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Journal of Thermodynamics
Volume 2011 (2011), Article ID 945047, 7 pages
Research Article

Corollary from the Exact Expression for Enthalpy of Vaporization

Department of Physics and Chemistry of New Materials, A. M. Prokhorov Academy of Engineering Sciences, 19 Presnensky Val, Moscow 123557, Russia

Received 14 November 2010; Revised 9 March 2011; Accepted 16 March 2011

Academic Editor: K. A. Antonopoulos

Copyright © 2011 A. A. Sobko. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.


A problem on determining effective volumes for atoms and molecules becomes actual due to rapidly developing nanotechnologies. In the present study an exact expression for enthalpy of vaporization is obtained, from which an exact expression is derived for effective volumes of atoms and molecules, and under certain assumptions on the form of an atom (molecule) it is possible to find their linear dimensions. The accuracy is only determined by the accuracy of measurements of thermodynamic parameters at the critical point.

1. Introduction

In the present study, the relationship is obtained that combines the enthalpy of vaporization with other thermodynamic evaporation parameters from the general expression for the heat of first-order phase transformations. A good agreement of the calculated enthalpy of vaporization with experimental data (within the accuracy of the order of several percent) proves the validity of the assumptions made. By using the obtained expression in the Clausius-Clapeyron equation, the relationship between thermodynamic parameters at the critical point is derived, which also well agrees with the experimental data. Also, the expression for determining atomic (ion, molecular) volumes from the thermodynamic parameters is obtained, which, by using geometrical models for atoms and molecules, may predict their linear dimensions.

2. Background

First- and second-order phase transitions are widely investigated, mainly in experiments. In the 1930s, L. D. Landau suggested the phenomenological theory of second-order phase transitions, from which the renormalization group approach and 𝜀-decomposition later were derived. However, by comparing the chapters devoted to first-order phase transitions in the first edition of “Statistical physics,” 1938 [2] with the edition from 1976 [3], we may find them actually similar. we may come to the same conclusion if we compare [2] with recent monograph by Prigogine and Kondepudi “Modern Thermodynamics” [4]. The chapters devoted to first-order phase transitions in both monographs are identical. One may assert that for the last 60–70 years no noticeable progress is observed in the theory of first-order phase transitions. There is a progress in studying critical points which is, however, connected with the fact that at a critical point we have Δ𝑉=0, Δ𝑆=0, that is, it becomes the second-order transition, theory for which, as was mentioned, is well developed.

The heat of a transition is an important characteristic for first-order phase transitions. In 1762, Black [5] was the first who discovered that water transformation to vapor consumes some heat that he called the latent evaporation heat. Then Black has conducted calorimetric investigations of melting ice.

Despite of longer than 200-year existence of the concept of transition heat we have no analytical expressions (except for empirical) binding the transition heat with other phase transfer parameters. For example, in the fundamental encyclopedia [6] the articles devoted to enthalpy of evaporation, enthalpy of melting, and so on include no formulae but only tables with experimental data. Similar situation is observed with other monographs in which, no expressions are given except for the common definition of transition heat 𝜆=𝑇Δ𝑆. This is why obtaining expressions that combine the transition heat with other measurable parameters of a first-order phase transfer would be a substantial contribution into the first-order phase transformations. In monographs [1, 7] a number of expressions are suggested for calculating the enthalpy of evaporation, for example, the Douglas-Avakyan method: Δ𝐻𝑣=𝑇Δ𝑉𝑣(397𝑛𝑃/1512𝛿𝑇𝑛73𝑃/216𝛿𝑇); the Riedel method: Δ𝐻𝑣𝑏=1.093𝑅𝑇𝑐(𝑇𝑏𝑟(ln𝑃𝑐1)/(0.930𝑇𝑏𝑟)); the Chen method: Δ𝐻𝑣𝑏=𝑅𝑇𝑇𝑏𝑟((3.978𝑇𝑏𝑟3.938+1.555ln𝑃𝑐)/(1.07𝑇𝑏𝑟)).

These methods help in the calculation of the enthalpy of evaporation for various complex organic substances with a high accuracy. As shown in [1, Table 6.3], the accuracy is several percent, and in particular, for inert gases the accuracy is 2.1–2.5%. In engineering calculations this is rather satisfactory. But, as P. Dirac noted “Physical law should have mathematical beauty,” which is not the case of the presented expressions. Presently the author is developing the model described below for calculating complex organic compounds.

