DOCSLIB.ORG

Corrected Values for Boiling Points and Enthalpies of Vaporization of Elements in Handbooks

Total Page：16

File Type：pdf, Size：1020Kb

Download full-text PDF Read full-text
Corrected Values for Boiling Points and Enthalpies of Vaporization of Elements in Handbooks CORE Metadata, citation and similar papers at core.ac.uk 328 J. Chem. Eng. Data 2011, 56, 328–337 Provided by e-Prints Soton Corrected Values for Boiling Points and Enthalpies of Vaporization of Elements in Handbooks Yiming Zhang Ningbo Institute of Material Technology & Engineering, Chinese Academy of Sciences, No. 519 Zhuangshi Road, Zhenhai District, Ningbo, Zhejiang Province, P.R. China 315201, and Department of Materials, Queen Mary University of London, Mile End Road, London E1 4NS, United Kingdom Julian R. G. Evans Department of Chemistry, University College London, 20 Gordon Street, London WC1H 0AJ, United Kingdom Shoufeng Yang* School of Engineering Sciences, University of Southampton, Southampton, SO17 1BJ, United Kingdom The scientific community relies upon the veracity of the scientific data in handbooks and databases. In a previous work, the authors developed a systematic, intelligent, and potentially automatic method to detect errors in such resources based on artificial neural networks (ANNs). This method revealed variations from (10 to 900) % in tables of property data for elements in the periodic table and pointed out the ones that are most probably correct. In this paper, we focus on the details of employing this method for analyzing the data of boiling points and enthalpies of vaporization recorded in different handbooks. The method points out the values that are likely to be correct. To verify the method employed, a detailed discussion of the data with reference to the original literature sources is given as well as factors that may affect the accuracy of the prediction. Introduction Experimental Details It is well-known that both the boiling point and the enthalpy Data Collection and Neural Network Construction. The data of vaporization are important thermodynamic properties that are are recorded from five different handbooks, including the required in product design and processes involving liquid and Chemistry Data Book (CDB),9 The Lange’s Handbook of vapor phase transitions such as distillation, vaporization, and Chemistry (LAG),10 The Elements (ELE),11 Table of Physical - drying1 3 and that, as a result, the quality and veracity of these and Chemical Constants (TPC),12 and CRC Handbook of data in handbooks are important for the academic and industrial Chemistry and Physics (CRC).13 The neural networks are scientific community.4 However, it is accepted that errors in constructed, trained, and simulated by employing MATLAB handbooks and databases are inescapable and are anticipated 7.4.0.287 (R2007a) software. A two-hidden layer network with 5-7 at rates of (1 to 5) %. tan-sigmoid transfer function in the first hidden layer and a linear This work challenges the inevitability of such high error rates. transfer function in the second hidden layer was established. A The values of boiling point and enthalpy of vaporization of the loop program was applied to redistribute the database to make elements were recorded for testing, because these data are the training set cover the problem domain.14,15 The detailed expected to be very reliable; only the elements with short half- process of data collection and neural network construction has lives were excluded. Tables 1 and 2 show the boiling point and been described in the authors’ related works.8 The ANN finds enthalpy of vaporization values of elements in the periodic table indirect relationships between data sets and then identifies values taken from five different handbooks. Considerable variation in which disobey the relationship. the values can be noticed, so it can be concluded that Stages of Error Correction. This includes four different inconsistencies are extant within these handbooks, and these stages. inconsistencies have persisted undetected into the 21st century. In the authors’ related work,8 we developed a systematic and Stage 1. During the exploration of the indirect relationship intelligent method based on artificial neural networks (ANNs) between boiling point and enthalpy of