Thermodynamics of Element Volatility and Its Application to Planetary Processes Paolo A
Total Page:16
File Type:pdf, Size:1020Kb
Load more
Recommended publications
-
Determining Volatile Organic Carbon by Differential Scanning Calorimetry
DETERMINING VOLATILE ORGANIC CARBON BY DIFFERENTIAL SCANNING CALORIMETRY By Roger L. Blaine TA Instrument, Inc. Volatile Organic Carbons (VOCs) are known to have serious environmental effects. Because of these deleterious effects, large scale attempts are being made to measure, reduce and regulate VOC use and emission. The California EPA, for example, requires characterization of the total volatility of pesticides based upon a TGA loss-on-drying test method [1, 2]. In another move, countries of the European market have reached a protocol agreement to reduce and stabilize VOC emissions by the year 2000 to 70% of the 1991 values [3]. And recently the Swiss Federal Government has imposed a tax on the amount of VOC [4]. Such regulatory agreements require qualitative and quantitative tools to assess what is a VOC and how much is present in a given formulation. Chief targets for VOC action include the paints and coatings industries, agricultural pesticides and solvent cleaning processes. VOC’s are defined as those organic materials having a vapor pressure greater than 10 Pa at 20 °C or having corresponding volatility at other operating temperatures associated with industrial processes [3]. Differential scanning calorimetry (DSC) is a useful tool for screening for potential VOC candidates as well as the actual determination of vapor pressure of suspect materials. Both of these measurements are based on the determination of the boiling (or sublimation) temperature; the former under atmospheric conditions, the latter under reduced pressures. Figure 1 725 ° exo 180 C µ size: 10 l 580 prog: 10°C / min atm: N2 Heat Flow Heat Flow 2.25mPa 435 (326 psi) [ ----] Pressure (psi) endo 290 50 100 150 200 250 300 Temperature (°C) TA250 Nielson and co-workers [5] have observed that: • All organic solvents with boiling temperatures below 170 °C are classified as VOCs, and • No organics solvents with boiling temperatures greater than 260 °C are VOCs. -
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. -
Transport of Dangerous Goods
ST/SG/AC.10/1/Rev.16 (Vol.I) Recommendations on the TRANSPORT OF DANGEROUS GOODS Model Regulations Volume I Sixteenth revised edition UNITED NATIONS New York and Geneva, 2009 NOTE The designations employed and the presentation of the material in this publication do not imply the expression of any opinion whatsoever on the part of the Secretariat of the United Nations concerning the legal status of any country, territory, city or area, or of its authorities, or concerning the delimitation of its frontiers or boundaries. ST/SG/AC.10/1/Rev.16 (Vol.I) Copyright © United Nations, 2009 All rights reserved. No part of this publication may, for sales purposes, be reproduced, stored in a retrieval system or transmitted in any form or by any means, electronic, electrostatic, magnetic tape, mechanical, photocopying or otherwise, without prior permission in writing from the United Nations. UNITED NATIONS Sales No. E.09.VIII.2 ISBN 978-92-1-139136-7 (complete set of two volumes) ISSN 1014-5753 Volumes I and II not to be sold separately FOREWORD The Recommendations on the Transport of Dangerous Goods are addressed to governments and to the international organizations concerned with safety in the transport of dangerous goods. The first version, prepared by the United Nations Economic and Social Council's Committee of Experts on the Transport of Dangerous Goods, was published in 1956 (ST/ECA/43-E/CN.2/170). In response to developments in technology and the changing needs of users, they have been regularly amended and updated at succeeding sessions of the Committee of Experts pursuant to Resolution 645 G (XXIII) of 26 April 1957 of the Economic and Social Council and subsequent resolutions. -
The Acidity of Atmospheric Particles and Clouds Havala O
