Discovery in Space of Ethanolamine, the Simplest Phospholipid Head Group
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United States Patent ‘ Patented Mar
r 2,786,869 United States Patent ‘ Patented Mar. 26, 1957 l 2 tically, mixtures of tert-alkylamine such as are available on the market. Typical mixtures are those containing ‘ 2,786,869 C12H25NH2 to C15H31NH2 or C18H3'INH2 to C24H49NH2 N-TRIALKYLCARBINYL-N-(HYDROXYETHYL or C15H31- to C24H49NH2. These may be represented by POLYOXYETHYL) GLYCINES the formula Peter L. de Benneville and Homer J. Sims, Philadelphia, 31 Pa., assignors to Rohrn & Haas Company, Philadelphia, R’-—-C—NH2 Pa., a corporation of Delaware Rs No Drawing. Application June 16, 1954, 10 As catalysts in the ?rst step of the process of this Serial No. 437,273 invention, wherein the hydroxyethyl group is introduced, 9 Claims.‘ (or. 260-534) there may be used any of the strong acids, such as hy drochloric, hydrobromic, sulfuric, arylsulfonic, alkanesul fonic, or phosphoric. The preferred amount of this cat This invention relatesto-compounds of the structure 15 alyst is 10 to 30 mole percent of the amine. With R1 '(CH2CH2O),.H ‘ , amines from 12 carbon atoms upward it is exceedingly di?icult to introduce more than one hydroxyethyl group in a tert-alkylamine molecule. Such amines‘yicld ?nal 3 \CHrCOOH products which have the desired balance of properties. ' wherein R1, R2, and R3 are alkyl groups containing a 20 The ?rst reaction with ethylene oxide is effected by total of 11 to 23 carbon atoms and n is an integer having bringing together ethylene oxide and tert-alkylamine, a value from 5 to about 50 or more, preferably 5 to 25. usually by passing ethylene oxide into amine and catalyst, These compounds may be called N-(trialkylcarbinyl)-N at temperatures from 0° to 180° C. -
Laboratory Studies for Planetary Sciences
Laboratory Studies for Planetary Sciences A Planetary Decadal Survey White Paper Prepared by the American Astronomical Society (AAS) Working Group on Laboratory Astrophysics (WGLA) http://www.aas.org/labastro Targeted Panels: Terrestrial Planets; Outer Solar System Satellites; Small Bodies Lead Author: Murthy S. Gudipati Ice Spectroscopy Lab, Science Division, Mail Stop 183-301, Jet Propulsion Laboratory, California Institute of Technology, 4800 Oak Grove Drive, Pasadena, CA 91109. [email protected], 818-354-2637 Co-Authors: Michael A'Hearn - University of Maryland [email protected], 301-405-6076 Nancy Brickhouse - Harvard-Smithsonian Center for Astrophysics [email protected], 617-495-7438 John Cowan - University of Oklahoma [email protected], 405-325-3961 Paul Drake - University of Michigan [email protected], 734-763-4072 Steven Federman - University of Toledo [email protected], 419-530-2652 Gary Ferland - University of Kentucky [email protected], 859-257-879 Adam Frank - University of Rochester [email protected], 585-275-1717 Wick Haxton - University of Washington [email protected], 206-685-2397 Eric Herbst - Ohio State University [email protected], 614-292-6951 Michael Mumma - NASA/GSFC [email protected], 301-286-6994 Farid Salama - NASA/Ames Research Center [email protected], 650-604-3384 Daniel Wolf Savin - Columbia University [email protected], 212-854-4124, Lucy Ziurys – University of Arizona [email protected], 520-621-6525 1 Brief Description: The WGLA of the AAS promotes collaboration and exchange of knowledge between astronomy and planetary sciences and the laboratory sciences (physics, chemistry, and biology). -
Monoethanolamine Diethanolamine Triethanolamine DSA9781.Qxd 1/31/03 10:21 AM Page 2
DSA9781.qxd 1/31/03 10:21 AM Page 1 ETHANOLAMINES Monoethanolamine Diethanolamine Triethanolamine DSA9781.qxd 1/31/03 10:21 AM Page 2 CONTENTS Introduction ...............................................................................................................................2 Ethanolamine Applications.........................................................................................................3 Gas Sweetening ..................................................................................................................3 Detergents, Specialty Cleaners, Personal Care Products.......................................................4 