Isobaric Vapour-Liquid Equilibrium of Binary Mixture of 1, 2-Di-chloroethane with 1-Heptanol at 95.72 Kpa

Isobaric Vapour-Liquid Equilibrium of Binary Mixture of 1, 2-Di-chloroethane with 1-Heptanol at 95.72 Kpa

Sai kumar Bitta Department Of Chemical Engineering

Chaitanya Bharathi Institute of Technology

Gandipet, Hyderabad 500075, INDIA

Guide: Mr. V. Ananth Kumar Thimmarusu

Associate Professor Department Of Chemical Engineering, Chaitanya Bharathi Institute of Technology, Gandipet, Hyderabad 500075, INDIA

1. Varsha Goud Department Of Chemical

   Engineering Chaitanya Bharathi Institute of

   Technology Gandipet, Hyderabad 500075,

   INDIA

   Abstract Experimentally the isobaric vaporliquid equilibrium (VLE) data for the binary system (1,2- Dichloroethane + 1-Heptanol) is found at pressure (720mm Hg) at varied mole fractions. The measurements have been performed using a vapor recirculating type (Swietoslawski ebulliometer) equilibrium still. The mixture shows positive deviation from ideality and does not form an azeotrope. The activity coefficients of the system were correlated with the Van Laar model. The relationship of the liquid composition (X1) as a function of temperature (T) was found to be well represented by the Van Laar Model. The results showed that the calculated values of the vapor phase mole fraction and boiling temperature are agreed well with the experimental data. Furthermore, the VLE data shown to be thermodynamically consistent and is determined by Herington Test. The calculations are done for Antoine constants to find vapour pressures, Van Laar equation to find the activity coefficients, excess Gibbs free energy. Vapour liquid equilibrium measurements are carried out for binary mixtures based on their industrial importance in chemical engineering separation operation and strongly non ideal behavior.

   Keywords: 1) SWIETOSLAWKI Ebulliometer, 2) Binary

   mixture, 3) Vapor-liquid equilibrium, 4) 1-Heptanol

   1. INTRODUCTION

      The measurement, modeling and computation of phase equilibria have been one of the most compelling problems of chemical engineering. The variety of experimental and computational methods developed by chemical engineers and physical chemists for measurement and thermodynamic interpretation of vapor-liquid equilibria

      (VLE) probably surpasses all other areas of chemical engineering research. The VLE information is useful in designing separation processes such as distillation, adsorption, stripping and liquid-liquid extraction, which are major components of industrial processes involving hydrocarbons, and their cost frequently represents a major fraction of total plant cost. Also the VLE studies have

      assumed greater importance with the expansion of petrochemical industry and the fast increase in number of pure components that are required to be distilled

      Very limited work has been reported on vapor- liquid equilibrium study of binary mixtures containing 1- Heptanol as one of the component. Such components form industrially important combinations in petroleum and petrochemical industries. In view of their close boiling point and varied binary interactions, separation becomes difficult. For the rigorous simulation and optimization of the separation of C9 aromatic compounds, an accurate description of vapor-liquid equilibria is required.

      As part of a wide experimental and theoretical study on thermodynamic and physicochemical properties of binary liquid mixtures containing C9 aromatic compounds and linear alcohols, and with the aim of studying in depth, the behavior of these kinds of mixtures, we are reporting experimental vapor-liquid equilibrium data for binary mixture of 1-Heptanol (H) and 1, 2Dichloroethane(DE). The measurements were performed under isobaric conditions at a pressure of

      95.72 kPa using a modified version of the recirculating type equilibrium still i.e. SWIETOSLAWKI type ebulliometer.

   2. EASE OF USE

      1. Industrial uses of this binary mixtures

         Heptan-1-ol (CAS RN:111-70-6) has a pleasant smell and is used in cosmetics for its fragrance. Pure 1, 2- dichloroethane (CAS RN: 107-06-2) nd its application in many pharmaceutical and chemical industries as the primary solvent, and for resins and cellulose esters. In addition to above-mentioned applications, the mixture of these alcohols nd uses in solubilization (reaction medium), extraction, and crystallization of active pharmaceutical ingredients.

