8_-_Experimental_investigation_of_the_vaporâ€“liquid_equ ilibrium at 313.15 K of the ternary system tert-amylmethyl_ether_(TAME)_+_n-heptane_+methanol

7/26/2019 8_-_Experimental_investigation_of_the_vaporliquid_equ ilibrium at 313.15 K of the ternary system tert-amylme

1/12

.Fluid Phase Equilibria 165 1999 197208

www.elsevier.nlrlocaterfluid

Experimental investigation of the vaporliquid equilibrium at 313.15K of the ternary system tert-amylmethyl ether

. 1TAME q n-heptane q methanol

Cesar R. Chamorro, Jose J. Segovia, Mara C. Martn, Miguel A. Villamanan ) Laboratorio de Termodinamica, Depto. Ingeniera Energetica y Fluidomecanica, E.T.S. de Ingenieros Industriales,

Uniersidad de Valladolid, E-47071, Valladolid, Spain

Received 12 October 1998; accepted 29 June 1999

Abstract

.Experimental isothermal Px data at 313.15 K for the ternary system tert-amylmethyl ether TAME q n-. heptaneq methanol and for one of the unmeasured constituent binary systems, tert-amylmethyl ether

. . ETAME q methanol are reported. Data reduction by Barkers method provides correlations for g using the

Margules equation for the binary systems and the Wohl expansion for the ternary system. Wilson, NRTL and

UNIQUAC models have been applied successfully to both the binary and the ternary systems. The presence of

azeotropes in the ternary system and constituent binaries are studied as well as the presence of immiscible

zones. q 1999 Elsevier Science B.V. All rights reserved.

Keywords:Data; VLE low pressure; Hydrocarbons; TAME; Excess Gibbs energy; Azeotropes; Correlations

1. Introduction

. .tert-amylmethyl ether TAME complements the use of methyl tert-butyl ether MTBE as analternative oxygenate additive in unleaded gasolines. This work will contribute with an experimental

.investigation of the thermodynamic parameters of VaporLiquid Equilibrium VLE at 313.15 K ofthe ternary system TAME q n-heptaneq methanol and the binary system TAME q methanol.

Methanol is present in the catalytic reaction to synthesize TAME from the isoolefine isopentene.

To design separation processes properly in the purification of TAME from methanol impurities,acurate VLE data are necessary. Thermodynamic phase behaviour of both components with gasoline

)

Corresponding author. Tel.: q34-983-423-364; fax:q34-983-423-363; e-mail: [email protected]

This paper is part of the Doctoral Thesis of C.R. Chamorro.

0378-3812r99r$ - see front matter q 1999 Elsevier Science B.V. All rights reserved. .P I I : S 0 3 7 8 - 3 8 1 2 9 9 0 0 2 6 8 - X


2/12

( )C.R. Chamorro et al.r Fluid Phase Equilibria 165 1999 197208198

hydrocarbons, represented here in a qualitative way by n-heptane, requires VLE equilibriummeasurements of the corresponding generated ternary system whose data are reported here Chamorro

w x w x. w x1 , Chamorro et al. 2 . A similar study has been done by our group concerning MTBE Segovia 3 ,w x.Segovia et al. 48 .

2. Materials

All the chemicals used here were purchased from Fluka Chemie and were of the highest purity .available, chromatography quality reagents of the series puriss. p.a. with a stated purity ) 97.0%

. . .GC for TAME, ) 99.5% GC for n-heptane and ) 99.8% GC for methanol. Only TAME wasdistilled, at atmospheric pressure, through a packed column, the first and last portions of the distillatewere discarded and the intermediate fraction distilling at constant temperature was collected.

All reagents were thoroughly degassed using a modified distillation method based on the onew xsuggested by Van Ness and Abbott 9 . The purity of the products after degassing was checked in our

.laboratory by gas chromatography, and the values obtained were ) 99.8% GC for all thecompounds.

In Table 1, the vapor pressures of the pure constituents measured in this work are compared withthose reported in the literature to check for complete degassing.