Textiles.................................................................................................................................4 Metalworking ......................................................................................................................5 Other Applications...............................................................................................................5 Ethanolamine Physical Properties ...............................................................................................6 Typical Physical Properties ....................................................................................................6 Vapor Pressure of Ethanolamines (Figure 1).........................................................................7 Heat of Vaporization of Ethanolamines (Figure 2)................................................................7 Specific -
Hydroxyacetonitrile (HOCH2CN) As a Precursor for Formylcyanide (CHOCN), Ketenimine (CH2CNH), and Cyanogen (NCCN) in Astrophysical Conditions
A&A 549, A93 (2013) Astronomy DOI: 10.1051/0004-6361/201219779 & c ESO 2013 Astrophysics Hydroxyacetonitrile (HOCH2CN) as a precursor for formylcyanide (CHOCN), ketenimine (CH2CNH), and cyanogen (NCCN) in astrophysical conditions G. Danger1, F. Duvernay1, P. Theulé1, F. Borget1, J.-C. Guillemin2, and T. Chiavassa1 1 Aix-Marseille Univ, CNRS, PIIM UMR 7345, 13397 Marseille, France e-mail: [email protected] 2 Institut des Sciences Chimiques de Rennes, École Nationale Supérieure de Chimie de Rennes, CNRS, UMR 6226, Avenue du Général Leclerc, CS 50837, 35708 Rennes Cedex 7, France Received 8 June 2012 / Accepted 19 November 2012 ABSTRACT Context. The reactivity in astrophysical environments can be investigated in the laboratory through experimental simulations, which provide understanding of the formation of specific molecules detected in the solid phase or in the gas phase of these environments. In this context, the most complex molecules are generally suggested to form at the surface of interstellar grains and to be released into the gas phase through thermal or non-thermal desorption, where they can be detected through rotational spectroscopy. Here, we focus our experiments on the photochemistry of hydroxyacetonitrile (HOCH2CN), whose formation has been shown to compete with aminomethanol (NH2CH2OH), a glycine precursor, through the Strecker synthesis. Aims. We present the first experimental investigation of the ultraviolet (UV) photochemistry of hydroxyacetonitrile (HOCH2CN) as a pure solid or diluted in water ice. Methods. We used Fourier transform infrared (FT-IR) spectroscopy to characterize photoproducts of hydroxyacetonitrile (HOCH2CN) and to determine the different photodegradation pathways of this compound. To improve the photoproduct identifications, irradiations of hydroxyacetonitrile 14N and 15N isotopologues were performed, coupled with theoretical calculations. -
Computational Surface Modelling of Ices and Minerals of Interstellar Interest—Insights and Perspectives
minerals Review Computational Surface Modelling of Ices and Minerals of Interstellar Interest—Insights and Perspectives Albert Rimola 1,* , Stefano Ferrero 1, Aurèle Germain 2 , Marta Corno 2 and Piero Ugliengo 2,3 1 Departament de Química, Universitat Autònoma de Barcelona, 08193 Bellaterra, Catalonia, Spain; [email protected] 2 Dipartimento di Chimica, Università degli Studi di Torino, 10125 Torino, Italy; [email protected] (A.G.); [email protected] (M.C.); [email protected] (P.U.) 3 Nanostructured Interfaces and Surfaces (NIS) Centre, Università degli Studi di Torino, 10125 Torino, Italy * Correspondence: [email protected]; Tel.: +34-93-581-3723 Abstract: The universe is molecularly rich, comprising from the simplest molecule (H2) to complex organic molecules (e.g., CH3CHO and NH2CHO), some of which of biological relevance (e.g., amino acids). This chemical richness is intimately linked to the different physical phases forming Solar-like planetary systems, in which at each phase, molecules of increasing complexity form. Interestingly, synthesis of some of these compounds only takes place in the presence of interstellar (IS) grains, i.e., solid-state sub-micron sized particles consisting of naked dust of silicates or carbonaceous materials that can be covered by water-dominated ice mantles. Surfaces of IS grains exhibit particular characteristics that allow the occurrence of pivotal chemical reactions, such as the presence of binding/catalytic sites and the capability to dissipate energy excesses through the grain phonons. The present know-how on the physicochemical features of IS grains has been obtained by the fruitful synergy of astronomical observational with astrochemical modelling and laboratory experiments. -