      2. Materials

      The reagents Heptanol-1, and 1, 2-Dichloroethane are purchased from Sigma-Aldrich Chemicals Pvt.

      Limited, India. The purities of the reagents are conrmed by gas chromatography with more than 0.99 mass fraction.

   3. METHODS FOR DETERMINATION OF VAPOUR LIQUID EQUILIBRIUM

      There are relatively few ideal system whose equilibrium relations can be calculated using Raoults law and Daltons law (i.e. from the known dependency of the vapour pressure of the pure constituents on temperature). On the other hand there are large numbers of industrially important systems whose equilibrium relations cannot be predicted from purely theoretical considerations of the both the phases analytically. The direct experimental determinations of vapour liquid equilibria require sampling of the liquid vapour, which are in thermodynamic equilibrium and determining the contacting of solutions.

      The methods for experimental determination of vapour-liquid-equilibria are classified into the following groups.

      1. Static method

      2. Distillation and Circulation method

      3. Dew and Bubble point method

      4. Flow method

      Distillation and circulation is direct method for the experimental determination of vapour- liquid-equilibria data.

      1. Apparatus for the estimation of vapour liquid equilibria:

         The apparatus used for the determination of vapour liquid equilibria is called EBULLIOMETER. There are different types of ebulliometers:

         1. Cottrell ebulliometer

         2. Washburn ebulliometer

         3. Swietoslawski ebulliometer

            The name ebulliometer has its roots in the Latin word "ebullio":meaning to boil or bubble up. An ebulliometer is designed to accurately measure the boiling point (temperature) of water or a water solution, by measuring the temperature of the vapour generated away from the heat source.

            An ebulliometer is designed to accurately m e a s u r e t h e boiling p o i n t of liquids by measuring the temperature of the vapor-liquid equilibrium either isobarically or isothermally. The method of using a vessel containing boiling substance into which the thermometer is immersed is not accurate. The boiling point measured by placing a thermometer in the boiling liquid above the vapour is not the actual boiling point.

            For example, a small amount of water may cause a large deviation of the condensation temperature from boiling point, COTTRELL and WASHBURN simultaneously published a method for this measurement of the boiling point of the liquid it was possible to determine the boiling point of liquid so accurately.

            B Equipment used:

            The equipment we used is SWIETOSLAWKI type ebulliometer is very similar to the one described by Halaetal (1958) was used for the experiments. One end of this ebulliometer was kept open so as to carry out experiment under a constant pressure equal to the atmospheric pressure.

            The thermometer bulb is located at the point in a thermo well filled with silicon oil where the gas liquid mixture impinges. The mixture samples to be studied are prepared by weighing the required amount of the pure liquids and stirring them well before charging them o the still. The heating rate is adjusted to yield the desired drop rate of about 30drops per minute [in accordance with

            suggestion of Hala(1958)]. The equilibrium temperature is recorded after steady state conditions judged by the constant temperature and uniform drop rate for at least 30 drops per minute.

            SKETCH OF EBULLIOMETER

            Figure-1

            An ebulliometer apparatus consists of-

            1. A chamber to hold the liquid whose boiling point is to be determined and is designed to allow for a semi-remote heat source.

            2. A condenser (reflux) to continually condense the vapour generated, to maintain the initial concentration of the liquid being tested.

            3. A special, precision thermometer calibrated in 0.02C with a range of 35-250C

            4. A heat source such as a heater.

            5. An outlet tap to allow removal of rinsing or tested liquid. A dedicated measuring cylinder marked at a 50ml volume.

      2. Experimental Determination Of Vapour Liquid Equilibria

      The test mixtures, in desired compositions were prepared gravimetrically using an electronic balance precise to ± 0.0001g. The prepared mixture was stirred well and charged to the ebulliometer and heated by gradually increasing the heat supply. The equilibrium state was observed by drop count of 30 per minute. The boiling point was ascertained by constancy of temperature for about 30 min. At this steady state, the temperature was noted by using a calibrated mercury thermometer (accurate to ± 1 K), and the samples withdrawn and analyzed.

