libet s

am, P.O L

Accepted 20 April 2010Available online 28 April 2010

dimethylamino-1-propanol components were measured by means of two static devices at temperatures

containing {methylethanolamine (MEA) + water}, or (4-methyl-morpholine + water) have been reported previously [1]. Thepurpose of the present work is to investigate VLE of {2-amino-2-methyl-1-propanol (AMP) (CAS # 124-68-5) + water},{N-benzylethanolamine (CAS # 104-63-2) + water}, or {3-dimeth-ylamino-1-propanol (CAS # 3179-63-3) + water} binary mixtureswith a view to use the results to determine interaction parameters

a static apparatus. The description of the apparatus and the exper-imental procedure can be found elsewhere [36], so only the mostsalient information is given here. The apparatus was equipped witha differential manometer from MKS, type 670, model 616A. Thepressure measurement consisted of applying the vapour pressureof the sample on the measurement side of the gauge. The referenceside was submitted to a permanent-dynamic pumping. The resid-ual pressure was 104 Pa and therefore can be neglected. Temper-ature measurements were carried out using a copper-constantanthermocouple calibrated against a 25X platinum resistance stan-dard thermometer (0.001 K, IPTS 90) and a Leeds and Northrup

* Corresponding author. Tel./fax: +213 43 28 65 30.

J. Chem. Thermodynamics 42 (2010) 11581162

Contents lists availab

rm

w.E-mail address: latifanegadi@yahoo.fr (L. Negadi).Aqueous alkanolamine solutions are widely used for theremoval of the acid gases (CO2 and H2S) from gas mixtures. In addi-tion to the well-established industrial uses of experimental datafor these completely miscible (alkanolamine + water) systems,there is a general scientic interest in using such experimentaldata in combination with theories or mathematical models toimprove our understanding of molecular interactions in non-idealliquid systems. (Vapour + liquid) equilibria (VLE) data for(alkanolamine + water) systems are rarely available in theliterature.

The present paper is part of a research program on (VLE) inaqueous mixtures of alkanolamines. VLE data for binary mixtures

(AMP + water) system [2].

2. Experimental

The alkanolamines were supplied by Aldrich Chem. (Milwau-kee, WI, USA). They were used without further purication. Thepurities, tested by GLC, were better than mass fraction purity0.99. Aqueous solutions were prepared from distilled and deion-ised water.

For the pure AMP and 3-dimethylamino-1-propanol compo-nents, the vapour pressure measurements were carried out usingKeywords:(Vapour + liquid) equilibriaIsoteniscopeAminesWaterExcess Gibbs free energy

1. Introduction0021-9614/$ - see front matter 2010 Elsevier Ltd. Adoi:10.1016/j.jct.2010.04.015between 283 K and 363 K. The data were correlated with the Antoine equation. From these data, excessGibbs functions (GE) were calculated for several constant temperatures and tted to a fourth-order Red-lichKister equation using the Barkers method. The {2-amino-2-methyl-1-propanol (AMP) + water} bin-ary mixture exhibits negative deviations in GE (at T < 353.15 K) and a sinusoidal shape for GE for thehigher temperatures over the whole composition range. For the aqueous N-benzylethanolamine solution,a S shape is observed for the GE for all investigated temperatures over the whole composition range. The(3-dimethylamino-1-propanol + water) binary mixture exhibits negative deviations in GE (atT < 293.15 K), positive deviations in GE (for 293.15 K < T < 353.15 K) and a sinusoidal shape for GE forthe higher temperatures over the whole composition range.

