Excess enthalpy, volume, and Gibbs free energy of cyclopentane-tetrachloroethylene mixtures at 25.deg.

Polák, Jiří; Murakami, Sachio; Lam, V. T.; Benson, George C.

doi:10.1021/je60045a041

Cited by 32 publications

(8 citation statements)

References 17 publications

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“…These plots yield the relations Figure 6. Back-calculated heat of mixing for the systems: (a) cyclopentane (l)-tetrachloroethylene (2) at 298.15 K (Polak et al, 1970) and acetonitrile (l)-benzene (2) at 318.15 K (Palmer and Smith, 1972); (b) methanol (l)-benzene (2) at 308.15 K (Mrazek and Van Ness, 1961) and methyl acetate (l)-benzene (2) at 308.15 K (Nagata et al, 1973). Results are excellent for both systems in (a), fair for methyl acetate-benzene, and poor for methanol-benzene.…”

Section: Discussionmentioning

confidence: 99%

“…Chlorobutane (l)-carbon tetrachloride (2), 1,2-dichloroethane (l)-carbon tetrachloride (2), and 1,2-dichloroethane (l)-chlorobutane (2): Munoz Embid et al (1990). Cyclopentane (l)-tetrachloroethylene (2): Polak et al (1970). Cyclohexane (l)-aniline (2) and acetone (l)-ethanol (2): Nicolaides and Eckert (1978b).…”

Section: Approachmentioning

confidence: 99%

“…The system cyclopentane (l)-tetrachloroethylene ( 2), for which isothermal VLE and heat of mixing data were available at 298.15 K (Polak et al, 1970), illustrates the degree to which the proposed approach works for simple nonpolar mixtures using three conventional means of representing isothermal binary VLE. Wilson and NRTL parameters were determined from the limiting partial molar excess enthalpies fliE" and 7Í2E", and isothermal VLE were predicted at 298.15 K using each of the four schemes described above.…”

Section: Application Of the Proposed Approachmentioning

confidence: 99%

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Calculation of vapor-liquid equilibria from infinite-dilution excess enthalpy data using the Wilson or NRTL equation

Gow¹

1993

Ind. Eng. Chem. Res.

111

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A study was undertaken to determine the potential for using infinite-dilution excess enthalpy data with activity coefficient models to predict vapor-liquid equilibria for binary systems. Expressions for the infinite-dilution reduced excess enthalpies in a binary liquid mixture derived from the Wilson or NRTL equation with temperature-independent parameters are solved for two unknown model parameters given limiting values of reduced excess enthalpy (partial molar excess enthalpy) IP/x 1X2. The Wilson equation is modified using the van der Waals covolume b in place of the pure-liquid molar volume, and an average value of the nonrandomness factor is chosen to obtain a two-parameter NRTL equation. Vapor-liquid equilibria were predicted for 19 isothermal and 8 isobaric binary systems. Good results are generally obtained for nearly ideal systems using either model; however, the Wilson equation is superior for moderately nonideal systems. The temperatureindependent Wilson model fails to accurately describe vapor-liquid equilibria for strongly nonideal mixtures with highly unsymmetric excess enthalpy profiles. The proposed method appears to be particularly well suited for estimating phase behavior of environmentally safe refrigerant mixtures.

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Section: Discussionmentioning

confidence: 99%

Section: Approachmentioning

confidence: 99%

Section: Application Of the Proposed Approachmentioning

confidence: 99%

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Calculation of vapor-liquid equilibria from infinite-dilution excess enthalpy data using the Wilson or NRTL equation

Gow¹

1993

Ind. Eng. Chem. Res.

111

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“…The method and equipment used in this study were described in earlier articles (8,10). 1 To whom correspondence should be addressed.…”

Section: Methodsmentioning

confidence: 99%

Vapor-liquid equilibriums of methyl propanoate-methanol and methyl propanoate-ethanol systems at 25.deg.