vaporization using data to detect wide levels of inconsistencies in handbooks and so from CDB (shown in Table 3) by an ANN, best linear fit stop their transmission to future researches and documents. In equations with a regression coefficient of R ) 0.973 and 0.972 this paper, we are going to show the details of application of were found (as shown in Figure 1). This result prompts us to this method in the case of correcting values of the boiling point raise the correlation hypothesis that the correlation applies to and enthalpy of vaporization for the elements. all of the elements. * Authors to whom correspondence should be addressed. E-mail: s.yang@ Stage 2. In this stage, a conformity criterion is selected. On soton.ac.uk. Tel.: 0044-23-8059-8697. Fax: 0044-23 8059 3016. the basis of the inconsistency within different handbooks, 10.1021/je1011086 2011 American Chemical Society Published on Web 01/11/2011 Journal of Chemical & Engineering Data, Vol. 56, No. 2, 2011 329 Table 1. List of Boiling Points Divided by Kelvin from Five Handbooksa element CDB LAGb ELE TPC CRC (max/min - 1) · 100 % Agc 2483 2483 2485 2433 2435 2.14 % Alc 2743 2743 2740 2793 2792 1.93 % Ar 87.15 87.15 87.29 87.29 87.3 0.17 % As (gray)d 886.2 886.2 889 883.2 876.2 1.46 % Au 3243 3243 3080 3123 3129 5.29 % Bae 1913 1913 1910 2173 2170 13.80 % Bee 2750 2750 3243f 2743 2744 18.20 % Bc 4203 4203 3931 4273 4273 8.70 % Bic 1833 1833 1883 1833 1837 2.73 % Br 331.7 332 331.9 332.1 332 0.12 % C (graphite)e 5103 5103 5100d - 4098d 24.50 % Ca 1760 1760 1757 1757 1757 0.17 % Cd 1038 1038 1038 1043 1040 0.48 % Cec 3743 3743 3699 3693 3716 1.35 % Cl 238.5 238.5 239.2 239.2 239.1 0.29 % Co 3173 3173 3143 3203 3200 1.91 % Cr 2755 2755 2945 2943 2944 6.90 % Cs 963.2 963.2 951.6 943.2 944.2 2.12 % Cu 2868 2868 2840 2833 2835 1.24 % Dy 2873 2873 2835 2833 2840 1.41 % Er 3173 3173 3136 3133 3141 1.28 % Eu 1713 1713 1870 1873 1802 9.34 % F 85.15 85.15 85.01 85.05 85.03 0.16 % Fe 3273 3273 3023 3133 3134 8.27 % Ga 2673 2673 2676 2473 2477 8.21 % Gd 3273 3273 3539 3533 3546 8.34 % Ge 3103 3103 3103 3103 3106 0.10 % H 21.15 21.15 20.28 20.28 20.28 4.29 % He 4.15 4.15 4.216 4.37 4.22 5.30 % Hfg 5673 5673 5470 4873 4876 16.40 % Hg 630.2 630.2 629.7 629.8 629.9 0.08 % Hoc 2873 2873 2968 2973 2973 3.48 % c I(I2) 457.2 457.2 457.5 457.2 457.6 0.09 % In 2273 2273 2353 2343 2345 3.52 % Irg 5573 5573 4403 4703 4701 26.60 % K 1047 1047 1047 1033 1032 1.45 % Krc 121.2 121.2 120.9 120 119.9 1.08 % La 3743 3743 3730 3733 3737 0.35 % Li 1603 1603 1620 1613 1615 1.06 % Lu 3603 3603 3668 3663 3675 2.00 % Mg 1383 1383 1363 1363 1363 1.47 % Mn 2373 2373 2235 2333 2334 6.17 % Mog 5833 5833 4885 4913 4912 19.40 % N 77.15 77.15 77.4 77.35 77.36 0.32 % Nac 1163 1163 1156 1153 1156 0.87 % Nbe 3573 3573 5015 4973 5017 40.40 % Nd 3303 3303 3341 3343 3347 1.33 % Ne 27.15 27.15 27.1 27.07 27.07 0.30 % Nib 3003 3003 3005 3263 3186 8.66 % O 90.15 90.15 90.19 90.19 90.2 0.06 % Osc 5273 5273 5300 5273 5285 0.51 % P (white)c 553.2 553.2 553 550.2 553.7 0.64 % Pb 2017 2017 2013 2023 2022 0.50 % Pde 4253 4253 3413 3233 3236 31.60 % Pre 3403 3403 3785 3783 3793 11.50 % Ptb,h 4803 4803 4100 4093 4098 17.40 % Rb 961.2 961.2 961 963.2 961.2 0.23 % Rec 5903 5903 5900 5873 5869 0.58 % Rhe 4773 4773 4000 3973 3968 20.30 % Ruh 5173 5173 4173 4423 4423 24.00 % S (monoclinic)c 718.2 718.2 717.8 717.8 717.8 0.06 % Sbg 1653 1653 1908 1860 1860 15.40 % Sc 3003 3003 3104 3103 3109 3.53 % Sec 958.2 958.2 958.1 958.2 958.2 0.01 % Sig 2633 2633 2628 3533 3538 34.60 % Smc 2173 2173 2064 2063 2067 5.33 % Sne 2543 2543 2543 2893 2875 13.80 % Sr 1653 1653 1657 1653 1655 0.24 % Ta 5693 5693 5698 5833 5731 2.46 % Tbg 3073 3073 3396 3493 3503 14.00 % Tec 1263 1263 1263 1263 1261 0.16 % Ti 3533 3533 3560 3563 3560 0.85 % Tl 1733 1733 1730 1743 1746 0.92 % Tme 2003 2003 2220 2223 2223 11.00 % Ve 3273 3273 3650 3673 3680 12.40 % W 6203 6203 5930 5823 5828 6.53 % 330 Journal of Chemical & Engineering Data, Vol. 56, No. 2, 2011 Table 1. Continued element CDB LAGb ELE TPC CRC (max/min - 1) · 100 % Xe 165.2 165.2 166.1 165.1 165 0.67 % Ybe 1703 1703 1466 1473 1469 16.20 % Ye 3203 3203 3611 3613 3618 13.00 % Zn 1180 1180 1180 1183 1180 0.25 % Zrg 3853 3853 4650 4673 4682 21.50 % a Acronyms as in text. This table does not have exclusions based on judgement.
