Avsec, J.

Marcic, M.

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Purdue UniversityPurdue e-PubsInternational Refrigeration and Air ConditioningConference School of Mechanical Engineering1998The Calculation of the Compressibility, ThermalExpansion Coefficient and the Determination theEvaporation Curve for Some ImportantRefrigerantsJ. AvsecUniversity of MariborM. MarcicUniversity of MariborFollow this and additional works at: http://docs.lib.purdue.edu/iraccThis document has been made available through Purdue e-Pubs, a service of the Purdue University Libraries. Please contact epubs@purdue.edu foradditional information.Complete proceedings may be acquired in print and on CD-ROM directly from the Ray W. Herrick Laboratories at https://engineering.purdue.edu/Herrick/Events/orderlit.htmlAvsec, J. and Marcic, M., "The Calculation of the Compressibility, Thermal Expansion Coefficient and the Determination theEvaporation Curve for Some Important Refrigerants" (1998). International Refrigeration and Air Conditioning Conference. Paper 425.http://docs.lib.purdue.edu/iracc/425THE CALCULATION OF THE COMPRESSmiLITY, THERMAL EXPANSION COEFFICIENT AND mE DETERMINATION THE EVAPORATION CURVE FOR SOME IMPORTANT REFRIGERANTS J. Avsec, M. Marcie University ofMaribor, Faculty of Mechanical Engineering,, Smetanova 17, 2000 Marihor, P.O. BOX 224, SLOVENIA ABSTRACT: The paper presents the mathematical model of computating the compessibility, thermal expansion coefficient, evaporation curve, velocity of sound and other thermophysical properties by means of statistical thermodynamics for some imortant refrigerants. The paper features all important forms of motion of molecules and atoms [translation, rotation, internal rotation, vibration], the influence of excitation of electrons and nuclei into higher energy levels as well as the effect of the intermolecular potential energy. Utilized as the intermolecular potential was the Lennard -Jones potential. To computate the thermodynamic values of the state in the realm of real fluids we used grand canonical distribution. For the realm of real fluids Johnson-Zollweg-Gubbins model based on the modified BWR and great number of Monte Carlo simulations was applied. For the calculation in two- phase region we applied the method of equilibrium conditions between two phases. The mathematical model enables the calculation in both sub-and supercritical region. By means of the mathematical model described above we were able to compute thermodynamical properties in one and two-phase region and to draw phase diagrams for some technically significant substances. The results of the analysis are compared with data on experiments showing a relatively good agreement. INTRODUCTION In refrigeration processes in liquid-gas region are of vital importance. In order to design devices for this field of activity, it is necessary to be familiar with the thermodynamic properties of state in a one-phase and two-phase environment. In most cases the thermodynamic tables and diagrams and different empirical functions obtained from measurements are used. Calculation of thermodynamic properties of state is possible by the claasical or statistical thermodynamics. Classical thermodynamics has no insight into the microstructure, but it allows the calculation of thermodynamic function of state with assistance of macroscopic observation of phenomenons. Unlike the classical thermodynamics, however, the statistical thermodynamics does enable the computation of the thermodynamic functions of the state by studying molecular structure of the matter. COMPUTATION OF THERMODYNAMIC PROPERTIES OF STATE To calculate thermodynamic functions of state we applied the canonical partitition (Lucas, 1992). Utilazing the semi-classical formulation for the purpose of the canonical ensemble for the N indistiguishable molecules can be expressed as follows (Lucas, 1992): Z==~J .. Jexi _..!!