The Acidity of Atmospheric Particles and Clouds Havala O. T. Pye1, Athanasios Nenes2,3, Becky Alexander4, Andrew P. Ault5, Mary C. Barth6, Simon L. Clegg7, Jeffrey L. Collett, Jr.8, Kathleen M. Fahey1, Christopher J. Hennigan9, Hartmut Herrmann10, Maria Kanakidou11, James T. Kelly12, I-Ting Ku8, V. Faye McNeill13, Nicole Riemer14, Thomas 5 Schaefer10, Guoliang Shi15, Andreas Tilgner10, John T. Walker1, Tao Wang16, Rodney Weber17, Jia Xing18, Rahul A. Zaveri19, Andreas Zuend20 1Office of Research and Development, U.S. Environmental Protection Agency, Research Triangle Park, NC, 27711, USA 2School of Architecture, Civil and Environmental Engineering, Ecole Polytechnique Fédérale de Lausanne, Lausanne, CH- 1015, Switzerland 10 3Institute for Chemical Engineering Sciences, Foundation for Research and Technology Hellas, Patras, GR-26504, Greece 4Department of Atmospheric Science, University of Washington, Seattle, WA, 98195, USA 5Department of Chemistry, University of Michigan, Ann Arbor, MI, 48109-1055, USA 6National Center for Atmospheric Research, Boulder, CO, 80307, USA 7School of Environmental Sciences, University of East Anglia, Norwich NR4 7TJ, UK 15 8Department of Atmospheric Science, Colorado State University, Fort Collins, CO, 80523, USA 9Department of Chemical, Biochemical, and Environmental Engineering, University of Maryland Baltimore County, Baltimore, MD, 21250, USA 10Leibniz Institute for Tropospheric Research (TROPOS), Atmospheric Chemistry Department (ACD), Leipzig, 04318, Germany 20 11Department of Chemistry, University -
Chapter 3 Equations of State
Chapter 3 Equations of State The simplest way to derive the Helmholtz function of a fluid is to directly integrate the equation of state with respect to volume (Sadus, 1992a, 1994). An equation of state can be applied to either vapour-liquid or supercritical phenomena without any conceptual difficulties. Therefore, in addition to liquid-liquid and vapour -liquid properties, it is also possible to determine transitions between these phenomena from the same inputs. All of the physical properties of the fluid except ideal gas are also simultaneously calculated. Many equations of state have been proposed in the literature with either an empirical, semi- empirical or theoretical basis. Comprehensive reviews can be found in the works of Martin (1979), Gubbins (1983), Anderko (1990), Sandler (1994), Economou and Donohue (1996), Wei and Sadus (2000) and Sengers et al. (2000). The van der Waals equation of state (1873) was the first equation to predict vapour-liquid coexistence. Later, the Redlich-Kwong equation of state (Redlich and Kwong, 1949) improved the accuracy of the van der Waals equation by proposing a temperature dependence for the attractive term. Soave (1972) and Peng and Robinson (1976) proposed additional modifications of the Redlich-Kwong equation to more accurately predict the vapour pressure, liquid density, and equilibria ratios. Guggenheim (1965) and Carnahan and Starling (1969) modified the repulsive term of van der Waals equation of state and obtained more accurate expressions for hard sphere systems. Christoforakos and Franck (1986) modified both the attractive and repulsive terms of van der Waals equation of state. Boublik (1981) extended the Carnahan-Starling hard sphere term to obtain an accurate equation for hard convex geometries. -
Carbon Dioxide and Chemical Looping: Current Research Trends Lukas C
Review Cite This: Ind. Eng. Chem. Res. XXXX, XXX, XXX−XXX pubs.acs.org/IECR 110th Anniversary: Carbon Dioxide and Chemical Looping: Current Research Trends Lukas C. Buelens, Hilde Poelman, Guy B. Marin, and Vladimir V. Galvita* Laboratory for Chemical Technology, Ghent University, Technologiepark 125, B-9052 Ghent, Belgium *S Supporting Information ABSTRACT: Driven by the need to develop technologies for converting CO2, an extraordinary array of chemical looping based process concepts has been proposed and researched over the past 15 years. This review aims at providing first a historical context of the molecule CO2, which sits at the center of these developments. Then, different types of chemical looping related to CO2 are addressed, with attention to process concepts, looping materials, and reactor configu- rations. Herein, focus lies on the direct conversion of carbon dioxide into carbon monoxide, a process deemed to have economic potential. 1. THE DISCOVERY OF CARBON DIOXIDE designate CO2 and CO probably occurred only after the Carbon dioxide was probably discovered around 1640 by Jan foundation of the International Union on Pure and Applied Baptist van Helmont, who named it spiritus sylvestre.1,2 When Chemistry (IUPAC) in 1919. burning a piece of wood, van Helmont noticed that the mass of 1,2 2. CARBON DIOXIDE AND THE EARTH’S CLIMATE the ash was considerably less than that of the original wood. He argued that a gas had volatilized from the wood.1,2 Over a In the 1820s, Joseph Fourier made heat transfer calculations hundred years later, around 1750, Joseph Black looked into based on knowledge of that time−between the Sun and the 9,10 carbon dioxide released by magnesium carbonate upon heating Earth. -
Molecular Corridors and Parameterizations of Volatility in the Chemical Evolution of Organic Aerosols