Table 1 sat.Average values of experimental vapor pressures P for the pure compounds measured in this work and literature valuesi

sat. . L . .P lit. , molar volumes of pure liquids V and the second virial coefficients B , B at 313.15 K used for the datai i ii i jreduction of the measured systems

. . .TAME is1 n-Heptane is 2 Methanol is3

sat .P kPa 19.567 12.351 35.463isat a c c . .P lit kPa 19.587 12.331 35.475i

b d f19.540 12.348 35.431e a12.335 35.445f h12.300 35.453g i12.363 35.470

L 3 j j j .V cm rmol 136 150 42ik k kB y1988 y2211 y923i1k k kB y2211 y2521 y622i2

k k kB y923 y622 y1964i3

a w xReported by Toghiani et al. 28 .b w xCalculated from the Antoine equation using constants reported by Cervenkova and Boublik 29 .c w xReported by Segovia 3 .d w xReported by Montero 30 .e w xCalculated from the Antoine equation using constants reported in Ref. 31 .f w xCalculated from the Antoine equation using constants reported by Reid et al. 32 .g w xReported by Reid et al. 33 .h w xReported by Goral et al. 34 .i w xReported by Boublik et al. 35 .

j w xReported in Ref. 36 .k w x w xCalculated by Hayden and OConnell 18 from Dymond and Smith 19 .


3/12

( )C.R. Chamorro et al.r Fluid Phase Equilibria 165 1999 197208 199

3. Experimental method

A static VLE apparatus, consisting of an isothermal total pressure cell, has been employed formeasuring the VLE of binary and ternary mixtures. The apparatus and measuring technique are based

w x w x.on that by Van Ness et al. Gibbs and Van Ness 10 ; DiElsi et al. 11 and whose performance has w x.been described in a previous paper Lozano et al. 12 .

3

.The piston injectors are three 100-cm positive displacement pumps Ruska, mod. 2200-801 witha resolution of 0.01 cm3 and an estimated total uncertainty of "0.03 cm3, allow the injection ofknown volumes of the pure components, previously degassed, into the cell immersed in a high

.precision water bath Hart Scientific model 6020 assuring an stability of 0.5 mK and thermostated at313.15 K.

The cell is a cylindrical stainless steel piece with a capacity of about 180 cm 3 and provided with amagnetic stirrer externally operated. An initial amount of about 50 cm 3 of one component is injectedinto the evacuated cell, the vapor pressure is recorded, and successive increases in composition of asecond or a third component are generated until we nearly fill the cell completing a desiredcomposition range. The total amount of mass injected is accurately determined from the volumedifferences read between two stop-points of the piston, the temperature of the injector and the value of

the density for that pure component allowing us assuring four digits in the value of the mole fraction.The stop-point for advancing the piston is in all cases determined by an accurate break-point torquewrench, set to overbalance the frictional effect of the packing around the piston.

Experimental values of total vapor pressure for the binary mixtures were obtained with twodifferent runs, the first one adding the second component to the first one up to a concentration close tox s 0.4, and the second run adding the first component to the second one up to x s 0.6, completing1 1in this way the whole concentration range. For the ternary mixtures data were obtained by addition of

.a pure species to a mixture of the other two at a fixed temperature. Six runs dilution lines were donestarting the corresponding binary system at mole fractions close to 0.3 or 0.7 and adding the thirdpure component up to a mole fraction of 0.5.

Table 2 . ..Total-pressure VLE data for TAME 1 qmethanol 2 at 313.15 K

. .x y P kPa x y P kPa1 1,calc 1 1,calc

0.0000 0.0000 35.467 0.5003 0.3550 39.066

0.0487 0.0967 37.574 0.5498 0.3722 38.598

0.1002 0.1616 38.860 0.5504 0.3724 38.603

0.1506 0.2055 39.555 0.5977 0.3897 38.048

0.1989 0.2368 39.910 0.6006 0.3908 38.019

0.2493 0.2628 40.060 0.6508 0.4111 37.296

0.2996 0.2845 40.061 0.6988 0.4332 36.433

0.3499 0.3036 39.939 0.7466 0.4595 35.376

0.3990 0.3209 39.751 0.7997 0.4968 33.822

0.3999 0.3212 39.740 0.8469 0.5419 31.998

0.4496 0.3380 39.456 0.9003 0.6186 29.113

0.4498 0.3381 39.459 0.9494 0.7396 25.353

0.4995 0.3548 39.082 1.0000 1.0000 19.573


4/12


Table 3 . . ..Total-pressure VLE data for TAME 1 q n-heptane 2 qmethanol 3 at 313.15 K