_)·dr1dr2 •• drNdp1dp2 .• dpN "(I) N!h l kT where f stands for the number of degrees of freedom of individual molecule, H designates the Hamiltonian molecule system. By means of the canonical ensemble for the system of N molecules can be like this: Z == ZoZtranszvibzrotzirzeiZnuczconf (2) 289 Thus the partition function Z is a product of terms of the ground state (0), the translation (trans), the vibration (vib), the rotation (rot), the internal rotation (ir),the influence of electrons excitation (el), the influence of nuclei excitation (nuc) and the influence of the potential intermolecular energy (con:f). Utilizing the canonical theory for computating the thermodynamic functions of the state can be put as follows (Smimova, 1983; Gray and Gubbins, 1984) Pressure: p = kT --(alnZ) av v Free energy: A= -kT ·ln Z Free enthalpy: G = -kT[ ln Z- v( a!; Z l], Internal energy: U = kT2 (a 1n z ) l ar v Entropy:S = k[ lnZ+T(a!~z l J J (alnZ) (atnzj] Enthalpy: H = k A l T l aT v + V l--ay Jr . (3) The computation of the individual terms of the partition function and their derivatives with the exception of the configuration integral is dealt with in the works of Lucas, 1992; Gray and Gubbins, 1984. The various derivatives and expressions of the fundamental equations (3) have an important physical significance. These paper presents expressions which are very important for planning the refi:igeration processes. The coefficient of thermal expansion: The isothermal compressibility: The heat capacity at contant volume per mole: The heat capacity at constant pressure per mole: ~=_!_(av) v ar p c =(au) v ar v c =-(aH 1 P ar k (4) The velocity of the mechanical longitudinal waves propagation between 16 s-1 and 20000 s-1 we call the velocity of sound (Gommon 1976). The calculation the speed of sound is very important in measurement (acoustic resonance level gauge. In real fluids we can calculate the isentropic speed of sound Co (Bird 1954, Younglove 1993): (5) In equation (5) is v specific volume and cp spcific heat capacity. 290 CONFIGURATIONAL INTEGRAL In the realm of real fluid Johnson-Zollweg-Gubbins (1993) model based on molecular dynamic and Monte Carlo simulations with help of Lennard-lones intermolecular potential and modified Benedict-Web-Rubin equation of state (MBWR) was used. On these basis we can express configurational free energy Aeon£: 8 *i 6 • ~ a-p ~ Aconf :::: ""-.t-~-. -+ L,;biGi' i=l I i=l (5) T* = kT ' £ A •- Aeon£ conf - NE (6) F = exp(- YP *2 ) , y=3 Table 1: oe Icients or c fi . fi MBWR f equation o state i a; b· I G; I . R . *2 *2 •3 (1 - F )1(2y) x 1T +x2 T +x 3 +x 4 1T +x5 1T x 20 IT + x 21 IT 2 * * *2 x 6T +x7 +x8 IT +x9 IT *2 *4 x 22 IT +x23 IT - Fp*2 -2G1 1(2y) 3 XIO T* +Xu + xl2 IT* *2 *3 x241T +X2siT -~ Fp'4 -4G2 l1(2y) 4 xu *2 *4 x26 IT +x27 IT -~ Fp*6 -6G3/(2y) 5 • *2 *2 *3 Fp •s- 8G4 1(2y) xt4T +xlsiT x28 IT +x 29 IT -6 xl6 IT* *2 *3 *4 x30 IT + x 31 IT + x32 IT -(Fp*10 -IOG 5 )1(2y) 7 • *2 x 17 IT +x18 IT 8 x 19 IT *2 The equation (5) accurately correlates thermophysical properties from 0.7 :5 r* :56. In equation (5) are xi's the sdjustable parameters in the equation of state. The equation (5) is especially accurate for vapour-liquid equilibrium conditions. DETERMINING THE EQUILIBRIUM STATES BETWEEN VAPOUR AND LIQUID Determining the equilibrium states between the liquid and the gasous phases conditions for equlibrium are applied: T' = T", p' = p", 1-1.' = 1-1.", (7) where ' in equation (7) means the liquid phase, " means the gaseous phase, J.1. constitutes the chemical potential. Due to complexity of the equations in the presented mathematical model the states on the coexistence curve are obtained on the numerical basis. By applying these states, thermodynamic properties in the two phase environment can be calculated. 