Gibbs duhem equation derivation pdf

Gibbs duhem equation derivation pdf
But the chemical potential is a function of (p,T) (remember that according to the Gibbs- Duhem equation, µ, p and T are not independent). Therefore, at two-phase coexistence
A more elegant derivation of equation (e) starts out with the equation (a) for the excess Gibbs energy written in the following form. [GE /mj ]/R ⋅T = 1−φ + 1n(γ j ) (f)
29/01/2015 · The Gibbs-Duhem is a relationship among the intensive parameters of the system. It follows that for a simple system with r components. a simple system with a single component will have two degrees of freedom.
not extensive and so there can, for example, be no Euler relation or Gibbs-Duhem equation applicable. Of course, the stated entropy expression is also not concave and
For a two-component system, a derivative that specifies the concentration-dependence of one chemical potential can be calculated from the corresponding derivative of the other chemical potential by applying the Gibbs–Duhem Equation.
Surface tension of surfactant solutions c << cmc c cmc saturation below cmc Slope corresponds to surface density
using the Gibbs-Duhem equation • Explain the origin of enthalpy, entropy, and volume changes due to mixing • Calculate the enthalpy of solution from the enthalpy of mixing and vice versa • Explain why the chemical potential is the relevant property for determining solution equilibrium CfE: Gibbs Free Energy (Balancing Energy and Entropy) Gibbs Free Energy (Balancing Energy and Entropy
This equation known as the Gibbs-Duhem equation is the starting point for many developments where equilibrium compositional changes occur under constant temperature and pressure. 10 Fundamental equations for open system An open system is the one that can exchange matter with its surroundings. Consider a two component system at temperature T and pressure p which is composed of n 1 moles …
6 Interfacial thermodynamics: Gibbs equation 6.1 Gibbs convention and Gibbs dividing plane 89 6.2 Surface excess functions 90 6.3 Gibbs equation 94 6.3.1 Derivation of the Gibbs equation and the
Chemistry 365: Gibbs-Duhem Relations ©David Ronis McGill University Here’saquick reviewofhow the so-called Gibbs-Duhem relation is obtained in thermody-
A Gibbs-Duhem equation describes the mutual dependence of state variables in an individual thermodynamic phase. Combination of the Gibbs-Duhem equations of coexisting phases enables one to derive a so-called Clapeyron equation.
The paper presents a rigorous thermodyna mic derivation of the augmented Biot equations for a general case of adsorbing fl uid mixture confined to nanoporous solid. The proposed approach extends the Gibbs excess adsorption thermodynamics to poroelastic nanomaterials. The augmented Biot equations contain additional terms associated with the adsorption stress, whic h represents the derivative of
which is known as the Gibbs-Thompson equation. It relates the difference in pressure at It relates the difference in pressure at an interface to its surface tension and curvature.
The normal derivation of the Gibbs-Duhem equation is performed using the theorem of Euler under the presupposition that the energy is a homogeneous function of order one.
The Duhem-Margules equation Fractional distillation of non ideal solution Partially miscible liquids Phenol-water system Triethylamine-water system Nicotine-water system Steam distillation. 2 Phase equilibrium Various heterogeneous equilibria (Box 10.1) have been studied by methods suitable to that type of equilibrium, such as vaporization by using Raoult’s law and Clausius-Clapeyron
The Gibbs–Duhem equation (GDE) considerably simplifies thermodynamic analysis of multicomponent solutions and is essential to derivation of the Gibbs phase rule. The GDE places a restriction on the simultaneous variations in the intensive thermodynamic variables of a phase.

Adsorption at Fluid–Fluid Interfaces Part I

Gibbs Free Energy (Balancing Energy and Entropy)
Some Terminology… M = XC i=1 y iM¯ i Gibbs-Duhem Equation: @M @P T,y dP + @M @T P,y XC i=1 y i dM¯ i =0 “Partial Molar” property ℳ -!arbitrary thermodynamic
The Gibbs–Duhem equation • When the compositions are changed infinitesimally, G of a binary system changes by • At constant pressure and temperature, a change in Gibbs energy is given by
Solution Behavior • Goal: Understand • Concepts Activity Partial molar properties Ideal solutions Non-ideal solutions Gibbs’-Duhem Equation Dilute solutions (Raoult’s law and Henry’s law) • Homework: 2 WS2002 2 Raoult’s Law • Describes the behavior of solvents with containing a small volume fraction of solute • The vapor pressure of a component A in a solution at
for the derivation of a number of important results, including the integrated form of the fundamental equation, the Gibbs-Duhem relation, and the internal conditions of equilib- rium.
The equation given is, however, most appropriately called the Gibbs-Helmholtz equation since it was first recognized by both Gibbs and Helmholtz (independently). The greatest utility of this equation lies in the presence of the temperature derivative of the Gibbs free energy.
P independent equations (of the Gibbs-Duhem form) that describe the energetics of the system–one equation for each phase. In mathematical terms, the variance (F) is determined by the difference between (C+2) variables and (P) equations.

