**Thermodynamic Properties and Applications of Modified van-der-Waals Equations of State**

Ronald J. Bakker

162 Thermodynamics – Fundamentals and Its Application in Science

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Kuča K. & Cabal, J. (2004a). In Vitro Reaktivace Acetylcholinesterázy Inhibované O-Isopropylmethylfluorofofonátem užitím biskvarterního oximu HS-6. *Česká a Slovenská* 

Kuča K. & Cabal, J. (2004b). In Vitro Reactivation of Tabun-Inhibited Acetylcholinesterase Using New Oximes – K027, K005, K033 and K048. *Central European Journal of Public* 

Kuča K.; Jun, D. & Musílek, K. (2006). Structural Requirements of Acetylcholinesterase Reactivators. *Mini-Reviews in Medicinal Chemistry*, Vol.6, No.3, pp. 269-277, ISSN 1389-

Additional information is available at the end of the chapter

http://dx.doi.org/10.5772/50315

## **1. Introduction**

Physical and chemical properties of natural fluids are used to understand geological processes in crustal and mantel rock. The fluid phase plays an important role in processes in diagenesis, metamorphism, deformation, magmatism, and ore formation. The environment of these processes reaches depths of maximally 5 km in oceanic crusts, and 65 km in continental crusts, e.g. [1, 2], which corresponds to pressures and temperatures up to 2 GPa and 1000 C, respectively. Although in deep environments the low porosity in solid rock does not allow the presence of large amounts of fluid phases, fluids may be entrapped in crystals as fluid inclusions, i.e. nm to µm sized cavities, e.g. [3], and fluid components may be present within the crystal lattice, e.g. [4]. The properties of the fluid phase can be approximated with equations of state (Eq. 1), which are mathematical formula that describe the relation between intensive properties of the fluid phase, such as pressure (*p*), temperature (*T*), composition (*x*), and molar volume (*V*m).

$$p\left(T, V\_{m'}x\right) \tag{1}$$

This pressure equation can be transformed according to thermodynamic principles [5], to calculate a variety of extensive properties, such as entropy, internal energy, enthalpy, Helmholtz energy, Gibbs energy, et al., as well as liquid-vapour equilibria and homogenization conditions of fluid inclusions, i.e. dew point curve, bubble point curve, and critical points, e.g. [6]. The partial derivative of Eq. 1 with respect to temperature is used to calculate total entropy change (*dS* in Eq. 2) and total internal energy change (*dU* in Eq. 3), according to the Maxwell's relations [5].

$$d\mathcal{S}\_{-}=\left.\left(\frac{\partial p}{\partial T}\right)\_{V,n\_{\Gamma}}dV\right.\tag{2}$$

$$d\mathcal{U}\_{\perp} = \left[ T \cdot \left( \frac{\mathcal{O}p}{\mathcal{O}T} \right)\_{V, n\_{\Gamma}} - p \right] dV \tag{3}$$

Thermodynamic Properties and Applications of Modified van-der-Waals Equations of State 165

<sup>2</sup>

2 2 2 2 2 1 34 4

*n RT* (12)

 

> 

4 according to van der Waals (W), Redlich and Kwong (RK), Soave

0 1 23 *aV aV aV a* 0 (15)

0 1 23 *bz bz bz b* 0 (16)

<sup>0</sup> *a p* (17)

*n RT* (18)

4 are defined according to the specific

(13)

(14)

*T pV <sup>z</sup>*

The general formulation that summarizes two-constant cubic equations of state according to van der Waals [7], Redlich and Kwong [8], Soave [9], and Peng and Robinson [10] is illustrated in Eq. 13 and 14, see also [11]. In the following paragraphs, these equations are

*<sup>p</sup> <sup>V</sup> VV V*

*T T*

*n RT n <sup>p</sup> V n V n Vn Vn*

 W RK S PR <sup>1</sup> *b b b b*  <sup>2</sup> *a a·T -0.5 a a*  <sup>3</sup> *- b b b*  <sup>4</sup> *- - - b* 

where *p* is pressure (in MPa), *T* is temperature (in Kelvin), *R* is the gas constant (8.3144621 J·mol-1K-1), *V* is volume (in cm3), *Vm* is molar volume (in cm3·mol-1), *n*T is the total amount of

equations of state (Table 1), and are assigned specific values of the two constants *a* and *b*, as originally designed by Waals [7]. The *a* parameter reflects attractive forces between

This type of equation of state can be transformed in the form of a cubic equation to define

where *a0*, *a1*, *a2*, and *a3* are defined in Eq. 17, 18, 19, and 20, respectively; *b0*, *b1*, *b2*, and *b3* are

 <sup>1</sup> *T T* <sup>341</sup> *a np* 

*m* 1 *m m* 34 4 *m*

*T TTT*

**2. Two-constant cubic equation of state** 

abbreviated with *Weos*, *RKeos, Seos*, and *PReos*.

substance (in mol). The parameters

1, 2, 3, and 

volume (Eq. 15) and compressibility factor (Eq. 16).

defined in Eq. 21, 22, 23, and 24, respectively.

**Table 1.** Definitions of

(S) and Peng and Robinson (PR).

*RT*

> > 1, 2, 3, and

3 2

3 2

molecules, whereas the *b* parameter reflects the volume of molecules.

where *nT* is the total amount of substance in the system. The enthalpy (*H*) can be directly obtained from the internal energy and the product of pressure and volume according to Eq. 4.

$$\begin{array}{rcl} \begin{array}{c} H \ \ \end{array} = & \begin{array}{c} \mathcal{U} \end{array} + \begin{array}{c} p \cdot V \end{array} \end{array} \tag{4}$$

The Helmholtz energy (*A*) can be calculated by combining the internal energy and entropy (Eq. 5), or by a direct integration of pressure (Eq. 1) in terms of total volume (Eq. 6).

$$A\_- = \downarrow \mathcal{U} - T\mathcal{S} \tag{5}$$

$$dA^{\quad} = \, -p dV\tag{6}$$

The Gibbs energy (*G*) is calculated in a similar procedure according to its definition in Eq. 7.

$$
\mathcal{G}\_- = \mathcal{U}\_- + p \cdot V\_- - T \cdot \mathcal{S} \tag{7}
$$

The chemical potential (*µ*i) of a specific fluid component (*i*) in a gas mixture or pure gas (Eq. 8) is obtained from the partial derivative of the Helmholtz energy (Eq. 5) with respect to the amount of substance of this component (*n*i).

$$
\mu\_i \quad = \left(\frac{\mathcal{\mathcal{D}A}}{\mathcal{\mathcal{O}n}\_i}\right)\_{T, V, n\_j} \tag{8}
$$

The fugacity (*f*) can be directly obtained from chemical potentials (Eq. 9) and from the definition of the fugacity coefficient (i) with independent variables *V* and *T* (Eq. 10).

$$RT\ln\left(\frac{f\_i}{f\_i^0}\right) = -\mu\_i - \mu\_i^0\tag{9}$$

where *µ*<sup>i</sup> 0 and *f*<sup>i</sup> 0 are the chemical potential and fugacity, respectively, of component *i* at standard conditions (0.1 MPa).

$$RT\ln\rho\_i = \int\_V^v \left[ \left(\frac{\partial p}{\partial n\_i}\right)\_{T,V,n\_j} - \frac{RT}{V} \right]dV - RT\ln z \,. \tag{10}$$

where i and z (compressibility factor) are defined according to Eq. 11 and 12, respectively.

$$
\rho\_i \quad = \frac{f\_i}{x\_i \cdot p} \tag{11}
$$

Thermodynamic Properties and Applications of Modified van-der-Waals Equations of State 165

$$
\omega\_{\perp} = \frac{pV}{n\_T RT} \tag{12}
$$

#### **2. Two-constant cubic equation of state**

164 Thermodynamics – Fundamentals and Its Application in Science

amount of substance of this component (*n*i).

definition of the fugacity coefficient (

where *µ*<sup>i</sup>

where  0 and *f*<sup>i</sup>

standard conditions (0.1 MPa).

4.

, *V nT*

(3)

*H U pV* (4)

*A U TS* (5)

*dA pdV* (6)

(8)

(9)

*G U pV TS* (7)

i) with independent variables *V* and *T* (Eq. 10).

. (10)

(11)

0

*i i*

0 are the chemical potential and fugacity, respectively, of component *i* at

*<sup>p</sup> dU T p dV <sup>T</sup>* 

where *nT* is the total amount of substance in the system. The enthalpy (*H*) can be directly obtained from the internal energy and the product of pressure and volume according to Eq.

The Helmholtz energy (*A*) can be calculated by combining the internal energy and entropy

The Gibbs energy (*G*) is calculated in a similar procedure according to its definition in Eq. 7.

The chemical potential (*µ*i) of a specific fluid component (*i*) in a gas mixture or pure gas (Eq. 8) is obtained from the partial derivative of the Helmholtz energy (Eq. 5) with respect to the

> *A n*

The fugacity (*f*) can be directly obtained from chemical potentials (Eq. 9) and from the

, , ln ln *j*

*<sup>p</sup> RT RT dV RT z n V*

i and z (compressibility factor) are defined according to Eq. 11 and 12, respectively.

*i*

*i f x p*

*V i TVn*

*i*

 

 

*i*

*<sup>f</sup> RT f*

*i*

 <sup>0</sup> ln *<sup>i</sup>*

*i*

, , *<sup>j</sup>*

*i TVn*

(Eq. 5), or by a direct integration of pressure (Eq. 1) in terms of total volume (Eq. 6).

 

The general formulation that summarizes two-constant cubic equations of state according to van der Waals [7], Redlich and Kwong [8], Soave [9], and Peng and Robinson [10] is illustrated in Eq. 13 and 14, see also [11]. In the following paragraphs, these equations are abbreviated with *Weos*, *RKeos, Seos*, and *PReos*.

$$p\_{\parallel} = \frac{RT}{V\_m - \zeta\_1} - \frac{\zeta\_2}{V\_m \cdot \left(V\_m + \zeta\_3\right) + \zeta\_4 \cdot \left(V\_m - \zeta\_4\right)}\tag{13}$$

$$p\_{\parallel} = \frac{n\_T RT}{V - n\_T \zeta\_1} - \frac{n\_T^{-2} \zeta\_2}{V^2 + n\_T \zeta\_3 V + n\_T \zeta\_4 V - n\_T^{-2} \zeta\_4^{-2}} \tag{14}$$

where *p* is pressure (in MPa), *T* is temperature (in Kelvin), *R* is the gas constant (8.3144621 J·mol-1K-1), *V* is volume (in cm3), *Vm* is molar volume (in cm3·mol-1), *n*T is the total amount of substance (in mol). The parameters 1, 2, 3, and 4 are defined according to the specific equations of state (Table 1), and are assigned specific values of the two constants *a* and *b*, as originally designed by Waals [7]. The *a* parameter reflects attractive forces between molecules, whereas the *b* parameter reflects the volume of molecules.


**Table 1.** Definitions of 1, 2, 3, and 4 according to van der Waals (W), Redlich and Kwong (RK), Soave (S) and Peng and Robinson (PR).

This type of equation of state can be transformed in the form of a cubic equation to define volume (Eq. 15) and compressibility factor (Eq. 16).

$$a\_0V^3 + a\_1V^2 + a\_2V + a\_3 = \begin{array}{c} 0 \end{array} \tag{15}$$

$$\begin{array}{ccccccccc}b\_0z^3 & + & b\_1z^2 & + & b\_2z & + & b\_3 & = & 0 & & & & \end{array} \tag{16}$$

where *a0*, *a1*, *a2*, and *a3* are defined in Eq. 17, 18, 19, and 20, respectively; *b0*, *b1*, *b2*, and *b3* are defined in Eq. 21, 22, 23, and 24, respectively.

<sup>0</sup> *a p* (17)

$$a\_1 \quad = \quad n\_T p \cdot \left(\mathcal{L}\_3 + \mathcal{L}\_4 - \mathcal{L}\_1\right) - \ \mathcal{n}\_T RT \tag{18}$$

$$\begin{array}{rcl} n\_2 &=& -n\_T \, ^2 p \cdot \left( \zeta\_4 \, ^2 + \zeta\_1 \zeta\_3 + \zeta\_1 \zeta\_4 \right) \\ &- \left( ^2 n \, ^2 \right) \cdot \left( \zeta\_3 + \zeta\_4 \right) + \left. n\_T \right|^2 \zeta\_2 \end{array} \tag{19}$$

$$\boldsymbol{a}\_{3} = \boldsymbol{n}\_{T}\boldsymbol{n}\_{T}^{3}\boldsymbol{p}\cdot\boldsymbol{\zeta}\_{1}\boldsymbol{\zeta}\_{4}^{2} + \boldsymbol{n}\_{T}^{3}\boldsymbol{\mathcal{R}}\boldsymbol{T}\cdot\boldsymbol{\zeta}\_{4}^{2} - \boldsymbol{n}\_{T}^{3}\cdot\boldsymbol{\zeta}\_{1}\boldsymbol{\zeta}\_{2} \tag{20}$$

$$\left| b\_0 \right| = \left( \frac{RT}{p} \right)^3 \tag{21}$$

Thermodynamic Properties and Applications of Modified van-der-Waals Equations of State 167

2 2

*T*

*n*

*TTT <sup>T</sup>*

*n Vn Vn n*

2 2 <sup>2</sup> 34 4 <sup>2</sup>

4 are usually independent of temperature, compare with the *b*

2 2 2 1 34 4 1 ( ) *T T <sup>T</sup> T TTT*

2 2 3 4

 

 

2 3 4 4 2 4

 

*T T T T*

*<sup>n</sup> <sup>n</sup> n n V n*

( ) () () <sup>2</sup>

*i i i*

*T*

  

> 

2 2

2 2 2

1

( )

 

2 2

*T T*

*T T*

1, 2, 3, and 4 are

 

 

 (29)

(30)

(31)

(32)

(33)

 

> 

2 2

*<sup>T</sup> V n Vn Vn*

*p nR nR n T V Vn V n Vn Vn T*

1 34 4 2 *T T*

1 34 4

*T TTT*

2 2 <sup>2</sup>

*<sup>p</sup> n RT <sup>n</sup> Vn n*

*<sup>p</sup> n RT <sup>n</sup> Vn n*

2 3 3 3 4 2 2 2

 

independent of volume. Finally, the partial derivative of pressure in respect to the amount of substance of a specific component in the fluid mixture (*n*i) is also used to characterize

1

( )

 

2 2

*nn n V n Vn Vn*

 

 

*T*

*n*

*T TTT*

Other important equations to calculate thermodynamic properties of fluids are partial

 

1 ( )

  <sup>1</sup> <sup>1</sup>

*TT T T <sup>T</sup> <sup>T</sup>*

2

 

 

derivatives of pressure with respect to volume (Eq. 31 and 32).

*<sup>V</sup> V n V n Vn Vn*

Eqs. 31 and 32 already include the assumption that the parameters

2

*T T*

1 ( )

 

> 

> 

*T TTT*

2

*V n Vn Vn*

*V n Vn Vn n*

*TTT i*

2 2 2 34 4

*TTT*

<sup>1</sup> <sup>1</sup>

*i T <sup>i</sup> <sup>T</sup>*

*p RT n RT n n Vn V n n*

2 2 2 34 4 2

*V V n V n Vn Vn*

*n*

2 2 <sup>2</sup> <sup>2</sup> 2 2 34 4

*T T*

 

*TTT*

<sup>2</sup> <sup>2</sup> 2 2 34 4

*V n Vn Vn T*

2 2 2 34 4

*p n R n R n RT n T V Vn T V n*

*TTT*

where

The parameters

1, 3, and 

parameter (Table 1). This reduces Eq. 29 to Eq. 30.

thermodynamic properties of fluid mixtures (Eq. 33).

2 2

$$b\_1 = \left(\frac{RT}{p}\right)^2 \cdot \left(\zeta\_3 + \zeta\_4 - \zeta\_1 - \frac{RT}{p}\right) \tag{22}$$

$$\left| b\_{2} \right| = \left( \frac{RT}{p} \right) \cdot \left( -\zeta\_{4} \right)^{2} - \left( \zeta\_{3} + \zeta\_{4} \right) \cdot \left( \zeta\_{1} + \frac{RT}{p} \right) + \frac{\zeta\_{2}}{p} \right) \tag{23}$$

$$\left(b\_3\right) = \left(\zeta\_1 + \frac{RT}{p}\right) \cdot \zeta\_4^{-2} - \frac{\zeta\_1 \zeta\_2}{p} \tag{24}$$

The advantage of a cubic equation is the possibility to have multiple solutions (maximally three) for volume at specific temperature and pressure conditions, which may reflect coexisting liquid and vapour phases. Liquid-vapour equilibria can only be calculated from the same equation of state if multiple solution of volume can be calculated at the same temperature and pressure. The calculation of thermodynamic properties with this type of equation of state is based on splitting Eq. 14 in two parts (Eq. 25), i.e. an ideal pressure (from the ideal gas law) and a departure (or residual) pressure, see also [6].

$$p\_- = \ p\_{ideal} + \ p\_{residual} \tag{25}$$

where

$$p\_{ideal} = \frac{n\_T RT}{V} \tag{26}$$

The residual pressure (*presidual*) can be defined as the difference (*p*, Eq. 27) between ideal pressure and reel pressure as expressed in Eq. 14 .

$$\Delta p = \left. p\_{\text{residual}} \right. \tag{27} \\ = \frac{n\_{\text{T}}RT}{V} + \frac{n\_{\text{T}}RT}{V - n\_{\text{T}}\zeta\_{1}} - \frac{n\_{\text{T}}^{\text{-2}}\zeta\_{2}}{V^{2} + n\_{\text{T}}\zeta\_{3}V + n\_{\text{T}}\zeta\_{4}V - n\_{\text{T}}^{\text{-2}}\zeta\_{4}^{\text{-2}}} \tag{27}$$

The partial derivative of pressure with respect to temperature (Eq. 28) is the main equation to estimate the thermodynamic properties of fluids (see Eqs. 2 and 3).

$$\frac{\partial \mathcal{P}}{\partial \mathcal{T}}\_{\mathcal{T}} = \frac{\partial p\_{\text{ideal}}}{\partial \mathcal{T}}\_{\mathcal{T}} + \frac{\partial \Delta p}{\partial \mathcal{T}}\_{\mathcal{T}} \tag{28}$$

where

166 Thermodynamics – Fundamentals and Its Application in Science

  

0

2 4 34 1 *RT RT <sup>b</sup>*

> 31 4 *RT <sup>b</sup>*

 

the ideal gas law) and a departure (or residual) pressure, see also [6].