2010 Elsevier Ltd. All rights reserved.

for predictive group contribution methods. A survey of the litera-ture shows that there is only one data set available for theReceived 14 February 2010Received in revised form 24 March 2010

The vapour pressures of (2-amino-2-methyl-1-propanol (AMP) + water), (N-benzylethanol-amine + water), or (3-dimethylamino-1-propanol + water) binary mixtures, and of pure AMP and 3-Investigation of the isothermal (vapour +2-amino-2-methyl-1-propanol (AMP), N-3-dimethylamino-1-propanol solutions a

Aouicha Belabbaci a, Nouria Chiali-Baba Ahmed a, IlhaUniversity Abou Bekr Belkaid of Tlemcen, Faculty of Sciences, Department of Chemistryb LSA, Laboratoire des Sciences Analytiques, CNRS-UMR 5180, Universit Claude Bernard

a r t i c l e i n f o

Article history:

a b s t r a c t

J. Chem. The

journal homepage: wwll rights reserved.quid) equilibria of aqueousnzylethanolamine, oreveral temperatures

Mokbel b, Latifa Negadi a,*

. Box 119, Tlemcen 13000, Algeriayon I, 43, Bd du 11 Novembre 1918, Villeurbanne Cedex 69622, France

le at ScienceDirect

odynamics

elsevier .com/locate / jc t

bridge (104X). During measurements the stability of the tem-perature is 0.02 K. The differential pressure gauge was calibratedagainst a U-manometer lled with mercury or Apiezon oil depend-ing on pressure range. The levels in both arms of the U-shapedmanometer were read by a cathetometer (reference 70298, fromBouty France) to the nearest 0.001 mm. The calibration was thenchecked by measuring the vapour and the sublimation pressures

TABLE 2Experimental and calculated (with the Antoine equation (1)) vapour pressures of pureAMP and 3-dimethylamino-1-propanol.

T/K P(experimental)/Pa P(from equation (1)/Pa 100dP/P

AMP293.29 41.5 41.0 1.21303.35 97.5 99.3 1.87313.24 219.1 219.1 0.02323.25 455.6 456.2 0.13332.57 874.5 856.0 2.11343.18 1658.6 1657.1 0.09353.17 2933.5 2942.1 0.29363.10 4987.5 4993.6 0.12373.00 8141.8 8159.0 0.21100dP/P 0.67

3-Dimethylamino-1-propanol283.15 7.0 7.0 0.04293.14 16.0 16.0 0.13303.09 34.6 34.5 0.27313.08 70.7 70.8 0.15323.28 141.8 140.8 0.69333.12 260.4 262.3 0.72343.12 474.2 475.1 0.20363.17 1419.4 1413.0 0.45373.10 2314.6 2318.4 0.17100dP/P 0.31

TABLE 3Values of the vapour pressure P, standard deviations dP/P (%), activity coefcients c1and c2 and excess molar Gibbs functions GE for the binary system {AMP (1) + water(2)}.

x1 P/kPa x1 P/kPa x1 P/kPa

T/K = 293.150.0000 2.2838 0.2603 1.6698 0.6692 0.69150.0498 2.1703 0.3598 1.4464 0.8203 0.36270.1001 2.0305 0.5408 1.0027 1.0000 0.04050.1800 1.9769

T/K = 303.150.0000 4.1478 0.2603 3.0389 0.6692 1.22690.0498 3.9584 0.3598 2.6179 0.8203 0.70810.1001 3.7225 0.5408 1.7898 1.0000 0.09760.1800 3.5283

T/K = 313.150.0000 7.2219 0.2603 5.3265 0.6692 2.10740.0498 6.9120 0.3598 4.5642 0.8203 1.29630.1001 6.5300 0.5408 3.0872 1.0000 0.21760.1800 6.0803

T/K = 323.150.0000 12.1071 0.2603 9.0231 0.6692 3.51380.0498 11.6081 0.3598 7.6914 0.8203 2.24460.1001 11.0120 0.5408 5.1605 1.0000 0.45310.1800 10.1488

T/K = 333.150.0000 19.6156 0.2603 14.8171 0.6692 5.70090.0498 18.8235 0.3598 12.5658 0.8203 3.70360.1001 17.9239 0.5408 8.3817 1.0000 0.88890.1800 16.4517

T/K = 343.150.0000 30.8154 0.2603 23.6497 0.6692 9.01900.0498 29.5745 0.3598 19.9565 0.8203 5.85870.1001 28.2571 0.5408 13.2592 1.0000 1.65440.1800 25.9642