PHYSICAL REVIEW E 88, 042135 (2013) Local thermodynamics and the generalized Gibbs-Duhem equation in systems with long-range interactions Ivan Latella* and Agust´ın Perez-Madrid´
Willard Gibbs and Hermann von Helmholtz (see History of Chemistry and Energy Balance of Reacting Systems ). Some of the scientists mentioned above are illustrated in
Read “Gibbs–Duhem-based relationships among derivatives expressing the concentration dependences of selected chemical potentials for a multicomponent system, Biophysical Chemistry” on DeepDyve, the largest online rental service for scholarly research with thousands of academic publications available at your fingertips.
The equation (1) is known as the Gibbs-Duhem equation. Applications of Gibbs-Duhem equation: (i) Gibbs-duhem equation is helpful in calculating partial molar quantity of a binary mixture by measuring the composition of the mixture which depends on the total molar quantity.

The Gibbs-Duhem equation for this partial molar quantity, and the one most normally associated with the name, is then: (2) This equation shows that the chemical potentials in a mixture are not all independent and that there is a constraint equation which they must satisfy.
The following derivation is based on the method of Gibbs involving the use of the thermodynamic potential. If is the surface energy per unit area and s is the surface area, then the free energy of a two component system is given by the Gibbs Duhem equation,
to consider the derivation revisited using Gibbs equations related to this problem. For the convenience of the reader, next to the regular numbers of equations the numbers given in curly brackets are the numbers of equations in the Gibbs’ original work (Gibbs, 1961). Symbols used in the equations are the same as in Gibbs’ book. The famous equation, known as Gibbs adsorption equation is (1
The relation between activity coefficients and excess Gibbs energy functions for mixtures of electrolytes and nonelectrolytes is examined under a general framework. It is shown that the use of molality, instead of mole fraction, as a composition
Gibbs–Helmholtz equation – Wikipedia. En.wikipedia.org The Gibbs–Helmholtz equation is a thermodynamic equation used for calculating changes in the Gibbs energy of a …
19/04/2017 · If we want to divide the Gibbs free energy terms into one part for the bulk and one part for the surface, it doesn’t really make much sense to put the surface tension work term into the bulk Gibbs energy. So it ends up in the surface free energy expression.
The derivation of the Butler equation is based here on the requirement of the minimum Gibbs energy of a solution, taking into account its surface. Thus, when the second part of the famous paper of Gibbs was published in 1878 [74] , everything was ready to derive the Butler equation.
Substituting Equation (11) into Equation (16) one gets Equation (17) is the Gibbs-Duhem equation for an adsorbed phase at constant temperature and spreading
The derivation of the expressions for the Gibbs energy of an ideal gas mixture and the chemical potentials of its components is a classi- cal topic, addressed in standard textbooks of thermodynamics ( …
Extensivity and Relativistic Thermodynamics arXiv
the Gibbs–Duhem relation, provides a relationship among the change of chemical potentials of the components in a solution at constant P–T condition. The partial property, Y
Lecture#24 1 Lecture 24 Objectives: 1. Be able to use two different methods to compute partial molar properties. 2. Be able to derive the generalized Gibbs-Duhem Equation from partial molar properties.
and µ), but now there is a Gibbs -Duhem equation for each of the phases, since each one has different s and v . Thus, the variance ( intensive degrees of freedom) of a …
Lecture Number & Topics 0. Introduction & Syllabus 1. Josiah Willard Gibbs Invents Colloid Thermodynamics ibbs Interface, Surface of Discontinuity, Surface Excess Variables, G Dividing Surfaces, Equipotential Dividing Surface, Surface Area of a Dividing Surface, Surface tension, Curvature of Surfaces, Types of Interfaces 2. Integral and Differential Calculus otal Differential Equations
Abstract: It is shown that the Gibbs-Duhem equation can be used for the calculation of (i) a partial molar quantity of a binary mixture from measurements of the composition dependence of the corresponding total molar quantity, (ii) the partial molar quantity of a
Two component systems Chemistry 433 Lecture 21 NC State University Total derivative for two components We consider the thermodynamics of two‐component systems. The ideas discussed here are easily generalized to multicomponentsystems. For a solution consisting of n1 moles of component 1 and n2 moles of component 2, the Gibbs energy is a function T and P and the two mole numbers n1 …
Abstract: The general form of the Gibbs-Duhem equation is derived for multiphase/multicomponent thermodynamic systems. The result illustrates that the form of the equation is invariant with respect to the number of phases present in the material.
Chapter 6: Solution Thermodynamics and Principles of Phase Equilibria In all the preceding chapters we have focused primarily on thermodynamic systems comprising pure – angle of elevation example problems Derivation from Gibbs–Duhem relation. from which the derivation of the Clapeyron equation continues as in the previous section. Ideal gas approximation at low temperatures. When the phase transition of a substance is between a gas phase and a condensed phase (liquid or solid), and occurs at temperatures much lower than the critical temperature of that substance, the specific volume of
The last step in the derivation simply takes the step before twice -say for the G and H at the begin and end of a process- and subtracts the two identical equations leading to a Δ symbol. In this differential form the Gibbs-Helmholtz equation can be applied to any process.
32 3 Thermodynamics of interfaces Q Example 3.1. To show how our choice of the position of the Gibbs dividing plane influ-ences the surface excess , we …
In each simulation, the pressure is adjusted to satisfy chemical potential equality according to the Gibbs-Duhem equation. Each coexistence point is determined by just one simulation, and particle insertions are never performed or attempted. Vapourliquid coexistence for the Lennard-Jones model is evaluated, and extensions are discussed.