Interstellar Dust Within the Life Cycle of the Interstellar Medium K
EPJ Web of Conferences 18, 03001 (2011) DOI: 10.1051/epjconf/20111803001 C Owned by the authors, published by EDP Sciences, 2011 Interstellar dust within the life cycle of the interstellar medium K. Demyk1,2,a 1Université de Toulouse, UPS-OMP, IRAP, Toulouse, France 2CNRS, IRAP, 9 Av. colonel Roche, BP. 44346, 31028 Toulouse Cedex 4, France Abstract. Cosmic dust is omnipresent in the Universe. Its presence influences the evolution of the astronomical objects which in turn modify its physical and chemical properties. The nature of cosmic dust, its intimate coupling with its environment, constitute a rich field of research based on observations, modelling and experimental work. This review presents the observations of the different components of interstellar dust and discusses their evolution during the life cycle of the interstellar medium. 1. INTRODUCTION Interstellar dust grains are found everywhere in the Universe: in the Solar System, around stars at all evolutionary stages, in interstellar clouds of all kind, in galaxies and in the intergalactic medium. Cosmic dust is intimately mixed with the gas-phase and represents about 1% of the gas (in mass) in our Galaxy. The interstellar extinction and the emission of diffuse interstellar clouds is reproduced by three dust components: a population of large grains, the BGs (Big Grains, ∼10–500 nm) made of silicate and a refractory mantle, a population of carbonaceous nanograins, the VSGs (Very Small Grains, 1–10 nm) and a population of macro-molecules the PAHs (Polycyclic Aromatic Hydrocarbons) [1]. These three components are more or less abundant in the diverse astrophysical environments reflecting the coupling of dust with the environment and its evolution according to the physical and dynamical conditions. -
Study of Various Aqueous and Non-Aqueous Amine Blends for Hydrogen Sulfide Removal from Natural Gas
processes Article Study of Various Aqueous and Non-Aqueous Amine Blends for Hydrogen Sulfide Removal from Natural Gas Usman Shoukat , Diego D. D. Pinto and Hanna K. Knuutila * Department of Chemical Engineering, Norwegian University of Science and Technology (NTNU), 7491 Trondheim, Norway; [email protected] (U.S.); [email protected] (D.D.D.P.) * Correspondence: [email protected] Received: 8 February 2019; Accepted: 8 March 2019; Published: 15 March 2019 Abstract: Various novel amine solutions both in aqueous and non-aqueous [monoethylene glycol (MEG)/triethylene glycol(TEG)] forms have been studied for hydrogen sulfide (H2S) absorption. The study was conducted in a custom build experimental setup at temperatures relevant to subsea operation conditions and atmospheric pressure. Liquid phase absorbed H2S, and amine concentrations were measured analytically to calculate H2S loading (mole of H2S/mole of amine). Maximum achieved H2S loadings as the function of pKa, gas partial pressure, temperature and amine concentration are presented. Effects of solvent type on absorbed H2S have also been discussed. Several new solvents showed higher H2S loading as compared to aqueous N-Methyldiethanolamine (MDEA) solution which is the current industrial benchmark compound for selective H2S removal in natural gas sweetening process. Keywords: H2S absorption; amine solutions; glycols; desulfurization; aqueous and non-aqueous solutions 1. Introduction Natural gas is considered one of the cleanest forms of fossil fuel. Its usage in industrial processes and human activities is increasing worldwide, providing 23.4% of total world energy requirement in 2017 [1]. Natural gas is half of the price of crude oil and produces 29% less carbon dioxide than oil per unit of energy output [2]. -
