ideal is good enough! For a representation of ternary equilibria a three-dimensional phase diagram is required. A phase diagram in physical chemistry, engineering, mineralogy, and materials science is a type of chart used to show conditions (pressure, temperature, volume, etc.) \end{equation}\]. As we increase the temperature, the pressure of the water vapor increases, as described by the liquid-gas curve in the phase diagram for water ( Figure 10.31 ), and a two-phase equilibrium of liquid and gaseous phases remains. If we extend this concept to non-ideal solution, we can introduce the activity of a liquid or a solid, \(a\), as: \[\begin{equation} When one phase is present, binary solutions require \(4-1=3\) variables to be described, usually temperature (\(T\)), pressure (\(P\)), and mole fraction (\(y_i\) in the gas phase and \(x_i\) in the liquid phase). This page looks at the phase diagrams for non-ideal mixtures of liquids, and introduces the idea of an azeotropic mixture (also known as an azeotrope or constant boiling mixture). Legal. Starting from a solvent at atmospheric pressure in the apparatus depicted in Figure 13.11, we can add solute particles to the left side of the apparatus. Since the vapors in the gas phase behave ideally, the total pressure can be simply calculated using Dalton's law as the sum of the partial pressures of the two components P TOT = P A + P B. [5] Other exceptions include antimony and bismuth. The chemical potential of a component in the mixture is then calculated using: \[\begin{equation} Make-up water in available at 25C. This reflects the fact that, at extremely high temperatures and pressures, the liquid and gaseous phases become indistinguishable,[2] in what is known as a supercritical fluid. We can now consider the phase diagram of a 2-component ideal solution as a function of temperature at constant pressure. For plotting a phase diagram we need to know how solubility limits (as determined by the common tangent construction) vary with temperature. \mu_{\text{non-ideal}} = \mu^{{-\kern-6pt{\ominus}\kern-6pt-}} + RT \ln a, For two particular volatile components at a certain pressure such as atmospheric pressure, a boiling-point diagram shows what vapor (gas) compositions are in equilibrium with given liquid compositions depending on temperature. You calculate mole fraction using, for example: \[ \chi_A = \dfrac{\text{moles of A}}{\text{total number of moles}} \label{4}\]. A phase diagramin physical chemistry, engineering, mineralogy, and materials scienceis a type of chartused to show conditions (pressure, temperature, volume, etc.) This is exemplified in the industrial process of fractional distillation, as schematically depicted in Figure 13.5. I want to start by looking again at material from the last part of that page. The solidus is the temperature below which the substance is stable in the solid state. As such, a liquid solution of initial composition \(x_{\text{B}}^i\) can be heated until it hits the liquidus line. \[ \underset{\text{total vapor pressure}}{P_{total} } = P_A + P_B \label{3}\]. Suppose you double the mole fraction of A in the mixture (keeping the temperature constant). The theoretical plates and the \(Tx_{\text{B}}\) are crucial for sizing the industrial fractional distillation columns. The second type is the negative azeotrope (right plot in Figure 13.8). This negative azeotrope boils at \(T=110\;^\circ \text{C}\), a temperature that is higher than the boiling points of the pure constituents, since hydrochloric acid boils at \(T=-84\;^\circ \text{C}\) and water at \(T=100\;^\circ \text{C}\). If you follow the logic of this through, the intermolecular attractions between two red molecules, two blue molecules or a red and a blue molecule must all be exactly the same if the mixture is to be ideal. Contents 1 Physical origin 2 Formal definition 3 Thermodynamic properties 3.1 Volume 3.2 Enthalpy and heat capacity 3.3 Entropy of mixing 4 Consequences 5 Non-ideality 6 See also 7 References \end{equation}\]. This behavior is observed at \(x_{\text{B}} \rightarrow 0\) in Figure 13.6, since the volatile component in this diagram is \(\mathrm{A}\). The \(T_{\text{B}}\) diagram for two volatile components is reported in Figure \(\PageIndex{4}\). There is also the peritectoid, a point where two solid phases combine into one solid phase during cooling. This is true whenever the solid phase is denser than the liquid phase. An orthographic projection of the 3D pvT graph showing pressure and temperature as the vertical and horizontal axes collapses the 3D plot into the standard 2D pressuretemperature diagram. \mu_{\text{solution}} (T_{\text{b}}) = \mu_{\text{solvent}}^*(T_b) + RT\ln x_{\text{solvent}}, There are two ways of looking at the above question: For two liquids at the same temperature, the liquid with the higher vapor pressure is the one with the lower boiling point. The global features of the phase diagram are well represented by the calculation, supporting the assumption of ideal solutions. The temperature decreases with the height of the column. Thus, the space model of a ternary phase diagram is a right-triangular prism. Phase separation occurs when free energy curve has regions of negative curvature. Figure 13.6: The PressureComposition Phase Diagram of a Non-Ideal Solution Containing a Single Volatile Component at Constant Temperature. This fact can be exploited to separate the two components of the solution.