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On the Gibbs-Duhem equation for thermodynamic systems of

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https://en.wikipedia.org/wiki/Duhem%E2%80%93Margules_equation
Thermodynamic modelling of solid solutions UA Geosciences
– Gibbs–Duhem-based relationships among DeepDyve
Derivation of the Butler equation from the requirement of

CHEM685F17

Clausius–Clapeyron relation Wikipedia

Gibbs–Duhem-based relationships among DeepDyve
Gibbs’ Phase Rule Where it all Begins

For a two-component system, a derivative that specifies the concentration-dependence of one chemical potential can be calculated from the corresponding derivative of the other chemical potential by applying the Gibbs–Duhem Equation.
The equation given is, however, most appropriately called the Gibbs-Helmholtz equation since it was first recognized by both Gibbs and Helmholtz (independently). The greatest utility of this equation lies in the presence of the temperature derivative of the Gibbs free energy.
The paper presents a rigorous thermodyna mic derivation of the augmented Biot equations for a general case of adsorbing fl uid mixture confined to nanoporous solid. The proposed approach extends the Gibbs excess adsorption thermodynamics to poroelastic nanomaterials. The augmented Biot equations contain additional terms associated with the adsorption stress, whic h represents the derivative of
The Gibbs–Duhem equation • When the compositions are changed infinitesimally, G of a binary system changes by • At constant pressure and temperature, a change in Gibbs energy is given by
Willard Gibbs and Hermann von Helmholtz (see History of Chemistry and Energy Balance of Reacting Systems ). Some of the scientists mentioned above are illustrated in
Two component systems Chemistry 433 Lecture 21 NC State University Total derivative for two components We consider the thermodynamics of two‐component systems. The ideas discussed here are easily generalized to multicomponentsystems. For a solution consisting of n1 moles of component 1 and n2 moles of component 2, the Gibbs energy is a function T and P and the two mole numbers n1 …
not extensive and so there can, for example, be no Euler relation or Gibbs-Duhem equation applicable. Of course, the stated entropy expression is also not concave and
which is known as the Gibbs-Thompson equation. It relates the difference in pressure at It relates the difference in pressure at an interface to its surface tension and curvature.