.x x y y P kPa1 2 1,calc 2,calc

1.0000 0.0000 1.0000 0.0000 19.561

0.6981 0.3019 0.7732 0.2268 17.923

0.6780 0.2932 0.5753 0.1762 23.564

0.6603 0.2856 0.4845 0.1539 27.088

0.6275 0.2714 0.3927 0.1327 31.527

0.5943 0.2570 0.3424 0.1226 34.351

0.5584 0.2415 0.3086 0.1170 36.379

0.5220 0.2257 0.2849 0.1142 37.809

0.4884 0.2112 0.2681 0.1127 38.788

0.4528 0.1958 0.2531 0.1119 39.596

0.4186 0.1810 0.2403 0.1116 40.208

0.3835 0.1658 0.2281 0.1115 40.724

0.3497 0.1512 0.2168 0.1117 41.134

0.0000 1.0000 0.0000 1.0000 12.348

0.3008 0.6992 0.4202 0.5798 15.148

0.2940 0.6836 0.2494 0.3621 24.709

0.2888 0.6714 0.2016 0.3032 29.3790.2750 0.6392 0.1507 0.2444 35.647

0.2564 0.5959 0.1265 0.2216 39.226

0.2398 0.5573 0.1156 0.2145 40.850

0.2258 0.5248 0.1091 0.2117 41.715

0.2111 0.4908 0.1035 0.2103 42.350

0.1960 0.4556 0.0983 0.2095 42.840

0.1809 0.4204 0.0934 0.2090 43.187

0.1655 0.3846 0.0886 0.2084 43.472

0.1504 0.3497 0.0840 0.2077 43.694

1.0000 0.0000 1.0000 0.0000 19.565

0.7023 0.0000 0.4349 0.0000 36.338

0.6859 0.0234 0.4186 0.0141 36.444

0.6670 0.0505 0.4004 0.0297 36.5620.6303 0.1028 0.3671 0.0576 36.770

0.5966 0.1508 0.3389 0.0807 36.926

0.5619 0.2003 0.3118 0.1022 37.074

0.5267 0.2505 0.2864 0.1219 37.214

0.4914 0.3007 0.2626 0.1399 37.332

0.4562 0.3508 0.2403 0.1563 37.439

0.4209 0.4011 0.2192 0.1716 37.529

0.3860 0.4507 0.1994 0.1859 37.597

0.3510 0.5005 0.1803 0.1995 37.647

0.0000 0.0000 0.0000 0.0000 35.467

0.3046 0.0000 0.2864 0.0000 40.048

0.2970 0.0252 0.2580 0.0355 40.641

0.2896 0.0498 0.2353 0.0628 41.074

0.2745 0.0996 0.1998 0.1031 41.706

0.2590 0.1505 0.1732 0.1314 42.135

0.2439 0.2002 0.1528 0.1522 42.441

0.2286 0.2504 0.1357 0.1692 42.680


5/12


.Table 3 continued

.x x y y P kPa1 2 1,calc 2,calc

0.2133 0.3008 0.1209 0.1836 42.889

0.1984 0.3495 0.1081 0.1955 43.053

0.1827 0.4011 0.0958 0.2063 43.214

0.1674 0.4513 0.0848 0.2151 43.345

0.1525 0.5002 0.0750 0.2224 43.452

0.0000 1.0000 0.0000 1.0000 12.3580.0000 0.6962 0.0000 0.2552 45.572

0.0244 0.6793 0.0108 0.2520 45.254

0.0504 0.6612 0.0228 0.2481 44.823

0.0992 0.6272 0.0460 0.2394 43.927

0.1489 0.5925 0.0702 0.2295 43.012

0.2014 0.5560 0.0963 0.2186 42.028

0.2497 0.5223 0.1211 0.2083 41.081

0.3002 0.4871 0.1479 0.1977 40.064

0.3502 0.4523 0.1760 0.1871 39.016

0.4004 0.4173 0.2063 0.1765 37.926

0.4497 0.3829 0.2386 0.1660 36.785

0.4999 0.3479 0.2745 0.1552 35.572

0.0000 0.0000 0.0000 0.0000 35.456

0.0000 0.3016 0.0000 0.2572 45.611

0.0251 0.2940 0.0163 0.2447 45.266

0.0503 0.2865 0.0325 0.2328 44.915

0.0997 0.2716 0.0634 0.2117 44.274

0.1502 0.2564 0.0938 0.1922 43.628

0.2001 0.2414 0.1227 0.1745 43.002

0.2500 0.2263 0.1506 0.1581 42.396

0.3002 0.2112 0.1780 0.1426 41.776

0.3500 0.1962 0.2048 0.1281 41.140

0.4003 0.1810 0.2318 0.1144 40.479

0.4502 0.1659 0.2588 0.1015 39.771

0.5000 0.1509 0.2865 0.0895 39.020

.Temperature was measured by a calibrated standard PRT-100 SDL model 5385r100 using as .indicator an AC resistance bridge ASL model F250 resolving 1 mK in the reading of temperature