The residual pressure (*presidual*) can be defined as the difference (

to estimate the thermodynamic properties of fluids (see Eqs. 2 and 3).

pressure and reel pressure as expressed in Eq. 14 .

*residual*

where

2 1 341 *RT RT <sup>b</sup>*

 

*RT <sup>b</sup>*

 

 2 2 <sup>2</sup> <sup>2</sup> <sup>2</sup> *<sup>T</sup>* 4 13 14 *T T* 3 4 <sup>2</sup> *a np*

3

3 23 23 <sup>3</sup> *TTT* 1 4 <sup>4</sup> 1 2 *a n p n RT n*

> *p*

*p p* 

*p p p*

 

*T*

*T T T*

The partial derivative of pressure with respect to temperature (Eq. 28) is the main equation

*ideal p p p T TT*

 

*n RT n RT <sup>n</sup> p p V Vn V n Vn Vn*

*n RT*

*ideal*

The advantage of a cubic equation is the possibility to have multiple solutions (maximally three) for volume at specific temperature and pressure conditions, which may reflect coexisting liquid and vapour phases. Liquid-vapour equilibria can only be calculated from the same equation of state if multiple solution of volume can be calculated at the same temperature and pressure. The calculation of thermodynamic properties with this type of equation of state is based on splitting Eq. 14 in two parts (Eq. 25), i.e. an ideal pressure (from

*p p*

 

<sup>2</sup> <sup>2</sup>

 

2 1 2

 

*ideal residual pp p* (25)

*<sup>p</sup> <sup>V</sup>* (26)

2 2 2 2 2 1 34 4

(28)

*T TTT*

*p*, Eq. 27) between ideal

  (27)

 

> 

 *n RT n* (19)

(21)

(20)

(22)

(24)

(23)

$$\begin{split} \frac{\partial \Delta p}{\partial T} &= -\frac{n\_T R}{V} + \frac{n\_T R}{V - n\_T \zeta\_1} + \frac{n\_T R T}{\left(V - n\_T \zeta\_1\right)^2} \cdot \frac{\mathcal{C}(n\_T \zeta\_1)}{\mathcal{C}T} \\ &- \frac{1}{V^2 + n\_T \zeta\_3 V + n\_T \zeta\_4 V - n\_T^2 \zeta\_4^2} \cdot \frac{\mathcal{C}(n\_T^{-2} \zeta\_2)}{\mathcal{C}T} \\ &+ \frac{n\_T^2 \zeta\_2}{\left(V^2 + n\_T \zeta\_3 V + n\_T \zeta\_4 V - n\_T^2 \zeta\_4^2\right)^2} \cdot \frac{\mathcal{C}\left(n\_T \zeta\_3 V + n\_T \zeta\_4 V - n\_T^2 \zeta\_4^2\right)}{\mathcal{C}T} \end{split} \tag{29}$$

The parameters 1, 3, and 4 are usually independent of temperature, compare with the *b* parameter (Table 1). This reduces Eq. 29 to Eq. 30.

$$\frac{\partial \Delta p}{\partial T} = -\frac{n\_T R}{V} + \frac{n\_T R}{V - n\_T \zeta\_1} - \frac{1}{V^2 + n\_T \zeta\_3 V + n\_T \zeta\_4 V - n\_T^2 \zeta\_4^2} \cdot \frac{\partial \langle n\_T^2 \zeta\_2 \rangle}{\partial T} \tag{30}$$

Other important equations to calculate thermodynamic properties of fluids are partial derivatives of pressure with respect to volume (Eq. 31 and 32).

$$\frac{\mathcal{CP}}{\mathcal{CP}}\_{\text{V}} = \left( -\frac{n\_{\text{T}}RT}{\left(V - n\_{\text{T}}\zeta\_{1}\right)^{2}} + \frac{n\_{\text{T}}^{\ast 2}\zeta\_{2}}{\left(V^{2} + n\_{\text{T}}\zeta\_{3}V + n\_{\text{T}}\zeta\_{4}V - n\_{\text{T}}^{\ast 2}\zeta\_{4}\right)^{2}} \cdot \left(2V + n\_{\text{T}}\zeta\_{3} + n\_{\text{T}}\zeta\_{4}\right) \tag{31}$$

$$\begin{split} \frac{\hat{\sigma}^2 p}{\hat{\sigma}V^2} &= \frac{2n\_\mathrm{T}RT}{\left(V - n\_\mathrm{T}\zeta\_1\right)^3} - \frac{2n\_\mathrm{T}^2 \zeta\_2}{\left(V^2 + n\_\mathrm{T}\zeta\_3 V + n\_\mathrm{T}\zeta\_4 V - n\_\mathrm{T}^2 \zeta\_4\right)^3} \cdot \left(2V + n\_\mathrm{T}\zeta\_3 + n\_\mathrm{T}\zeta\_4\right)^2 \\ &+ \frac{2n\_\mathrm{T}^2 \zeta\_2}{\left(V^2 + n\_\mathrm{T}\zeta\_3 V + n\_\mathrm{T}\zeta\_4 V - n\_\mathrm{T}^2 \zeta\_4\right)^2} \end{split} \tag{32}$$

Eqs. 31 and 32 already include the assumption that the parameters 1, 2, 3, and 4 are independent of volume. Finally, the partial derivative of pressure in respect to the amount of substance of a specific component in the fluid mixture (*n*i) is also used to characterize thermodynamic properties of fluid mixtures (Eq. 33).

$$\begin{split} \frac{\partial \hat{p}}{\partial \eta\_{i}} &= \frac{RT}{V - n\_{T}\zeta\_{1}} + \frac{n\_{T}RT}{\left(V - n\_{T}\zeta\_{1}\right)^{2}} \cdot \frac{\partial (n\_{T}\zeta\_{1})}{\partial n\_{i}} \\ &- \frac{1}{V^{2} + n\_{T}\zeta\_{3}V + n\_{T}\zeta\_{4}V - n\_{T}^{2}\zeta\_{4}^{2}} \cdot \frac{\partial (n\_{T}^{-2}\zeta\_{2})}{\partial n\_{i}} \\ &+ \frac{n\_{T}\zeta\_{2}}{\left(V^{2} + n\_{T}\zeta\_{3}V + n\_{T}\zeta\_{4}V - n\_{T}^{2}\zeta\_{4}^{2}\right)^{2}} \cdot \left[\left(\frac{\partial (n\_{T}\zeta\_{3})}{\partial n\_{i}} + \frac{\partial (n\_{T}\zeta\_{4})}{\partial n\_{i}}\right) \cdot V - 2n\_{T}\zeta\_{4}\frac{\partial (n\_{T}\zeta\_{4})}{\partial n\_{i}}\right] \end{split} \tag{33}$$

#### **3. Thermodynamic parameters**

The entropy (*S*) is obtained from the integration defined in Eq. 2 at constant temperature (Eqs. 34 and 35).

$$\int\_{S\_0}^{S} dS \quad = \int\_{V\_0}^{V} \left(\frac{\partial p}{\partial T}\right)\_{V, n\_T} dV \tag{34}$$

Thermodynamic Properties and Applications of Modified van-der-Waals Equations of State 169

(42)

*<sup>p</sup>* (43)

2

3 4

2( )

2

*T*

2 2

 

 

 

  3 = 0 and

The entropy change that is caused by a volume change of ideal gases corresponds to the second term on the right-hand side of Eqs. 36 and 37. This term can be used to express the behaviour of an ideal mixture of perfected gases. Each individual gas in a mixture expands from their partial volume (*v*i) to the total volume at a pressure of 0.1 MPa, which results in a

1 1

*i i ideal mix*

0 *i*

0 1 2

2

*T T T*

*S ns* (46)

(47)

*T*

<sup>1</sup> ( ) ln ln *T T*

(44)

0 1 2 3 4

0

0 is the molar entropy of a pure component *i* in an ideal gas mixture at temperature T.

*n RT V q T Vn q*

 

<sup>1</sup> ( ) 2( ) ln ln ln

 (45)

*n RT V VT*

*n RT*

0 .

*i*

volume according to the two-constant cubic equation of state is given by Eq. 44 for

*p V V n <sup>n</sup> S S nR n R*

*i i T p V Vn n Vn q S S nR n R*

The subscripts "1" for the upper limit of integration is eliminated to present a pronounced equation. The standard state entropy (*S*0) of a mixture of ideal gases is defined according to

> 0 *i i i*

The internal energy (*U*, see Eq. 3) is obtained from the pressure equation (Eq. 14) and its

*<sup>p</sup> dU T p dV <sup>T</sup>* 

34 4

*<sup>n</sup> U U n T dV*

<sup>1</sup> ( ) *<sup>V</sup>*

*V n Vn Vn T*

 

 (48)

*i T*

*i i*

partial derivative with respect to temperature (Eqs. 28 and 30):

1

0

1 1

*U V*

0 0

*U V*

1 0 2 2 2 2

*V TTT*

*i T*

*v*

ln ln *T i*

*V V n R n R V v*

where *ni* is the amount of substance of component *i* in the fluid mixture. In addition, the partial volume of an ideal gas is related to the standard pressure *p*0 (0.1 MPa) according to

Finally, the entropy of fluid phases containing gas mixtures at any temperature and total

new expression for this term (Eq. 42)

4 = 0, and Eq. 45 for

0

where si

the ideal gas law (Eq. 43, compare with Eq. 26).

3 > 0.

0

the arithmetic average principle (Eq. 46).

$$\begin{array}{rcl} S\_1 & = & S\_0 \ & + \ \int\_{V\_0}^{V\_1} \left( \frac{\mathcal{O}p\_{\text{ideal}}}{\mathcal{O}T} + \frac{\partial \Delta p}{\mathcal{J}T} \right) dV \end{array} \tag{35}$$

The limits of integration are defined as a reference ideal gas at *S*0 and *V*0, and a real gas at *S*<sup>1</sup> and *V*1. This integration can be split into two parts, according to the ideal pressure and residual pressure definition (Eqs. 25, 26, and 27). The integral has different solutions dependent on the values of 3 and 4: Eq. 36 for 3 = 0 and 4 = 0, and Eqs. 37 and 38 for 3 > 0.

$$S\_1 = S\_0 + n\_T R \ln\left(\frac{V\_1}{V\_0}\right) + n\_T R \ln\left(\frac{V\_1 - n\_T \zeta\_1}{V\_0 - n\_T \zeta\_1} \cdot \frac{V\_0}{V\_1}\right) + \left(\frac{1}{V\_1} - \frac{1}{V\_0}\right) \cdot \frac{\mathcal{E}(\nu\_T^2 \zeta\_2)}{\mathcal{E}T} \tag{36}$$

$$\begin{split} S\_{1} &= \ S\_{0} + n\_{T}R\ln\left(\frac{V\_{1}}{V\_{0}}\right) + n\_{T}R\ln\left(\frac{V\_{1} - n\_{T}\zeta\_{1}}{V\_{0} - n\_{T}\zeta\_{1}} \cdot \frac{V\_{0}}{V\_{1}}\right) \\ &- \frac{1}{q} \cdot \frac{\mathcal{E}(n\_{T}^{-2}\zeta\_{2})}{\mathcal{E}T} \cdot \ln\left(\frac{2V\_{1} + n\_{T}(\zeta\_{3} + \zeta\_{4}) - q}{2V\_{1} + n\_{T}(\zeta\_{3} + \zeta\_{4}) + q}\right) + \frac{1}{q} \cdot \frac{\mathcal{E}(n\_{T}^{-2}\zeta\_{2})}{\mathcal{E}T} \cdot \ln\left(\frac{2V\_{0} + n\_{T}(\zeta\_{3} + \zeta\_{4}) - q}{2V\_{0} + n\_{T}(\zeta\_{3} + \zeta\_{4}) + q}\right) \end{split} \tag{37}$$

where

$$\left(q\right) \quad = \left(m\_T \sqrt{4\zeta\_4^{'}\,^2 + \left(\zeta\_3 + \zeta\_4\right)^2}\right) \tag{38}$$

The *RKeos* and *Seos* define *q* as *Tn b* , whereas in the *PReos q* is equal to 8 *Tn b* , according to the values for 3 and 4 listed in Table 1. Eqs. 36 and 37 can be simplified by assuming that the lower limit of the integration corresponds to a large number of *V*0. As a consequence, part of the natural logarithms in Eqs. 36 and 37 can be replaced by the unit value 1 or 0 (Eqs. 39, 40, and 41).

$$\lim\_{V\_0 \to \infty} \left( \frac{V\_0}{V\_0 - n\_T \zeta\_1} \right) \tag{39}$$

$$\lim\_{V\_0 \to \infty} \left(\frac{1}{V\_0}\right) = \quad 0 \tag{40}$$

$$\lim\_{N\_0 \to \infty} \left( \frac{2V\_0 + n\_T(\zeta\_3 + \zeta\_4) - q}{2V\_0 + n\_T(\zeta\_3 + \zeta\_4) + q} \right) \\ = 1 \tag{41}$$

The entropy change that is caused by a volume change of ideal gases corresponds to the second term on the right-hand side of Eqs. 36 and 37. This term can be used to express the behaviour of an ideal mixture of perfected gases. Each individual gas in a mixture expands from their partial volume (*v*i) to the total volume at a pressure of 0.1 MPa, which results in a new expression for this term (Eq. 42)

168 Thermodynamics – Fundamentals and Its Application in Science

The entropy (*S*) is obtained from the integration defined in Eq. 2 at constant temperature

0 0 , *<sup>T</sup>*

The limits of integration are defined as a reference ideal gas at *S*0 and *V*0, and a real gas at *S*<sup>1</sup> and *V*1. This integration can be split into two parts, according to the ideal pressure and residual pressure definition (Eqs. 25, 26, and 27). The integral has different solutions

*ideal*

*T T*

3 = 0 and

0 0 11 1 0

*T*

2 2 1 34 0 34

*n n Vn q Vn q q T Vn q q T Vn q*

1 1 ( ) 2() ( ) 2 () ln ln

4 34 4( ) *<sup>T</sup> q n* 

The *RKeos* and *Seos* define *q* as *Tn b* , whereas in the *PReos q* is equal to 8 *Tn b* , according to

the lower limit of the integration corresponds to a large number of *V*0. As a consequence, part of the natural logarithms in Eqs. 36 and 37 can be replaced by the unit value 1 or 0 (Eqs.

> 0 0 1 lim 1

> > <sup>1</sup> lim <sup>0</sup>

 

0 34 0 34 2 () lim <sup>1</sup> 2 () *T*

 

*Vn q Vn q* 

*V*

 

1 1 1 0 2

1 1 ( ) ln ln *T T*

*V Vn V V V T* 

1 34 0 34

4 listed in Table 1. Eqs. 36 and 37 can be simplified by assuming that

2() 2 ()

 

*T T*

2 2

 

 

(34)

(35)

4 = 0, and Eqs. 37 and 38 for

3 > 0.

(36)

(37)

2

> 

> 

(38)

(39)

(40)

(41)

 

*S V V n <sup>p</sup> dS dV T* 

1

*V*

0

*V <sup>p</sup> <sup>p</sup> S S dV*

4: Eq. 36 for

1 1 1 0

0 0 11 2 2

*V Vn V*

 

 

0

*<sup>V</sup> <sup>T</sup>*

0

*<sup>V</sup> <sup>T</sup>*

*V n*

<sup>0</sup> 0

*<sup>V</sup> V*

*V Vn <sup>V</sup> <sup>n</sup> S S nR nR*

*T*

*T T T T T*

1 1

*S V*

1 0

3 and 

ln ln

*T T*

*V Vn <sup>V</sup> S S nR nR*

*T T*

**3. Thermodynamic parameters** 

(Eqs. 34 and 35).

dependent on the values of

1 0

 

3 and 

1 0

the values for

39, 40, and 41).

where

$$m\_T R \ln\left(\frac{V\_1}{V\_0}\right)\_{ideal.mix} = \sum\_i \left[n\_i R \ln\left(\frac{V\_1}{v\_i}\right)\right] \tag{42}$$

where *ni* is the amount of substance of component *i* in the fluid mixture. In addition, the partial volume of an ideal gas is related to the standard pressure *p*0 (0.1 MPa) according to the ideal gas law (Eq. 43, compare with Eq. 26).

$$w\_i \quad = \frac{n\_i \mathbb{R} T}{p\_0} \tag{43}$$

Finally, the entropy of fluid phases containing gas mixtures at any temperature and total volume according to the two-constant cubic equation of state is given by Eq. 44 for 3 = 0 and 4 = 0, and Eq. 45 for 3 > 0.

$$S\_{\rm in} = S\_0 + \sum\_{i} \left[ n\_i R \ln \left( \frac{p\_0 V}{n\_i R T} \right) \right] + n\_T R \ln \left( \frac{V - n\_T \zeta\_1}{V} \right) + \frac{1}{V} \cdot \frac{\mathcal{E}(n\_T^2 \zeta\_2)}{\mathcal{E}T} \tag{44}$$

$$S\_{-}=S\_{0}+\sum\_{i}\left[n\_{i}R\ln\left(\frac{p\_{0}V}{n\_{i}RT}\right)\right]+n\_{T}R\ln\left(\frac{V-n\_{T}\zeta\_{1}}{V}\right)-\frac{1}{q}\cdot\frac{\mathcal{O}(n\_{T}^{2}\zeta\_{2})}{\mathcal{ol}T}\cdot\ln\left(\frac{2V+n\_{T}(\zeta\_{3}+\zeta\_{4})-q}{2V+n\_{T}(\zeta\_{3}+\zeta\_{4})+q}\right) \tag{45}$$

The subscripts "1" for the upper limit of integration is eliminated to present a pronounced equation. The standard state entropy (*S*0) of a mixture of ideal gases is defined according to the arithmetic average principle (Eq. 46).

$$\mathcal{S}\_0 \quad = \sum\_i \boldsymbol{n}\_i \cdot \boldsymbol{s}\_i^0 \tag{46}$$

where si 0 is the molar entropy of a pure component *i* in an ideal gas mixture at temperature T.