Chapter 6 Solution Thermodynamics and Principles of Phase
Lecture35 MIT OpenCourseWare

The Gibbs–Duhem equation (GDE) considerably simplifies thermodynamic analysis of multicomponent solutions and is essential to derivation of the Gibbs phase rule. The GDE places a restriction on the simultaneous variations in the intensive thermodynamic variables of a phase.
6 Interfacial thermodynamics: Gibbs equation 6.1 Gibbs convention and Gibbs dividing plane 89 6.2 Surface excess functions 90 6.3 Gibbs equation 94 6.3.1 Derivation of the Gibbs equation and the
The derivation of the expressions for the Gibbs energy of an ideal gas mixture and the chemical potentials of its components is a classi- cal topic, addressed in standard textbooks of thermodynamics ( …
The last step in the derivation simply takes the step before twice -say for the G and H at the begin and end of a process- and subtracts the two identical equations leading to a Δ symbol. In this differential form the Gibbs-Helmholtz equation can be applied to any process.
19/04/2017 · If we want to divide the Gibbs free energy terms into one part for the bulk and one part for the surface, it doesn’t really make much sense to put the surface tension work term into the bulk Gibbs energy. So it ends up in the surface free energy expression.
and µ), but now there is a Gibbs -Duhem equation for each of the phases, since each one has different s and v . Thus, the variance ( intensive degrees of freedom) of a …
The normal derivation of the Gibbs-Duhem equation is performed using the theorem of Euler under the presupposition that the energy is a homogeneous function of order one.
for the derivation of a number of important results, including the integrated form of the fundamental equation, the Gibbs-Duhem relation, and the internal conditions of equilib- rium.
A more elegant derivation of equation (e) starts out with the equation (a) for the excess Gibbs energy written in the following form. [GE /mj ]/R ⋅T = 1−φ 1n(γ j ) (f)
In each simulation, the pressure is adjusted to satisfy chemical potential equality according to the Gibbs-Duhem equation. Each coexistence point is determined by just one simulation, and particle insertions are never performed or attempted. Vapourliquid coexistence for the Lennard-Jones model is evaluated, and extensions are discussed.
the Gibbs–Duhem relation, provides a relationship among the change of chemical potentials of the components in a solution at constant P–T condition. The partial property, Y
using the Gibbs-Duhem equation • Explain the origin of enthalpy, entropy, and volume changes due to mixing • Calculate the enthalpy of solution from the enthalpy of mixing and vice versa • Explain why the chemical potential is the relevant property for determining solution equilibrium CfE: Gibbs Free Energy (Balancing Energy and Entropy) Gibbs Free Energy (Balancing Energy and Entropy
Chemistry 365: Gibbs-Duhem Relations ©David Ronis McGill University Here’saquick reviewofhow the so-called Gibbs-Duhem relation is obtained in thermody-
29/01/2015 · The Gibbs-Duhem is a relationship among the intensive parameters of the system. It follows that for a simple system with r components. a simple system with a single component will have two degrees of freedom.
Derivation from Gibbs–Duhem relation. from which the derivation of the Clapeyron equation continues as in the previous section. Ideal gas approximation at low temperatures. When the phase transition of a substance is between a gas phase and a condensed phase (liquid or solid), and occurs at temperatures much lower than the critical temperature of that substance, the specific volume of

Thermodynamic modelling of solid solutions UA Geosciences
Adsorption at Fluid–Fluid Interfaces Part I

In each simulation, the pressure is adjusted to satisfy chemical potential equality according to the Gibbs-Duhem equation. Each coexistence point is determined by just one simulation, and particle insertions are never performed or attempted. Vapourliquid coexistence for the Lennard-Jones model is evaluated, and extensions are discussed.
Read “Gibbs–Duhem-based relationships among derivatives expressing the concentration dependences of selected chemical potentials for a multicomponent system, Biophysical Chemistry” on DeepDyve, the largest online rental service for scholarly research with thousands of academic publications available at your fingertips.
The following derivation is based on the method of Gibbs involving the use of the thermodynamic potential. If is the surface energy per unit area and s is the surface area, then the free energy of a two component system is given by the Gibbs Duhem equation,
The Gibbs–Duhem equation (GDE) considerably simplifies thermodynamic analysis of multicomponent solutions and is essential to derivation of the Gibbs phase rule. The GDE places a restriction on the simultaneous variations in the intensive thermodynamic variables of a phase.
Substituting Equation (11) into Equation (16) one gets Equation (17) is the Gibbs-Duhem equation for an adsorbed phase at constant temperature and spreading
Chemistry 365: Gibbs-Duhem Relations ©David Ronis McGill University Here’saquick reviewofhow the so-called Gibbs-Duhem relation is obtained in thermody-
19/04/2017 · If we want to divide the Gibbs free energy terms into one part for the bulk and one part for the surface, it doesn’t really make much sense to put the surface tension work term into the bulk Gibbs energy. So it ends up in the surface free energy expression.
the Gibbs–Duhem relation, provides a relationship among the change of chemical potentials of the components in a solution at constant P–T condition. The partial property, Y
Two component systems Chemistry 433 Lecture 21 NC State University Total derivative for two components We consider the thermodynamics of two‐component systems. The ideas discussed here are easily generalized to multicomponentsystems. For a solution consisting of n1 moles of component 1 and n2 moles of component 2, the Gibbs energy is a function T and P and the two mole numbers n1 …
Willard Gibbs and Hermann von Helmholtz (see History of Chemistry and Energy Balance of Reacting Systems ). Some of the scientists mentioned above are illustrated in