3. Derivation of the Enthalpy of Evaporation and Comparison with Experimental Data

In [8], the general expression for the heat of first-order phase transitions was derived from the first law of thermodynamics𝜆=𝑇𝑣2𝑣1𝜕𝑆𝜕𝑉𝑇𝑑𝑉+Δ𝐴,or𝜆=𝑇Δ𝑇𝑆+Δ𝐴,(1) where 𝑇 is the transition temperature, Δ𝐴 is the work performed by the system, and 𝑉2𝑉1(𝜕𝑆/𝜕𝑉)𝑇𝑑𝑉, Δ𝑇𝑆 is the entropy variation for the phase transition at constant temperature.

Numerical calculations require that 𝑆(𝑉) is found. The entropy is calculated from the general definition [3]: 𝑆=𝑘ln𝑉ph/(2𝜋)𝑠 and Δ𝑆=𝑘ln(𝑉ph)𝑛/(𝑉ph)𝑜, where 𝑘 is the Boltzmann constant, 𝑉ph is the volume of phase space occupied by the system, 𝑠 is the number of degrees of freedom, Δ𝑆 is the entropy change in the phase transition, (𝑉ph)𝑛 is the phase volume of a new phase, and (𝑉ph)𝑜 is the phase volume for the previous phase.

Thus, the heat of first-order phase transition takes the form𝑉𝜆=𝑘𝑇lnph𝑛𝑉ph𝑜+Δ𝐴.(2) The volumes of phase spaces and expressions for the work are specified for each particular phase transition. In the present paper all calculations are made per one mole of substance, hence, all extensive parameters refer to one mole.

In [9], the approximation method is suggested for calculating the entropy from the general expression 𝑆=𝑘ln𝑉ph/(2𝜋)𝑁, where 𝑉ph is the volume of the phase space for the system.

For liquid and gas states the system energy has the form𝑝2𝑥12𝑚1+𝑝2𝑦12𝑚1+𝑝21𝑧2𝑚1𝑝++2𝑧𝑁2𝑚𝑁𝐫+𝑈1,,𝐫𝑛=𝐸,1𝑛𝑁𝐴.(3)

Since we deal with one mole of single-component sample all the masses are equal and 𝑁=𝑁𝐴 is the Avogadro constant so that the volume of the phase space is 𝑉ph=6𝑁𝑁𝐴𝑛=1𝑑3𝑝𝑛𝑑3𝑟𝑛.

Equation (3) can be written in the form 𝑖𝑛𝑝2𝑖𝑛=(2𝑚(𝐸𝑈(𝐫1,,𝐫𝑛))), which describes a 3N-dimension sphere in 𝐩-space. Hence, the 3N-dimensional integral over pulses 𝐩 is equal to the volume of the sphere of radius (2𝑚(𝐸𝑈(𝐫1,,𝐫𝑛)))1/2, and the expression for the phase space volume takes the form3𝑁𝜋3𝑁/2𝑟(3𝑁/2)!2𝑚𝐸𝑈1,𝑟𝑛𝑁3𝑁/2𝐴𝑛=1𝑑3𝑟.(4)

The integration results in a reduction of the dimension from 6𝑁 to 3𝑁. Nevertheless, it is impossible to take the rest integral without additional assumptions. To approximately take the needed 3𝑁-dimensional integral we will consider the behavior of the distribution function for the kinetic energy of particles near the point of phase transition. Not specifying the particular distribution function we may assert that it has a bell shape with the maximum that moves right with temperature. Near the phase transition point such evolution of the distribution function is impossible because the system temperature is constant and the heat still passes to the system. The only possible variation of the distribution function in this case is its narrowing and transformation to the delta function in the limit 𝑇𝑇ph. In this case the most probable and the mean values of the kinetic energy coincide. This is not a rigorous proof for narrowing the distribution function. However, we can make the basic assumption, which is confirmed by satisfactory agreement between experimental and calculation results: most of atoms (molecules, ions) near the first-order phase transition are in the state with a mean kinetic energy.