Load more

Recommended publications
  • Physical Model for Vaporization
    Physical model for vaporization Jozsef Garai Department of Mechanical and Materials Engineering, Florida International University, University Park, VH 183, Miami, FL 33199 Abstract Based on two assumptions, the surface layer is flexible, and the internal energy of the latent heat of vaporization is completely utilized by the atoms for overcoming on the surface resistance of the liquid, the enthalpy of vaporization was calculated for 45 elements. The theoretical values were tested against experiments with positive result. 1. Introduction The enthalpy of vaporization is an extremely important physical process with many applications to physics, chemistry, and biology. Thermodynamic defines the enthalpy of vaporization ()∆ v H as the energy that has to be supplied to the system in order to complete the liquid-vapor phase transformation. The energy is absorbed at constant pressure and temperature. The absorbed energy not only increases the internal energy of the system (U) but also used for the external work of the expansion (w). The enthalpy of vaporization is then ∆ v H = ∆ v U + ∆ v w (1) The work of the expansion at vaporization is ∆ vw = P ()VV − VL (2) where p is the pressure, VV is the volume of the vapor, and VL is the volume of the liquid. Several empirical and semi-empirical relationships are known for calculating the enthalpy of vaporization [1-16]. Even though there is no consensus on the exact physics, there is a general agreement that the surface energy must be an important part of the enthalpy of vaporization. The vaporization diminishes the surface energy of the liquid; thus this energy must be supplied to the system.
    [Show full text]
  • Equation of State for Benzene for Temperatures from the Melting Line up to 725 K with Pressures up to 500 Mpa†
    High Temperatures-High Pressures, Vol. 41, pp. 81–97 ©2012 Old City Publishing, Inc. Reprints available directly from the publisher Published by license under the OCP Science imprint, Photocopying permitted by license only a member of the Old City Publishing Group Equation of state for benzene for temperatures from the melting line up to 725 K with pressures up to 500 MPa† MONIKA THOL ,1,2,* ERIC W. Lemm ON 2 AND ROLAND SPAN 1 1Thermodynamics, Ruhr-University Bochum, Universitaetsstrasse 150, 44801 Bochum, Germany 2National Institute of Standards and Technology, 325 Broadway, Boulder, Colorado 80305, USA Received: December 23, 2010. Accepted: April 17, 2011. An equation of state (EOS) is presented for the thermodynamic properties of benzene that is valid from the triple point temperature (278.674 K) to 725 K with pressures up to 500 MPa. The equation is expressed in terms of the Helmholtz energy as a function of temperature and density. This for- mulation can be used for the calculation of all thermodynamic properties. Comparisons to experimental data are given to establish the accuracy of the EOS. The approximate uncertainties (k = 2) of properties calculated with the new equation are 0.1% below T = 350 K and 0.2% above T = 350 K for vapor pressure and liquid density, 1% for saturated vapor density, 0.1% for density up to T = 350 K and p = 100 MPa, 0.1 – 0.5% in density above T = 350 K, 1% for the isobaric and saturated heat capaci- ties, and 0.5% in speed of sound. Deviations in the critical region are higher for all properties except vapor pressure.