Atmos. Chem. Phys., 16, 3327–3344, 2016 www.atmos-chem-phys.net/16/3327/2016/ doi:10.5194/acp-16-3327-2016 © Author(s) 2016. CC Attribution 3.0 License. Molecular corridors and parameterizations of volatility in the chemical evolution of organic aerosols Ying Li1,2, Ulrich Pöschl1, and Manabu Shiraiwa1 1Multiphase Chemistry Department, Max Planck Institute for Chemistry, Mainz, Germany 2State Key Laboratory of Atmospheric Boundary Layer Physics and Atmospheric Chemistry (LAPC), Institute of Atmospheric Physics, Chinese Academy of Sciences, Beijing, China Correspondence to: Manabu Shiraiwa ([email protected]) Received: 23 September 2015 – Published in Atmos. Chem. Phys. Discuss.: 15 October 2015 Revised: 1 March 2016 – Accepted: 3 March 2016 – Published: 14 March 2016 Abstract. The formation and aging of organic aerosols (OA) 1 Introduction proceed through multiple steps of chemical reaction and mass transport in the gas and particle phases, which is chal- lenging for the interpretation of field measurements and lab- Organic aerosols (OA) consist of a myriad of chemical oratory experiments as well as accurate representation of species and account for a substantial mass fraction (20–90 %) OA evolution in atmospheric aerosol models. Based on data of the total submicron particles in the troposphere (Jimenez from over 30 000 compounds, we show that organic com- et al., 2009; Nizkorodov et al., 2011). They influence regional pounds with a wide variety of functional groups fall into and global climate by affecting radiative budget of the at- molecular corridors, characterized by a tight inverse cor- mosphere and serving as nuclei for cloud droplets and ice relation between molar mass and volatility. -
United States Patent (19) 11) 4,080,491 Kobayashi Et Al
United States Patent (19) 11) 4,080,491 Kobayashi et al. 45) Mar. 21, 1978 54) PROCESS OF PRODUCING RING-OPENING 56 References Cited POLYMERIZATION PRODUCTS U.S. PATENT DOCUMENTS (75) Inventors: Yukio Kobayashi; Takashi Ueshima; 3,798,175 3/1974 Streck .................................. 526/136 Shoichi Kobayashi, all of Yokohama, 3,856,758 - 12/1974 Ueshima ............................... 526/169 Japan 3,859,265 1/1975 Hepworth ............................ 526/281 3,959,234 5/1976 Kurosawa ............................ 526/281 Assignee: Showa Denko K.K., Tokyo, Japan (73) Primary Examiner-Paul R. Michl 21 Appl. No.: 714,833 Attorney, Agent, or Firm-Fitzpatrick, Cella, Harper & 22) Filed: Aug. 16, 1976 Scinto Foreign Application Priority Data 57 ABSTRACT (30) A process of producing a ring-opening polymerization Aug. 27, 1975 Japan ................................ 50-103060 product of a norbornene derivative containing at least Mar. 26, 1976 Japan .................................. 51-32464 one polar group or aromatic group, a norbornadiene Mar. 26, 1976 Japan .................................. 51-32465 derivative containing at least one of said groups or a Apr. 5, 1976 Japan .................................. 51-37274 cycloolefin using a catalyst system prepared from an Apr. 27, 1976 Japan .................................. 51-47268 organometallic compound and the reaction product of May 25, 1976 Japan .................................. 51-59642 tungsten oxide or molybdenum oxide and a phosphorus 51 Int. C.’................................................ C08F 4/78 pentahalide or phosphorus oxytrihalide or these com (52) U.S. C. ..... o e s p s 8 v 8 526/137; 526/113; pounds and other third components. The catalyst sys 526/127; 526/136; 526/169; 526/281; 526/308 temi possesses a high polymerization activity. (58) Field of Search .................... -
Theoretical and Experimental Aspects of Current and Future Research on Nbo2 Thin Film Devices
crystals Review Theoretical and Experimental Aspects of Current and Future Research on NbO2 Thin Film Devices Denis Music 1,* , Andreas M. Krause 1 and Pär A. T. Olsson 1,2 1 Department of Materials Science and Applied Mathematics, Malmö University, SE-205 06 Malmö, Sweden; [email protected] (A.M.K.); [email protected] (P.A.T.O.) 2 Division of Mechanics, Lund University, Box 118, SE-221 00 Lund, Sweden * Correspondence: [email protected]; Tel.: +46-40-6658709 Abstract: The present research front of NbO2 based memory, energy generation, and storage thin film devices is reviewed. Sputtering plasmas contain NbO, NbO2, and NbO3 clusters, affecting nucleation and growth of NbO2, often leading to a formation of nanorods and nanoslices. NbO2 (I41/a) undergoes the Mott topological transition at 1081 K to rutile (P42/mnm), yielding changes in the electronic structure, which is primarily utilized in memristors. The Seebeck coefficient is a key physical parameter governing the performance of thermoelectric devices, but its temperature behavior is still controversial. Nonetheless, they