and estimating an overall uncertainty of "10 mK. The measurement of the pressure was doneindirectly through a differential pressure cell and indicator Ruska models 2413-705 and 2416-711,

.respectively . Once air balances the vapor pressure of the cell a Bourdon fused quartz precision .pressure gauge Texas Instruments mod. 801 reads the pressure with an estimated uncertainty of"5

Pa for the 125 kPa range.

3.1. Experimental results and correlations

The use of the measuring technique described above allows a static equilibrium between phases,assuring a true thermodynamic equilibrium. Direct sampling, particularly of the vapor phase, upsetsthe equilibrium, the mass of vapor in the cell is very small; yet an appreciable mass must be


6/12


withdrawn to yield an amount of condensate suitable for accurate analysis. However, as a conse-quence of Duhems theorem, sampling of the phases is not, in fact, necessary. Given a set ofequilibrium x, P data at constant T, thermodynamics allows calculation of the y-values. Thus, theequilibrium vapor need not be sampled for analysis and the data are thermodynamically consistent

w x w x.per se. Van Ness et al. 13 ; Van Ness 14w xData reduction for the binary and ternary mixtures was done by Barkers method 15 according to

w x.well established procedures Abbott and Van Ness 16,17 developing a computer program described w x.in detail earlier. Lozano et al. 12

The non-ideality of the vapor phase was taken into account with the virial equation of state, .truncated in the second term. The second virial coefficients B are indicated in Table 1. They wereii

w xcalculated by the Hayden and OConnell method 18 using the parameters given by Dymond andw xSmith 19 . Correction for the vapor phase was also applied to x.

The quality of the data of the present VLE technique for ternaries has been assessed previously andw xreported in Refs. 38 .

The ternary system TAMEq n-heptaneq methanol has been measured together with the binarysystem TAME q methanol at 313.15 K. The other binary systems involved in this ternary TAMEq n-

w xheptane and n-heptaneq methanol have been already published Chamorro et al. 2 ; Segovia et

w x.al. 8 , using the same experimental procedure and data reduction.Data for this ternary system are adequately correlated by the three-parameter Wohl equation, Eq.

. w x.1 Van Ness and Abbott 13 , which also includes the parameters of the corresponding binaries.

g E

g s g q g q g q C q C x q C x x x x 1 . .123 12 13 23 0 1 1 2 2 1 2 3RT

.Correlations for the g are given by Eq. 2 ; parameters C , C and C are found by regression ofi j 0 1 2 .the ternary data. The Margules equation with three parameters, Eq. 2 , has been chosen for the

binaries.

g E

g s s A x qA x ylx x x x 2 .i j ji i i j j i j i jRt

w x w xBinary and ternary systems have also been correlated using Wilson 20 , NRTL 21 andw xUNIQUAC 22 models, whose expressions for the excess Gibbs energy are indicated by the Eqs.