    [Show full text]
  • Determination of the Identity of an Unknown Liquid Group # My Name the Date My Period Partner #1 Name Partner #2 Name
    Determination of the Identity of an unknown liquid Group # My Name The date My period Partner #1 name Partner #2 name Purpose: The purpose of this lab is to determine the identity of an unknown liquid by measuring its density, melting point, boiling point, and solubility in both water and alcohol, and then comparing the results to the values for known substances. Procedure: 1) Density determination Obtain a 10mL sample of the unknown liquid using a graduated cylinder Determine the mass of the 10mL sample Save the sample for further use 2) Melting point determination Set up an ice bath using a 600mL beaker Obtain a ~5mL sample of the unknown liquid in a clean dry test tube Place a thermometer in the test tube with the sample Place the test tube in the ice water bath Watch for signs of crystallization, noting the temperature of the sample when it occurs Save the sample for further use 3) Boiling point determination Set up a hot water bath using a 250mL beaker Begin heating the water in the beaker Obtain a ~10mL sample of the unknown in a clean, dry test tube Add a boiling stone to the test tube with the unknown Open the computer interface software, using a graph and digit display Place the temperature sensor in the test tube so it is in the unknown liquid Record the temperature of the sample in the test tube using the computer interface Watch for signs of boiling, noting the temperature of the unknown Dispose of the sample in the assigned waste container 4) Solubility determination Obtain two small (~1mL) samples of the unknown in two small test tubes Add an equal amount of deionized into one of the samples Add an equal amount of ethanol into the other Mix both samples thoroughly Compare the samples for solubility Dispose of the samples in the assigned waste container Observations: The unknown is a clear, colorless liquid.
    [Show full text]
  • The Basics of Vapor-Liquid Equilibrium (Or Why the Tripoli L2 Tech Question #30 Is Wrong)
    The Basics of Vapor-Liquid Equilibrium (Or why the Tripoli L2 tech question #30 is wrong) A question on the Tripoli L2 exam has the wrong answer? Yes, it does. What is this errant question? 30.Above what temperature does pressurized nitrous oxide change to a gas? a. 97°F b. 75°F c. 37°F The correct answer is: d. all of the above. The answer that is considered correct, however, is: a. 97ºF. This is the critical temperature above which N2O is neither a gas nor a liquid; it is a supercritical fluid. To understand what this means and why the correct answer is “all of the above” you have to know a little about the behavior of liquids and gases. Most people know that water boils at 212ºF. Most people also know that when you’re, for instance, boiling an egg in the mountains, you have to boil it longer to fully cook it. The reason for this has to do with the vapor pressure of water. Every liquid wants to vaporize to some extent. The measure of this tendency is known as the vapor pressure and varies as a function of temperature. When the vapor pressure of a liquid reaches the pressure above it, it boils. Until then, it evaporates until the fraction of vapor in the mixture above it is equal to the ratio of the vapor pressure to the total pressure. At that point it is said to be in equilibrium and no further liquid will evaporate. The vapor pressure of water at 212ºF is 14.696 psi – the atmospheric pressure at sea level.
    [Show full text]
  • Liquid-Vapor Equilibrium in a Binary System
    Liquid-Vapor Equilibria in Binary Systems1 Purpose The purpose of this experiment is to study a binary liquid-vapor equilibrium of chloroform and acetone. Measurements of liquid and vapor compositions will be made by refractometry. The data will be treated according to equilibrium thermodynamic considerations, which are developed in the theory section. Theory Consider a liquid-gas equilibrium involving more than one species. By definition, an ideal solution is one in which the vapor pressure of a particular component is proportional to the mole fraction of that component in the liquid phase over the entire range of mole fractions. Note that no distinction is made between solute and solvent. The proportionality constant is the vapor pressure of the pure material. Empirically it has been found that in very dilute solutions the vapor pressure of solvent (major component) is proportional to the mole fraction X of the solvent. The proportionality constant is the vapor pressure, po, of the pure solvent. This rule is called Raoult's law: o (1) psolvent = p solvent Xsolvent for Xsolvent = 1 For a truly ideal solution, this law should apply over the entire range of compositions. However, as Xsolvent decreases, a point will generally be reached where the vapor pressure no longer follows the ideal relationship. Similarly, if we consider the solute in an ideal solution, then Eq.(1) should be valid. Experimentally, it is generally found that for dilute real solutions the following relationship is obeyed: psolute=K Xsolute for Xsolute<< 1 (2) where K is a constant but not equal to the vapor pressure of pure solute.