13 Multi-Component Phase Diagrams and Solutions Notice from Figure 13.10 how the depression of the melting point is always smaller than the elevation of the boiling point. That means that there are only half as many of each sort of molecule on the surface as in the pure liquids.
Chapter 7 Simple Mixtures - Central Michigan University 1. The corresponding diagram is reported in Figure 13.2. The obvious difference between ideal solutions and ideal gases is that the intermolecular interactions in the liquid phase cannot be neglected as for the gas phase. \begin{aligned} The condensed liquid is richer in the more volatile component than Single-phase, 1-component systems require three-dimensional \(T,P,x_i\) diagram to be described. This is why the definition of a universally agreed-upon standard state is such an essential concept in chemistry, and why it is defined by the International Union of Pure and Applied Chemistry (IUPAC) and followed systematically by chemists around the globe., For a derivation, see the osmotic pressure Wikipedia page., \(P_{\text{TOT}}=P_{\text{A}}+P_{\text{B}}\), \[\begin{equation} Overview[edit] The lines also indicate where phase transition occur. Under these conditions therefore, solid nitrogen also floats in its liquid. \end{equation}\].
PDF Analysis of ODE Models - Texas A&M University What is total vapor pressure of this solution? Figure 1 shows the phase diagram of an ideal solution. Attention has been directed to mesophases because they enable display devices and have become commercially important through the so-called liquid-crystal technology. which shows that the vapor pressure lowering depends only on the concentration of the solute. . The liquidus is the temperature above which the substance is stable in a liquid state.
Phase Diagrams and Thermodynamic Modeling of Solutions \end{equation}\]. (1) High temperature: At temperatures above the melting points of both pure A and pure B, the . At the boiling point of the solution, the chemical potential of the solvent in the solution phase equals the chemical potential in the pure vapor phase above the solution: \[\begin{equation} Chart used to show conditions at which physical phases of a substance occur, For the use of this term in mathematics and physics, see, The International Association for the Properties of Water and Steam, Alan Prince, "Alloy Phase Equilibria", Elsevier, 290 pp (1966) ISBN 978-0444404626. In practice, this is all a lot easier than it looks when you first meet the definition of Raoult's Law and the equations! As is clear from Figure 13.4, the mole fraction of the \(\text{B}\) component in the gas phase is lower than the mole fraction in the liquid phase. { Fractional_Distillation_of_Ideal_Mixtures : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.
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The page will flow better if I do it this way around. For cases of partial dissociation, such as weak acids, weak bases, and their salts, \(i\) can assume non-integer values. The elevation of the boiling point can be quantified using: \[\begin{equation} How these work will be explored on another page. You can discover this composition by condensing the vapor and analyzing it. The following two colligative properties are explained by reporting the changes due to the solute molecules in the plot of the chemical potential as a function of temperature (Figure 12.1). Single phase regions are separated by lines of non-analytical behavior, where phase transitions occur, which are called phase boundaries. The curve between the critical point and the triple point shows the carbon dioxide boiling point with changes in pressure. For an ideal solution the entropy of mixing is assumed to be. This occurs because ice (solid water) is less dense than liquid water, as shown by the fact that ice floats on water. This flow stops when the pressure difference equals the osmotic pressure, \(\pi\). His studies resulted in a simple law that relates the vapor pressure of a solution to a constant, called Henrys law solubility constants: \[\begin{equation} The curves on the phase diagram show the points where the free energy (and other derived properties) becomes non-analytic: their derivatives with respect to the coordinates (temperature and pressure in this example) change discontinuously (abruptly). \tag{13.18} Liquid and Solid Solution phase changes - First Year General Chemistry