The internal energy (*U*, see Eq. 3) is obtained from the pressure equation (Eq. 14) and its partial derivative with respect to temperature (Eqs. 28 and 30):

$$\bigcup\_{II\_0}^{II\_1} dII \quad = \iint\_{V\_0} (T \cdot \frac{\partial p}{\partial T} - p)dV \tag{47}$$

$$\mathcal{U}\_{1} = \mathcal{U}\_{0} + \int\_{V\_{0}}^{V\_{1}} \left( \frac{1}{V^{2} + n\_{T}\zeta\_{3}V + n\_{T}\zeta\_{4}V - n\_{T}^{2}\zeta\_{4}^{2}} \cdot \left( n\_{T}^{-2}\zeta\_{2} - T \frac{\hat{\mathcal{C}}(n\_{T}^{-2}\zeta\_{2})}{\tilde{\sigma}T} \right) \right) dV \tag{48}$$

Similar to the integral in the entropy definition (see Eqs. 44 and 45), Eq. 48 has different solutions dependent on the values of 3 and 4: Eq. 49 for 3 = 0 and 4 = 0, and Eq. 50 for 3 > 0.

$$
\delta \mathcal{U}\_- = \mathcal{U}\_0 - \frac{1}{V} \cdot \left( n\_T^{-2} \mathcal{L}\_2 - T \frac{\mathcal{C}(n\_T^{-2} \mathcal{L}\_2)}{\mathcal{C}T} \right) \tag{49}
$$

Thermodynamic Properties and Applications of Modified van-der-Waals Equations of State 171

<sup>2</sup> ln ln *TT T*

0 1

*i i T*

3 4 34 4

*T TTT*

*n RT V Vn V* 

(58)

*i i T*

ln ln

i) of a component in either vapour or liquid phase gas mixtures (compare with

00 0 1

*U S p V V n T RT RT RT n n n RT V*

2

ln ln

3 4

( ) ln ln

*i*

 

 

4 4 3

 

 

> 

3 = b and

*i T*

*q Vn q V n Vn Vn*

The Helmholtz energy equation (Eqs. 55, 56, and 57) is used for the definition of chemical

1 2

 

> 

00 0 1 1

*ii i T i*

*U S pV V n n RT n T RT RT RT n n n RT V Vn n*

2( )

 

> 

 

> 

> >

 

 

*p V V n n RTV G U TS RT n n RT*

*i T*

2( ) ln 2( )

 

 

*p V V n n RTV n G U TS RT n n RT*

2 2 2 2 3 4

*n Vn q n V*

*T T T*

4 = 0, and Eq. 62 for

( ) 1

*TT T Ti i*

*n RT n n Vn n V n*

2 2 3 4

*n n q Vn q n q n Vn q q*

<sup>1</sup> 2( ) ln

 

> 

 

*T i ii*

4 3 4 <sup>1</sup> 4 () *T T <sup>T</sup>*

*nq n n n*

4 = 0 [8, 9] is illustrated in Eq. 64, and

*i i i i q n n n*

The definitions of the partial derivative of *q* in respect to amount of substance (Eq. 63)

 

 

 

*T T*

*n n*

 

*T i i*

2 4 3

2 4 3

*n n n q q Vn q n n n*

*n n n q q Vn q n n n*

*ii i*

0 0

potential (

*i*

where

according to

Eq. 8), Eq. 61 for

equations of state.

0 0

*i*

2

2

3 = b and

 3 = 0 and

2 2

 

  1

2

 

*T T T i iT T T T*

 

*T T T*

1 2( )

1 2( )

3 4

3 4

 

  *A*0 00 *U TS* (57)

2 2 2

 

*G U TS n RT* 0 00 *<sup>T</sup>* (60)

0 1 2

*n RT V Vn*

2

1

(61)

(62)

(59)

1

 

*T T*

3 > 0, calculated with two-constant cubic

*T*

*T TT*

1

 

> 

(63)

4 = b [10] in Eq. 65.

$$\mathcal{U}\_{-}=\mathcal{U}\_{0}+\frac{1}{q}\cdot\left(n\_{T}^{-2}\zeta\_{2}-T\frac{\mathcal{O}(n\_{T}^{-2}\zeta\_{2})}{\mathcal{O}T}\right)\cdot\ln\left(\frac{2V+n\_{T}(\zeta\_{3}+\zeta\_{4})-q}{2V+n\_{T}(\zeta\_{3}+\zeta\_{4})+q}\right)\tag{50}$$

The definition of *q* is given in Eq. 38. The standard state internal energy (*U*0) of a mixture of ideal gases is defined according to the arithmetic average principle (Eq. 51).

$$\mathcal{U}\_0 \quad = \sum\_i \mathbf{n}\_i \cdot \mathbf{u}\_i^0 \tag{51}$$

where *u*<sup>i</sup> 0 is the molar internal energy of a pure component *i* in an ideal gas mixture at temperature T.

Enthalpy (Eq. 52 for 3 = 0 and 4 = 0, and Eq. 53 for 3 > 0), Helmholtz energy (Eq. 55 for 3 = 0 and 4 = 0, and Eq. 56 for 3 > 0), and Gibbs energy (Eq. 58 for 3 = 0 and 4 = 0, and Eq. 59 for 3 > 0) can be obtained from the definitions of pressure, entropy and internal energy according to standard thermodynamic relations, as illustrated in Eq. 4, 5, and 7. Standard state enthalpy (*H*0), standard state Helmholtz energy (*A*0), and standard state Gibbs energy (*G*0) of an ideal gas mixture at 0.1 MPa and temperature T are defined in Eqs. 54, 57, and 60, respectively.

$$\left| H \right| = \left| U\_0 \right| + \frac{n\_T RTV}{V - n\_T \zeta\_1} - \frac{1}{V} \cdot \left( 2n\_T \, ^2 \zeta\_2 - T \frac{\partial (n\_T \, ^2 \zeta\_2)}{\partial T} \right) \tag{52}$$

$$\begin{split} H &= \; \mathcal{U}\_0 + \frac{n\_T RTV}{V - n\_T \mathcal{\zeta}\_1} - \frac{n\_T \, ^2 \mathcal{\zeta}\_2 V}{V^2 + n\_T \mathcal{\zeta}\_3 V + n\_T \mathcal{\zeta}\_4 V - n\_T \, ^2 \mathcal{\zeta}\_4 ^2} \\ &+ \frac{1}{q} \cdot \left( n\_T \, ^2 \mathcal{\zeta}\_2 - T \, \frac{\mathcal{\mathcal{E}}(n\_T \, ^2 \mathcal{\zeta}\_2)}{\mathcal{\mathcal{E}}T} \right) \cdot \ln \left( \frac{2V + n\_T (\mathcal{\zeta}\_3 + \mathcal{\zeta}\_4) - q}{2V + n\_T (\mathcal{\zeta}\_3 + \mathcal{\zeta}\_4) + q} \right) \end{split} \tag{53}$$

$$H\_0 \quad = \ \mathcal{U}\_0 \, + \ \ n\_T RT \,\tag{54}$$

$$A\_{\perp} = \left. \mathcal{U}\_{0} - TS\_{0} - \sum\_{i} \left[ n\_{i}RT\ln\left(\frac{p\_{0}V}{n\_{i}RT}\right) \right] - \left. n\_{T}RT\ln\left(\frac{V - n\_{T}\zeta\_{1}}{V}\right) - \frac{n\_{T}^{2}\zeta\_{2}}{V} \right. \tag{55}$$

$$\begin{split} A &= \begin{aligned} \mathcal{U}\_0 & - & \mathcal{TS}\_0 & - \sum\_i \Bigg[ n\_i RT \ln \Bigl( \frac{p\_0 V}{n\_i RT} \Bigg) \Bigg] - n\_T RT \ln \Bigl( \frac{V - n\_T \mathcal{L}\_1}{V} \Bigg) \\ &+ \frac{n\_T^{-2} \mathcal{L}\_2}{q} \cdot \ln \Bigl( \frac{2V + n\_T (\mathcal{L}\_3 + \mathcal{L}\_4) - q}{2V + n\_T (\mathcal{L}\_3 + \mathcal{L}\_4) + q} \Bigg) \end{aligned} \tag{56}$$

Thermodynamic Properties and Applications of Modified van-der-Waals Equations of State 171

$$A\_0 \quad = \ \mathcal{U}\_0 \ - \ \mathcal{TS}\_0 \tag{57}$$

$$\begin{array}{rcl} \text{G} &=& \text{U}\_{0} - \text{TS}\_{0} - \text{RT} \sum\_{i} \left[ n\_{i} \ln \left( \frac{p\_{0}V}{n\_{i}\text{RT}} \right) \right] - n\_{T}\text{RT} \ln \left( \frac{V - n\_{T}\zeta\_{1}}{V} \right) + \frac{n\_{T}\text{RT}V}{V - n\_{T}\zeta\_{1}} - \frac{2n\_{T}^{2}\zeta\_{2}}{V} \end{array} \tag{58}$$

$$\begin{aligned} G &= \begin{aligned} \boldsymbol{U}\_{0} & \cdots & \boldsymbol{T} \mathbf{S}\_{0} & -\boldsymbol{R} \boldsymbol{T} \sum\_{i} \Bigg[ n\_{i} \ln \Bigl( \frac{p\_{0} \boldsymbol{V}}{n\_{i} \boldsymbol{R} \boldsymbol{T}} \Bigg) \Bigg] - n\_{\Gamma} \boldsymbol{R} \boldsymbol{T} \ln \Bigl( \frac{\boldsymbol{V} - n\_{\Gamma} \boldsymbol{\zeta}\_{1}}{\boldsymbol{V}} \Bigg) & + \frac{n\_{\Gamma} \boldsymbol{R} \boldsymbol{T} \boldsymbol{V}}{\boldsymbol{V} - n\_{\Gamma} \boldsymbol{\zeta}\_{1}} \\ & + \frac{n\_{\Gamma} \prescript{2}{}{\boldsymbol{\zeta}\_{2}}}{\boldsymbol{q}} \cdot \ln \Bigl( \frac{2 \boldsymbol{V} + n\_{\Gamma} (\boldsymbol{\zeta}\_{3} + \boldsymbol{\zeta}\_{4}) - \boldsymbol{q}}{2 \boldsymbol{V} + n\_{\Gamma} (\boldsymbol{\zeta}\_{3} + \boldsymbol{\zeta}\_{4}) + \boldsymbol{q}} \Bigg) - \frac{n\_{\Gamma} \prescript{2}{}{\boldsymbol{\zeta}\_{2}} \boldsymbol{V}}{\boldsymbol{V}^{2} + n\_{\Gamma} \boldsymbol{\zeta}\_{3} \boldsymbol{V} + n\_{\Gamma} \boldsymbol{\zeta}\_{4} \boldsymbol{V} - n\_{\Gamma}^{2} \boldsymbol{\zeta}\_{4}^{2}} \end{aligned} \tag{59}$$

*G U TS n RT* 0 00 *<sup>T</sup>* (60)

The Helmholtz energy equation (Eqs. 55, 56, and 57) is used for the definition of chemical potential (i) of a component in either vapour or liquid phase gas mixtures (compare with Eq. 8), Eq. 61 for 3 = 0 and 4 = 0, and Eq. 62 for 3 > 0, calculated with two-constant cubic equations of state.

$$\begin{split} \mu\_{i} &= \frac{\partial \mathcal{U}\_{0}}{\partial \boldsymbol{n}\_{i}} - T \frac{\partial \mathbb{S}\_{0}}{\partial \boldsymbol{n}\_{i}} - RT \ln \left( \frac{p\_{0}V}{n\_{i}RT} \right) + RT - RT \ln \left( \frac{V - n\_{T}\zeta\_{1}}{V} \right) \\ &+ \frac{n\_{T}RT}{V - n\_{T}\zeta\_{1}} \cdot \frac{\partial (\boldsymbol{n}\_{T}\zeta\_{1})}{\partial \boldsymbol{n}\_{i}} - \frac{1}{V} \cdot \frac{\partial n\_{T}^{2}\zeta\_{2}}{\partial \boldsymbol{n}\_{i}} \end{split} \tag{61}$$

$$\begin{split} \mu\_{i} &= \frac{\partial \mathcal{U}\_{0}}{\partial n\_{i}} - T \frac{\partial \mathcal{S}\_{0}}{\partial n\_{i}} - RT \ln \left( \frac{p\_{0}V}{n\_{i}RT} \right) + RT - RT \ln \left( \frac{V - n\_{T}\zeta\_{1}}{V} \right) + \frac{n\_{T}RT}{V - n\_{T}\zeta\_{1}} \cdot \frac{\partial (n\_{T}\zeta\_{1})}{\partial n\_{i}} \\ &+ \left( \frac{\partial n\_{T}^{T}\zeta\_{2}}{\partial n\_{i}} \cdot \frac{1}{q} - \frac{n\_{T}^{T}\zeta\_{2}}{q^{2}} \cdot \frac{\partial q}{\partial n\_{i}} \right) \cdot \ln \left( \frac{2V + n\_{T}(\zeta\_{3} + \zeta\_{4}) - q}{2V + n\_{T}(\zeta\_{3} + \zeta\_{4}) + q} \right) \\ &+ \frac{n\_{T}^{2}\zeta\_{2}}{q} \cdot \frac{1}{2V + n\_{T}(\zeta\_{3} + \zeta\_{4}) - q} \cdot \left( \frac{\partial n\_{T}\zeta\_{3}}{\partial n\_{i}} + \frac{\partial n\_{T}\zeta\_{4}}{\partial n\_{i}} - \frac{\partial q}{\partial n\_{i}} \right) \\ &- \frac{n\_{T}^{2}\zeta\_{2}}{q} \cdot \frac{1}{2V + n\_{T}(\zeta\_{3} + \zeta\_{4}) + q} \cdot \left( \frac{\partial n\_{T}\zeta\_{3}}{\partial n\_{i}} + \frac{\partial n\_{T}\zeta\_{4}}{\partial n\_{i}} + \frac{\partial q}{\partial n\_{i}} \right) \end{split} \tag{62}$$

where

170 Thermodynamics – Fundamentals and Its Application in Science

solutions dependent on the values of

where *u*<sup>i</sup>

0 and 

for 

temperature T.

respectively.

Enthalpy (Eq. 52 for

4 = 0, and Eq. 56 for

3 = 0 and

Similar to the integral in the entropy definition (see Eqs. 44 and 45), Eq. 48 has different

*T <sup>n</sup> UU n T*

2

*<sup>n</sup> Vn q UU n T*

The definition of *q* is given in Eq. 38. The standard state internal energy (*U*0) of a mixture of

0 *i i i*

3 > 0), and Gibbs energy (Eq. 58 for

3 > 0) can be obtained from the definitions of pressure, entropy and internal energy according to standard thermodynamic relations, as illustrated in Eq. 4, 5, and 7. Standard state enthalpy (*H*0), standard state Helmholtz energy (*A*0), and standard state Gibbs energy (*G*0) of an ideal gas mixture at 0.1 MPa and temperature T are defined in Eqs. 54, 57, and 60,

0 2

 

4 = 0, and Eq. 53 for

0 2 1

2

*p V Vn n A U TS n RT n RT*

*i i*

 

 

*p V V n A U TS n RT n RT*

*T T*

*T n RTV <sup>n</sup> H U n T*

*n RTV n V H U*

 

*i i*

2 3 4

*n Vn q q Vn q*

*T T*

2( ) ln 2( )

*T*

2

*T*

0 0 2

 4: Eq. 49 for

*V T*

<sup>1</sup> ( ) 2( ) ln

 2 2

*T T*

2 2 3 4

0

0 is the molar internal energy of a pure component *i* in an ideal gas mixture at

<sup>1</sup> ( ) <sup>2</sup> *T T T*

> 2 2

1 34 4

*Vn V T*

0 2 2 2

*V n V n Vn Vn*

<sup>1</sup> ( ) 2( ) ln

0 0 ln ln *T T i T*

3 4

2 2 3 4

*<sup>n</sup> Vn q n T q T Vn q*

*i T*

ln ln

*T TTT T T*

*q T Vn q*

 

1 ( ) *<sup>T</sup>*

3 = 0 and

2

3 4

3 > 0), Helmholtz energy (Eq. 55 for

3 = 0 and

2( )

 

 

*U nu* (51)

2

3 4

 

*T*

2 2

2( )

 

 

*H U n RT* 0 0 *<sup>T</sup>* (54)

0 1 2

0 1

*n RT V V*

*n RT V*

(55)

*T*

 

> 

*T*

4 = 0, and Eq. 50 for

(49)

3 > 0.