    [Show full text]
  • Pressure Vs Temperature (Boiling Point)
    Boiling Points and Vapor Pressure Background Boiling Points and Vapor Pressure Background: Definitions Vapor Pressure: The equilibrium pressure of a vapor above its liquid; the pressure of the vapor resulting from the evaporation of a liquid above a sample of the liquid in a closed container. Boiling Point: The temperature at which the vapor pressure of a liquid is equal to the atmospheric (or applied) pressure. As the temperature of the liquid increases, the vapor pressure will increase, as seen below: https://www.chem.purdue.edu/gchelp/liquids/vpress.html Vapor pressure is interpreted in terms of molecules of liquid converting to the gaseous phase and escaping into the empty space above the liquid. In order for the molecules to escape, the intermolecular forces (Van der Waals, dipole- dipole, and hydrogen bonding) have to be overcome, which requires energy. This energy can come in the form of heat, aka increase in temperature. Due to this relationship between vapor pressure and temperature, the boiling point of a liquid decreases as the atmospheric pressure decreases since there is more room above the liquid for molecules to escape into at lower pressure. The graph below illustrates this relationship using common solvents and some terpenes: Pressure vs Temperature (boiling point) Ethanol Heptane Isopropyl Alcohol B-myrcene 290.0 B-caryophyllene d-Limonene Linalool Pulegone 270.0 250.0 1,8-cineole (eucalyptol) a-pinene a-terpineol terpineol-4-ol 230.0 p-cymene 210.0 190.0 170.0 150.0 130.0 110.0 90.0 Temperature (˚C) Temperature 70.0 50.0 30.0 10 20 30 40 50 60 70 80 90 100 200 300 400 500 600 760 10.0 -10.0 -30.0 Pressure (torr) 1 Boiling Points and Vapor Pressure Background As a very general rule of thumb, the boiling point of many liquids will drop about 0.5˚C for a 10mmHg decrease in pressure when operating in the region of 760 mmHg (atmospheric pressure).
    [Show full text]
  • Freezing and Boiling Point Changes
    Freezing Point and Boiling Point Changes for Solutions and Solids Lesson Plans and Labs By Ranald Bleakley Physics and Chemistry teacher Weedsport Jnr/Snr High School RET 2 Cornell Center for Materials Research Summer 2005 Freezing Point and Boiling Point Changes for Solutions and Solids Lesson Plans and Labs Summary: Major skills taught: • Predicting changes in freezing and boiling points of water, given type and quantity of solute added. • Solving word problems for changes to boiling points and freezing points of solutions based upon data supplied. • Application of theory to real samples in lab to collect and analyze data. Students will describe the importance to industry of the depression of melting points in solids such as metals and glasses. • Students will describe and discuss the evolution of glass making through the ages and its influence on social evolution. Appropriate grade and level: The following lesson plans and labs are intended for instruction of juniors or seniors enrolled in introductory chemistry and/or physics classes. It is most appropriately taught to students who have a basic understanding of the properties of matter and of solutions. Mathematical calculations are intentionally kept to a minimum in this unit and focus is placed on concepts. The overall intent of the unit is to clarify the relationship between changes to the composition of a mixture and the subsequent changes in the eutectic properties of that mixture. Theme: The lesson plans and labs contained in this unit seek to teach and illustrate the concepts associated with the eutectic of both liquid solutions, and glasses The following people have been of great assistance: Professor Louis Hand Professor of Physics.
