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Isobaric Vapor-Liquid Equilibrium for Methyldichlorosilane- * Methyltrichlorosilane-Dimethyldichlorosilane System

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Isobaric Vapor-Liquid Equilibrium for Methyldichlorosilane- * Methyltrichlorosilane-Dimethyldichlorosilane System 中国科技论文在线 http://www.paper.edu.cn Qiu et al. / J Zhejiang Univ SCI 2005 6B(6):559-562 559 Journal of Zhejiang University SCIENCE ISSN 1009-3095 http://www.zju.edu.cn/jzus E-mail: [email protected] Isobaric vapor-liquid equilibrium for methyldichlorosilane- * methyltrichlorosilane-dimethyldichlorosilane system †1,2 1 1 1 QIU Zu-min (邱祖民) , XIE Xin-liang (谢心亮) , LUO Mei (罗 美) , XIE Feng-xia (谢凤霞) (1School of Environmental Science and Engineering, Nanchang University, Nanchang 330029, China) (2Key Laboratory of Poyang Lake Ecology and Bio-resource Utilization, Nanchang University, Nanchang 330029, China) †E-mail: [email protected] Received Oct. 26, 2004; revision accepted Mar. 1, 2005 Abstract: This paper describes measurement of vapor-liquid equilibrium (VLE) data of methyldichlorosilane-methyltrichloro- silane-dimethyldichlorosilane system and that of the three binary systems at 101.325 kPa with a new pump-ebulliometer. The equilibrium composition of the vapor phase was calculated from pTx by indirect method. The model parameters of the liquid activity coefficient of the Wilson, NRTL, Margules and van Laar equations was corrected by the least square method. The ternary system VLE data were predicted by the Wilson equation, with the calculated boiling points showing good agreement with the experimental data. Key words: Ebulliometer, Vapor-liquid equilibrium, Methyldichlorosilane, Methyltrichlorosilane, Dimethyldichlorosilane doi:10.1631/jzus.2005.B0559 Document code: A CLC number: O642.42 INTRODUCTION vapor-liquid equilibrium for multicomponent systems containing halogenated silane. In order to provide Vapor-liquid equilibrium (VLE) data are very some necessary basic data on silicon derivatives, important in the design and operation of separation these systems are selected for study. The VLE data processes in chemical industry. Such information can are measured by the total pressure-temperature-liquid be obtained experimentally or estimated by using composition (pTx) method. In this study, the VLE generalized methods for calculation of the properties data are determined at 101.325 kPa for methyldi- of mixtures. For ideal system, it is relatively easy to chloroslane-methyltrichlorosilane-dimethyldichloro- estimate vapor-liquid equilibrium. However, most silane and constituent binary system. The results systems of industrial interest show deviations from calculated by the activity coefficient models were the ideal behavior. shown to be in good agreement with the experimental The methyldichlorosilane-methyltrichlorosilane- data. dimethyldichlorosilane and constituent binary system are of importance in the production of silicon, while VLE data of these systems are very scarce in the lit- EXPERIMENTAL erature. Only in the past several years did some re- searchers (Ana et al., 1995; Liviu et al., 1995; Wu and Materials Cai, 1997; Xie et al., 1998) begin to study isobaric Methyldichlorosilane, methyltrichlorosilane and dimethyldichlorosilane were obtained from Xinhuo Chemical Factory, Jiangxi. All the chemicals were * Project supported by the Foundation of Science and Technology, the Ministry of Education (No. 03071), and The Natural Science Foun- purified by distillation in a laboratory column to a dation of Jiangxi Province (No. 0320013), China purity of more than 99.5% by gas chromatography 转载 中国科技论文在线 http://www.paper.edu.cn 560 Qiu et al. / J Zhejiang Univ SCI 2005 6B(6):559-562 (GC) analysis. Methyldichlorosilane, methyltri- RESULTS AND DISCUSSION chlorosilane and dimethyldichlorosilane should be purified just before measurement because they may At low and moderate pressures, the pointing easily react with water when exposed to the air. factor is negligible, so the equilibrium relations is as Comparison between some of the measured data and follows literature data is given Table 1. PyPxϕˆ = ssϕγ (1) Table 1 Boiling point of pure component ii i iii Boiling point (K) Component where yi is the mole fraction of component i in the Lit. Exp. vapor phase, ϕˆ is the fugacity coefficient of com- Methyldichlorosilane 314.15 (Dean, 2003) 314.41 i ponent i in the vapor phase, P is the total pressure, γ is Methyltrichlorosilane 339.55 (Dean, 2003) 339.50 i Dimethyldichlorosilane 343.15 (Dean, 2003) 343.46 the activity coefficient of component i in the vapor phase, xi is the mole fraction of component i in the s Apparatus and procedure liquid phase, ϕi is the pure component fugacity co- s A new type of magnetical pump-ebulliometer, efficient at saturation, and Pi is the vapor pressure of described in detail by Qiu et al.