(50)

3 =

4 = 0, and Eq. 59

(52)

(53)

(56)

2

3 and 

0 2

*T*

ideal gases is defined according to the arithmetic average principle (Eq. 51).

$$\frac{\partial \hat{q}\_{1}}{\partial n\_{i}} = -\frac{1}{q} \cdot \left[ 4n\_{T}\zeta\_{4}\frac{\partial n\_{T}\zeta\_{4}}{\partial n\_{i}} + \left. n\_{T}(\zeta\_{3} + \zeta\_{4}) \cdot \left( \frac{\partial n\_{T}\zeta\_{3}}{\partial n\_{i}} + \frac{\partial n\_{T}\zeta\_{4}}{\partial n\_{i}} \right) \right| \right] \tag{63}$$

The definitions of the partial derivative of *q* in respect to amount of substance (Eq. 63) according to 3 = b and 4 = 0 [8, 9] is illustrated in Eq. 64, and 3 = b and 4 = b [10] in Eq. 65.

$$\frac{\partial \mathfrak{q}}{\partial \mathfrak{n}\_i} = \frac{\partial \mathfrak{l}(\mathfrak{n}\_T \mathfrak{b})}{\partial \mathfrak{n}\_i} \tag{64}$$

Thermodynamic Properties and Applications of Modified van-der-Waals Equations of State 173

 

0

(68)

(69)

(70)

(71)

(72)

(73)

(74)

1 2 1 11 21 2 12 22

*VV n V n V Vn n n n n*

*AAA AAA*

*Vn n n n n*

This matrix is square and contains a specific number of columns that is defined by the number of differentiation variables, i.e. volume and number of components in the fluid mixture minus 1. The individual components of this matrix are defined according to Eqs. 69, 70, 71, 72, 73, and 74. The exact definition of these components according to two-constant cubic equations of state can be obtained from the web site http://fluids.unileoben.ac.at (see

> 2 2

*V* 

> 2 2 1 , ,

*n* 

> 2 2 2 , ,

*n* 

1 1 2

1 , *n V V n n*

2 2 1

 

2 , *n V V n n*

1 2 2 1

 

1 2 , *n n n n V*

The determinant in Eq. 68 is calculated with the Laplacian expansion that contains "*minors*" and "*cofactors*", e.g. see [13]. The mathematical computation time increases exponential with increasing number of components. Therefore, the *LU* decomposition [14] can be applied in

The spinodal curve, binodal curve and critical point of a binary CO2-CH4 mixture with *x*(CO2) = 0.9 are illustrated in Figure 1, which are calculated with the *PReos* [10]. The spinodal has a small loop near the critical point, and may reach negative pressures at lower temperatures. The binodal remains within the positive pressure part at all temperatures. The binodal is obtained from equality of fugacity (Eq. 66 and 67) of each component in both

*V V*

1 1

2 2

*n n*

*n n*

*<sup>A</sup> <sup>A</sup>*

*<sup>A</sup> <sup>A</sup>*

*<sup>A</sup> <sup>A</sup>*

2

2

*<sup>A</sup> A A n V* 

2

*<sup>A</sup> A A n n* 

 

 

 

computer programming to reduce this time.

*<sup>A</sup> A A n V* 

 

*AAA*

1 2

*n n*

2

1

*n V*

*n V*

, ,

*spin*

*D*

also [6]).

$$\frac{\partial \overline{\boldsymbol{\sigma}}}{\partial \mathbf{n}\_i} = -\sqrt{8} \cdot \frac{\partial (\boldsymbol{n}\_T \boldsymbol{b})}{\partial \mathbf{n}\_i} \tag{65}$$

The fugacity coefficient (i) is defined according to Eqs. 9 and 10 from the difference between the chemical potential of a real gas mixture and an ideal gas mixture at standard conditions (0.1 MPa), see Eq. 66 for 3 = 0 and 4 = 0, and Eq. 67 for 3 > 0. Fugacity coefficient defined in Eq. 66 is applied to *Weos* and Eq. 67 is applied to *RKeos*, *Seos*, and *PReos.*

$$RT\ln\left(\rho\_{i}\right) = -RT\ln\left(\frac{pV}{n\_{T}RT}\right) - RT\ln\left(\frac{V - n\_{T}\zeta\_{1}}{V}\right) + \frac{n\_{T}RT}{V - n\_{T}\zeta\_{1}} \cdot \frac{\partial(n\_{T}\zeta\_{1})}{\partial n\_{i}} - \frac{1}{V} \cdot \frac{\partial n\_{T}^{2}\zeta\_{2}}{\partial n\_{i}}\tag{66}$$

$$\begin{split} RT\ln\left(\rho\_{i}\right) &= \ -RT\ln\left(\frac{pV}{n\_{\mathrm{T}}RT}\right) - RT\ln\left(\frac{V - n\_{\mathrm{T}}\zeta\_{1}}{V}\right) + \frac{n\_{\mathrm{T}}RT}{V - n\_{\mathrm{T}}\zeta\_{1}} \cdot \frac{\mathcal{E}(n\_{\mathrm{T}}\zeta\_{1})}{\mathcal{D}n\_{i}} \\ &+ \left(\frac{\partial n\_{\mathrm{T}}\zeta\_{2}}{\partial n\_{i}}\cdot\frac{1}{q} - \frac{n\_{\mathrm{T}}\,^{2}\zeta\_{2}}{q^{2}} \cdot \frac{\mathcal{E}q}{\partial n\_{i}}\right) \cdot \ln\left(\frac{2V + n\_{\mathrm{T}}(\zeta\_{3} + \zeta\_{4}) - q}{2V + n\_{\mathrm{T}}(\zeta\_{3} + \zeta\_{4}) + q}\right) \\ &+ \frac{n\_{\mathrm{T}}\,^{2}\zeta\_{2}}{q} \cdot \frac{1}{2V + n\_{\mathrm{T}}(\zeta\_{3} + \zeta\_{4}) - q} \cdot \left(\frac{\partial n\_{\mathrm{T}}\zeta\_{3}}{\partial n\_{i}} + \frac{\partial n\_{\mathrm{T}}\zeta\_{4}}{\partial n\_{i}} - \frac{\partial q}{\partial n\_{i}}\right) \\ &- \frac{n\_{\mathrm{T}}\,^{2}\zeta\_{2}}{q} \cdot \frac{1}{2V + n\_{\mathrm{T}}(\zeta\_{3} + \zeta\_{4}) + q} \cdot \left(\frac{\partial n\_{\mathrm{T}}\zeta\_{3}}{\partial n\_{i}} + \frac{\partial n\_{\mathrm{T}}\zeta\_{4}}{\partial n\_{i}} + \frac{\partial q}{\partial n\_{i}}\right) \end{split} \tag{67}$$

#### **4. Spinodal**

The stability limit of a fluid mixture can be calculated with two-constant cubic equations of state, e.g. see [6]. This limit is defined by the spinodal line, i.e. the locus of points on the surface of the Helmholtz energy or Gibbs energy functions that are inflection points, e.g. see [12] and references therein. The stability limit occurs at conditions where phase separation into a liquid and vapour phase should take place, which is defined by the binodal. Metastability is directly related to spinodal conditions, for example, nucleation of a vapour bubble in a cooling liquid phase within small constant volume cavities, such as fluid inclusions in minerals (< 100 µm diameter) occurs at conditions well below homogenization conditions of these phases in a heating experiment. The maximum temperature difference of nucleation and homogenization is defined by the spinodal. In multi-component fluid systems, the partial derivatives of the Helmholtz energy with respect to volume and amount of substance of each component can be arranged in a matrix that has a determinant (*Dspin*) equal to zero (Eq. 68) at spinodal conditions.

$$D\_{\text{spin}} = \begin{vmatrix} A\_{VV} & A\_{n\_1V} & A\_{n\_2V} & \cdots \\ A\_{Vn\_1} & A\_{n\_1n\_1} & A\_{n\_2n\_1} & \cdots \\ A\_{Vn\_2} & A\_{n\_1n\_2} & A\_{n\_2n\_2} & \cdots \\ \vdots & \vdots & \vdots & \ddots \end{vmatrix}\_{\text{-}1} = \begin{array}{c} 0 \\ \end{array} \tag{68}$$

This matrix is square and contains a specific number of columns that is defined by the number of differentiation variables, i.e. volume and number of components in the fluid mixture minus 1. The individual components of this matrix are defined according to Eqs. 69, 70, 71, 72, 73, and 74. The exact definition of these components according to two-constant cubic equations of state can be obtained from the web site http://fluids.unileoben.ac.at (see also [6]).

172 Thermodynamics – Fundamentals and Its Application in Science

2

2

*T*

*n*

The fugacity coefficient (

**4. Spinodal** 

68) at spinodal conditions.

*i*

conditions (0.1 MPa), see Eq. 66 for

*i*

 ( ) *<sup>T</sup>*

( ) <sup>8</sup> *<sup>T</sup>*

 

(64)

(65)

1 12

*T TT*

1

 

 

> 

3 4

1

2( )

 

 

 

> 

*n n q*

*T T*

 

 

3 > 0. Fugacity coefficient

 

   2

(67)

i) is defined according to Eqs. 9 and 10 from the difference

4 = 0, and Eq. 67 for

*T Ti i*

(66)

*T T i*

*n RT V Vn n*

*T i ii*

*T i ii*

 

 

 

 

 

*n RT V Vn n V n*

2 2 3 4

*n n q Vn q n q n Vn q q*

<sup>1</sup> 2( ) ln

2 4 3

*n n n q q Vn q n n n*

*q Vn q n n n*

*i i q n b n n*

*i i q n b n n*

between the chemical potential of a real gas mixture and an ideal gas mixture at standard

1 1

( ) ln ln ln

 

> *T T T i iT T T T*

( ) <sup>1</sup> ln ln ln *T TT T*

2

 

*pV V n n RT n RT RT RT*

1 2( )

1 2( )

3 4

 2 4 <sup>3</sup> 3 4

The stability limit of a fluid mixture can be calculated with two-constant cubic equations of state, e.g. see [6]. This limit is defined by the spinodal line, i.e. the locus of points on the surface of the Helmholtz energy or Gibbs energy functions that are inflection points, e.g. see [12] and references therein. The stability limit occurs at conditions where phase separation into a liquid and vapour phase should take place, which is defined by the binodal. Metastability is directly related to spinodal conditions, for example, nucleation of a vapour bubble in a cooling liquid phase within small constant volume cavities, such as fluid inclusions in minerals (< 100 µm diameter) occurs at conditions well below homogenization conditions of these phases in a heating experiment. The maximum temperature difference of nucleation and homogenization is defined by the spinodal. In multi-component fluid systems, the partial derivatives of the Helmholtz energy with respect to volume and amount of substance of each component can be arranged in a matrix that has a determinant (*Dspin*) equal to zero (Eq.

*pV V n n RT n <sup>n</sup> RT RT RT*

 

2 2

3 = 0 and

defined in Eq. 66 is applied to *Weos* and Eq. 67 is applied to *RKeos*, *Seos*, and *PReos.*

$$A\_{VV} = \left(\frac{\partial^2 A}{\partial V^2}\right)\_{n\_1, n\_2, \dots} \tag{69}$$

$$A\_{n\_1 n\_1} = \left(\frac{\hat{\sigma}^2 A}{\hat{\sigma} n\_1^2}\right)\_{n\_2, V, \dots} \tag{70}$$

$$A\_{n\_2 n\_2} = \left. \left( \frac{\partial^2 A}{\partial n\_2^{\prime}} \right)\_{n\_1, V\_{\prime}, \dots} \right. \tag{71}$$

$$A\_{\mathfrak{n}\_1 V} = \left(\frac{\partial^2 A}{\partial \mathfrak{n}\_1 \mathcal{O} V}\right)\_{\mathfrak{n}\_2, \dots} = \left. A\_{V \mathfrak{n}\_1} \right. \tag{72}$$

$$A\_{n\_2 V} = \left(\frac{\partial^2 A}{\partial n\_2 \partial V}\right)\_{n\_1, \dots} = \left. A\_{V n\_2} \right| \tag{73}$$

$$A\_{\boldsymbol{n}\_1 \boldsymbol{n}\_2} = \left. \left( \frac{\partial^2 A}{\partial \boldsymbol{n}\_1 \partial \boldsymbol{n}\_2} \right)\_{\boldsymbol{V}\_{\boldsymbol{\cdot}}, \dots} \right|\_{\boldsymbol{V}\_{\boldsymbol{\cdot}}, \boldsymbol{n}\_1} = \left. A\_{\boldsymbol{n}\_2 \boldsymbol{n}\_1} \right|\_{\boldsymbol{V}\_{\boldsymbol{\cdot}}, \dots} \tag{74}$$

The determinant in Eq. 68 is calculated with the Laplacian expansion that contains "*minors*" and "*cofactors*", e.g. see [13]. The mathematical computation time increases exponential with increasing number of components. Therefore, the *LU* decomposition [14] can be applied in computer programming to reduce this time.

The spinodal curve, binodal curve and critical point of a binary CO2-CH4 mixture with *x*(CO2) = 0.9 are illustrated in Figure 1, which are calculated with the *PReos* [10]. The spinodal has a small loop near the critical point, and may reach negative pressures at lower temperatures. The binodal remains within the positive pressure part at all temperatures. The binodal is obtained from equality of fugacity (Eq. 66 and 67) of each component in both liquid and vapour phase, and marks the boundary between a homogeneous fluid mixture and fluid immiscibility [6, 15].

Thermodynamic Properties and Applications of Modified van-der-Waals Equations of State 175

 

<sup>3</sup> (78)

<sup>3</sup> 3.847322

*<sup>b</sup> RKeos : V <sup>b</sup>* (81)

*<sup>m</sup> PReos : V Q b b* (82)

3 3 *Q* 48 48 (83)

2 1

1 1

where *Q* is defined according to Eq. 83, the superscript "*pc*" is the abbreviation for "*pseudo* 

*Equation of state f g b in Eqs. 80-82 b in Eqs. 94-96 difference van der Waals [7]* -3b2 -2b3 31.3727 42.8453 37 % *Redlich and Kwong [8]* -6b2 -6b3 24.4633 29.6971 21 % *Soave [9]* -6b2 -6b3 24.4633 29.6971 21 % *Peng and Robinson [10]* -6b2 -8b3 23.8191 26.6656 12 %

**Table 2.** Definitions of *f* and *g* according to Eq. 77 and 78, respectively. The values of *b* are calculated for the critical conditions of pure CO2: *V*m,C = 94.118 cm3·mol-1, *T*C = 304.128 K and *p*C = 7.3773 MPa [18]. The

The temperature at pseudo critical conditions is obtained from the combination of Eqs. 80-82

> 

2

 

2 2 <sup>8</sup> 0.29629630

2 4 <sup>3</sup> 0.17014442

*bR bR*

*bR bR*

2 2

*bR bR*

(84)

(85)

(86)

last column gives the percentage of difference between the values of *b* (Eqs. 80-82 and 94-96).

27

 <sup>2</sup> <sup>3</sup> 2 2 <sup>3</sup> 2 1 0.20267686 *pc RKeos : T*

4 2

*<sup>Q</sup> <sup>Q</sup>*

and the first partial derivative of pressure with respect to volume (Eq. 31).

*pc Weos : T*

*pc <sup>Q</sup> PReos : T*

 

<sup>3</sup> *pc Weos : V b <sup>m</sup>* (80)

 

(79)

<sup>2</sup> 3 2 2 2

1 1 4 34 34 4 1 *g* 2 2

*V x <sup>m</sup>* <sup>1</sup>

The values of *f* and *g* in terms of the *b* parameters for the individual two-constant cubic equations of state are given in Table 2. The molar volume at pseudo critical conditions is directly related to the *b* parameter in each equation of state: *Weos* Eq. 80; *RKeos* Eq. 81; *Seos*

 

also Eq. 81; and *PReos* Eq. 82.

*critical*".

 

 

> *pc m*

1 3.951373 *pc*

**Figure 1.** (**a**) Temperature-pressure diagram of a binary CO2-CH4 fluid mixture, with *x*(CO2) = 0.9. The shaded area illustrates *T-p* condition of immiscibility of a CO2-rich liquid phase and a CH4-rich vapour phase (the binodal). The red dashed line is the spinodal. All lines are calculated with the equation of state according to *PReos* [10]. The calculated critical point is indicated with *cPR*. *cDK* is the interpolated critical point from experimental data [16]. (**b**) enlargement of (**a**) indicated with the square in thin lines.