. .3 5 , respectively.

g E

s y x ln x A 3 . i j i j /RT i jA G x j i ji jEg j

s x 4 . iRT G xi

ki k

k

g E w z qi is x ln q q x ln y q x ln q A 5 . i i i i i j ji /RT x 2 qi ii i i j

. . . . .where, G s exp ya A , qs q x r q x ; ws r x r r x and z s 10.ji ji ji i i i j j j i i i j j j


7/12


Table 4 . ..Summary of the data reduction results and azeotrope situation obtained for the binary system TAME 1 qmethanol 2 at

313.15 Ka b .Margules 3p Wilson NRTL NRTL UNIQUAC

A 1.5372 0.3996 0.8593 0.9723 0.214612A 1.5096 0.4189 0.9015 1.0111 1.252321l 0.5045

a 0.47 0.613812 .rms D P kPa 0.007 0.081 0.113 0.007 0.203 .max D P kPa 0.023 0.180 0.252 0.014 0.455

.x azeotrope 0.2737 0.2788 0.2736 0.28701 . .P azeotrope kPa 40.076 40.014 40.072 39.948

aThis column contains a s 0.47 as recommended, but the fitting is rather poor.12

bThis column contains a simultaneous adjustment of the three parameters.

Table 2 gives experimental values of total pressure and the corresponding compositions of the .liquid and vapor phases for the binary system TAMEq methanol , reduced by Margules equation.

.Table 3 gives the same type of information for the ternary system TAMEq n-heptaneq methanol ,

where Wohl expansion has been used in the data reduction.Results of data correlation for the binary system TAME q methanol are summarized in Table 4.

The results of the correlations for the other binaries involved in the ternary system TAMEq n-. w x w x.heptaneq methanol have been published previously Chamorro et al. 2 ; Segovia et al. 8 . For the

ternary system, the results of the correlation are given in Table 5. All these tables contain values ofthe adjustable parameters of the different models which lead to the correlated results using Barkers

Table 5 . . ..Summary of the data reduction results obtained for the ternary system TAME 1 q n-heptane 2 qmethanol 3 at 313.15

Ka bWohl Wilson NRTL UNIQUAC

C 1.74160C 2.60071C 2.39992A 0.7071 0.4237 1.401112A 1.0561 y0.1962 0.551721A 0.4133 0.9958 0.220513A 0.4044 0.9585 1.237931A 0.0594 2.6495 0.061623A 0.0296 2.7360 1.142532a 0.312a 0.613813a 0.435623

.rms

DP kPa 0.159 0.118 0.212 0.620< < .max D P kPa 0.470 0.407 0.774 2.096

aThe values for the correlation parameters of the two constituent binaries, not reported in this paper, were taken from Refs.

w x2,8 .b

The recommended value of a s0.3 has been taken, since it has been found that the outcome of the fitting was the same12using an adjusted ad hoc value.


8/12


. ..Fig. 1. Comparison for the binary system TAME 1 qmethanol 2 at 313.15 K of the pressure residuals, P y P ,calcdefined as differences between experimental pressures, P, and calculated pressures, P . A"0.1% band of the experimen-calctal pressure in each point is indicated on the diagram.

method. The root mean square of the difference between experimental and calculated pressures rms. <


9/12


Table 6 . ..Values of the azeotrope composition, x , and total vapor pressure, P, for the binary system TAME 1 qmethanol 2 at1

313.15 K, calculated with different correlation models, and comparison with values reported from literature

.x P kPa1

Margules 0.2737 40.076

Wilson 0.2788 40.014

NRTL 0.2736 40.072

UNIQUAC 0.2870 39.948a bw xReported by Gmehling et al. 23 0.2731a bw xReported by Coto et al. 24 0.2749

aObtained by interpolation of values at different temperatures.

b w xNot determined by the referred authors 23,24 at 313.15 K.

w x .Chamorro et al. 2 . The remaining binary system methanolq n-heptane presents a large immiscibil- w x.ity gap between x s 0.2263 and x s 0.8714 as has been determined by us Segovia et al. 8 .1 1