Polák¹,

Lu²

1972

J. Chem. Eng. Data

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The experimental vapor-liquid equilibrium data are presented in Table 11. The liquid-phase activity coefficients were evaluated using the classical thermodynamic relationship: Equation 1 allows for the effect of pressure on the liquid fugacity, and for the nonideality in the gas phase. For the latter, the virial equation was truncated to the second term. Wohl's (5) equation was employed to estimate the values of the second virial coefficients. Volumetric data were taken from the literature. For our systems, the contribution of the second term on the right-hand side of Equation 1 was very small.During the experimental determinations, some difficulty was experienced in establishing the equilibrium pressure. Though pressures could be read accurately, pressure changes of 10-15 mm Hg showed no observable effect on the temperature. This was particularly true for the systems containing di-npropyl ether. The following procedure was therefore adopted to determine the equilibrium pressure. The pressure was deliberately changed in small steps until the measured equilibrium temperature differed from 90°C. This gave pressures corresponding to temperatures of approximately 90 + O.05"CJ and the mean pressure was taken to be the equilibrium pressure a t 90°C.The activity coefficients for these systems are close to unity. Considerable scatter was noted in the activity coefficient data, possibly due, a t least in part, to the uncertainty in pressure. The equilibrium data were compared with ideal values calculated from Pi021 2 P*"Xi Yc = -i = 1,2 and are shown in Figures 2-4. Po = pure component vapor pressure, mm Hg R = gas constant, (mm Hg)(cc)/(g mol)(OK) T = temp,"K u = molal volume, cc/g mol x = mole fraction in liquid y = mole fraction in vapor GREEK LETTERS p = second virial coefficient y = activity coefficient A = total pressure, mm Hg SUBSCRIPTS 1,2,i = component 1, 2, or i SUPERSCRIPT L = liquid LITERATURE CITED (1) American Petroleum Institute, Research Project-44, "Selected Values of Physical and Thermodynamic Properties of Hydrccarbons and Vapor-liquid equi,libria of the systems methyl propanoate-methanol and methyl propanoate-ethanol measured at 25°C are reported along with the results of the volumes of mixing at the same temperature.Vapor-liquid equilibria a t 25°C for the two binary systems, methyl propanoate-methanol and methyl propanoate-ethanol, were measured by a circulation method. The experimental equilibrium pressures and compositions, together with the liquid activity coefficients and excess Gibbs free energies, are presented. The excess volumes of the systems were calculated using the density values obtained by means of a pycnometer a t 25°C. EXPERIMENTALThe method and equipment used in this study were described in earlier articles (8, IO).A circulation still with a total capacity of about 150 ml was used for the determination of vapor-liquid equilibrium compositions. When the temperature of 25°C was obtained in the still head, this temperature was maintained for 3 hr to ensure the establishment of equilibr...

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“…Details of the design and of the operating technique are given in ref. 12. The pressure in the still was measured with a quartz spiral gage (Texas Instruments) which was calibrated by comparison with a mercury manometer.…”

Section: (Ii) Apparatus and Techniquesmentioning

confidence: 99%

Excess enthalpy, volume, and Gibbs free energy of n-propanol – isopropanol mixtures at 25 °C

Polák¹,

Murakami²,

Benson³

et al. 1970

Can. J. Chem.

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Excess enthalpy, volume, and Gibbs free energy of cyclopentane-tetrachloroethylene mixtures at 25.deg.

Cited by 32 publications

References 17 publications

Calculation of vapor-liquid equilibria from infinite-dilution excess enthalpy data using the Wilson or NRTL equation

Calculation of vapor-liquid equilibria from infinite-dilution excess enthalpy data using the Wilson or NRTL equation

Vapor-liquid equilibriums of methyl propanoate-methanol and methyl propanoate-ethanol systems at 25.deg.

Excess enthalpy, volume, and Gibbs free energy of n-propanol – isopropanol mixtures at 25 °C

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