291 1-T=l66K 4-T=222K 160 120 RESULTS AND COMPARISSON WITH EXPERIMENTAL DATA 2-T=188 K 3-T=210K 5-T=255K &-T=282K V [m3/kmol] ....... = 1E+7r--------~----.. E::. IE+6 c. 80 1E+:5~---.-----.---r---.---.---""T"-~ 0.01 0.1 100 160 200 T{K) 240 280 · Figure 1: Entropy and vapour pressure in one- and two- phase region for C2IL (R-1150) Table 2: The comparisson between the analytical calculation (Simul) and the experimental data (Exp) for argon (Rw740 ) in the region of compressed liquid T v p Cv cp X Co K ml/ :MPa kJikmolK kJikmolK Gpa·• mls lonol Simul. Exp. Simul EXJ>. Simul. Exp. Simul. ~-Simul. ~!Q. llO .0317 4.65 4.5 17.7 18.9 43.3 45.6 4.09 3.42 678 701 200 .0329 110 100 17.1 17.8 32.1 34:5 2.39 804 851 300 .1187 22 20 13.3 13.8 28.0 30.5 40.40 42.96 386 371 300 .0521 63 60 14.3 14.9 29.1 32.4 7.99 574 570 300 .0412 110 100 15.1 15.7 29.4 31.0 3.8 3.72 716 731 400 .0507 106 100 14.1 14.6 26.3 26.8 4.9 685 689 500 .0602 105 100 13.6 14.1 24.9 26.4 5.9 685 683 600 .0702 110 100 13.3 13.7 23.4 25.0 5.4 755 731 Table 3: The comparisson between the analytical calculation (Simul) and the experimental data (Exp) for carbon d ioxide rn • 144) in the ree:ion of boiling liquid T v p cp 13 K m3/kmol bar kJikmolK 1/K Simul. E~. Simul. Exp. Simul. Exp. 253 .04253 1.62 1.96 902 94.7 0.0037 263 .04465 2.82 2.64 94.4 98.8 0.0052 273 .04753 3.33 3.48 105.6 106.0 0.0072 0.0080 283 .05102 4.26 4.49 118.2 126.8 0.0114 293 .05683 5.41 5.72 213.2 216.2 0.0159 0.0014 298 .06186 6.52 6.43 407.5 445.8 0.0017 292 Table 4: The comparisson between the analytical calculation (Simul) and the experimental data (Exp.) for carbon dioxide (R-744) · th · f d m e regwn o saturate vapour T v p Co K m31kmol bar m/s Simul. Exp. Simul. E~ 223 2.432 7.11 6.83 226.7 223.6 233 1.667 10.58 8.9 227.5 224.2 243 1.144 15.52 14.3 226.9 222.9 253 0.843 21.10 19.7 223.5 220.8 263 0.613 27.82 26.5 219.3 217.5 273 0.448 36.37 34.8 214.4 212.7 283 0.325 47.20 44.9 209.9 206.3 293 0.228 61.7 57.3 203.7 197.9 301 0.155 76.5 73.7 194.1 189.8 Table 5:The comparisson between the analytical calculation (Simul.) and the experimental data (Exp) for diflo urdichlormethane R -12) in the region of superheated vapour 10 bar 20 bar T v H s v H s K m31krnol kJ!kmol kJ/kmolK m3/kmol kJikrnol kJ/kmolK 373 Simul. 2.81 29120 97.1 1.25 28440 91.0 Exp 2.79 29936 97.9 1.21 28646 89.6 423 Simul. 3.30 36900 106.1 1.55 35380 105.4 Exp 3.29 34637 109.1 1.53 33358 101.8 473 Simul. 1.82 40840 114.1 Exp. 1.79 38274 104.5 Figure I features the graphic course of thermodynamic functions of the state computated by means of the mathematical model. The values presented the liquid, gas and two-phase regions. The results presented feature ethylene (C2If.t). The constants necessary for the computation like the characteristic rotation-, vibration-, electronic etc. temperatures are obtained by means of experimental data (Herzberg,I966; Herzberg,1984; Bellamy). The inertia moments are obtained analytically applying the know-how of atomic structure of the molecule. Constants for Lennard-Janes potential are obtained from literature of Gray 1984, Bird 1954 and Lucas 1992. Similarly as with athylene (R-1150), the analytical calculation was also carried out for argon (R-740), diflourdichlormethane (R-12), and carbon dixide (R-744) . The comparisson of our analytical (Simul) with experimental resoults (Exp) by Maxwell1955, Edmister 1964, Ecker & Drake 1959 and Petrak 1993, 1980, Ashrae Refrigerant Tables and Chart, 