The molar excess Gibbs function, g E, shows a positive deviation from ideality with maximum .values close to equimolar concentrations at 1672 Jrmol for methanolq n-heptane , 910 Jrmol for

. . E

TAME q n-heptane and 107.4 Jrmol for TAME q n-heptane . This behaviour of g showsquantitatively the strong gradation of the nature of the binary mixtures, ranging from nearly an ideal . solution in the case of TAME q n-heptane to the high non-ideality with separation for methanolq

.n-heptane .Concerning the measured ternary system, the results of the correlation give a root mean square

pressure residuals between 0.118 kPa for Wilson equation and 0.620 kPa for UNIQUAC, being the

Fig. 2. Total vapor pressure as a function of the liquid, x , and vapor composition, y , of TAME for the VLE of the binary1 1 . ..system TAME 1 qmethanol 2 at 313.15 K. The azeotrope showed occurs at x s 0.2737 and P s40.076 kPa.1


10/12


Fig. 3. Isobar lines in kPa as a function of the ternary liquid composition, x , for the VLE at 313.15 K of the ternary systemi . . ..TAME 1 q n-heptane 2 qmethanol 3 .

former the best fit for all the miscible region. Figs. 3 and 4 show, respectively isobar and the iso-g E

lines as a function of the ternary liquid composition.

Fig. 4. Iso-g E lines in Jrmol as a function of the ternary liquid composition, x , for the VLE at 313.15 K of the ternaryi . . ..system TAME 1 q n-heptane 2 qmethanol 3 .


11/12


.The investigated ternary system TAMEq n-heptaneq mehtanol shows good miscibility in thewhole range of our measurements, nevertheless, it is to expect a really very narrow immiscible zone

.close to binary line of methanolq n-heptane which is impossible to precise with our experimentaltechnique due to the very low concentrations of TAME at which it appears. In fact, very lowquantities of TAME representing according to our measurements values lower than 0.1 molar destroys

.the immiscibility of the binary methanolq n-heptane .

The search for ternary azeotropes either homogeneous or heterogeneous using the calculationw x w x w xprocedures indicated by Gmehling and Menke 25 ; Demirel 26 and Chapman and Goodwin 27have been negative in all the concentration range for the correlated data by Wilson, NRTL orUNIQUAC. Concerning the g E function the maximum value occurs at the maximum value for the

.binary methanolq n-heptane already given.

5. Nomenclature

A , A adjustable parameters of the correlation modelsi j jiB , B , B second virial coefficientsii i j j j

.C , C , C parameters in Eq. 10 1 2g E molar excess Gibbs energyg value of g ErRT for a binary or a ternary mixturei,j constituent identification: 1, 2 or 3lit literature valuemax maximum value of the indicated quantityP total pressureP sat vapor pressure of pure constituent iiR universal gas constant

rms root mean squareT absolute temperatureVL molar volume of pure liquid i s 1,2,3ix mole fraction, liquid phasey mole fraction, vapor phaseGreek lettersD signifies difference

.l parameter in Eq. 2

Acknowledgements

Support for this work came from the DGICYT, Direccion General de Investigacion Cientfica y Tecnica of the Spanish Ministery of Education, Project PB-95-0704 and from Junta de Castilla y Leon .Consejera de Educacion y Cultura project VA 42r96.


12/12


References

w x1 C.R. Chamorro, PhD Thesis, University of Valladolid, Spain, 1998.w x .2 C.R. Chamorro, J.J. Segovia, M.C. Martn, E.A. Montero, M.A. Villamanan, Fluid Phase Equilibria 156 1999 7387. w x3 J.J. Segovia, PhD Thesis, University of Valladolid, Spain, 1997.w x .4 J.J. Segovia, M.C. Martn, C.R. Chamorro, M.A. Villamanan, Fluid Phase Equilibria 133 1997 163172. w x .5 J.J. Segovia, M.C. Martn, C.R. Chamorro, E.A. Montero, M.A. Villamanan, Fluid Phase Equilibria 152 1998