Derivation of the Butler equation from the requirement of
Thermodynamic modelling of solid solutions UA Geosciences

32 3 Thermodynamics of interfaces Q Example 3.1. To show how our choice of the position of the Gibbs dividing plane influ-ences the surface excess , we …
For a two-component system, a derivative that specifies the concentration-dependence of one chemical potential can be calculated from the corresponding derivative of the other chemical potential by applying the Gibbs–Duhem Equation.
A Gibbs-Duhem equation describes the mutual dependence of state variables in an individual thermodynamic phase. Combination of the Gibbs-Duhem equations of coexisting phases enables one to derive a so-called Clapeyron equation.
the Gibbs–Duhem relation, provides a relationship among the change of chemical potentials of the components in a solution at constant P–T condition. The partial property, Y
In each simulation, the pressure is adjusted to satisfy chemical potential equality according to the Gibbs-Duhem equation. Each coexistence point is determined by just one simulation, and particle insertions are never performed or attempted. Vapourliquid coexistence for the Lennard-Jones model is evaluated, and extensions are discussed.
Substituting Equation (11) into Equation (16) one gets Equation (17) is the Gibbs-Duhem equation for an adsorbed phase at constant temperature and spreading
The Gibbs–Duhem equation • When the compositions are changed infinitesimally, G of a binary system changes by • At constant pressure and temperature, a change in Gibbs energy is given by
Gibbs–Helmholtz equation – Wikipedia. En.wikipedia.org The Gibbs–Helmholtz equation is a thermodynamic equation used for calculating changes in the Gibbs energy of a …
PHYSICAL REVIEW E 88, 042135 (2013) Local thermodynamics and the generalized Gibbs-Duhem equation in systems with long-range interactions Ivan Latella* and Agust´ın Perez-Madrid´
A more elegant derivation of equation (e) starts out with the equation (a) for the excess Gibbs energy written in the following form. [GE /mj ]/R ⋅T = 1−φ 1n(γ j ) (f)
The equation (1) is known as the Gibbs-Duhem equation. Applications of Gibbs-Duhem equation: (i) Gibbs-duhem equation is helpful in calculating partial molar quantity of a binary mixture by measuring the composition of the mixture which depends on the total molar quantity.
using the Gibbs-Duhem equation • Explain the origin of enthalpy, entropy, and volume changes due to mixing • Calculate the enthalpy of solution from the enthalpy of mixing and vice versa • Explain why the chemical potential is the relevant property for determining solution equilibrium CfE: Gibbs Free Energy (Balancing Energy and Entropy) Gibbs Free Energy (Balancing Energy and Entropy
The last step in the derivation simply takes the step before twice -say for the G and H at the begin and end of a process- and subtracts the two identical equations leading to a Δ symbol. In this differential form the Gibbs-Helmholtz equation can be applied to any process.
Solution Behavior • Goal: Understand • Concepts Activity Partial molar properties Ideal solutions Non-ideal solutions Gibbs’-Duhem Equation Dilute solutions (Raoult’s law and Henry’s law) • Homework: 2 WS2002 2 Raoult’s Law • Describes the behavior of solvents with containing a small volume fraction of solute • The vapor pressure of a component A in a solution at