1985; Ermakova at al., Younglove 1995, are presented in the tables 2,3,4,5. Table 2 shows The comparisson between the analytical calculation and the experimental data for argon (R-740) in the region of liquid. Tables 3 and 4 show the deviation of the results for carbon dioxide between the analytical computation with help of statistical thermodynamics and experimental data. Table 5 shows the deviation of the results for diflourdichlormethane (R-12) for the real gas region between the analytical computation and the experimental values. The results show relatively good harmony. In the region of real gases (Tables 4,5) the results are an equally good match. Somewhat larger deviations can howewer be found in the region of real liquid (Table 2,3) due to the large influence of the attraction forces, whereas the Lennard-Janes potential is a crude simplification 293 NOMENCLATURE A free energy s entropy Co velocity of soWld T temperature Cv heat capacity at contant volume per mole u internal energy Cp specific heat capacity at constant pressure v specific volume CP heat capacity at contant pressure per mole v volume E potential energy z partition function G free enthalpy ~ coefficient of thermal expansion H enthalpy, hamiltonian Jl chemical potential k Boltzmann consstant X isothermal compressibility N number of molecules in system p density p pressure, momentum Superscripts and subscripts 0 groWld state pot potential energy conf configuration rot rotation el influence of electron excitation trans translation rr internal rotation vib vibration nuc influence of nuclear excitation REFERENCES Ashrae Refrigerant Tables and Charts, 1985, Atlanta Bellamy, L.J., 1980 The Infrared Spectra of Complex Molecules, Chapman & Hall, London, Bird, L., 1954. Molecular Theory of Gases and Liquids, John Willey & Sons, Eckert, R.L., Drake, R.M., 1959, Heat and Mass Transfer, McGraw-Hill Company, New York Edmister, W.C., Lee B. L, 1964. Hydrocarbon Thermodynamics 1,11, GulfPublishing Company, 1964, London Gammon, B.E., Douslin D.R., 1976, J.Chem. Phys. 64:203 Ermakova E., Solca J., Huber H. Marc Welker, Argon in condensed phase, The Journal of Chemical Physics, VoL 102, No.12, 1995 Gray, C.G., Gubbins, K.E., 1984. Theory of Molecular Fluids, Clarendon Press, Oxford Herzberg G., 1966. Electronic Spectra of Polyatomic Molecules, Van Nostrand Reinhold Company, 1966, London. Toronto, Melbourne Herzberg, G., 1984. Infrared and Raman Spectra of Polyatomic molecules, Van Nostrand Reinhold Company, New York Johnson, J.K., Zollweg, J.A., Gubbins K.E., The Lennard-Janes equation of state revisited, Molecular Physics, 1993, 78:591 Lucas, K., 1992. Applied Statistical Thermodynamics, Springer- Verlag, New York Maxwell, J.B., 1955. Data Book on Hydrocarbons, Van Nostrand Company, New York McClelland, B.J., 1980. Statistical Thermodynamics, Chapman & Hall, London Reichl, L.E., 1990. A Modem Course in Statistical Physics, University in Texas Petrak, J., Ludek, L., Termokinetic properties ofrefrigerants, 1993, Faculty ofMechanical Engineering, Praha Smimova, N.A., 1982. Methods of the Statistical thermodynamics in the Physical Chemistry, University of Moscow, Moscow YoWlglove, B.A., Frederick, N.V., McCarthy, R.D., Speed ofsoWld Data and Related Models for Mixtures ofNatural Gas Constituents, 1993, NIST, Washington 294 

The Calculation of the Compressibility, Thermal Expansion Coefficient and the Determination the Evaporation Curve for Some Important Refrigerants

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The Calculation of the Compressibility, Thermal Expansion Coefficient and the Determination the Evaporation Curve for Some Important Refrigerants

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