T/K = 353.150.0000 47.0737 0.2603 36.7767 0.6692 13.93990.0498 45.1559 0.3598 30.8832 0.8203 8.93060.1001 43.2785 0.5408 20.4713 1.0000 2.93860.1800 39.9802

T/K = 363.150.0000 70.1022 0.2603 55.8377 0.6692 21.0863

A. Belabbaci et al. / J. Chem. Thermodynamics 42 (2010) 11581162 1159of water and naphthalene [4]. The uncertainty of the measure-ments is estimated to be: r( P) = 0.03(P/Pa) for P < 600 Pa;r(P) = 0.01(P/Pa) for P in the range (600 to 1300) Pa,r(P) = 0.03(P/Pa) for P over 1300 Pa, and r(T) = 0.02 K for thetemperature range 203 6 T/K 6 463.

For the three binary systems, the experimental vapour pressure,P, data were obtained with an apparatus described in detail byBlondel-Telouk et al. [7,8], as a function of the temperature, T, forconstant mole fraction composition, xi. The apparatus allows mea-surements at pressures from 27 Pa to 200 103 Pa and at tempera-tures from (258.15 to 468.15) K. The pressure was measured with apressure gauge (Rosemount, Model 1151 DPE 22S2, Minneapolis,MN, USA), separated from the working uid by a differential pres-sure indicator (MKS, Model 615D, MKS Instruments, USA). Thepressure gauges were periodically checked against a Hg or oilmanometer and a Bouty (Paris, France) Type 70298 cathetometer,which when combined provide pressures with an uncertainty of1 Pa. The temperature of the oil-lled thermostat was maintainedconstant to 0.01 K. The temperature was measured by means ofa copper-constantan thermocouple calibrated against a Leeds andNorthrup standard platinum resistance thermometer 8163-B, cali-brated by the National Bureau of Standards (NIST) (Washington,DC, USA) and connected to Mueller type G2 bridge (with a preci-sion 104X). All temperatures are reported on ITS-90. The esti-mated uncertainties in pressure, temperature and mole fractionare: r(P) = 0.15(P/Pa) for P < 13.3 Pa, r(P) = 0.05(P/Pa) at pressurebetween (13.3 and 200) Pa, r(P) = 0.005(P/Pa) in the range (200to 1000) Pa, r(P) = 0.002(P/Pa) for the range (1000 to200 103) Pa, r(T) = 0.01 K and r(xi) = 0.0002. Mixtures were pre-pared bymass and thoroughly degassed by distillation as describedby Blondel-Tellouk et al. [7,8].

3. Results and discussion

The experimental vapour pressure data were tted to the Antoine equation:

lg10P=Torr AB

C t=C : 1

The objective function Q was the sum of the squared relative deviations in pressure:

Q X Pcalc Pexp

Pexp

2: 2

The overall mean relative deviation in pressure is:

dPP% 100

N

X Pcalc PexpPexp

; 3

where N is the total number of experimental values.Table 1 lists, for the pure AMP and 3-dimethylamino-1-propanol components,

the temperature range, the coefcients A, B, C of the Antoine equation and the over-all mean relative deviation in pressure. The comparison of the calculated vapour

TABLE 1Coefcients A, B, C and overall mean relative deviation in pressure of the Antoineequation (1).

Compound T/K A B C 100(dP/P)

AMP 3 293.29373.00 7.73031 1698.90 185.9906 0.673-Dimethylamino-

1-propanol283.1573.10 8.87465 2767.22 262.5195 0.31100dP=P 1NPN

i1100PcalcPexp

Pexp

, where N is the total number of experimental

values.

0.0498 67.1789 0.3598 46.6687 0.8203 13.17480.1001 64.5689 0.5408 30.9057 1.0000 5.00680.1800 60.1821

pressures of AMP or 3-dimethylamino-1-propanol from equation (1) with the mea-sured values is shown in table 2. Our vapour pressure data for pure AMP are in goodagreement with those reported by Pappa et al. [2] or given by the NIST database [9].For pure 3-dimethylamino-1-propanol, no vapour pressure data are available in theliterature. For pure water and N-benzylethanolamine, the vapour pressures used inthis work have been reported previously [1,10].