## **5. Pseudo critical point**

The pseudo critical point is defined according to the first and second partial derivatives of pressure with respect to volume (Eqs. 31 and 32). This point is defined in a *p-V* diagram where the inflection point and extremum coincide at a specific temperature, i.e. Eqs. 31 and 32 are equal to 0. The pseudo critical point is equal to the critical point for pure gas fluids, however, the critical point in mixtures cannot be obtained from Eqs. 31 and 32. The pseudo critical point estimation is used to define the two-constants (*a* and *b*) for pure gas fluids in cubic equations of state according to the following procedure. The molar volume of the pseudo critical point that is derived from Eqs 31 and 32 is presented in the form of a cubic equation (Eq. 75).

$$\mathbf{0} = \left| \mathbf{V}\_m^3 - \mathbf{3}\boldsymbol{\zeta}\_1 \cdot \mathbf{V}\_m \right|^2 + \left[ \mathbf{3}\boldsymbol{\zeta}\_4^2 - \mathbf{3}\boldsymbol{\zeta}\_1 \cdot \left( \boldsymbol{\zeta}\_3 + \boldsymbol{\zeta}\_4 \right) \right] \cdot \mathbf{V}\_m - \boldsymbol{\zeta}\_1 \cdot \left[ \boldsymbol{\zeta}\_4^2 + \left( \boldsymbol{\zeta}\_3 + \boldsymbol{\zeta}\_4 \right)^2 \right] + \boldsymbol{\zeta}\_4^{\prime \cdot 2} \cdot \left( \boldsymbol{\zeta}\_3 + \boldsymbol{\zeta}\_4 \right) \tag{75}$$

The solution of this cubic equation can be obtained from its reduced form, see page 9 in [15]:

$$\begin{array}{rcl} \mathbf{x}^3 + f \cdot \mathbf{x} + \mathbf{g} &=& \mathbf{0} \\\\ \end{array} \tag{76}$$

where

$$f\_{\perp} = \mathbf{3} \cdot \left[ \boldsymbol{\zeta}\_{4}^{\prime 2} - \boldsymbol{\zeta}\_{1}^{\prime} \cdot \left( \boldsymbol{\zeta}\_{1}^{\prime} + \boldsymbol{\zeta}\_{3}^{\prime} + \boldsymbol{\zeta}\_{4}^{\prime} \right) \right] \tag{77}$$

Thermodynamic Properties and Applications of Modified van-der-Waals Equations of State 175

$$\log \mathbf{s} = -2\boldsymbol{\zeta}\_1^{\prime \cdot 3} + \boldsymbol{\zeta}\_1^{\prime} \cdot \left[ 2\boldsymbol{\zeta}\_4^{\prime \cdot 2} - \left( \boldsymbol{\zeta}\_3^{\prime} + \boldsymbol{\zeta}\_4 \right)^2 \right] + \left( \boldsymbol{\zeta}\_3^{\prime} + \boldsymbol{\zeta}\_4 \right) \cdot \left[ \boldsymbol{\zeta}\_4^{\prime \cdot 2} - 3\boldsymbol{\zeta}\_1^{\prime \cdot 2} \right] \tag{78}$$

$$V\_m = \|\mathbf{x} + \boldsymbol{\zeta}\_1\|\tag{79}$$

The values of *f* and *g* in terms of the *b* parameters for the individual two-constant cubic equations of state are given in Table 2. The molar volume at pseudo critical conditions is directly related to the *b* parameter in each equation of state: *Weos* Eq. 80; *RKeos* Eq. 81; *Seos* also Eq. 81; and *PReos* Eq. 82.

174 Thermodynamics – Fundamentals and Its Application in Science

and fluid immiscibility [6, 15].

**5. Pseudo critical point** 

equation (Eq. 75).

where

   

liquid and vapour phase, and marks the boundary between a homogeneous fluid mixture

**Figure 1.** (**a**) Temperature-pressure diagram of a binary CO2-CH4 fluid mixture, with *x*(CO2) = 0.9. The shaded area illustrates *T-p* condition of immiscibility of a CO2-rich liquid phase and a CH4-rich vapour phase (the binodal). The red dashed line is the spinodal. All lines are calculated with the equation of state according to *PReos* [10]. The calculated critical point is indicated with *cPR*. *cDK* is the interpolated critical point from experimental data [16]. (**b**) enlargement of (**a**) indicated with the square in thin lines.

The pseudo critical point is defined according to the first and second partial derivatives of pressure with respect to volume (Eqs. 31 and 32). This point is defined in a *p-V* diagram where the inflection point and extremum coincide at a specific temperature, i.e. Eqs. 31 and 32 are equal to 0. The pseudo critical point is equal to the critical point for pure gas fluids, however, the critical point in mixtures cannot be obtained from Eqs. 31 and 32. The pseudo critical point estimation is used to define the two-constants (*a* and *b*) for pure gas fluids in cubic equations of state according to the following procedure. The molar volume of the pseudo critical point that is derived from Eqs 31 and 32 is presented in the form of a cubic

<sup>2</sup> 3 22 <sup>2</sup> <sup>2</sup>

 

<sup>2</sup>

 

<sup>3</sup> *x fx g* 0 (76)

(77)

(75)

   

1 4 13 4 14 3 4 4 3 4 0 3 33 *V V m m Vm*

The solution of this cubic equation can be obtained from its reduced form, see page 9 in [15]:

4 11 3 4 *<sup>f</sup>* <sup>3</sup>

 

$$\text{Weos}: \qquad V\_m^{\;\;\;\;pc} = \; \mathbf{3} \cdot \mathbf{b} \tag{80}$$

$$\text{RKeos}: \qquad V\_m^{\;pc} = \begin{array}{c c c} b \\ \sqrt[3]{2} - 1 \end{array} \approx \begin{array}{c c} \text{3.847322 } \cdot b \\ \end{array} \tag{81}$$

$$\text{PReos}: \quad V\_{\text{in}}{}^{\text{pc}} = \begin{bmatrix} 1 \ + \ Q \end{bmatrix} \cdot b \quad \approx \text{ 3.951373} \cdot b \tag{82}$$

where *Q* is defined according to Eq. 83, the superscript "*pc*" is the abbreviation for "*pseudo critical*".

$$\begin{array}{ccccccccc}\hline\text{Equation of state} & f & \text{g} & b \text{ in Eqs. 80-82} & b \text{ in Eqs. 94-96} & \text{difference} \\ \hline \text{van der Waals [7]} & -\text{3b}^2 & -\text{2b}^3 & \text{31.3727} & 42.8453 & \text{37.\%} \\ \text{Rellich and Knong [8]} & -\text{6b}^2 & -\text{6b}^3 & 24.4633 & \text{29.6971} & \text{21\%} \\ \text{Soave [9]} & -\text{6b}^2 & -\text{6b}^3 & 24.4633 & \text{29.6971} & \text{21\%} \\ \text{Peng and Rohinson [10]} & -\text{6b}^2 & -\text{8b}^3 & 23.8191 & \text{26.6656} & \text{12\%} \\ \hline \end{array}$$

 1 1 3 3 *Q* 48 48 (83)

**Table 2.** Definitions of *f* and *g* according to Eq. 77 and 78, respectively. The values of *b* are calculated for the critical conditions of pure CO2: *V*m,C = 94.118 cm3·mol-1, *T*C = 304.128 K and *p*C = 7.3773 MPa [18]. The last column gives the percentage of difference between the values of *b* (Eqs. 80-82 and 94-96).

The temperature at pseudo critical conditions is obtained from the combination of Eqs. 80-82 and the first partial derivative of pressure with respect to volume (Eq. 31).

$$\text{Weos}: \qquad T^{\text{pc}} = \frac{8}{27} \cdot \frac{\zeta\_2}{bR} \approx \quad 0.29629630 \cdot \frac{\zeta\_2}{bR} \tag{84}$$

$$R \text{Keros}: \qquad T^{pc} = \left(\sqrt[3]{2} - 1\right)^2 \cdot \left(\frac{3\zeta\_2}{bR}\right) \quad \approx \quad 0.20267686 \cdot \frac{\zeta\_2}{bR} \tag{85}$$

$$P\text{Reos}:\qquad T^{\text{pc}} = \frac{2Q+4}{\left(Q+4+\sqrt{Q}\right)^2} \cdot \left(\frac{3\zeta\_2}{bR}\right) \approx \quad 0.17014442\cdot \frac{\zeta\_2}{bR} \tag{86}$$

where *Q* is defined according to Eq. 83. The order of equations (84, 85, 86) is according to the order of equations of state in Eq. 80, 81,and 82. The parameter 2 is used in Eqs. 84, 85 and, 86 instead of the constant *a* (see Table 1). Eq. 87 illustrates the transformation of Eq. 85 for the *RKeos* [8] by substitution of 2 according to its value given in Table 1.

$$T^{pc} = \begin{pmatrix} \sqrt[3]{2} - & 1 \end{pmatrix}^{\not\xi} \cdot \begin{pmatrix} \frac{3a}{bR} \end{pmatrix}^{\not\xi} \tag{87}$$

Thermodynamic Properties and Applications of Modified van-der-Waals Equations of State 177

0.08664035

(95)

0.07779607

(96)

*C C C C*

*C C C C*

*p p*

*Q Q p p*

<sup>3</sup> 2 1

*RT RT RKeos : b*

3

2 2

equation in Table 2 (11% for pure CO2).

(*D*crit) of the matrix illustrated in Eq. 97, see also [6].

*crit*

*D*

**6. Critical point and curve** 

determinant *D*spin from Eq. 68:

2 2

2

*<sup>Q</sup> RT RT PReos : b*

where *TC* and *pC* are the critical temperature and critical pressure, and *Q* is defined according to Eq. 83. The order of equations (91-93, and 94-96) is according to the order of equations of state in Eqs. 80-82. Comparison of the value of b calculated with experimental critical volume (Eqs. 80, 81 and 82) and critical temperature and pressure (Eqs. 94, 95, and 96) is illustrated in Table 2. The difference indicates the ability of a specific equation of state to reproduce fluid properties of pure gases. A large difference indicates that the geometry or morphology of the selected equation of state in the *p-V-T-x* parameter space is not exactly reproducing fluid properties of pure gases. The empirical modifications of the van-der-Waals equation of state according to Peng and Robinson [10] result in the most accurate

The critical point is the highest temperature and pressure in a pure gas system where boiling may occur, i.e. where a distinction can be made between a liquid and vapour phase at constant temperature and pressure. At temperatures and pressures higher than the critical point the pure fluid is in a homogeneous supercritical state. The critical point of pure gases and multi-component fluid mixtures can be calculated exactly with the Helmholtz energy equation (Eqs. 55-57) that is obtained from two-constant cubic equations of state, e.g. see [17, 18], and it marks that part of the surface described with a Helmholtz energy function where two inflection points of the spinodal coincide. Therefore, the conditions of the spinodal are also applied to the critical point. In addition, the critical curve is defined by the determinant

> 1 2 1 11 21

*VV n V n V Vn n n n n*

*AAA AAA*

*Vn n*

The number of rows in Eq.97 is defined by the differentiation variables volume and number of components minus 2. The last row is reserved for the partial derivatives of the

*DDD*

*V*

*D*

1 2

*spin*

*V*

*D*

0

(98)

(97)

 

Any temperature dependency of the *a* constant has an effect on the definition of the pseudo critical temperature. The pressure at pseudo critical condition (Eqs. 88-90) is obtained from a combination of the pressure equation (Eq.14), pseudo critical temperature (Eqs. 84-87) and pseudo critical molar volume (Eqs. 80-82).

$$\text{Weos}: \qquad p^{\text{pc}} = \frac{1}{27} \cdot \frac{\zeta\_2}{b^2} \quad \approx \quad 0.03703704 \cdot \frac{\zeta\_2}{b^2} \tag{88}$$

$$\text{RKeos}: \qquad p^{\text{pc}} = \left(\sqrt[3]{2} - 1\right)^3 \cdot \frac{\zeta\_2}{b^2} \quad \approx \quad 0.01755999 \cdot \frac{\zeta\_2}{b^2} \tag{89}$$

$$PR\cos:\quad p^{\rm pc} = \frac{Q^2 - 2}{\left(Q^2 + 4Q + 2\right)^2} \cdot \frac{\zeta\_2}{b^2} \approx \quad 0.01227198 \cdot \frac{\zeta\_2}{b^2} \tag{90}$$

where *Q* is defined according to Eq. 83. The order of equations (88, 89, and 90) is according to the order of equations of state in Eqs. 80, 81, and 82. These equations define the relation between the *a* and *b* constant in two-constant cubic equations of state and critical conditions, i.e. temperature, pressure, and molar volume of pure gas fluids. Therefore, knowledge of these conditions from experimental data can be used to determine the values of *a* (or 2) and *b*, which can be defined as a function of only temperature and pressure (Eqs. 91-93, and 94- 96, respectively).

$$\text{Weos}: \qquad \zeta\_2 \quad = \frac{27}{64} \cdot \frac{R^2 T\_\odot^2}{p\_\odot} \quad = \ 0.421875 \cdot \frac{R^2 T\_\odot^2}{p\_\odot} \tag{91}$$

$$\text{RKcos}: \quad \zeta\_2 \quad = \frac{1}{9 \cdot \left(\sqrt[3]{2} - 1\right)} \cdot \frac{R^2 T\_\odot^{-2}}{p\_\odot} \approx \quad 0.42748024 \cdot \frac{R^2 T\_\odot^{-2}}{p\_\odot} \tag{92}$$

$$P\text{Reos}:\quad \zeta\_{2} = \frac{\left(Q^{2} + 4Q + 2\right)^{2} \cdot \left(Q^{2} - 2\right)}{4Q^{2} \cdot \left(Q + 2\right)^{2}} \cdot \frac{R^{2}T\_{\text{C}}^{-2}}{p\_{\text{C}}} \approx \ 0.45723553 \cdot \frac{R^{2}T\_{\text{C}}^{-2}}{p\_{\text{C}}}\tag{93}$$

$$\text{Weos}: \qquad b \quad = \ \frac{1}{8} \cdot \frac{RT\_{\text{\textdegree}}}{p\_{\text{\textdegree}}} \quad = \ 0.125 \cdot \frac{RT\_{\text{\textdegree}}}{p\_{\text{\textdegree}}} \tag{94}$$

Thermodynamic Properties and Applications of Modified van-der-Waals Equations of State 177

$$\text{RKeos}: \qquad b \quad = \frac{\left(\sqrt[3]{2} - 1\right)}{3} \cdot \frac{RT\_{\odot}}{p\_{\odot}} \quad \approx \quad 0.08664035 \cdot \frac{RT\_{\odot}}{p\_{\odot}} \tag{95}$$

$$PReos: \quad b \quad = \frac{\left(Q^2 - 2\right)}{2Q^2 \cdot \left(Q + 2\right)} \cdot \frac{RT\_{\odot}}{p\_{\odot}} \quad \approx \quad 0.07779607 \cdot \frac{RT\_{\odot}}{p\_{\odot}} \tag{96}$$

where *TC* and *pC* are the critical temperature and critical pressure, and *Q* is defined according to Eq. 83. The order of equations (91-93, and 94-96) is according to the order of equations of state in Eqs. 80-82. Comparison of the value of b calculated with experimental critical volume (Eqs. 80, 81 and 82) and critical temperature and pressure (Eqs. 94, 95, and 96) is illustrated in Table 2. The difference indicates the ability of a specific equation of state to reproduce fluid properties of pure gases. A large difference indicates that the geometry or morphology of the selected equation of state in the *p-V-T-x* parameter space is not exactly reproducing fluid properties of pure gases. The empirical modifications of the van-der-Waals equation of state according to Peng and Robinson [10] result in the most accurate equation in Table 2 (11% for pure CO2).

#### **6. Critical point and curve**

176 Thermodynamics – Fundamentals and Its Application in Science

the *RKeos* [8] by substitution of

96, respectively).

pseudo critical molar volume (Eqs. 80-82).

order of equations of state in Eq. 80, 81,and 82. The parameter

where *Q* is defined according to Eq. 83. The order of equations (84, 85, 86) is according to the

86 instead of the constant *a* (see Table 1). Eq. 87 illustrates the transformation of Eq. 85 for

<sup>3</sup> <sup>3</sup> <sup>3</sup> 2 1 *pc <sup>a</sup> <sup>T</sup>*

27 *pc Weos : p b b* 

these conditions from experimental data can be used to determine the values of *a* (or

64

9 21

4 2

8

*RT RT Weos : b*

42 2

2

2 3

<sup>2</sup> <sup>2</sup> <sup>2</sup>

*Weos :*

*RKeos :*

*PReos :*

2

2 2 2 1 0.01755999 *pc RKeos : p b b*

4 2 *pc <sup>Q</sup> PReos : p b b Q Q* 

where *Q* is defined according to Eq. 83. The order of equations (88, 89, and 90) is according to the order of equations of state in Eqs. 80, 81, and 82. These equations define the relation between the *a* and *b* constant in two-constant cubic equations of state and critical conditions, i.e. temperature, pressure, and molar volume of pure gas fluids. Therefore, knowledge of

*b*, which can be defined as a function of only temperature and pressure (Eqs. 91-93, and 94-

2 according to its value given in Table 1.