APPENDIX G Acid Dissociation Constants
harxxxxx_App-G.qxd 3/8/10 1:34 PM Page AP11 APPENDIX G Acid Dissociation Constants § ϭ 0.1 M 0 ؍ (Ionic strength ( † ‡ † Name Structure* pKa Ka pKa ϫ Ϫ5 Acetic acid CH3CO2H 4.756 1.75 10 4.56 (ethanoic acid) N ϩ H3 ϫ Ϫ3 Alanine CHCH3 2.344 (CO2H) 4.53 10 2.33 ϫ Ϫ10 9.868 (NH3) 1.36 10 9.71 CO2H ϩ Ϫ5 Aminobenzene NH3 4.601 2.51 ϫ 10 4.64 (aniline) ϪO SNϩ Ϫ4 4-Aminobenzenesulfonic acid 3 H3 3.232 5.86 ϫ 10 3.01 (sulfanilic acid) ϩ NH3 ϫ Ϫ3 2-Aminobenzoic acid 2.08 (CO2H) 8.3 10 2.01 ϫ Ϫ5 (anthranilic acid) 4.96 (NH3) 1.10 10 4.78 CO2H ϩ 2-Aminoethanethiol HSCH2CH2NH3 —— 8.21 (SH) (2-mercaptoethylamine) —— 10.73 (NH3) ϩ ϫ Ϫ10 2-Aminoethanol HOCH2CH2NH3 9.498 3.18 10 9.52 (ethanolamine) O H ϫ Ϫ5 4.70 (NH3) (20°) 2.0 10 4.74 2-Aminophenol Ϫ 9.97 (OH) (20°) 1.05 ϫ 10 10 9.87 ϩ NH3 ϩ ϫ Ϫ10 Ammonia NH4 9.245 5.69 10 9.26 N ϩ H3 N ϩ H2 ϫ Ϫ2 1.823 (CO2H) 1.50 10 2.03 CHCH CH CH NHC ϫ Ϫ9 Arginine 2 2 2 8.991 (NH3) 1.02 10 9.00 NH —— (NH2) —— (12.1) CO2H 2 O Ϫ 2.24 5.8 ϫ 10 3 2.15 Ϫ Arsenic acid HO As OH 6.96 1.10 ϫ 10 7 6.65 Ϫ (hydrogen arsenate) (11.50) 3.2 ϫ 10 12 (11.18) OH ϫ Ϫ10 Arsenious acid As(OH)3 9.29 5.1 10 9.14 (hydrogen arsenite) N ϩ O H3 Asparagine CHCH2CNH2 —— —— 2.16 (CO2H) —— —— 8.73 (NH3) CO2H *Each acid is written in its protonated form. -
Experimental Study Into Carbon Dioxide Solubility and Species Distribution in Aqueous Alkanolamine Solutions
Air Pollution XX 515 Experimental study into carbon dioxide solubility and species distribution in aqueous alkanolamine solutions H. Yamada, T. Higashii, F. A. Chowdhury, K. Goto S. Kazama Research Institute of Innovative Technology for the Earth, Japan Abstract We investigated the solubility of CO2 in aqueous solutions of alkanolamines at 40C and 120C over CO2 partial pressures ranging from a few kPa to 100 kPa to evaluate the potential for CO2 capture from flue gas. CO2 capacities were compared between monoethanolamine, N-ethyl ethanolamine and N-isopropyl ethanolamine. Speciation analyses were conducted in the alkanolamine solutions 13 at different CO2 loadings by accurate quantitative C nuclear magnetic resonance spectroscopy. N-isopropyl ethanolamine showed a large capacity for CO2 because of the formation of bicarbonate. However, we also found that at a lower CO2 loading a significant amount of carbamate was present in the aqueous N-isopropyl ethanolamine solutions. Keywords: carbon capture, amine absorbent, CO2 solubility, vapour-liquid equilibrium, nuclear magnetic resonance. 1 Introduction Carbon capture and storage is of central importance for the reduction of anthropogenic CO2 emissions in the atmosphere. Amine scrubbing is the most promising and currently applicable technology used in an industrial scale for the capture of CO2 from a gas stream [1]. To maximise the capture efficiency and to reduce energy costs we previously developed CO2 capture systems and high performance CO2 absorbents [2–5]. Recently, we demonstrated that hindered amino alcohols for the promotion of CO2 capture can be developed by rational molecular design and by the placement of functional groups [4, 5]. For aqueous solutions of primary and secondary amines the CO2 absorption proceeds by the formation of a carbamate anion or a bicarbonate anion. -
United States Patent Office Patented Jan
2,700,668 United States Patent Office Patented Jan. 25, 1955 1. 2 Glycolonitrile, as is known, is readily prepared by re acting formaldehyde and hydrogen cyanide. Cf. Prepa 2,700,668 ration of Formaldehyde Cyanohydrin, p. 168 in "Prepara PREPARATION OF KETOPPERAZINES tion of Organic Intermediates' by Shirley, John Wiley & 5 Sons, New York, 1951. See also, p. 176 of "Chemistry James S. Strong and W. E. Craig, Philadelphia, and Vin of Organic Cyanogen Compounds,” Migridichian, 1947 cent T. Elkind, Roslyn, Pa., assignors to Rohm & Haas ed. Glycolonitrile may also be prepared in the reaction Company, Philadelphia, Pa., a corporation of Delaware mixture as described in the next example wherein form No Drawing. Application February 8, 1952, aldehyde and hydrogen cyanide are reacted in the pres Serial No. 270,761 O ence of an amine catalyst. 7 Claims. (C. 260-268) Example 2 To 83 parts of a 36.3% aqueous formaldehyde solution there were added a trace of piperidine to serve as catalyst This invention concerns a method for preparing keto 5 and 27 parts of hydrogen cyanide. During addition of piperazines having the formula the hydrogen cyanide the temperature was kept between N. R. 27 and 30° C. by cooling. After the cyanide had been added, the temperature of the mixture was allowed to, cá, Yo4R, rise to 50° C. The mixture was allowed to stand for bH, d-o 20 3.5 hours. This solution was then slowly added to 78 N parts of 76.7% ethylenediamine in water, which was stirred and held at 100° C. -