For the three binary mixtures, the vapour pressures were measured at temper-atures between (283.15 (or 293.15) and 363.15) K and the results tted to the An-toine equation and the molar excess Gibbs functions GE were estimated from theRedlichKister equation using the method of Barker [11]:

GE x11 x1Xmj1

RTGj2x1 1j1; 4

where x1 is the mole fraction for the alkanolamine. The coefcients Gj were deter-mined by regression through minimization of the sum of deviations in pressure. Va-pour phase imperfection and variation of the Gibbs function of the pure liquid

components with pressure were accounted for in terms of the second molar virialcoefcients, estimated by the method of Tsonopoulos [12,13] and the molar volumesunder saturation pressure.

TABLE 4Values of the vapour pressure P, standard deviations dP/P (%), activity coefcients c1and c2 and excess molar Gibbs functions GE for the binary system {N-benzylethanol-amine (1) + water (2)}.

x1 P/kPa x1 P/kPa x1 P/kPa

T/K = 283.150.0000 1.1995 0.3589 0.9828 0.7546 0.21920.0746 1.1797 0.4879 0.6833 0.8358 0.10870.1798 1.1600 0.6368 0.3759 1.0000 0.00030.2599 1.1242

T/K = 293.150.0000 2.2838 0.3589 1.8102 0.7546 0.44340.0746 2.2513 0.4879 1.3596 0.8358 0.21830.1798 2.1784 0.6368 0.7557 1.0000 0.00080.2599 2.0655

T/K = 298.150.0000 3.0950 0.3589 2.4174 0.7546 0.61670.0746 3.0538 0.4879 1.8667 0.8358 0.30400.1798 2.9377 0.6368 1.0465 1.0000 0.00130.2599 2.7628

T/K = 303.150.0000 4.1478 0.3589 3.1963 0.7546 0.84640.0746 4.0959 0.4879 2.5217 0.8358 0.41870.1798 3.9223 0.6368 1.4287 1.0000 0.00220.2599 3.6646

T/K = 313.150.0000 7.2219 0.3589 5.4334 0.7546 1.53590.0746 7.1404 0.4879 4.4051 0.8358 0.77080.1798 6.7991 0.6368 2.5597 1.0000 0.00530.2599 6.2965

T/K = 323.150.0000 12.1071 0.3589 8.9249 0.7546 2.66420.0746 11.9800 0.4879 7.3076 0.8358 1.36660.1798 11.3869 0.6368 4.3745 1.0000 0.01250.2599 10.5045

T/K = 333.15

TABLE 5Values of the vapour pressure P, standard deviations dP/P (%), activity coefcients c1and c2 and excess molar Gibbs functions GE for the binary system {3-dimethylamino-1-propanol (1) + water (2)}.

x1 P/kPa x1 P/kPa x1 P/kPa

T/K = 283.150.0000 1.1995 0.2599 0.8687 0.7189 0.33220.0501 1.1288 0.3602 0.7398 0.8119 0.23100.1005 1.0745 0.4998 0.5619 1.0000 0.007

T/K = 293.150.0000 2.2838 0.2599 1.6884 0.7189 0.65100.0501 2.1704 0.3602 1.4182 0.8119 0.51630.1005 2.0696 0.4998 1.1314 1.0000 0.0160

T/K = 303.150.0000 4.1478 0.2599 3.1272 0.7189 1.21370.0501 3.9719 0.3602 2.6069 0.8119 1.02060.1005 3.7980 0.4998 2.1465 1.0000 0.0346

T/K = 313.150.0000 7.2219 0.2599 5.5479 0.7189 2.16370.0501 6.9561 0.3602 4.6130 0.8119 1.83150.1005 6.6752 0.4998 3.8649 1.0000 0.0712

T/K = 323.150.0000 12.1070 0.2599 9.4688 0.7189 3.70590.0501 11.7119 0.3602 7.8849 0.8119 3.04160.1005 11.2862 0.4998 6.6449 1.0000 0.1396