265276.w x .6 J.J. Segovia, M.C. Martn, C.R. Chamorro, M.A. Villamanan, J. Chem. Eng. Data 43 1998 10141020. w x .7 J.J. Segovia, M.C. Martn, C.R. Chamorro, M.A. Villamanan, J. Chem. Eng. Data 43 1998 10211026. w x8 J.J. Segovia, M.C. Martn, C.R. Chamorro, M.A. Villamanan, J. Chem. Thermodyn., 1999, in print. w x .9 H.C. Van Ness, M.M. Abbott, Ind. Eng. Chem. Fundam. 17 1978 6667.

w x .10 R.E. Gibbs, H.C. Van Ness, Ind. Eng. Chem. Fundam. 11 1972 410413.w x .11 D.P. DiElsi, R.B. Patel, M.M. Abbott, H.C. Van Ness, J. Chem. Eng. Data 23 1978 242245.w x .12 L.M. Lozano, E.A. Montero, M.C. Martn, M.A. Villamanan, Fluid Phase Equilibria 110 1995 219230. w x13 H.C. Van Ness, M.M. Abbott. Classical Thermodynamics of Nonelectrolyte Solutions with Applications to Phase

Equilibria, Mc-Graw Hill, New York, 1982.w x .14 H.C. Van Ness, J. Chem. Thermodyn. 27 1995 113134.w x .15 J.A. Barker, Aust. J. Chem. 6 1953 207210.w x .16 M.M. Abbott, H.C. Van Ness, AIChE Journal 21 1975 6271.

w x .17 M.M. Abbott, J.K. Floess, G.E. Walsh Jr., H.C. Van Ness, AIChE Journal 21 1975 7276.w x .18 J.G. Hayden, J.P. OConnell, Ind. Eng. Chem. Process Des. Dev. 14 1975 209216.w x19 J.H. Dymond, E.B. Smith, The Virial Coefficients of Pure Gases and Mixtures A Critical Compilation, Clarendon

Press, Oxford, 1980.w x .20 G.M. Wilson, J. Am. Chem. Soc. 86 1964 127130.w x .21 H. Renon, J.M. Prausnitz, AIChE Journal 14 1968 135144.w x .22 D.S. Abrams, J.M. Prausnitz, AIChE Journal 21 1975 116128.w x .23 J. Gmehling, J. Menke, J. Krafczyck, K. Fisher, Fluid Phase Equilibria 103 1995 5176.w x .24 B. Coto, F. Mosner, C. Pando, R.G. Rubio, J.A.R Renuncio, Fluid Phase Equilibria 133 1997 89103.w x25 J. Gmehling and B. Menke, Thermodynamik, VCH Verlag, Weiheim, 1992.w x .26 Y. Demirel, Fluid Phase Equilibria 86 1993 113.w x .27 R.G. Chapman, S.P. Goodwin, Fluid Phase Equilibria 85 1993 5569.w x .28 R.K. Toghiani, H. Toghiani, G. Venkateswarlu, Fluid Phase Equilibria 122 1996 157168.w x .29 I. Cervenkova, T. Boublik, J. Chem. Eng. Data 29 1984 425427.w x30 E.A. Montero, PhD Thesis, University of Valladolid, Spain, 1996.w x31 TRC-Thermodynamic Tables Hydrocarbons, Thermodynamics Research Center. The Texas A&M University

System, College Station, Vapor Pressures, 1976.w x32 R.C. Reid, J.M. Prausnitz, B.E. Poling, The Properties of Gases and Liquids, Mc-Graw Hill, New York, 1987.w x33 R.C. Reid, J.M. Prausnitz, T.K. Sherwood, The Properties of Gases and Liquids, 3rd edn., Mc-Graw Hill, New York,

1977.w x .34 M. Goral, Fluid Phase Equilibria 102 1994 275286.w x35 T. Boublik, V. Fried, E. Hala, The Vapor Pressures of Pure Liquids, Elsevier, Amsterdam, 1973.w x36 TRC-Thermodynamic Tables Hydrocarbons, Thermodynamics Research Center. The Texas A&M University

System, College Station, Densities, 1973.

Documents

8_-_Experimental_investigation_of_the_vaporâ€“liquid_equ ilibrium at 313.15 K of the ternary system tert-amylmethyl_ether_(TAME)_+_n-heptane_+methanol