   4. CALCULATIONS

      1. Mole fraction or composition (X1):-

         Isobaric Vapour-Liquid Equilibrium of Binary Mixture of 1,2-di-chloroethane with 1-Heptanol at 95.72 Kpa

         The given equation is used for calculation the mole fraction of given solution.

         1,2Dichloromethane(DE) + 1Heptanol(H).

         X1 = {[W1/M1[/[(W1/M1)+[W2/M2]} (1)

         Where W1 is weight, V1 is volume, 1 is density, X1 is the mole fraction and M1 is molar mass of low boiling substance i.e. 1, 2 Dichloroethane (DE) and W2 is weight, V2 is volume, 2 is density, X2 is the mole fraction and M2 is molar mass of high boiling substance i.e.

         1Heptanol (H).

         Low boiling substance (DE): High boiling substance (H):

         V1 = 5ml, 1 =1.168 and V2 = 48 ml,

         2= 0.822 and M1 = 98.96, M2= 116.

         X1= {[5*1.168/98.96]/[(5*1.168/98.96)+(48

         *0.822/116.204)]

         = 0.0590/0.0590+0.3985

         *X1 = 0.1478

         X2 = 1-X1 (2)

         1-0.1478 = 0.852

         X1=0.1478 X2=0.852

      2. Calculation of saturated vapour pressure ( P1s,P2s): Calculation of saturated vapour pressures using Antoine Equation.

         The equation is given by

         ln (p1) = A-[B/T(K)+C] (3)

         Where A, B and Care Antoine Constance and T(K) is temperature in Kelvin.

         • Antoine Constants are taken from property Data bank. Antoine constants for 1, 2-dichloroethane is

           Low boiling substance (DE):

           A= 16.1764, B = 2927.17, C= -50.22

           Antoine constants for1-heptanol is High boiling substance (H):

           A = 15.3068, B = 2626.42, C = -146.6

           ln (P1s)=16.1764-[2927.17/416.15-50.22] ln (P2s)=15.3068-[2626.42/416.15-146.6]

           • P1s = 3558.65 mmHg.

           • P2s = 260.624 mmHg.

      3. calculation of Activity coefficients (1,2)

         Calculation of activity coefficients by using Vanlaar equation, given by

         RT(K)ln1=A1 [1+ (A1X1/B1X 2 ] – 2 ( 4 )

         Where R is ideal gas constant A1=M1/1 and B1= M2/2

         R= 1.987(Kcal/Kmol. K), T = 416.15K, A1= 84.726 and B1= 141.367

         1.987*416.15ln1=

         84.726* [1+(84.726*0.148/141.367*0.8514)]-2

         826.890 ln1= 84.726[1+ 0.1046]-2

         826.890 ln1= 69.4342 ln1= 69.4342/826.890

         • 1= 1.0874

           Similarly 2

           R T (K)ln 2=B1[1+(B1X2/A1X2)]-2 (5)

         • 2= 1.0011

      4. Calculation of Excess Gibbs free energy (GE):

      GE = RT (K) [X1ln 1+X2ln 2] (6)

      =826.89* [0.1486*0.0839+0.8514*(1.5341*103)]

      • GE = 11.0769

      X1	Tk	P1s	P2s	1	2	log1/2	Y1	E G
      0.0715	424.15	4222.89	395.593	1.0962	1.0003	0.0397	0.0826	5.7872
      0.1486	416.15	3558.65	260.624	1.0875	1.0015	0.0357	0.7212	11.333
      0.2101	406.15	2842.37	179.051	1.0812	1.0033	0.0324	0.8081	15.353
      0.2579	403.15	2650.46	159.069	1.0751	1.0052	0.0291	0.8609	18.017
      0.3395	391.15	1979.42	96.2591	1.0657	1.0105	0.0230	0.9176	22.120
      0.4100	384.15	1653.38	70.1416	1.0568	1.0161	0.017	0.944	24.455
      0.4649	381.15	1527.08	60.8918	1.0495	1.0221	0.0149	0.9572	25.799
      0.5601	378.15	1408.38	52.6687	1.0369	1.0018	0.0149	0.9572	15.790
      0.6612	376.15	1333.13	61.5724	1.0243	1.0565	-0.013	0.9724	26.084
      0.7621	374.15	1261.39	43.1478	1.0134	1.0856	-0.029	0.9886	22.046
      0.8002	368.15	1063.69	31.565	1.0	1.1012	-0.037	0.992	19.918
      0.8890	365.15	974.311	26.8246	1.0	1.1464	-0.057	0.996	13.378
      0.9412	362.15	890.99	22.6931	1.0	1.1748	-0.069	0.9983	6.8454
      1.000	355.15	718.322	15.075	1.1275	1.2218	-0.348	1	84.689