Ethanolamines Storage Guide Dow Manufactures Ethanolamines for A
DSA9782.qxd 1/29/03 2:34 PM Page 1 DSA9782.qxd 1/29/03 2:34 PM Page 2 DSA9782.qxd 1/29/03 2:34 PM Page 3 Contents PAGE Introduction 2 Product Characteristics 3 Occupational Health 3 Reactivity 3 Oxidation 4 Liquid Thermal Stability 4 Materials of Construction 5 Pure Ethanolamines 5 Aqueous Ethanolamines 6 Gaskets and Elastomers 7 Transfer Hose 8 Preparation for Service 9 Thermal Insulation Materials 10 Typical Storage System 11 Tank and Line Heating 11 Drum Thawing 11 Special Considerations 14 Vent Freezing 14 Color Buildup in Traced Pipelines 14 Thermal Relief for Traced Lines 14 Product Unloading 15 Unloading System 15 Shipping Vessel Descriptions 16 General Unloading Procedure 17 Product Handling 18 Personal Protective Equipment 18 Firefighting 18 Equipment Cleanup 18 Product Shipment 19 Environmental Considerations 19 Product Safety 20 1 DSA9782.qxd 1/29/03 2:34 PM Page 4 Ethanolamines Storage and Handling The Dow Chemical Company manufactures high-quality ethanolamines for a wide variety of end uses. Proper storage and handling will help maintain the high quality of these products as they are delivered to you. This will enhance your ability to use these products safely in your processes and maximize performance in your finished products. Ethanolamines have unique reactivity and solvent properties which make them useful as intermediates for a wide variety of applications. As a group, they are viscous, water-soluble liquids. In their pure, as-delivered state, these materials are chemically stable and are not corrosive to the proper containers. Ethanolamines can freeze at ambient temperatures. -
Interstellar Ice Photochemistry and the Deuterium Enrichment and Chemical Properties of Meteoritic Polycyclic Aromatic Hydrocarbons S
63rd Annual Meteoritical Society Meeting 5003.pdf INTERSTELLAR ICE PHOTOCHEMISTRY AND THE DEUTERIUM ENRICHMENT AND CHEMICAL PROPERTIES OF METEORITIC POLYCYCLIC AROMATIC HYDROCARBONS S. A. Sandford1, M. P. Bernstein1,2, L. J. Allamandola1, J. S. Gillette3, and R. N. Zare3, 1NASA-Ames Research Center, MS 245-6, Moffett Field CA 94035 ([email protected]), 2SETI Institute, 2035 Landings Drive, Mountain View CA 94043, USA, 3Department of Chemistry, Stanford University, Stanford CA 94305, USA. Introduction: Polycyclic aromatic hydrocarbons surroundings over time. However, exchanged D atoms (PAHs) are known to be abundant and ubiquitous in at the other sites are labile only under UV irradiation; the interstellar medium (ISM) [1]. At the temperatures once irradiation ceases these atoms will not exchange typical of dense interstellar molecular clouds (T = 10–- with the environment. 50 K), the birth sites of stars and planetary systems, Because the aromatic fractions of meteoritic PAHs will be frozen out of the gas phase into icy grain organics are known to be enriched in deuterium [6], mantles. These mantles contain a number of molecular this raises the possibility that interstellar species, the most abundant being H2O, CH3OH, CO, photoprocessing of PAHs in D-enriched interstellar CO2, NH3, CH 4, and possibly N2 and O2 [2]. Many of ices has occurred [7]. The measured D/H ratios of these molecules are expected to be enriched in interstellar ices [8] and the observed exchange rates for deuterium via a number of interstellar chemical coronene (C 24H12)-D2O and d12-coronene (C24D12)-H2O processes [2]. While frozen in these D-enriched ices, isotopic substitution experiments show that PAHs in the PAHs will be exposed to ultraviolet photons from interstellar ices could easily attain the D/H levels nearby stars, the attenuated diffuse ISM radiation field, observed in meteorites [7].