Since (𝐸𝑈(𝐫1,,𝐫𝑛)) is the system kinetic energy we, according to the theorem on equal distribution of kinetic energy over degrees of freedom [10], can substitute it with the mean value 3𝑁𝐴𝑘𝑇/2=3𝑅𝑇/2, where 𝑅=𝑘𝑁𝐴 is the absolute gas constant. Then,𝑉ph=3𝑁𝜋3𝑁/23(3𝑁/2)!22𝑚𝑅𝑇𝑁3𝑁/2𝐴𝑛=1𝑑3𝑟𝑛=𝜋3𝑁/2(3𝑁/2)!(2𝑚𝑅𝑇)3𝑁/2𝑉𝑁.(5)

Hence, the volume of the phase space has the form: 𝑉ph𝐿=(3𝜋𝑚𝑅𝑇)3𝑁/2𝑉(3𝑁/2)!𝑁𝐿,𝑉(6)ph𝐺=(3𝜋𝑚𝑅𝑇)3𝑁/2𝑉(3𝑁/2)!𝑁𝐺,(7) where 𝑉𝐿 and 𝑉𝐺 are the volumes of liquid and gas, respectively. The expression for the evaporation heat at the saturation curve can be found from general expression (2). One can see from (6) and (7) that the expressions for the volumes of phase spaces coincide for liquid and gas. One can easily write the expression for the entropy variation in this case:𝑘ln(2𝜋𝑚𝑅𝑇)3𝑁/2𝑉(3𝑁/2)!𝑁,𝜕𝑆𝜕𝑉𝑇=𝑘𝑁𝑉=𝑅𝑉,𝑇𝑣2𝑣1𝑅𝑉𝑉𝑑𝑉=𝑅𝑇ln𝐺𝑉𝐿=𝑅𝑇ln1+Δ𝑉𝑉𝐿,(8) where Δ𝑉 is the volume change, 𝑉𝐿 is the volume of liquid, and 𝑉𝐺 is that of gas.

Work on volume enlarging is 𝐴1=𝑃Δ𝑉. In the liquid-gas transfer in addition to the work on volume enlarging the work is performed against surface tension force 𝐴2=𝜎𝐹𝑁1, where 𝜎 is the surface tension coefficient, 𝐹 is the surface of liquid, 𝑁1=𝑉𝑎/𝐹𝑑 is the number of single-molecular layers, 𝑉𝑎 is the volume occupied by atoms (molecules, ions), 𝑑 is the width of single-molecular layer that in the present paper is, 𝑟 is radius of atom (molecule, ion), and 𝛼=1.717 is the packing index.

Hence, 𝐴2=𝜎𝐹𝑁1=𝜎𝐹𝑉𝑎/𝐹𝑑=𝜎𝑉𝑎/𝛼𝑟.

The expression for evaporation heat along the saturation curve has the form𝜆=𝑅𝑇ln1+Δ𝑉𝑉𝐿+𝑃Δ𝑉+𝜎𝑉𝑎𝛼𝑟.(9) It is not clear which volume of liquid phase 𝑉𝐿 should be used in the calculations, the geometrical volume or “free volume” 𝑉𝑓𝐿=𝑉𝐿𝑉𝑎, where 𝑉𝑎 is the volume occupied by atoms (molecules, ions). This is why the calculations are performed for both the geometrical (experimental) volume and “free volume.” The experimental data on saturation curve were taken from [11], and atomic radii were used from [12]. For the radii of twoatomic molecules we took half the distance between the centers of nuclei [13] plus Van der Waals radii [12]. The results are presented in Table 1.

Table 1: Calculation of evaporation heat.

One can see that the evaporation heat calculated by using the “free volume” noticeably better agrees with the experimental data, hence, the expression for the evaporation heat can be finally written in the form𝜆=𝑅𝑇ln1+Δ𝑉𝑉fL+𝑃Δ𝑉+𝜎𝑉𝑎𝛼𝑟𝑎.(10) Expression (10) includes the term with a surface tension coefficient. A contribution of the term into the enthalpy of evaporation is on the order of 10%. Unfortunately, the author has no data on the surface tension coefficient in the interval from the triple to boiling point for most of substances, and the results for only several values of the enthalpy of evaporation are given in the table. For hydrogen, the surface tension coefficient is known over the whole interval from the triple to boiling point, which gives a possibility to draw a temperature dependence for the enthalpy of evaporation. The result is shown in Figure 1.

Figure 1: Temperature dependence of the experimental enthalpy of evaporation 𝜆exp=𝑓1(𝑇) and calculated enthalpy of evaporation 𝜆cal=𝑓2(𝑇) for hydrogen.

As one can see, the experimental values of enthalpy of evaporation well agree with those calculated by formula (10). A distinction at low temperatures is explained by that at those temperatures the calculation of the phase space volume should take into account quantum corrections.

Note that, in [14], the method used above gives a good agreement between calculated and experimental values for the enthalpy of fusion.