T/K = 333.150.0000 19.6156 0.2599 15.6059 0.7189 6.12270.0501 19.0343 0.3602 13.0589 0.8119 4.74260.1005 18.4285 0.4998 10.9668 1.0000 0.2627

T/K = 343.150.0000 30.8153 0.2599 24.9205 0.7189 9.79210.0501 29.9641 0.3602 21.0130 0.8119 7.02040.1005 29.1571 0.4998 17.4516 1.0000 0.4760

T/K = 353.150.0000 47.0737 0.2599 38.6685 0.7189 15.20600.0501 45.8291 0.3602 32.9293 0.8119 9.95120.1005 44.8321 0.4998 26.8798 1.0000 0.8328

T/K = 363.150.0000 70.1021 0.2599 58.4529 0.7189 22.98940.0501 68.2833 0.3602 50.3645 0.8119 13.59940.1005 67.1660 0.4998 40.2065 1.0000 1.4116

1160 A. Belabbaci et al. / J. Chem. Thermodynamics 42 (2010) 115811620.0000 19.6156 0.3589 14.2113 0.7546 4.43970.0746 19.4190 0.4879 11.5917 0.8358 2.34140.1798 18.4827 0.6368 7.1709 1.0000 0.02760.2599 17.0558

T/K = 343.150.0000 30.8154 0.3589 21.9986 0.7546 7.13760.0746 30.5123 0.4879 17.6823 0.8358 3.88850.1798 29.1565 0.6368 11.3275 1.0000 0.05780.2599 27.0090

T/K = 353.150.0000 47.0737 0.3589 33.1874 0.7546 11.11080.0746 46.6090 0.4879 26.0629 0.8358 6.27570.1798 44.8102 0.6368 17.3127 1.0000 0.11590.2599 41.7925

T/K = 363.150.0000 70.1022 0.3589 48.9020 0.7546 16.80030.0746 69.3943 0.4879 37.2688 0.8358 9.8664

0.1798 67.2411 0.6368 25.6896 1.0000 0.22270.2599 63.2972FIGURE 1. Plot of pressure against mole fraction to show the experimental and

calculated Px(y) behaviour of the system {AMP (1) + water (2)} at differenttemperatures: , 293.15 K; d, 323.15 K; j, 343.15; N, 363.15 K; 3, calculatedvalues using Barkers method.

For the three binary mixtures, a fourth-order RedlichKister equation has beenchosen because it was the most suitable to represent the excess Gibbs free energiesfor all investigated temperatures (it gives the best representations of GE for the low-est values of dP/P).

The vapour pressure as a function of the mole fraction for each binary mixture islisted in tables 3 to 5, and shown in gures 1 to 3.

The Gj coefcients and standard deviations r(Gj) for (AMP + water), (N-benzy-

increases with increasing temperature from 203 J mol1 at T = 293.15 K to136 J mol1 at T = 313.15 K than decreases with increasing temperature to333 J mol1 at T = 363.15 K.

The (N-benzylethanolamine + water) binary mixture shows a sinusoidal shapefor GE values calculated from the vapour pressure data for all investigated temper-atures over the whole composition range. The equimolar GE of (N-benzylethanol-amine + water) increases with increasing temperature from 377 J mol1 at

1

FIGURE 2. Plot of pressure against mole fraction to show the experimental andcalculated Px(y) behaviour of the system {N-benzylethanolamine (1) + water (2)}at different temperatures: , 293.15 K; d, 323.15 K; j, 343.15; N, 363.15 K; 3,calculated values using Barkers method.

FIGURE 3. Plot of pressure against mole fraction to show the experimental andcalculated Px(y) behaviour of the system {3-dimethylamino-1-propanol(1) + water (2)} at different temperatures: , 293.15 K; d, 323.15 K; j, 343.15; N,363.15 K; 3, calculated values using Barkers method.

n (4

+ w0.060.04

A. Belabbaci et al. / J. Chem. Thermodynamics 42 (2010) 11581162 1161lethanolamine + water), or (3-dimethylamino-1-propanol + water) binary systemare reported in table 6.