*bR*

2 2 2 2 <sup>1</sup> 0.03703704

<sup>3</sup> <sup>3</sup> 2 2

2 2 <sup>2</sup> <sup>2</sup> <sup>2</sup> 0.01227198

2 2 2 2

*p p*

<sup>2</sup> 2 2 2 2 2 2

*Q Q p p*

*C C C C*

*QQ Q R T R T*

<sup>1</sup> 0.125

<sup>1</sup> 0.42748024

*C C C C R T R T*

(91)

2 2 2 2

*p p*

*C C C C R T R T*

0.45723553

*C C C C*

*p p* (94)

<sup>27</sup> 0.421875

 (88)

(89)

2 2

 

(90)

2) and

(92)

(93)

<sup>2</sup> 4 3

Any temperature dependency of the *a* constant has an effect on the definition of the pseudo critical temperature. The pressure at pseudo critical condition (Eqs. 88-90) is obtained from a combination of the pressure equation (Eq.14), pseudo critical temperature (Eqs. 84-87) and

2 is used in Eqs. 84, 85 and,

(87)

The critical point is the highest temperature and pressure in a pure gas system where boiling may occur, i.e. where a distinction can be made between a liquid and vapour phase at constant temperature and pressure. At temperatures and pressures higher than the critical point the pure fluid is in a homogeneous supercritical state. The critical point of pure gases and multi-component fluid mixtures can be calculated exactly with the Helmholtz energy equation (Eqs. 55-57) that is obtained from two-constant cubic equations of state, e.g. see [17, 18], and it marks that part of the surface described with a Helmholtz energy function where two inflection points of the spinodal coincide. Therefore, the conditions of the spinodal are also applied to the critical point. In addition, the critical curve is defined by the determinant (*D*crit) of the matrix illustrated in Eq. 97, see also [6].

$$D\_{crit} = \begin{vmatrix} A\_{VV} & A\_{n\_1V} & A\_{n\_2V} & \cdots \\ A\_{Vn\_1} & A\_{n\_1n\_1} & A\_{n\_2n\_1} & \cdots \\ \vdots & \vdots & \vdots & \vdots \\ D\_V & D\_{n\_1} & D\_{n\_2} & \cdots \end{vmatrix}\_{n\_2} = \begin{array}{c} 0 \\ \end{array} \tag{97}$$

The number of rows in Eq.97 is defined by the differentiation variables volume and number of components minus 2. The last row is reserved for the partial derivatives of the determinant *D*spin from Eq. 68:

$$D\_V = \frac{\partial \mathcal{D}\_{\text{spin}}}{\partial V} \tag{98}$$

$$D\_{n\_1} = \begin{array}{c} \mathcal{O}D\_{\text{spin}}\\ \mathcal{O}n\_1 \end{array} \tag{99}$$

Thermodynamic Properties and Applications of Modified van-der-Waals Equations of State 179

*<sup>4</sup>* to fit experimental data. The original definition

(105)

(103)

(104)

is the acentric factor.

been used to calculate the determinant in Eq. 97. The determinants in Eqs. 68 and 97 are both used to calculate exactly the critical point of any fluid mixture and pure gases, based on

An example of a calculated critical curve, i.e. critical points for a variety of compositions in a binary fluid system, is illustrated in Figure 2. The prediction of critical temperatures of fluid mixtures corresponds to experimental data [16, 19], whereas calculated critical pressures are slightly overestimated at higher fraction of CH4. This example illustrates that the *PReos* [10] is a favourable modification that can be used to calculate sub-critical conditions of CO2-CH4

All modifications of the van-der-Waals two-constant cubic equation of state [7] have an empirical character. The main modifications are defined by Redlich and Kwong, Soave and Peng and Robinson (see Table 1), and all modification can by summarized by specific

93, and 94-96). This principle is adapted in most modifications of the van-der-Waals equation of state, e.g. *RKeos* [8]. Soave [9] and Peng and Robinson [10] adjusted the

2 *C*

1 1

*m*

0, 1, 2

The summation in Eq. 105 does not exceed *i* = 2 for Soave [9] and Peng and Robinson [10]. The definition of the acentric factor is arbitrary and chosen for convenience [5] and is a purely empirical modification. These two equations of state have different definitions of pseudo critical conditions (see Eqs. 91-93 and 94-96), therefore, the values of *m*i must be

*Soave [9] Peng and Robinson [10]* 

*i m m*

*a*

where *a*c is defined by the pseudo critical conditions (Eqs. 91-93), and

*m0* 0.480 0.37464 *m1* 1.574 1.54266 *m2* -0.176 -0.26992

*<sup>2</sup>* with a temperature dependent correction parameter (Eqs. 103-105).

 

2

*C T*

*i i*

*T*

*<sup>2</sup> (a)* for pure gases is obtained from the pseudo critical conditions (Eqs. 91-

two-constant cubic equations of state that define the Helmholtz energy function.

**7. Mixing rules and definitions of 1 and <sup>2</sup>**

*1, 2, 3, and* 

fluid mixtures.

[7] of *1 (b)* and

definition of

adaptations of the values of

different for each equation (Table 3).

**Table 3.** Values of the constant *mi* in Eq. 105.

$$D\_{n\_2} = \begin{array}{c} \mathcal{O}D\_{\text{spin}}\\ \mathcal{O}n\_2 \end{array} \tag{100}$$

The derivatives of the spinodal determinant (Eqs. 98-100) are calculated from the sum of the element-by-element products of the matrix of "cofactors" (or adjoint matrix) of the spinodal (Eq. 101) and the matrix of the third derivatives of the Helmholtz energy function (Eq. 102).

$$
\begin{vmatrix}
\mathbb{C}\_{V,V} & \mathbb{C}\_{n\_1 V} & \mathbb{C}\_{n\_2 V} & \cdots \\
\mathbb{C}\_{V,n\_1} & \mathbb{C}\_{n\_1 n\_1} & \mathbb{C}\_{n\_2 n\_1} & \cdots \\
\mathbb{C}\_{V,n\_2} & \mathbb{C}\_{n\_1 n\_2} & \mathbb{C}\_{n\_2 n\_2} & \cdots \\
\vdots & \vdots & \vdots & \ddots
\end{vmatrix}
\tag{101}$$

$$\begin{vmatrix} A\_{VVK} & A\_{n\_1VK} & A\_{n\_2VK} & \cdots \\ A\_{Vn\_1K} & A\_{n\_1n\_1K} & A\_{n\_2n\_1K} & \cdots \\ A\_{Vn\_2K} & A\_{n\_1n\_2K} & A\_{n\_2n\_2K} & \cdots \\ \vdots & \vdots & \vdots & \ddots \end{vmatrix} \tag{102}$$

**Figure 2.** Calculated critical points of binary CO2-CH4 fluid mixtures in terms of temperature (red line) and pressure (green line), obtained from the *PReos* [10]. Solid circles are experimental data [16, 19]. The open squares are the critical point of pure CO2 [20].

where *C*xy are the individual elements in the matrix of "cofactors", as obtained from the Laplacian expansion. The subscript *K* refers to the variable that is used in the third differentiation (volume, amount of substance of the components 1 and 2. To reduce computation time in software that uses this calculation method, the *LU* decomposition has been used to calculate the determinant in Eq. 97. The determinants in Eqs. 68 and 97 are both used to calculate exactly the critical point of any fluid mixture and pure gases, based on two-constant cubic equations of state that define the Helmholtz energy function.

An example of a calculated critical curve, i.e. critical points for a variety of compositions in a binary fluid system, is illustrated in Figure 2. The prediction of critical temperatures of fluid mixtures corresponds to experimental data [16, 19], whereas calculated critical pressures are slightly overestimated at higher fraction of CH4. This example illustrates that the *PReos* [10] is a favourable modification that can be used to calculate sub-critical conditions of CO2-CH4 fluid mixtures.

## **7. Mixing rules and definitions of 1 and <sup>2</sup>**

178 Thermodynamics – Fundamentals and Its Application in Science

1

2

*n*

*D*

*n*

*D*

1 *spin*

2 *spin*

> 

> >

*n*

(99)

(100)

(101)

(102)

*n*

*D*

*D*

The derivatives of the spinodal determinant (Eqs. 98-100) are calculated from the sum of the element-by-element products of the matrix of "cofactors" (or adjoint matrix) of the spinodal (Eq. 101) and the matrix of the third derivatives of the Helmholtz energy function (Eq. 102).

> 1 2 1 11 21 2 12 22

1 2

1 11 21 2 12 22

**Figure 2.** Calculated critical points of binary CO2-CH4 fluid mixtures in terms of temperature (red line) and pressure (green line), obtained from the *PReos* [10]. Solid circles are experimental data [16, 19]. The

where *C*xy are the individual elements in the matrix of "cofactors", as obtained from the Laplacian expansion. The subscript *K* refers to the variable that is used in the third differentiation (volume, amount of substance of the components 1 and 2. To reduce computation time in software that uses this calculation method, the *LU* decomposition has

open squares are the critical point of pure CO2 [20].

*VVK n VK n VK Vn K n n K n n K Vn K n n K n n K*

*AAA AAA AAA*

*VV n V n V Vn n n n n Vn n n n n*

*CCC CCC CCC*

All modifications of the van-der-Waals two-constant cubic equation of state [7] have an empirical character. The main modifications are defined by Redlich and Kwong, Soave and Peng and Robinson (see Table 1), and all modification can by summarized by specific adaptations of the values of *1, 2, 3, and <sup>4</sup>* to fit experimental data. The original definition [7] of *1 (b)* and *<sup>2</sup> (a)* for pure gases is obtained from the pseudo critical conditions (Eqs. 91- 93, and 94-96). This principle is adapted in most modifications of the van-der-Waals equation of state, e.g. *RKeos* [8]. Soave [9] and Peng and Robinson [10] adjusted the definition of *<sup>2</sup>* with a temperature dependent correction parameter (Eqs. 103-105).

$$
\mathcal{L}\_2 \, :\, \begin{array}{c} \text{ $a\_\odot$ } \, :\, a \, \text{ $a\_\odot$ } \, \end{array} \tag{103}
$$

$$\begin{array}{rcl} \alpha & = & \left[1 + m\left(1 - \sqrt{\frac{T}{T\_{\odot}}}\right)\right]^2 \\\\ & & \left[1 - m\left(1 - \sqrt{\frac{T}{T\_{\odot}}}\right)\right]^2 \end{array} \tag{104}$$

$$\mathfrak{m}\_{\parallel} = \sum\_{i=0,1,2} m\_i \cdot o^i \tag{105}$$

where *a*c is defined by the pseudo critical conditions (Eqs. 91-93), and is the acentric factor. The summation in Eq. 105 does not exceed *i* = 2 for Soave [9] and Peng and Robinson [10]. The definition of the acentric factor is arbitrary and chosen for convenience [5] and is a purely empirical modification. These two equations of state have different definitions of pseudo critical conditions (see Eqs. 91-93 and 94-96), therefore, the values of *m*i must be different for each equation (Table 3).


**Table 3.** Values of the constant *mi* in Eq. 105.

The two-constant cubic equation of state can be applied to determine the properties of fluid mixtures by using "*mixing rules*" for the parameters *1* and *<sup>2</sup>* which are defined for individual pure gases according to pseudo critical conditions. These mixing rules are based on simplified molecular behaviour of each component (*i* and *j)* in mixtures [21, 22] that describe the interaction between two molecules:

$$\left.\boldsymbol{\zeta}\_{1}^{\text{mix}}\right.\quad =\sum\_{i}\sum\_{j} \mathbf{x}\_{i} \cdot \boldsymbol{\zeta}\_{1}(i)\tag{106}$$

Thermodynamic Properties and Applications of Modified van-der-Waals Equations of State 181

**Figure 3.** Modelled immiscibility of binary CO2-CH4 gas mixtures (shaded areas) in a pressure - amount CH4 fraction diagram (**a**) and amount CH4 fraction - molar volume diagram (**b**) at 15 C. The solid and open circles are experimental data [16]. The red squares are the properties of pure CO2 [20]. The yellow triangle (*Cexp*) is the interpolated critical point for experimental data, and the green triangle (*CRK*) is the calculated critical point [8]. *tie1* and *tie 2* in (**b**) are calculated tie-lines between two phases at constant

*cm3·mol-1 W RK S PR CO2 CH4 N2* 0.8 0.1 0.1 56.64 64.61 (14.1%) 54.90 (-3.1%) 57.94 (2.3%) 53.59 (-5.4%) 0.8 0.2 0.2 58.92 65.81 (11.7%) 56.61 (-3.9%) 59.61 (1.2%) 56.93 (-6.1%) 0.4 0.3 0.3 61.08 67.08 (9.6%) 58.27 (-4.6%) 61.12 (0.1%) 56.93 (-6.8%) 0.2 0.4 0.4 62.90 68.28 (8.6%) 59.83 (-4.9%) 62.42 (-0.8%) 58.28 (-7.3%) **Table 4.** Comparison of supercritical experimental molar volumes [23] at 100 MPa and 200 C with two-

constant cubic equations of state (abbreviations see Table 1). The percentage of deviation from

Figure 3 and Table 4 illustrate that these modified two-constant cubic equations of state still need to be modified again to obtain a better model to reproduce fluid properties at sub- and

The number of publications that have modified the previously mentioned two-constant cubic equations of state are numerous, see also [11], and they developed highly complex, but

gases by Chueh and Prausnitz [24]. This equation is an arbitrary modification of the *RKeos*

*1* and  *1* and *<sup>2</sup>* (Eqs. 92 and 95) are modified for individual

*<sup>2</sup>*. A few examples are

experimentally obtained molar volumes is indicated in brackets.

**9. Modifications of modified equations of state** 

purely empirical equations to define the parameters

illustrated in the following paragraphs.

The constant values in the definition of

**9.1. Chueh and Prausnitz [24]** 

pressures 6.891 and 6.036 MPa, respectively.

*composition Vm(exp)*

supercritical conditions.

$$\left| \mathcal{L}\_2^{\min} \right\rangle = \sum\_{i} \sum\_{j} \mathbf{x}\_i \mathbf{x}\_j \cdot \mathcal{L}\_2 \langle i, j \rangle \tag{107}$$

where

$$
\mathcal{L}\_2(\mathbf{i}, \mathbf{j}) \quad = \sqrt{\mathcal{L}\_2(\mathbf{i}) \cdot \mathcal{L}\_2(\mathbf{j})} \tag{108}
$$

These mixing rules have been subject to a variety of modifications, in order to predict fluid properties of newly available experimental data of mixtures. Soave [9] and Peng and Robinson [10] modified Eq. 108 by adding an extra correction factor (Eq. 109).

$$
\zeta\_2(i,j) = \left(1 - \delta\_{ij}\right) \cdot \sqrt{\zeta\_2(i) \cdot \zeta\_2(j)}\tag{109}
$$

where *ij* has a constant value dependent on the nature of component *i* and *j*.

#### **8. Experimental data**

As mentioned before, modifications of two-constant cubic equation of state was mainly performed to obtain a better fit with experimental data for a multitude of possible gas mixtures and pure gases. Two types of experimental data of fluid properties were used: 1. homogeneous fluid mixtures at supercritical conditions; and 2. immiscible two-fluid systems at subcritical conditions (mainly in petroleum fluid research). The experimental data consist mainly of pressure, temperature, density (or molar volume) and compositional data, but can also include less parameters. Figure 3 gives an example of the misfit between the first type of experimental data for binary CO2-CH4 mixtures [19] and calculated fluid properties with *RKeos* [8] at a constant temperature (15 C). The *RKeos* uses the pseudo critical defined parameters *1* and *<sup>2</sup>* (Eqs. 92 and 95) and mixing rules according to Eqs. 106-108 and is only approximately reproducing the fluid properties of CO2-CH4 mixtures at subcritical conditions

Experimental data of homogeneous supercritical gas mixtures in the ternary CO2-CH4-N2 system [23] are compared with the two-constant cubic equations of state in Table 4. The *Weos* [7] clearly overestimates (up to 14.1 %) experimentally determined molar volumes at 100 MPa and 200 C. The *Seos* [9] is the most accurate model in Table 4, but still reach deviations of up to 2.3 % for CO2-rich gas mixtures. The *PReos* [10] gives highly underestimated molar volumes at these conditions.

**Figure 3.** Modelled immiscibility of binary CO2-CH4 gas mixtures (shaded areas) in a pressure - amount CH4 fraction diagram (**a**) and amount CH4 fraction - molar volume diagram (**b**) at 15 C. The solid and open circles are experimental data [16]. The red squares are the properties of pure CO2 [20]. The yellow triangle (*Cexp*) is the interpolated critical point for experimental data, and the green triangle (*CRK*) is the calculated critical point [8]. *tie1* and *tie 2* in (**b**) are calculated tie-lines between two phases at constant pressures 6.891 and 6.036 MPa, respectively.


**Table 4.** Comparison of supercritical experimental molar volumes [23] at 100 MPa and 200 C with twoconstant cubic equations of state (abbreviations see Table 1). The percentage of deviation from experimentally obtained molar volumes is indicated in brackets.

Figure 3 and Table 4 illustrate that these modified two-constant cubic equations of state still need to be modified again to obtain a better model to reproduce fluid properties at sub- and supercritical conditions.

## **9. Modifications of modified equations of state**

The number of publications that have modified the previously mentioned two-constant cubic equations of state are numerous, see also [11], and they developed highly complex, but purely empirical equations to define the parameters *1* and *<sup>2</sup>*. A few examples are illustrated in the following paragraphs.

## **9.1. Chueh and Prausnitz [24]**

180 Thermodynamics – Fundamentals and Its Application in Science

describe the interaction between two molecules:

where

where 

parameters

conditions

*1* and 

volumes at these conditions.

**8. Experimental data** 

mixtures by using "*mixing rules*" for the parameters

Robinson [10] modified Eq. 108 by adding an extra correction factor (Eq. 109).