perform efficiently above 900 K. There is a great potential to improve NbO2 batteries since the theoretical capacity has not been reached, which may be addressed by future diffusion studies. Thermal management of functional materials, comprising thermal stress, thermal fatigue, and thermal shock, is often overlooked even though it can lead to failure. NbO2 exhibits relatively low thermal expansion and high elastic modulus. The future for NbO2 thin film devices looks promising, but there are issues that need to be tackled, such as dependence of properties on strain and grain size, multiple interfaces with point and extended defects, and interaction with various natural and artificial environments, enabling multifunctional Citation: Music, D.; Krause, A.M.; applications and durable performance. -
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. -
Mineral Commodity Summareis 2013
U.S. Department of the Interior U.S. Geological Survey MINERAL COMMODITY SUMMARIES 2013 Abrasives Fluorspar Mercury Silver Aluminum Gallium Mica Soda Ash Antimony Garnet Molybdenum Sodium Sulfate Arsenic Gemstones Nickel Stone Asbestos Germanium Niobium Strontium Barite Gold Nitrogen Sulfur Bauxite Graphite Peat Talc Beryllium Gypsum Perlite Tantalum Bismuth Hafnium Phosphate Rock Tellurium Boron Helium Platinum Thallium Bromine Indium Potash Thorium Cadmium Iodine Pumice Tin Cement Iron and Steel Quartz Crystal Titanium Cesium Iron Ore Rare Earths Tungsten Chromium Iron Oxide Pigments Rhenium Vanadium Clays Kyanite Rubidium Vermiculite Cobalt Lead Salt Wollastonite Copper Lime Sand and Gravel Yttrium Diamond Lithium Scandium Zeolites Diatomite Magnesium Selenium Zinc Feldspar Manganese Silicon Zirconium U.S. Department of the Interior KEN SALAZAR, Secretary U.S. Geological Survey Marcia K. McNutt, Director U.S. Geological Survey, Reston, Virginia: 2013 Manuscript approved for publication January 24, 2013. For more information on the USGS—the Federal source for science about the Earth, its natural and living resources, natural hazards, and the environment— visit http://www.usgs.gov or call 1–888–ASK–USGS. For an overview of USGS information products, including maps, imagery, and publications, visit http://www.usgs.gov/pubprod For sale by the Superintendent of Documents, U.S. Government Printing Office Mail: Stop IDCC; Washington, DC 20402–0001 Phone: (866) 512–1800 (toll-free); (202) 512–1800 (DC area) Fax: (202) 512–2104 Internet: bookstore.gpo.gov Any use of trade, product, or firm names is for descriptive purposes only and does not imply endorsement by the U.S. Government. Although this report is in the public domain, permission must be secured from the individual copyright owners to reproduce any copyrighted material contained within this report. -
Chaotic Temperatures Vs Coefficients of Thermodynamic Activity: the Advantage of the Method of Chemical Dynamics
CHAOTIC TEMPERATURES VS COEFFICIENTS OF THERMODYNAMIC ACTIVITY: THE ADVANTAGE OF THE METHOD OF CHEMICAL DYNAMICS B. Zilbergleyt Bank One, IT Department, Chicago E-mail: [email protected] ABSTRACT. The article compares traditional coefficients of thermodynamic activity as a parameter related to individual chemical species to newly introduced reduced chaotic temperatures as system characteristics, both regarding their usage in thermodynamic simulation of open chemical systems. Logical and mathematical backgrounds of both approaches are discussed. It is shown that usage of reduced chaotic temperatures and the Method of Chemical Dynamics to calculate chemical and phase composition in open chemical systems is much less costly, easier to perform and potentially leads to better precision. PROBABILISTIC MODEL OF COMPLEX CHEMICAL EQUILIBRIUM. It is well known how easily the Guldberg-Waage’s equation can be derived from the probabilistic considerations. Being based on the particle collisions, typical for the reactions in gases, it states that chance of the reaction to happen is proportional to joint probability P(A) of reactant particles to occur simultaneously at the same point of the reaction space. This probability merely equals to product of concentrations of the colliding particles. If multiplied by the rate constant it defines the reaction rate. When the rates of the forward and the reverse reactions are equal then the state of equilibrium exists. Less known is the fact that the above derivation is valid only in the case when no one of reactants can be consumed in any other collision with different outcome than A. Chemical system with only one type of collision represents isolated by the reactants (more traditionally referred to as closed) is a simple chemical system: one type of collision – one outcome.