The three binary mixtures do not show azeotropic behaviour. No comparisonwith literature data was possible for the investigated temperaturepressure-com-position (TPx) range.

For each system, the molar excess Gibbs functions GE at different temperatures,calculated from our vapour pressure data, are plotted in gures 4 to 6 against themole fraction x1 of alkanolamine.

The aqueous AMP solution exhibits negative deviations in GE values calculatedfrom the vapour pressure data for the temperatures less than 313.15 K. For highertemperatures, the S shape is observed for GE. The equimolar GE of (AMP + water)

TABLE 6Coefcients Gj and standard deviations r for least-squares representations by equatio

T/K G1 r G2 r

{AMP293.15 0.32708 (0.073) 0.09084 (303.15 0.25737 (0.049) 0.05707 (

313.15 0.22532 (0.034) 0.14214 (0.03323.15 0.22461 (0.025) 0.17368 (0.02333.15 0.24995 (0.021) 0.15868 (0.02343.15 0.29680 (0.019) 0.10279 (0.02353.15 0.36109 (0.019) 0.01104 (0.02363.15 0.43904 (0.022) 0.11161 (0.02

{N-benzylethanola283.15 0.66497 (0.058) 0.97724 (0.06293.15 0.55486 (0.066) 0.98497 (0.07298.15 0.51108 (0.071) 0.97419 (0.07303.15 0.47358 (0.075) 0.95554 (0.07313.15 0.41456 (0.079) 0.89891 (0.08323.15 0.37303 (0.077) 0.82204 (0.08333.15 0.34546 (0.071) 0.72991 (0.07343.15 0.32912 (0.065) 0.62617 (0.06353.15 0.32191 (0.060) 0.51353 (0.06363.15 0.32209 (0.062) 0.39406 (0.06

{3-Dimethylamino-1-p283.15 0.07768 (0.022) 0.19259 (0.02293.15 0.24091 (0.051) 0.36242 (0.05303.15 0.40801 (0.093) 0.40559 (0.09313.15 0.46532 (0.115) 0.35689 (0.11323.15 0.44194 (0.121) 0.24142 (0.12333.15 0.35885 (0.113) 0.07751 (0.11343.15 0.23130 (0.095) 0.12118 (0.09353.15 0.07056 (0.070) 0.34445 (0.07363.15 0.11493 (0.042) 0.58458 (0.04T = 283.15 K to 224 J mol at T = 343.15 K than decreases with increasing tem-perature to 236 J mol1 at T = 363.15 K.

The aqueous 3-dimethylamino-1-propanol binary solution exhibits negativedeviations in GE (for T < 293.15 K), positive deviations in GE (for293.15 K < T < 353.15 K) and a sinusoidal shape for GE for the higher temperaturesover the whole composition range. The equimolar GE of (3-dimethylamino-1-propa-nol + water) increases with increasing temperature from 46 J mol1 atT = 283.15 K to +303 J mol1 at T = 313.15 K than decreases with increasing tem-perature to 87 J mol1 (at T = 363.15 K).

The S shape for GE depends essentially on the combined effects of the tempera-ture and composition on the behaviour of the system.

).

G3 r G4 r

ater}5) 0.01169 (0.168) 0.17132 (0.319)5) 0.23712 (0.115) 0.02375 (0.219)

2) 0.40370 (0.081) 0.14916 (0.153)4) 0.51883 (0.062) 0.21356 (0.116)1) 0.58682 (0.054) 0.22302 (0.100)0) 0.61019 (0.051) 0.18184 (0.094)1) 0.59088 (0.052) 0.09354 (0.096)5) 0.53140 (0.060) 0.03819 (0.111)mine + water}1) 0.67194 (0.128) 0.10927 (0.259)0) 0.46884 (0.145) 0.87686 (0.295)5) 0.38922 (0.155) 0.81446 (0.318)9) 0.32281 (0.164) 0.77749 (0.336)3) 0.22567 (0.171) 0.76796 (0.353)1) 0.17008 (0.167) 0.82823 (0.345)6) 0.14958 (0.155) 0.94296 (0.319)8) 0.15863 (0.141) 1.10021 (0.288)4) 0.19254 (0.131) 1.29050 (0.268)6) 0.24735 (0.136) 1.50616 (0.276)ropanol + water}2) 0.02247 (0.047) 0.14096 (0.088)0) 0.39851 (0.106) 0.32640 (0.199)2) 0.60643 (0.194) 0.53317 (0.366)4) 0.66308 (0.240) 0.54754 (0.455)0) 0.61051 (0.252) 0.41862 (0.478)3) 0.47817 (0.237) 0.18229 (0.449)6) 0.28694 (0.201) 0.13473 (0.379)1) 0.05187 (0.149) 0.51233 (0.280)3) 0.21608 (0.090) 0.93512 (0.167)