The two-constant cubic equation of state can be applied to determine the properties of fluid

individual pure gases according to pseudo critical conditions. These mixing rules are based on simplified molecular behaviour of each component (*i* and *j)* in mixtures [21, 22] that

1 1( ) *mix*

2 2(,) *mix i j*

*i j*

2 22

These mixing rules have been subject to a variety of modifications, in order to predict fluid properties of newly available experimental data of mixtures. Soave [9] and Peng and

<sup>2</sup> 2 2 (, ) 1 () () *ij*

As mentioned before, modifications of two-constant cubic equation of state was mainly performed to obtain a better fit with experimental data for a multitude of possible gas mixtures and pure gases. Two types of experimental data of fluid properties were used: 1. homogeneous fluid mixtures at supercritical conditions; and 2. immiscible two-fluid systems at subcritical conditions (mainly in petroleum fluid research). The experimental data consist mainly of pressure, temperature, density (or molar volume) and compositional data, but can also include less parameters. Figure 3 gives an example of the misfit between the first type of experimental data for binary CO2-CH4 mixtures [19] and calculated fluid properties with *RKeos* [8] at a constant temperature (15 C). The *RKeos* uses the pseudo critical defined

approximately reproducing the fluid properties of CO2-CH4 mixtures at subcritical

Experimental data of homogeneous supercritical gas mixtures in the ternary CO2-CH4-N2 system [23] are compared with the two-constant cubic equations of state in Table 4. The *Weos* [7] clearly overestimates (up to 14.1 %) experimentally determined molar volumes at 100 MPa and 200 C. The *Seos* [9] is the most accurate model in Table 4, but still reach deviations of up to 2.3 % for CO2-rich gas mixtures. The *PReos* [10] gives highly underestimated molar

*<sup>2</sup>* (Eqs. 92 and 95) and mixing rules according to Eqs. 106-108 and is only

*ij* has a constant value dependent on the nature of component *i* and *j*.

 

*i i j*

 

  *1* and 

*x i* (106)

*xx i j* (107)

(, ) () () *ij i j* (108)

*i j i j* (109)

*<sup>2</sup>* which are defined for

The constant values in the definition of *1* and *<sup>2</sup>* (Eqs. 92 and 95) are modified for individual gases by Chueh and Prausnitz [24]. This equation is an arbitrary modification of the *RKeos*

[8]. Consequently, the calculation of the value of *1* and *<sup>2</sup>* is not any more defined by pseudo critical conditions, which give exact mathematical definition of these constants. Although the prediction of fluid properties of a variety of gas mixtures was improved by these modifications, the morphology of the Helmholtz energy equation in the *p-V-T-x*  parameter space is not any more related to observed fluid properties. The theory of pseudo critical conditions is violated according to these modifications.

The mixing rules in Eqs. 106-108 were further refined by arbitrary definitions of critical temperature, pressure, volume and compressibility for fluid mixtures.

$$\text{Tr}\_2(i,j) \quad = \frac{\Omega\_i + \Omega\_j}{2} \cdot \frac{\mathbf{R}^2 T\_{\text{Cij}}^2}{p\_{\text{Cij}}} \tag{110}$$

Thermodynamic Properties and Applications of Modified van-der-Waals Equations of State 183

temperature was subjected to a variety of best-fit procedures [25, 26]. The fitting was improved from four experimental data points [25] to six [26] (Figure 5), but was restricted to temperatures above 350 C. Bakker [27] improved the best-fit equation by including the

**Figure 4.** See Figure 3 for details. The *RKeos* is indicated by dashed lines in (**a**) and (**b**). The shaded areas are immiscibility conditions calculated with the Chueh-Prausnitz equation. *tie1* and *tie 2* in (**b**) are calculated tie-lines between two phases at constant pressures 6.944 and 5.984 MPa, respectively.

**Figure 5.** Temperature dependence of the *a* constant for pure H2O in the modified cubic equation of state [25, 26]. The open circles are calculated experimental data [29]. *fit [25]* is the range of fitting in the definition of Holloway [25], and *fit [26]* of Holloway [26]. *RK* illustrates the constant value calculated

from pseudo critical condition [8].

entire data set [29], down to 50 C (Eq. 112).

$$a\_{ij} = \frac{\Omega\_i + \Omega\_j}{2} \cdot \frac{\mathbb{R}^2 T\_{C\bar{j}}^{2.5}}{p\_{C\bar{j}}} \tag{111}$$

where *i* and *<sup>j</sup>* are the newly defined constant values of component *i* and *j*, and *TCij* and *pCij* are defined according to complex mixing rules [see 24]. The values of *TCij* and *pCij* are not related to true critical temperatures and pressures of specific binary gas mixtures.

The prediction of the properties of homogeneous fluids at supercritical conditions (Table 5) is only slightly improved compared to *RKeos* [10], but it is not exceeding the accuracy of the *Seos* [11]. At sub-critical condition (Figure 4), the Chueh-Prausnitz equation is less accurate than the Redlich-Kwong equation (compare Figure 3) in the binary CO2-CH4 fluid mixture at 15 C.


**Table 5.** The same experimental molar volumes as in Table 4 compared with two-constant equations of state according to Chueh and Prausnitz [24] (CP), Holloway [25, 26] (H), Bakker [27] [B1], and Bakker [28] (B2). The percentage of deviation from experimentally obtained molar volumes is indicated in brackets.

### **9.2. Holloway [25, 26] and Bakker [27]**

The equation of Holloway [25, 26] is another modification of the *RKeos* [8]. The modification is mainly based on the improvement of predictions of homogenous fluid properties of H2O and CO2 mixtures, using calculated experimental data [29]. The value for *1* and *<sup>3</sup>* (both *b*) of H2O is arbitrarily selected at 14.6 cm3·mol-1, whereas other pure gases are defined according to pseudo critical conditions. The definition of *<sup>2</sup>* (i.e. *a*) for H2O as a function of temperature was subjected to a variety of best-fit procedures [25, 26]. The fitting was improved from four experimental data points [25] to six [26] (Figure 5), but was restricted to temperatures above 350 C. Bakker [27] improved the best-fit equation by including the entire data set [29], down to 50 C (Eq. 112).

182 Thermodynamics – Fundamentals and Its Application in Science

where *i* and 

*composition Vm(exp)* 

**9.2. Holloway [25, 26] and Bakker [27]** 

*CO2 CH4 N2*

indicated in brackets.

[8]. Consequently, the calculation of the value of

critical conditions is violated according to these modifications.

temperature, pressure, volume and compressibility for fluid mixtures.

*i j*

*ij*

*a*

*1* and 

2 2

(110)

(111)

*1* and 

*<sup>2</sup>* (i.e. *a*) for H2O as a function of

*<sup>3</sup>* (both *b*)

*R T*

*p*

2 2.5

*R T*

*p*

*<sup>j</sup>* are the newly defined constant values of component *i* and *j*, and *TCij* and *pCij*

*cm3·mol-1 CP H B1 B2* 

*Cij*

*Cij*

*i j Cij*

*i j Cij*

pseudo critical conditions, which give exact mathematical definition of these constants. Although the prediction of fluid properties of a variety of gas mixtures was improved by these modifications, the morphology of the Helmholtz energy equation in the *p-V-T-x*  parameter space is not any more related to observed fluid properties. The theory of pseudo

The mixing rules in Eqs. 106-108 were further refined by arbitrary definitions of critical

2

are defined according to complex mixing rules [see 24]. The values of *TCij* and *pCij* are not

The prediction of the properties of homogeneous fluids at supercritical conditions (Table 5) is only slightly improved compared to *RKeos* [10], but it is not exceeding the accuracy of the *Seos* [11]. At sub-critical condition (Figure 4), the Chueh-Prausnitz equation is less accurate than the Redlich-Kwong equation (compare Figure 3) in the binary CO2-CH4 fluid mixture at 15 C.

0.8 0.1 0.1 56.64 56.42 (-0.4%) 55.96 (-0.6%) 56.84 (0.4%) 56.53 (-0.2%) 0.8 0.2 0.2 58.92 57.85 (-1.8%) 57.68 (-2.1%) 59.43 (0.9%) 58.81 (-0.2%) 0.4 0.3 0.3 61.08 59.21 (-3.1%) 59.17 (-3.1%) 61.67 (1.0%) 60.79 (-0.5%) 0.2 0.4 0.4 62.90 60.44 (-3.9%) 60.38 (-4.0%) 63.45 (0.9%) 62.40 (-0.8%) **Table 5.** The same experimental molar volumes as in Table 4 compared with two-constant equations of state according to Chueh and Prausnitz [24] (CP), Holloway [25, 26] (H), Bakker [27] [B1], and Bakker [28] (B2). The percentage of deviation from experimentally obtained molar volumes is

The equation of Holloway [25, 26] is another modification of the *RKeos* [8]. The modification is mainly based on the improvement of predictions of homogenous fluid properties of H2O

of H2O is arbitrarily selected at 14.6 cm3·mol-1, whereas other pure gases are defined

and CO2 mixtures, using calculated experimental data [29]. The value for

according to pseudo critical conditions. The definition of

<sup>2</sup>(,) <sup>2</sup>

related to true critical temperatures and pressures of specific binary gas mixtures.

*<sup>2</sup>* is not any more defined by

**Figure 4.** See Figure 3 for details. The *RKeos* is indicated by dashed lines in (**a**) and (**b**). The shaded areas are immiscibility conditions calculated with the Chueh-Prausnitz equation. *tie1* and *tie 2* in (**b**) are calculated tie-lines between two phases at constant pressures 6.944 and 5.984 MPa, respectively.

**Figure 5.** Temperature dependence of the *a* constant for pure H2O in the modified cubic equation of state [25, 26]. The open circles are calculated experimental data [29]. *fit [25]* is the range of fitting in the definition of Holloway [25], and *fit [26]* of Holloway [26]. *RK* illustrates the constant value calculated from pseudo critical condition [8].

$$a\_{H\_2O} = \left(9.4654 - \frac{2.0246 \cdot 10^3}{T} + \frac{1.4928 \cdot 10^6}{T^2} + \frac{7.57 \cdot 10^8}{T^3}\right) \cdot 10^6 \tag{112}$$

Thermodynamic Properties and Applications of Modified van-der-Waals Equations of State 185

mathematical formulation and the use of different independent variables, which are temperature and pressure in Eq. 118. The integration to calculate the fugacity coefficient can be graphically obtained by measuring the surface of a diagram of the difference between the ideal molar volume and the partial molar volume (i.e. *V*m,i - *V*mideal) as a function of pressure (Figure 6). The surface obtained from experimental data can be directly compared to

The dashed line in Figure 6 is calculated with another type of equation of state: a modification of the Lee-Kesler equation of state [33] that is not treated in this manuscript because it is not a two-constant cubic equation of state. Fugacity estimations of H2O are similar according to both equations, and reveal only a minor improvement for the twoconstant cubic equation of state [27]. The experimental data to determine fugacity of CO2 in this fluid mixture is inconsistent at relative low pressures (< 100 MPa). The calculated

fugacity [27] is approximately compatible with the experimental data from [31, 32].

**Figure 6.** Fugacity estimation in a pressure - dv diagram at 873 K and a composition of *x*(CO2) = 0.3 in the binary H2O-CO2 system, where dv is the molar volume difference of an ideal gas and the partial molar volume of either H2O or CO2 in binary mixtures. Experimental data are illustrated with circles, triangles and squares (solid for CO2 and open for H2O. The red lines are calculated with Bakker [27],

and the shaded area is a measure for the fugacity coefficient of H2O (Eq. 118).

calculated curves from equations of state, according to Eq. 10 (Table 6).

where *T* is temperature in Kelvin, and the dimension of *a* is cm6·MPa·K0.5·mol-2. The properties of homogeneous pure CO2, CH4 and N2 fluids [27] were also used to obtain a temperature dependent *a* constant (Eqs. 113, 114, and 115, respectively).

$$a\_{\rm CO\_2} = \left(-1.2887 + \frac{5.9363 \cdot 10^3}{T} - \frac{1.4124 \cdot 10^6}{T^2} + \frac{1.1767 \cdot 10^8}{T^3}\right) \cdot 10^6\tag{113}$$

$$a\_{CH\_4} = \left(-1.1764 + \frac{3.5216 \cdot 10^3}{T} - \frac{1.155 \cdot 10^6}{T^2} + \frac{1.1767 \cdot 10^8}{T^3}\right) \cdot 10^6\tag{114}$$

$$a\_{N\_2} = \left(0.060191 - \frac{0.20059 \cdot 10^3}{T} + \frac{0.15386 \cdot 10^6}{T^2}\right) \cdot 10^6\tag{115}$$

The *aij* value of fluid mixtures with a H2O and CO2 component (as in Eqs. 106-108 and 110- 111) is not defined by the value of pure H2O and CO2 (Eqs. 112 and 113), but from a temperature independent constant value (Eqs. 116 and 117, respectively). In addition, a correction factor is used only for binary H2O-CO2 mixtures, see [25, 29].

$$a\_0 \left( H\_2O \right) \quad = \ 3.5464 \cdot 10^6 \quad MPa \cdot cm^6 \cdot K^{0.5} \cdot mol^2 \tag{116}$$

$$a\_0 \left(\text{CO}\_2\right) \quad = \ 4.661 \cdot 10^6 \quad \text{MPa} \cdot \text{cm}^6 \cdot \text{K}^{0.5} \cdot \text{mol}^2 \tag{117}$$

Table 5 illustrates that the equation of Holloway [25] is not improving the accuracy of predicted properties of supercritical CO2-CH4-N2 fluids, compared to Chueh-Prausnitz [24] or *Seos* [9], and it is only a small improvement compared to the *RKeos* [8]. The accuracy of this equation is highly improved by using the definitions of *a* constants according to Bakker [27] (see Eqs. 112-115), and result in a maximum deviation of only 1% from experimental data in Table 5.

Experimental data, including molar volumes of binary H2O-CO2 fluid mixtures at supercritical conditions [30, 31, 32] are used to estimate fugacities of H2O and CO2 according to Eq. 118 (compare Eq. 10).

$$RT\ln p\_i \quad = \int\_0^p \left[V\_{m,i} - V\_m^{\
i \text{ideal}}\right] dp \tag{118}$$

where *V*m,i - *V*mideal is the difference between the partial molar volume of component i and the molar volume of an ideal gas (see also Eq. 43). The difference between Eqs. 118 and 10 is the mathematical formulation and the use of different independent variables, which are temperature and pressure in Eq. 118. The integration to calculate the fugacity coefficient can be graphically obtained by measuring the surface of a diagram of the difference between the ideal molar volume and the partial molar volume (i.e. *V*m,i - *V*mideal) as a function of pressure (Figure 6). The surface obtained from experimental data can be directly compared to calculated curves from equations of state, according to Eq. 10 (Table 6).

184 Thermodynamics – Fundamentals and Its Application in Science

3 68

368

36 8

3 6

0 2 *a HO* 3.5464 10 *MPa cm K mol* (116)

0 2 *a CO* 4.661 10 *MPa cm K mol* (117)

(118)

2 3

2 3

2

*T T T*

*T T T*

*T T T*

*T T*

2.0246 10 1.4928 10 7.57 10 9.4654 <sup>10</sup> *H O <sup>a</sup>*

where *T* is temperature in Kelvin, and the dimension of *a* is cm6·MPa·K0.5·mol-2. The properties of homogeneous pure CO2, CH4 and N2 fluids [27] were also used to obtain a

5.9363 10 1.4124 10 1.1767 10 1.2887 <sup>10</sup> *CO <sup>a</sup>*

3.5216 10 1.155 10 1.1767 10 1.1764 <sup>10</sup> *CH <sup>a</sup>*

0.20059 10 0.15386 10 0.060191 <sup>10</sup> *Na*

The *aij* value of fluid mixtures with a H2O and CO2 component (as in Eqs. 106-108 and 110- 111) is not defined by the value of pure H2O and CO2 (Eqs. 112 and 113), but from a temperature independent constant value (Eqs. 116 and 117, respectively). In addition, a

<sup>6</sup> 6 0.5 2

<sup>6</sup> 6 0.5 2

Table 5 illustrates that the equation of Holloway [25] is not improving the accuracy of predicted properties of supercritical CO2-CH4-N2 fluids, compared to Chueh-Prausnitz [24] or *Seos* [9], and it is only a small improvement compared to the *RKeos* [8]. The accuracy of this equation is highly improved by using the definitions of *a* constants according to Bakker [27] (see Eqs. 112-115), and result in a maximum deviation of only 1% from experimental

Experimental data, including molar volumes of binary H2O-CO2 fluid mixtures at supercritical conditions [30, 31, 32] are used to estimate fugacities of H2O and CO2 according

,

0

where *V*m,i - *V*mideal is the difference between the partial molar volume of component i and the molar volume of an ideal gas (see also Eq. 43). The difference between Eqs. 118 and 10 is the

*p ideal RT <sup>i</sup> V V dp mi m*

ln

 

 

 

temperature dependent *a* constant (Eqs. 113, 114, and 115, respectively).

correction factor is used only for binary H2O-CO2 mixtures, see [25, 29].

 

2 3

6

6

6

6

(112)

(113)

(114)

(115)

2

2

4

data in Table 5.

to Eq. 118 (compare Eq. 10).

2

The dashed line in Figure 6 is calculated with another type of equation of state: a modification of the Lee-Kesler equation of state [33] that is not treated in this manuscript because it is not a two-constant cubic equation of state. Fugacity estimations of H2O are similar according to both equations, and reveal only a minor improvement for the twoconstant cubic equation of state [27]. The experimental data to determine fugacity of CO2 in this fluid mixture is inconsistent at relative low pressures (< 100 MPa). The calculated fugacity [27] is approximately compatible with the experimental data from [31, 32].

**Figure 6.** Fugacity estimation in a pressure - dv diagram at 873 K and a composition of *x*(CO2) = 0.3 in the binary H2O-CO2 system, where dv is the molar volume difference of an ideal gas and the partial molar volume of either H2O or CO2 in binary mixtures. Experimental data are illustrated with circles, triangles and squares (solid for CO2 and open for H2O. The red lines are calculated with Bakker [27], and the shaded area is a measure for the fugacity coefficient of H2O (Eq. 118).