4. Conclusion and Test of the Relationship Binding Critical Parameters

The Clausius-Clapeyron equation𝑑𝑃=𝑑𝑇Δ𝑆=𝜆Δ𝑉𝑇Δ𝑉(11) is rigorously derived from thermodynamic relationships and experimentally verified. Expression (10) for the evaporation heat is also sufficiently rigorously obtained, and the calculation results agree with the experimental data. Hence, by substituting (10) into (11) and passing to the critical point limit Δ𝑉0 we obtain the relationship between the thermodynamic parameters at a critical point 𝑑𝑃=𝑑𝑇𝑅𝑇𝑇Δ𝑉ln1+Δ𝑉𝑉fL+𝑃Δ𝑉+𝑇Δ𝑉𝜎𝑉𝑎𝛼𝑟𝑎,=𝑅𝑇Δ𝑉Δ𝑉ln1+Δ𝑉𝑉fL+𝑃𝑇+𝜎𝑉𝑎𝛼𝑟𝑎,𝑇Δ𝑉limΔ𝑉0𝑑𝑃𝑑𝑇=limΔ𝑉0𝑅Δ𝑉ln1+Δ𝑉𝑉fL+limΔ𝑉0𝑃𝑇+limΔ𝑉0𝜎𝑉𝑎𝛼𝑟𝑎,𝑇Δ𝑉limΔ𝑉0𝑑𝑃=𝑑𝑇𝑑𝑃𝑑𝑇𝑐,limΔ𝑉0𝑃𝑇=𝑃𝑐𝑇𝑐,limΔ𝑉0𝑅Δ𝑉ln1+Δ𝑉𝑉fL=limΔ𝑉0𝑅Δ𝑉Δ𝑉𝑉fL=limΔ𝑉0𝑅𝑉fL=𝑅𝑉c,limΔ𝑉0𝜎𝑉𝑎𝛼𝑟𝑎𝑇Δ𝑉=0.(12)

The latter statement can be proved. As was shown [15] near the critical point we have 𝜎𝜎0(1𝑇/𝑇𝑐)3/2 and (see [4]) Δ𝑉(1(𝑇/𝑇𝑐))𝛽, where the theoretical value is 𝛽=1/2 and experimental values are 𝛽=0.30.4. Thus, we have limΔ𝑉0𝜎𝑉𝑎𝛼𝑟𝑎=𝜎𝑇Δ𝑉0𝑉𝑎𝛼𝑟𝑎lim𝑇𝑇𝑐1𝑇/𝑇𝑐3/2𝑇1𝑇/𝑇𝑐𝛽=0.(13) At the critical point the following relationship should hold:𝑑𝑃𝑑𝑇𝑐=𝑅𝑉fLc+𝑃𝑐𝑇𝑐.(14) Subscript 𝑐 indicates that all the thermodynamic parameters are taken at the critical point.

Formula (14) is rigorously obtained from the exact Clausius-Clapeyron equation and (10) that is confirmed by a good description for the evaporation heat. However, it is worth verifying for particular substances. We can calculate the derivative (𝑑𝑃/𝑑𝑇)𝑐,𝑇 from experimental data [1113] by using formula (14) and from expression (𝑑𝑃/𝑑𝑇)𝑐,ex=(𝑃c𝑃1)/(𝑇𝑐𝑇1), where 𝑃1, 𝑇1 are experimental pressure and temperature closest to the critical point on the equilibrium curve. A good agreement between the derivatives (𝑑𝑃/𝑑𝑇)𝑐,𝑇 and (𝑑𝑃/𝑑𝑇)𝑐,ex will be an argument for the validity of (14). The calculation results are presented in Table 2.

Table 2: Experimental and calculated values for derivatives.

Small deviations in the values of derivatives (on the order of several percent) are explained by an insufficient measurement accuracy near the critical point and by approximate character for values of molecule radii. For example, the values of atomic radii given in [16] and calculated by eight various authors differ by several percent and even by 10 or more percent.

5. Definition of Volumes and the Linear Sizes of Atoms and Molecules

Formula (14) whose validity was rigorously proved and experimentally verified includes the “free” system critical volume 𝑉fc=𝑉𝑐𝑁A𝑉0, where 𝑉𝑐 is the experimental value for the critical volume, 𝑁𝐴=6.021023 is the Avogadro constant, and 𝑉0 is the volume of atom (molecule, ion). Hence, one can obtain the following formula for determining the effective volumes of atoms (molecules, ions) via the thermodynamic parameters at a critical point:𝑉0=1𝑁𝐴𝑉𝑐𝑅(𝑑𝑃/𝑑𝑇)𝑐𝑃𝑐/𝑇𝑐.(15) By using geometrical models for atoms (molecules) one can calculate their linear parameters.