    [Show full text]
  • Methods for the Determination of the Normal Boiling Point of a High
    Metalworking Fluids & VOC, Today and Tomorrow A Joint Symposium by SCAQMD & ILMA South Coast Air Quality Management District Diamond Bar, CA, USA March 8, 2012 Understanding & Determining the Normal Boiling Point of a High Boiling Liquid Presentation Outline • Relationship of Vapor Pressure to Temperature • Examples of VP/T Curves • Calculation of Airborne Vapor Concentration • Binary Systems • Relative Volatility as a function of Temperature • GC Data and Volatility • Everything Needs a Correlation • Conclusions Vapor Pressure Models (pure vapor over pure liquid) Correlative: • Clapeyron: Log(P) = A/T + B • Antoine: Log(P) = A/(T-C) + B • Riedel: LogP = A/T + B + Clog(T) + DTE Predictive: • ACD Group Additive Methods • Riedel: LogP = A/T + B + Clog(T) + DTE Coefficients defined, Reduced T = T/Tc • Variations: Frost-Kalkwarf-Thodos, etc. Two Parameters: Log(P) = A/T + B Vaporization as an CH OH(l) CH OH(g) activated process 3 3 G = -RTln(K) = -RTln(P) K = [CH3OH(g)]/[CH3OH(l)] G = H - TS [CH3OH(g)] = partial P ln(P) = -G/RT [CH3OH(l)] = 1 (pure liquid) ln(P) = -H/RT+ S/R K = P S/R = B ln(P) = ln(K) H/R = -A Vapor pressure Measurement: Direct versus Distillation • Direct vapor pressure measurement (e.g., isoteniscope) requires pure material while distillation based determination can employ a middle cut with a relatively high purity. Distillation allows for extrapolation and/or interpolation of data to approximate VP. • Direct vapor pressure measurement requires multiple freeze-thaw cycles to remove atmospheric gases while distillation (especially atmospheric distillation) purges atmospheric gases as part of the process. • Direct measurement OK for “volatile materials” (normal BP < 100 oC) but involved for “high boilers” (normal BP > 100 oC).
    [Show full text]
  • Corollary from the Exact Expression for Enthalpy of Vaporization
    Hindawi Publishing Corporation Journal of Thermodynamics Volume 2011, Article ID 945047, 7 pages doi:10.1155/2011/945047 Research Article Corollary from the Exact Expression for Enthalpy of Vaporization A. A. Sobko Department of Physics and Chemistry of New Materials, A. M. Prokhorov Academy of Engineering Sciences, 19 Presnensky Val, Moscow 123557, Russia Correspondence should be addressed to A. A. Sobko, [email protected] Received 14 November 2010; Revised 9 March 2011; Accepted 16 March 2011 Academic Editor: K. A. Antonopoulos Copyright © 2011 A. A. Sobko. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited. A problem on determining effective volumes for atoms and molecules becomes actual due to rapidly developing nanotechnologies. In the present study an exact expression for enthalpy of vaporization is obtained, from which an exact expression is derived for effective volumes of atoms and molecules, and under certain assumptions on the form of an atom (molecule) it is possible to find their linear dimensions. The accuracy is only determined by the accuracy of measurements of thermodynamic parameters at the critical point. 1. Introduction 1938 [2] with the edition from 1976 [3], we may find them actually similar. we may come to the same conclusion if In the present study, the relationship is obtained that we compare [2] with recent monograph by Prigogine and combines the enthalpy of vaporization with other thermody- Kondepudi “Modern Thermodynamics” [4]. The chapters namic evaporation parameters from the general expression devoted to first-order phase transitions in both monographs for the heat of first-order phase transformations.
    [Show full text]
  • Liquid Equilibrium Measurements in Binary Polar Systems
    DIPLOMA THESIS VAPOR – LIQUID EQUILIBRIUM MEASUREMENTS IN BINARY POLAR SYSTEMS Supervisors: Univ. Prof. Dipl.-Ing. Dr. Anton Friedl Associate Prof. Epaminondas Voutsas Antonia Ilia Vienna 2016 Acknowledgements First of all I wish to thank Doctor Walter Wukovits for his guidance through the whole project, great assistance and valuable suggestions for my work. I have completed this thesis with his patience, persistence and encouragement. Secondly, I would like to thank Professor Anton Friedl for giving me the opportunity to work in TU Wien and collaborate with him and his group for this project. I am thankful for his trust from the beginning until the end and his support during all this period. Also, I wish to thank for his readiness to help and support Professor Epaminondas Voutsas, who gave me the opportunity to carry out this thesis in TU Wien, and his valuable suggestions and recommendations all along the experimental work and calculations. Additionally, I would like to thank everybody at the office and laboratory at TU Wien for their comprehension and selfless help for everything I needed. Furthermore, I wish to thank Mersiha Gozid and all the students of Chemical Engineering Summer School for their contribution of data, notices, questions and solutions during my experimental work. And finally, I would like to thank my family and friends for their endless support and for the inspiration and encouragement to pursue my goals and dreams. Abstract An experimental study was conducted in order to investigate the vapor – liquid equilibrium of binary mixtures of Ethanol – Butan-2-ol, Methanol – Ethanol, Methanol – Butan-2-ol, Ethanol – Water, Methanol – Water, Acetone – Ethanol and Acetone – Butan-2-ol at ambient pressure using the dynamic apparatus Labodest VLE 602.