Thermodynamic Properties and Applications of Modified van-der-Waals Equations of State 187

analytical technique that directly uses equations of state to obtain fluid composition and density of fluid inclusions. For example, cooling and heating experiment may reveal fluid phase changes at specific temperatures, such as dissolution and homogenization, which can

The calculation method of fluid properties is extensive and is susceptible to errors, which is obvious from the mathematics presented in the previous paragraphs. The computer package FLUIDS [6, 40, 41] was developed to facilitate calculations of fluid properties in fluid inclusions, and fluids in general. This package includes the group "Loners" that handles a large variety of equations of state according to individual publications. This group allows researchers to perform mathematical experiments with equations of state and to test the

The equations of state handled in this study can be downloaded from the web site **http://fluids.unileoben.ac.at** and include 1. "*LonerW*" [7]; 2. "*LonerRK*" [8]; 3. "*LonerS*" [9]; 4. "*LonerPR*" [10]; 5. "*LonerCP*" [24]; 6. "*LonerH*" [25, 26, 27]; and 7. "*LonerB*" [28, 34]. Each program has to possibility to calculate a variety of fluid properties, including pressure, temperature, molar volume, fugacity, activity, liquid-vapour equilibria, homogenization conditions, spinodal, critical point, entropy, internal energy, enthalpy, Helmholtz energy, Gibbs energy, chemical potentials of pure gases and fluid mixtures. In addition, isochores can be calculated and exported in a text file. The diagrams and tables presented in this study

*Department of Applied Geosciences and Geophysics, Resource Mineralogy, Montanuniversitaet,* 

[1] Dziewonski AM, Anderson DL (1981) Preliminary reference Earth model. Phys. Earth

[3] Roedder E (1984) Fluid inclusions, Reviews in Mineralogy 12, Mineralogical Association

[4] Bakker RJ (2009) Reequilibration of fluid inclusions: Bulk diffusion. Lithos 112: 277-288. [5] Prausnitz JM, Lichtenthaler RN, Gomes de Azevedo E (1986) Molecular thermodynamics of fluid-phase equilibria. Prentice-Hall, Englewood Cliffs, NJ, 600 p. [6] Bakker RJ (2009) Package FLUIDS. Part 3: correlations between equations of state,

[2] Press F, Siever R (1999) Understanding Earth. Freeman, New York, 679 p.

thermodynamics and fluid inclusions. Geofluids 9: 63-74.

be transformed in composition and density by using the proper equations of state.

accuracy by comparison with experimental data.

are all calculated with these programs.

**Author details** 

Ronald J. Bakker

*Leoben, Austria* 

**11. References** 

Planet. In. 25: 297-356.

of America, 646 p.

**Table 6.** Fugacities of H2O in H2O-CO2 fluid mixtures, *x*(CO2) = 0.3, at 873.15 K and variable pressures. B1 fugacity is calculated with Bakker [27]. The deviation (in %) is illustrated in brackets.

## **9.3. Bowers and Helgeson [34] and Bakker [28]**

Most natural occurring fluid phases in rock contain variable amounts of NaCl, which have an important influence on the fluid properties. Bowers and Helgeson [34] modified the *RKeos* [8] to be able to reproduce the properties of homogeneous supercritical fluids in the H2O-CO2-NaCl system, but only up to 35 mass% NaCl. The model is originally restricted between 350 and 600 C and pressures above 50 MPa, according to the experimental data [35] that was used to design this equation. This model was modified by Bakker [28] including CH4, N2, and additionally any gas with *a* (2) and b (1) constants defined by the pseudo critical conditions (Eqs. 91-93 and 94-96). Experimental data in this multi-component fluid system with NaCl can be accurately reproduced up to 1000 MPa and 1300 K. Table 5 illustrates that this modification results in the best estimated molar volumes in the ternary CO2-CH4-N2 fluid system at 100 MPa and 673 K. Similar to all modifications of the *RKeos* [8], this model cannot be used in and near the immiscibility conditions and critical points (i.e. sub-critical conditions).

## **10. Application to fluid inclusion research**

Knowledge of the properties of fluid phases is of major importance in geological sciences. The interaction between rock and a fluid phase plays a role in many geological processes, such as development of magma [36], metamorphic reactions [37] and ore formation processes [38]. The fluid that is involved in these processes can be entrapped within single crystal of many minerals (e.g. quartz), which may be preserved over millions of years. The information obtained from fluid inclusions includes 1. fluid composition; 2. fluid density; 3. temperature and pressure condition of entrapment; and 4. a temporal evolution of the rock can be reconstructed from presence of various generation of fluid inclusions. An equation of state of fluid phases is the major tool to obtain this information. Microthermometry [39] is an analytical technique that directly uses equations of state to obtain fluid composition and density of fluid inclusions. For example, cooling and heating experiment may reveal fluid phase changes at specific temperatures, such as dissolution and homogenization, which can be transformed in composition and density by using the proper equations of state.

The calculation method of fluid properties is extensive and is susceptible to errors, which is obvious from the mathematics presented in the previous paragraphs. The computer package FLUIDS [6, 40, 41] was developed to facilitate calculations of fluid properties in fluid inclusions, and fluids in general. This package includes the group "Loners" that handles a large variety of equations of state according to individual publications. This group allows researchers to perform mathematical experiments with equations of state and to test the accuracy by comparison with experimental data.

The equations of state handled in this study can be downloaded from the web site **http://fluids.unileoben.ac.at** and include 1. "*LonerW*" [7]; 2. "*LonerRK*" [8]; 3. "*LonerS*" [9]; 4. "*LonerPR*" [10]; 5. "*LonerCP*" [24]; 6. "*LonerH*" [25, 26, 27]; and 7. "*LonerB*" [28, 34]. Each program has to possibility to calculate a variety of fluid properties, including pressure, temperature, molar volume, fugacity, activity, liquid-vapour equilibria, homogenization conditions, spinodal, critical point, entropy, internal energy, enthalpy, Helmholtz energy, Gibbs energy, chemical potentials of pure gases and fluid mixtures. In addition, isochores can be calculated and exported in a text file. The diagrams and tables presented in this study are all calculated with these programs.

## **Author details**

186 Thermodynamics – Fundamentals and Its Application in Science

**9.3. Bowers and Helgeson [34] and Bakker [28]** 

**10. Application to fluid inclusion research** 

sub-critical conditions).

*Pressure (MPa) Exp. fugacity (MPa) B1 fugacity (MPa)* 

**Table 6.** Fugacities of H2O in H2O-CO2 fluid mixtures, *x*(CO2) = 0.3, at 873.15 K and variable pressures.

Most natural occurring fluid phases in rock contain variable amounts of NaCl, which have an important influence on the fluid properties. Bowers and Helgeson [34] modified the *RKeos* [8] to be able to reproduce the properties of homogeneous supercritical fluids in the H2O-CO2-NaCl system, but only up to 35 mass% NaCl. The model is originally restricted between 350 and 600 C and pressures above 50 MPa, according to the experimental data [35] that was used to design this equation. This model was modified by Bakker [28] including CH4, N2, and additionally any gas with *a* (2) and b (1) constants defined by the pseudo critical conditions (Eqs. 91-93 and 94-96). Experimental data in this multi-component fluid system with NaCl can be accurately reproduced up to 1000 MPa and 1300 K. Table 5 illustrates that this modification results in the best estimated molar volumes in the ternary CO2-CH4-N2 fluid system at 100 MPa and 673 K. Similar to all modifications of the *RKeos* [8], this model cannot be used in and near the immiscibility conditions and critical points (i.e.

Knowledge of the properties of fluid phases is of major importance in geological sciences. The interaction between rock and a fluid phase plays a role in many geological processes, such as development of magma [36], metamorphic reactions [37] and ore formation processes [38]. The fluid that is involved in these processes can be entrapped within single crystal of many minerals (e.g. quartz), which may be preserved over millions of years. The information obtained from fluid inclusions includes 1. fluid composition; 2. fluid density; 3. temperature and pressure condition of entrapment; and 4. a temporal evolution of the rock can be reconstructed from presence of various generation of fluid inclusions. An equation of state of fluid phases is the major tool to obtain this information. Microthermometry [39] is an

B1 fugacity is calculated with Bakker [27]. The deviation (in %) is illustrated in brackets.

10 6.692 6.659 (-0.5%) 50 27.962 27.3061 (-2.3%) 100 45.341 44.6971 (-1.4%) 200 77.278 75.0515 (-2.9%) 300 114.221 111.072 (-2.8%) 400 160.105 157.145 (-1.8%) 500 219.252 216.817 (-1.1%) 600 295.350 294.216 (-04%)

> Ronald J. Bakker *Department of Applied Geosciences and Geophysics, Resource Mineralogy, Montanuniversitaet, Leoben, Austria*

## **11. References**


[7] Waals JD van der (1873) De continuiteit van den gas- en vloeistof-toestand. PhD Thesis, University Leiden, 134 p.

Thermodynamic Properties and Applications of Modified van-der-Waals Equations of State 189

[24] Chueh PL, Prausnitz JM (1967) Vapor-liquid equilibria at high pressures. Vapor-phase fugacity coefficients in non-polar and quantum-gas mixtures. Ind. Eng. Chem. Fundam.

[25] Holloway JR (1977) Fugacity and activity of molecular species in supercritical fluids. In:

[26] Holloway JR (1981) Composition and volumes of supercritical fluids in the earth's crust. In Hollister LS, Crawford MI, editors. Short course in fluid inclusions: Applications to

[27] Bakker RJ (1999a) Optimal interpretation of microthermometrical data from fluid inclusions: thermodynamic modelling and computer programming. Habilitation Thesis,

[28] Bakker RJ (1999b) Adaptation of the Bowers and Helgeson (1983) equation of state to

[29] Santis R de, Breedveld GJF, Prausnitz JM (1974) Thermodynamic properties of aqueous gas mixtures at advanced pressures. Ind. Eng. Chem. Process, Dess, Develop. 13: 374-

[30] Greenwood HJ (1969) The compressibility of gaseous mixtures of carbon dioxide and water between 0 and 500 bars pressure and 450 and 800 Centigrade. Am. J.Sci. 267A:

[31] Franck EU, Tödheide K (1959) Thermische Eigenschaften überkritischer Mischungen von Kohlendioxyd und Wasser bis zu 750 C und 2000 Atm. Z. Phys. Chem. Neue Fol.

[32] Sterner SM, Bodnar RJ (1991) Synthetic fluid inclusions X. Experimental determinations of the P-V-T-X properties in the CO2-H2O system to 6 kb and 700 C. Am. J. Sci. 291: 1-

[33] Duan Z, Møller N, Weare JH (1996) A general equation of state for supercritical fluid mixtures and molecular simulation of mixtures PVTX properties. Geochim.

[34] Bowers TS, Helgeson HC (1983) Calculation of the thermodynamic and geochemical consequences of non-ideal mixing in the system H2O-CO2-NaCl on phase relations in geological systems: equation of state for H2O-CO2-NaCl fluids at high pressures and

[35] Gehrig M (1980) Phasengleichgewichte und pVT-daten ternärer Mischungen aus Wasser, Kohlendioxide und Natriumchlorid bis 3 kbar und 550 C. University

[36] Thompson JFH (1995) Magmas, fluids, and ore deposits. Short course 23, Mineralogical

[37] Spear FS (1995) Metamorphic phase equilibria and pressure-temperature-time paths.

[38] Wilkinson JJ (2001) Fluid inclusions in hydrothermal ore deposits. Lithos 55: 229-272.

Fraser DG, editor. Thermodynamics in geology, pp 161-182.

the H2O-CO2-CH4-N2-NaCl system. Chem. Geol. 154: 225-236.

temperatures. Geochim. Cosmochim. Acta 47: 1247-1275.

Karlsruhe, PhD-thesis, Hochschul Verlag, Freiburg, 109 p.

Mineralogical Society of America, Monograph, 799 p.

6: 492-498.

377.

191-208.

22: 232-245.

54.

petrology, pp. 13-38.

University Heidelberg, 50 p.

Cosmochim. Acta 60: 1209-1216.

Association of Canada.


[24] Chueh PL, Prausnitz JM (1967) Vapor-liquid equilibria at high pressures. Vapor-phase fugacity coefficients in non-polar and quantum-gas mixtures. Ind. Eng. Chem. Fundam. 6: 492-498.

188 Thermodynamics – Fundamentals and Its Application in Science

state. Chem. Eng. Sci. 27: 1197-1203.

Hill Book Company, NJ, 741 p.

Ind. Eng. Chem. 46: 511-517.

Eng. Japan 4: 113-122.

Chem. Ref. Data 25:1509-1596.

Theorie der Gase. Ann. Phys. 12: 127-136.

Stoffen besteht. Z. Ph. Chem. 5: 133-173

data. Geochim. Cosmochim. Acta 58: 1065-1071.

University Leiden, 134 p.

Fundam. 15: 59-64.

Amsterdam, 302 p.

Raton, Fl, 609 p.

561 p.

[7] Waals JD van der (1873) De continuiteit van den gas- en vloeistof-toestand. PhD Thesis,

[8] Redlich OR, Kwong JNS (1949) On the thermodynamics of solutions, V: An equation of

[9] Soave G (1972) Equilibrium constants from a modified Redlich-Kwong equation of

[10] Peng DY, Robinson DB (1976) A new two constant equation of state. Ind. Eng. Chem.

[11] Reid RC, Prausnitz JM, Poling BE (1989) The properties of gases and liquids. McGraw-

[12] Levelt-Sengers J (2002) How fluids unmix, discoveries by the school of van der Waals and Kamerlingh Onnes. Koninklijke Nederlandse Akademie van Wetenschappen,

[13] Beyer WH (1991) CRC Standard mathematical tables and formulae. CRC Press, Boca

[14] Horn RA, Johnson CR (1985) Matrix analysis. Cambridge University Press, Cambridge,

[15] Prausnitz JM, Anderson TF, Grens EA, Eckert CA, Hsieh R, O'Connell JP (1980) Computer calculations for the multicomponent vapor-liquid and liquid-liquid

[16] Donnelly HG, Katz DL (1954) Phase equilibria in the carbon dioxide - methane system.

[17] Baker LE, Luks KD (1980) Critical point and saturation pressure calculations for

[18] Konynenburg PH van, Scott RL (1980) Critical lines and phase equilibria in binary van

[19] Arai Y, Kaminishi GI, Saito S (1971) The experimental determination of the P-V-T-X relations for carbon dioxide-nitrogen and carbon dioxide-methane systems. J. Chem.

[20] Span R, Wagner W (1996) A new equation of state for carbon dioxide covering the fluid region from the triple point temperature to 1100 K at pressures up to 800 MPa. J. Phys.

[21] Lorentz HA (1881) Über die Anwendung des Satzes vom Virial in den kinetischen

[22] Waals JD van der (1890) Molekulartheorie eines Körpers, der aus zwei verschiedenen

[23] Seitz JC, Blencoe JG, Joyce DB, Bodnar RJ (1994) Volumetric properties of CO2-CH4-N2 fluids at 200 C and 1000 bars: a comparison of equations of state and experimental

state, fugacities of gaseous solutions. Chem Rev. 44: 233-244.

equilibria. Prentice-Hall, Englewood Cliffs, NJ, 353 p.

multipoint systems. Soc. Petrol. Eng. J. 20: 15-4.

der Waals mixtures. Philos. T. Roy. Soc. 298: 495-540.

	- [39] Shepherd TJ, Rankin AH, Alderton DHM (1985) A practical guide to fluid inclusion studies. Blackie, Glasgow, 239 p.

**Chapter 8** 

© 2012 Blanquet and Nuta, licensee InTech. This is an open access chapter distributed under the terms of the Creative Commons Attribution License (http://creativecommons.org/licenses/by/3.0), which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

© 2012 The Author(s). Licensee InTech. This chapter is distributed under the terms of the Creative Commons Attribution License http://creativecommons.org/licenses/by/3.0), which permits unrestricted use, distribution,

**Thermodynamics Simulations Applied to** 

**Gas-Solid Materials Fabrication Processes** 

The development and the design of materials and/or the processes of their fabrication are generally very time consumer and with expensive operations. Various methods of development can be conceived. Often, "empirical" approaches are adopted: the choice of the experimental parameters is established either on technological or commercial criteria, the optimization being the results of a "trial and error" approach, or on the results of design of experiments (DOE) approach targeted at a property of a material or a parameter of a very particular process. Another approach is to use process modeling: to simulate the process by a more or less simplified model. The modeling of gas-solid materials fabrication processes brings together several physical and chemical fields with variable complexity, starting from thermodynamics and\or kinetics studies up to the mass and heat transport coupled with

The objective of this chapter is to illustrate the interest areas computer-aided materials design and of processes optimization based on the thermodynamic simulation and giving some interesting examples in different domains. Databases as well as their necessary tools

The thermodynamic simulations of multicomponent systems contribute at two important points: the selection of the material and the optimization of the conditions of fabrication. In order to obtain a finely targeted product which meet specific functionalities, it is necessary




and reproduction in any medium, provided the original work is properly cited.

databases and with thermodynamic and/or kinetics transport properties.

for the implementation of the thermodynamic calculations will be described.

Elisabeth Blanquet and Ioana Nuta

http://dx.doi.org/10.5772/51377

to answer the following questions:

and which operating conditions?

such properties?

**1. Introduction** 

Additional information is available at the end of the chapter


**Chapter 8** 