The negative values of GE shows that the entropic effect is more important thanthe enthalpic one. It is, essentially, due to the presence of the strong hydrogenbonding which decrease the enthalpic effect.

4. Summary

Vapour pressures of pure AMP and 3-dimethylamino-1-propa-nol have been measured using a static device and correlated withthe Antoine equation. Isothermal VLE data of aqueous AMP, N-ben-zylethanolamine, or 3-dimethylamino-1-propanol solutions werestudied at several temperatures using a second static device. Theaqueous AMP solution exhibits negative deviations in GE (at

E

[6] S. Sarraute, I. Mokbel, M.F. Costa Gomes, V. Majer, J. Jose, Atmos. Environ. 42

110 (1995) 315339.[9] http://webbook.nist.gov.

FIGURE 4. Plot of GE against x1 for the {AMP (1) + water (2)} system: T = ,293.15 K; d, 323.15 K; j, 343.15 K; N, 363.15 K; 3, calculated values usingequation (4).

FIGURE 5. Plot of GE against x1 for the {N-benzylethanolamine (1) + water (2)}system: T = , 293.15 K; d, 323.15 K; j, 343.15; N, 363.15 K; 3, calculated valuesusing equation (4).

FIGURE 6. Plot of GE against x1 for the {3-dimethylamino-1-propanol (1) + water(2)} system: T = , 293.15 K; d, 323.15 K; j, 343.15; N, 363.15 K; 3, calculatedvalues using equation (4).

1162 A. Belabbaci et al. / J. Chem. Thermodynamics 42 (2010) 11581162[10] A. Razzouk, A. Hajjaji, I. Mokbel, P. Mougin, J. Jose, Fluid Phase Equilib. 282(2009) 1113.

[11] J.A. Barker, Aust. J. Chem. 6 (3) (1953) 207210.[12] C. Tsonopoulos, AIChE J. 20 (1974) 263272.[13] C. Tsonopoulos, AIChE J. 21 (1975) 827829.

JCT 1055(2008) 47244734.[7] A. Blondel-Telouk, Conception et mise au point dun dispositif statique pour la

dtermination de la masse molaire moyenne des coupes ptrolires partonomtrie, Etude dquilibres liquidevapeur de quatre systmes binaires,Thse de Doctorat (Universit Lyon I, France), 1994, pp. 1272.

[8] A. Blondel-Telouk, H. Loiseleur, A. Barreau, E. Behar, J. Jose, Fluid Phase Equilib.T < 313.15 K) and a sinusoidal shape for G for the higher temper-atures. For the (N-benzylethanolamine + water) binary mixture, aS shape is observed for the GE for all investigated temperaturesover the whole composition range. The aqueous 3-dimethyl-amino-1-propanol binary mixture exhibits negative deviations inGE (at T < 293.15 K), positive deviations in GE (for 293.15 K < T< 353.15 K) and a sinusoidal shape for GE for the higher tempera-tures over the whole composition range.

Acknowledgement

This work has been done in the framework of the internationalproject PHC TASSILI (Ref. 09 MDU 761).

References

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Investigation of the isothermal (vapour+liquid) equilibria of aqueous 2-amino-2-methyl-1-propanol (AMP), N-benzylethanolamine, or 3-dimethylamino-1-propanol solutions at several temperaturesIntroductionExperimentalResults and discussionSummaryAcknowledgementReferences