    [Show full text]
  • Vapor-Liquid Equilibrium Data and Other Physical Properties of the Ternary System Ethanol, Glycerine, and Water
    University of Louisville ThinkIR: The University of Louisville's Institutional Repository Electronic Theses and Dissertations 1936 Vapor-liquid equilibrium data and other physical properties of the ternary system ethanol, glycerine, and water Charles H. Watkins 1913-2004 University of Louisville Follow this and additional works at: https://ir.library.louisville.edu/etd Part of the Chemical Engineering Commons Recommended Citation Watkins, Charles H. 1913-2004, "Vapor-liquid equilibrium data and other physical properties of the ternary system ethanol, glycerine, and water" (1936). Electronic Theses and Dissertations. Paper 1940. https://doi.org/10.18297/etd/1940 This Master's Thesis is brought to you for free and open access by ThinkIR: The University of Louisville's Institutional Repository. It has been accepted for inclusion in Electronic Theses and Dissertations by an authorized administrator of ThinkIR: The University of Louisville's Institutional Repository. This title appears here courtesy of the author, who has retained all other copyrights. For more information, please contact [email protected]. l •1'1k- UNIVESSITY OF LOUISVILLE VAPOR-LIQUID EQUILIBRImr. DATA AND " OTHER PHYSICAL PROPERTIES OF THE TERNARY SYSTEM ETHANOL, GLYCERINE, AND WATER A Dissertation Submitted to the Faculty Of the Graduate School of the University of Louisville In Partial Fulfillment of the Requirements for the Degree Of Master of Science In Chemical Engineering Department of Chemical Engineering :By c CP.ARLES H. WATK INS 1936 i - J TABLE OF CONTENTS Chapter I Introduotlon-------------------2 II Theoretloal--------------------5 III Apparatue ~ Prooedure----------12 IV Experlnental Mater1ale--~----~---~~-~--~-~~~22 Preparation of Samplee---------22 BpecIflc Reats-----------------30 ~oI11n~ Polnts-----------------34 Vapor rressure-----------------37 Latent Heats-------------------51 Vapor-LiquId EquI1Ibrlum-------53 Freez1ne Points----------------62 V Concluclone--------------------67 VI RIbl1ography-------------------69 J .____ ~~ ___________.
    [Show full text]
  • Song and Mason Equation of State for Refrigerants © 2014, Sociedad Química De México235 ISSN 1870-249X Song and Mason Equation of State for Refrigerants
    J. Mex. Chem. Soc. 2014, 58(2), 235-238 ArticleSong and Mason Equation of State for Refrigerants © 2014, Sociedad Química de México235 ISSN 1870-249X Song and Mason Equation of State for Refrigerants Farkhondeh Mozaffari Department of Chemistry, College of Sciences, Persian Gulf University, Boushehr, Iran. [email protected] Received February 10th, 2014; Accepted April 21st, 2014 Abstract. In this work, the Song and Mason equation of state has been Resumen. En este trabajo, la ecuación de estado de Song y Mason se applied to calculate the PVT properties of refrigerants. The equation ha utilizado para calcular las propiedades PVT de los refrigerantes. of state is based on the statistical-mechanical perturbation theory of La ecuación de estado se basa en la teoría de la perturbación de la hard convex bodies. The theory has considerable predictive power, mecánica estadística de cuerpos convexos duros. La teoría tiene una since it permits the construction of the PVT surface from the normal gran capacidad de predicción, ya que permite la construcción de la boiling temperature and the liquid density at the normal boiling point. superficie PVT sólo a partir de la temperatura y de la densidad del The average absolute deviation for the calculated densities of 11 re- líquido en el punto de ebullición normal. La desviación absoluta media frigerants is 1.1%. de las densidades calculadas de 11 refrigerantes es del 1.1%. Key words: equation of state; liquid density; normal boiling point; Palabras clave: Ecuación de estado; densidad del líquido; punto de refrigerants; statistical mechanics. ebullición normal; refrigerantes; mecánica estadística. Introduction thermophysical behavior of refrigerants over a wide range of temperatures and pressures.
    [Show full text]