      Table: 1 calculation of 1,2 Dichloroethane (DE) + 1 Heptanol (H)

      1

      0.8

      0.6

      0.4

      0.2

      0

      0.06

      0.04

      0.02

      0

      1.2

      1

      0.8

      0.6

      0.4

      0.2

      0

      H with DA

      Y1

      log1/2

      D. G r a p h s

      X1

      -0.04

      -0.06

      -0.08

      -0.02

      0.8 1 1.2

      0.6

      X1

      0 0.2 0.4

      Figure 2

      This graph shows the comparison between the liquid composition (X1) and vapor composition (Y1) of binary mixture DE +

      H.

      Figure 3

      This graph shows the comparison between the liquid composition (X1) and activity coefficients (log 1 / 2) of binary

      mixture DE + H.

      160

      140

      120

      100

      80

      60

      40

      20

      0

      0 0.2

      0.4 0.6 0.8

      X1 Y1

      1 1.2

      TEMP

      Figure 4

      -0.02

      This graph shows the comparison between the liquid (X1) and vapor (Y1) composition with temperature (T) of binary mixture DE

      + H.

      Discussions:

      Consistency of experimental values is determined by using HERINGTON TEST.

      (area above X-axis area below Y-axis)

      /(area above X-axis + area below Y-axis)

      < 0.02.

      1

      0.8

      0.6

      0.4

      0.2

      0

      0.06

      0.04

      0.02

      0

      log1/2

      Graph of log1/2vs x1

      -0.04

      -0.06

      -0.08

      X1

      30

      25

      20

      15

      10

      5

      0

      Figure 6

      GE

      Consistency Test:

      (0.011-0.044)/ (0.011+0.044) = -0.6 <0.02.

      Therefore value obtained by the above test is found to be true.

      0

      0.2

      0.4

      0.6

      X1

      0.8

      1

      1.2

      Figure 5

      This graph shows the comparison between the liquid composition (X1) and Excess Gibbs Free energy (GE) of binary

      mixture DE + H.

   5. RESULTS AND DISCUSSIONS:

      Vapour liquid equilibrium measurements are carried out for one binary mixture based on the its industrial importance in chemical engineering separation operation and strongly non ideal behavior.

      A thorough literature research has been conducted and revealed that no information is available for this system. Temperaturecomposition measurements are carried out at atmospheric pressures i.e.716 mmHg or718 mmHg. The calculations are done for Antoine constants to find vapour pressures, Vanlaar equation to find the activity coefficients, excess gibbs free energy.

   6. REFERENCES

1. Distillation by Van Winkle

2. Encyclopedia of chemical technology, fifth edition,volume2; Author Kirk-othmer.

3. Encyclopedia of science and technology, s i x t h e d i t i o n , v o l u m e 1 , 7 ;Author:GrawHill.

4. Encyclopedia of Industrial chemistry, fifth edition, volume 9;Author: Ullmanns.

5. Mass Transfer Operations by Robert E. Treybal.

6. T.E. Vittal Prasad, A.Sravan Kumar, D.H.L. Prasad; Fluid Phase Equilibria:201,(2002),4755

7. J.A. Riddick, W.S. Bunger, T,K.Sakno;

8. Organic Solvents: physical properties and methods of purification; Vol2, fourth edition, New York, 1986.

9. Journals of Chemical &Thermodynamic

10. Journals of Chemical & Fluid Phase Equilibria.

11. Properties of Liquids and Gases by Reid & Sherwood.