5.1. Spherical Model

Spherical model is adequate to noble gases, alkali metal ions, CH4 and NH3 molecules due to smallness of hydrogen atoms. The corresponding atomic (molecular) radii can be found by using (15) from the relationship 𝑉0=(4/3)𝜋𝑟3 or 𝑟=33𝑉0/4𝜋. The constant 𝑏=𝑉𝑐/3 in Van der Waals equation is treated as the volume occupied by molecules, and the effective radii in the spherical Van der Waals model can be calculated by the formula 𝑟𝑊=3𝑉𝑐/4𝜋𝑁𝐴. These results are presented in Table 3.

Table 3: Volumes and radii of molecules in spherical model.

One can see from Table 3 that the results calculated by formula (15) well agree with the reference data; however, they are more reliable because most of methods for determining molecule dimensions are approximate whereas the method suggested is accurate and its accuracy is only determined by the measurement accuracy for the thermodynamic parameters at a critical point.

5.2. Ellipsoidal Model

For twoatomic molecules that are symmetric and for those combined from the atoms of close dimensions the ellipsoid of revolution can be suggested as the geometrical model:𝑥2𝑎2+𝑦2𝑏2+𝑧2𝑏2=1.(16) The volume of the ellipsoid of revolution is 𝑉0=(4/3)𝜋𝑎𝑏2=(4/3)𝜋(𝑎2𝑐2)𝑎, where 2𝑐 is the distance between the atomic centers taken from [13]. The volume 𝑉0 is calculated by formula (14). Thus, the equation for finding the major semiaxis takes the form𝑎3𝑐2𝑎3𝑉04𝜋=0.(17) As expected, the equation parameters are so that there is one real solution and two complex solutions. The equation assumes an analytical solution [17], namely, sin(𝜔)=8𝜋𝑐393𝑉0,𝑡𝑔(𝜑)=3𝜔𝑡𝑔2,𝑎=2𝑐.3sin(2𝜑)(18) By using 𝑎 one can find 𝑏=𝑎2𝑐2. The calculation results are given in Table 4.

Table 4: Volumes and linear dimensions for twoatomic molecules in ellipsoidal model.

For the model of twoatomic molecules one can also suggest the body of revolution formed by the Cassinian oval:𝑥2+𝑦222𝑐2𝑥2𝑦2𝑑4𝑐4=0,(19) where 𝑑2 is the product of the distances from the centers to an arbitrary point on the curve, and 2𝑐 is the distance between the atomic centers. The obtained body of revolution, in contrast to an ellipsoid that has a convex surface, may have a dumbbell shape with a “waist” at 𝑐<𝑑<2. At 𝑑<𝑐 it may transfer to two ovals, which can be interpreted as two atoms of the molecule separated by large distance. The results of calculations in the case of Cassinian oval do not noticeably differ from those in the case of ellipsoidal model.

In Table 5, the values of calculated evaporation heat are presented obtained by using the data on molecule volumes and linear dimensions given above.

Table 5: Calculation results for evaporation heat.

As one can see from Table 5, employment of the results obtained in the present work gives, generally, better agreement between the calculated and experimental enthalpy of evaporation.

6. Conclusions

(1)The evaporation heat is determined by expression (9): 𝜆=𝑅𝑇ln1+Δ𝑉𝑉fL+𝑃Δ𝑉+𝜎𝑉𝑎𝛼𝑟𝑎.(20)(2)At a critical point the thermodynamic parameters should satisfy relationship (14) 𝑑𝑃𝑑𝑇𝑐=𝑅𝑉fLc+𝑃𝑐𝑇𝑐.(21)(3)The effective volumes of atoms (molecules, ions) are calculated from exact formula (15) 𝑉0=1𝑁𝐴𝑉𝑐𝑅(𝑑𝑃/𝑑𝑇)𝑐𝑃𝑐/𝑇𝑐.(22) The volume calculation accuracy is only determined by the measurement accuracy for the thermodynamic parameters at the critical point. By using geometrical models for atoms (molecules, ions) one can determine their linear parameters as well.(4)Rapid development of nanotechnology necessitates accurate determination of geometrical parameters for atoms (molecules, ions), which can be made by means of the method suggested.


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