(1995) was used for pure component i. The coefficients of ϕˆ and ϕ s measuring the boiling points with different liquid i i were evaluated using the second virial coefficients phase compositions (Qiu et al., 1997). The apparatus from the critical data, respectively. The vapor pres- was an all-glass dynamic recirculation still with total −4 3 s volume of about 1.00×10 m . During the run, the sure of pure component, Pi is calculated by the An- still was submerged in a constant temperature bath toine equation. The critical data and Antoine con- about 3 °C below the equilibrium boiling point. The stants of the pure component are given in Table 2. atmospheric pressure, P, was measured by a The experimental data were correlated using the Fortin-type mercury barometer. Since the barometric Wilson, NRTL, Margules and van Laar equations f. pressure changed slightly, the experimental tem- The optimal parameters were obtained by minimiza- peratures were automatically corrected to that at tion of the objective function F (Qiu et al., 1994). 101.325 kPa. The equilibrium temperature, T, was measured using a standard mercury thermometer with 22 Frfarfa=∑|ln(1 ) cal − 1 (ik )| +∑ |ln( 2 ) cal − 2 ( ik )| (2) accuracy of 0.1 K. In each experiment, a known mass of the material was introduced into the still from the where γ , γ are the activity coefficient of component injector and was heated at a fixed pressure of 101.325 1 2 kPa by an automatic regulation system. The accuracy 1and component 2 in the liquid phase, ai is model of the liquid and vapor phase was constant. The liquid parameter. k is the point of difference. compositions component was added into the still. The The binary systems VLE data were used to plot vapor compositions, yi, were calculated from the ex- the three graphs in Fig.1. perimental pTx data by an indirect method (Qiu et al., The model parameters of liquid activity coeffi- 1994). This pTx method was based on the Q function cient and the absolute average deviations are listed in (The function of molar excess Gibbs energy) and had Table 3 showing that the deviations of Wilson, NRTL, rigorous thermodynamic consistency (Hu, 1982). Margules equations are reasonably small, especially * Table 2 Antoine constants, critical temperature, pressure and volume of the pure components −6 3 Component A B C Tc (K) Pc (kPa) Vc (10 m /mol) Methyldichlorosilane 7.0484 1179 242 475 3901.1 290 (Rugina and Sacarescu, 1992) Methyltrichlorosilane 6.8721 1167 226 518 5562.7 339 (Rugina and Sacarescu, 1992) Dimethyldichlorosilane 7.1435 1328 241 520 3485.6 350 (Rugina and Sacarescu, 1992) * A, B, C: Antoine constants; Tc: Critical temperature; Pc: Critical pressure; Vc: Critical volume 中国科技论文在线 http://www.paper.edu.cn Qiu et al. / J Zhejiang Univ SCI 2005 6B(6):559-562 561 1.0 1.0 345 1.0 340 344 344 336 0.8 340 0.8 0.8 336 332 343 0.6 332 0.6 0.6 328 (K) (K) 342 328 T T (K) (mol/mol) (mol/mol) 324 0.4 T 0.4 0.4 y (mol/mol) 324 y 341 320 y 320 0.2 0.2 340 0.2 316 316 312 0.0 312 0.0 339 0.0 0.0 0.2 0.4 0.6 0.8 1.0 0.0 0.2 0.4 0.6 0.8 1.0 0.0 0.2 0.4 0.6 0.8 1.0 x (mol/mol) x (mol/mol) x (mol/mol) (a) (b) (c) Fig.1 VLE curve of (a) methyldichlorosilane+methylltrichlorosilane; (b) methyldichlorosilane+dimethyldichlorosilane; (c) methyltrichlorosilane+dimethyldichlorosilane • Calculated vapor phase points; − Calculated temperature curve; ◦ Experimental temperature data that of the Wilson equation, while the deviations of dichlorosilane and constituent binary systems were the van Laar equation is a little bigger. So the activity measured at 101.325 kPa. The equilibrium compo- coefficient models are suitable for representing the sition of the vapor phase was calculated from pTx by binary experimental data. The binary parameters of the indirect method. The experimental data were the Wilson model given in Table 3 were used to pre- correlated using the Wilson, NRTL, Margules and dict the VLE data of the ternary system. The results van Laar equations. It was shown that the deviations were satisfactory. The VLE data of the ternary system of the Wilson, NRTL, Margules equations were and the average deviation in boiling temperatures are reasonably small, while the deviation of the van Laar listed in Table 4. equation was a little bigger. Ternary system VLE data were predicted by the Wilson equation; the calculated boiling points accorded well with ex- CONCLUSION perimental data. The results showed that the calcu- lated boiling point is fitted by the models which sat- Vapor-liquid equilibrium for a ternary system of isfied the need for the design and operation of sepa- methyldichloroslane-methyltrichlorosilane-dimethyl- ration processes. Table 3 Model parameters and the absolute average deviations Parameters and Methyldichlorosilane (1)+ Methyldichlorosilane (1)+ Methyltrichloroslane (1)+ Equation deviations methyltrichlorosilane (2) dimethyldichlorosilane (2) dimethyldichloroslane (2) Wilson A −38.1 −120.1 −28.9 B 0.05 0.1 0.11 * dt 0.17 0.14 0.07 ** dy 0.004 0.0089 0.006 NRTL A −66.5 −0.1 −142.2 B 0.01 −148.7 −1.4 Aij 0.05 0.3 0.08 dt 0.14 0.15 0.09 d 0.0038 0.0081 0.0039 y Margules A −0.125 −0.41 −0.34 B −0.11 −0.12 −0.13 dt 0.15 0.5 0.28 dy 0.0039 0.0042 0.007 van Laar A 0.001 0.0001 0.0001 B 0.003 0.05 0.03 dt 0.61 1.34 1.15 dy 0.0074 0.0157 0.0155 * ** dt=∑|T-Tmod|/N, dy=∑|ycal-ymod|/N, N=Number of data points; Tmod: Calculated boiling point from model (K); ycal: Calculated vapor phase mole fraction from pTx; ymol: Calculated vapor phase mole fraction from mode 中国科技论文在线 http://www.paper.edu.cn 562 Qiu et al.
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