Adsorption at Fluid–Fluid Interfaces Part I
Lecture 7 phase equilibrium kau

which is known as the Gibbs-Thompson equation. It relates the difference in pressure at It relates the difference in pressure at an interface to its surface tension and curvature.
the Gibbs–Duhem relation, provides a relationship among the change of chemical potentials of the components in a solution at constant P–T condition. The partial property, Y
The Gibbs–Duhem equation (GDE) considerably simplifies thermodynamic analysis of multicomponent solutions and is essential to derivation of the Gibbs phase rule. The GDE places a restriction on the simultaneous variations in the intensive thermodynamic variables of a phase.
The Gibbs–Duhem equation • When the compositions are changed infinitesimally, G of a binary system changes by • At constant pressure and temperature, a change in Gibbs energy is given by
for the derivation of a number of important results, including the integrated form of the fundamental equation, the Gibbs-Duhem relation, and the internal conditions of equilib- rium.
This equation known as the Gibbs-Duhem equation is the starting point for many developments where equilibrium compositional changes occur under constant temperature and pressure. 10 Fundamental equations for open system An open system is the one that can exchange matter with its surroundings. Consider a two component system at temperature T and pressure p which is composed of n 1 moles …
The derivation of the Butler equation is based here on the requirement of the minimum Gibbs energy of a solution, taking into account its surface. Thus, when the second part of the famous paper of Gibbs was published in 1878 [74] , everything was ready to derive the Butler equation.
A Gibbs-Duhem equation describes the mutual dependence of state variables in an individual thermodynamic phase. Combination of the Gibbs-Duhem equations of coexisting phases enables one to derive a so-called Clapeyron equation.
The equation given is, however, most appropriately called the Gibbs-Helmholtz equation since it was first recognized by both Gibbs and Helmholtz (independently). The greatest utility of this equation lies in the presence of the temperature derivative of the Gibbs free energy.

Chapter 6 Solution Thermodynamics and Principles of Phase
Deriving the Gibbs-Duhem equation Journal of Chemical

Gibbs–Helmholtz equation – Wikipedia. En.wikipedia.org The Gibbs–Helmholtz equation is a thermodynamic equation used for calculating changes in the Gibbs energy of a …
The Duhem-Margules equation Fractional distillation of non ideal solution Partially miscible liquids Phenol-water system Triethylamine-water system Nicotine-water system Steam distillation. 2 Phase equilibrium Various heterogeneous equilibria (Box 10.1) have been studied by methods suitable to that type of equilibrium, such as vaporization by using Raoult’s law and Clausius-Clapeyron
The paper presents a rigorous thermodyna mic derivation of the augmented Biot equations for a general case of adsorbing fl uid mixture confined to nanoporous solid. The proposed approach extends the Gibbs excess adsorption thermodynamics to poroelastic nanomaterials. The augmented Biot equations contain additional terms associated with the adsorption stress, whic h represents the derivative of
In each simulation, the pressure is adjusted to satisfy chemical potential equality according to the Gibbs-Duhem equation. Each coexistence point is determined by just one simulation, and particle insertions are never performed or attempted. Vapourliquid coexistence for the Lennard-Jones model is evaluated, and extensions are discussed.
Abstract: The general form of the Gibbs-Duhem equation is derived for multiphase/multicomponent thermodynamic systems. The result illustrates that the form of the equation is invariant with respect to the number of phases present in the material.
Surface tension of surfactant solutions c << cmc c cmc saturation below cmc Slope corresponds to surface density
Derivation from Gibbs–Duhem relation. from which the derivation of the Clapeyron equation continues as in the previous section. Ideal gas approximation at low temperatures. When the phase transition of a substance is between a gas phase and a condensed phase (liquid or solid), and occurs at temperatures much lower than the critical temperature of that substance, the specific volume of
6 Interfacial thermodynamics: Gibbs equation 6.1 Gibbs convention and Gibbs dividing plane 89 6.2 Surface excess functions 90 6.3 Gibbs equation 94 6.3.1 Derivation of the Gibbs equation and the
The Gibbs–Duhem equation (GDE) considerably simplifies thermodynamic analysis of multicomponent solutions and is essential to derivation of the Gibbs phase rule. The GDE places a restriction on the simultaneous variations in the intensive thermodynamic variables of a phase.
P independent equations (of the Gibbs-Duhem form) that describe the energetics of the system–one equation for each phase. In mathematical terms, the variance (F) is determined by the difference between (C 2) variables and (P) equations.