DOCSLIB.ORG

25WORDS ETHYLENE Ethylene, C2H4 ,Is an Unsaturated

Total Page：16

File Type：pdf, Size：1020Kb

Download full-text PDF Read full-text

Load more

25WORDS ETHYLENE Ethylene, C2H4 ,is an unsaturated hydrocarbon that is used in industrial plants and sometimes as a hormone in an average medicine cabinet. It also is the most globally produced organic compound in the world. Ethylene, C2H4, is a hydrocarbon gas that is widely used in the world's industry for purposes like ripening fruit, making detergents, and for making soda. It is also highly flammable and colorless. Ethylene is an unsaturated hydrocarbon, composed of four hydrogen atoms bound to a pair of carbon atoms by means of a double bond. Ethylene has a molar mass of 28.05 g/mol Ethylene is the simplest member of the class called alkenes. It is a colorless, quite sweet- smelling gas. This gas is very reactive and burns with a very bright flame. ethylene (C2H4); Ethylene is known as the simplest alkene and an important hormone in organic chemistry. Over 80% of ethylene is used as a main component of polyethylene and to ripen fruit faster. Ethylene, C2H4, is a colorless gas that can be used as an inhalation anesthetic. This gas is also commonly used to keep fruit ripe as well as to cut and wield metals. Ethylene, C2H4, is an unsaturated hydrocarbon. It is used in anesthetic agents and in detergents. It is the most widely produced organic compound in the world. Ethylene (C2H4): Ethylene is an unsaturated hydrocarbon that is used in the production of polyethylene, a widely used plastic. It can be modified to become ethylene glycol (an antifreeze) and ethylene dichloride (used in creating polyvinyl chloride Ethlyene; Ethylene, C2H4, is a colorless, odorless gas that can be produced in nature as well as man-made processes. Ethylene affects the growth, development, ripening and aging of all plants. Ethylene is an unsaturated hydrocarbon with the chemical formula C2H4. It is used to make polyethylene, a packaging material used so widely that there is more demand for ethylene than any other organic compound. Ethylene is a chemical compound and is the simplest alkene. It contains a double bond making it a unsaturated hydrocarbon. It is the most produced organic compound in the world. Ethylene; is a chemical compound with the formula C2H4. Ethylene is the most produced organic compound in the world due to it's important uses in industry and biology. Ethylene is a hydrocarbon and colorless gas. Molar mass is 28.05g/mol and ethylene also is associated with the hormone that ripens fruit. It is a flammable gas that is made in nature and also by man. Ethylene, C2H4, is a colorless, odorless gas emitted by all plants and fruit. This unsaturated hydrocarbon, also known as olefin, is used to regulate their ripening process. Ethylene is an unsaturated hydrocarbon, composed of four hydrogen atoms bound to a pair of carbon atoms by means of a double bond. Ethylene has a molar mass of 28.05 g/mol Ethylene; Ethylene, C2H4. Ethylene is a chemical compound. It is called an unsaturated hydrocarbon and it is extremely important in industry and even has a role in biology as a hormone. Ethylene;C2H4; Ethylene is the world's biggest organic chemical seller. It is mainly used on plants as a hormone. Polyethylenes are used for packaging and wiring insulation. Ethylene, C2H4, is a chemical compound. This is a hydrocarbon with four hydrogen atoms bound to two carbon atoms connected with a double bond. Ethylene is extremely flammable. Ethylene is the most produced organic compound in the world and to meet the never ending demand for ethylene, increases in production facilities have been added globally. Ethylene, C2H2, is the simplest alkene. It is composed of a double bond between two carbon atoms and two hydrogen atoms. Ethylene is a gas and it is used in many compounds. Ethylene (C2H4) is a colorless gas with a slightly sweet odor and taste. Ethylene affects the growth, development, ripening, and senescence of all plants. It is the simplest alkene. Ethylene is a flammable colorless gas. It is the most produced organic compound in the world. In small quantities, ethylene is used as an anesthetic agent which is used to hasten the ripping of fruit. Ethylene has a double bond between the carbons so it is classified as unsaturated hydrocarbon. It's the simplest alkene with the IUPAC name ethene. It is the most produced in the world. Ethylene: A colorless flammable gas resulting from natural gas and oil and used as a source of many organic compounds, to color citrus fruits and as an anesthetic. Ethylene (or ethene), C2H4, is a simple hydrocarbon. It can be used to create polyethylene. (which is used to make plastic shopping bags Ethylene is the simplest alkene. Also ethylene has a double bond so it is an unaturated hydrocarbon. Ethylene is the most produce compound in organic chemistry. Ethylene (also called Ethene; C2H4), the simplest Alkene, is an organic compound containing a C=C double bond. Ethylene is a coplanary unsaturated hydrocarbon (also called olefin) which is the most produced for industrial use. Ethylene, C2H4, is an odorless, colorless gas that exists in nature and is produced from methionine. It stimulates fruit ripening, flower opening, leaf and fruit abscission, and shoot and root growth. Ethylene is the simplest alkene and the most produced organic compound in the world. It contains four hydrogen atoms and two carbon atoms that are connected by a double bond. Ethylene is a chemical compound, the formula is C2H4. It contains a double bond, it called an unsaturated hydrocarbon. it is extremely important in industry and even has a role in biology as a hormone. ethylene; Since 1795, ethylene has been referred to as the olefiant gas due to it's combination with chlorine, thus producing the "oil of the Dutch". This came due to a group of four Dutch chemists. Ethylene, an unsaturated hydrocarbon, is extremely important in industry and biology for the reason that it can undergo many types of reaction, such as oxidation, polymerization, hydration, and many more. Ethylene gas (C2H4) is the most common gas which found in plant tissues. It also can be man make by combustion. It’s a colorless compound which pound in double bond. Ethylene, also named ethene, is a chemical with the formula C2H4. It is the simplest alkene and also one of the most produced organic compounds in the world. Ethylene, C2H4 ,is an unsaturated hydrocarbon that is used in industrial plants and sometimes as a hormone in an average medicine cabinet. It also is the most globally produced organic compound in the world. Ethylene is a gaseous unsaturated hydrocarbon. Ethylene is colorless, has a slightly sweet taste, and has a faint odor. Since there is a double bond in its molecule, ethylene is very reactive. Ethylene, C2H4, is a colorless gas. It is the simplest alkene. Because it contains a double bond, it it called an unsaturated hydrocarbon or an olefin. Ethylene is an odorless and colorless gas that is created by man-made sources. A person can find this in plants and plant products. Ethylene, also known as “ripening hormone” plays a part of plant growth Ethylene is the chemical compound with the formula C2H4. Ethylene is called an unsaturated hydrocarbon or an olefin. It is extremely important in industry and even has a role in biology as a hormone. Ethylene, C2H4, is an unsaturated hydrocarbon, which is produced in the petrochemical industry. It is used to create other organic compounds, and is also used as an anesthetic agent and as welding gas. Ethylene is the chemical compound with formula C2H4. Ethylene is the most produced organic compound in the world. All six atoms in ethylene are coplanar. .
Recommended publications
  • United States Patent C Patented Aug

    United States Patent C Patented Aug

    3,336,412 United States Patent C Patented Aug. 15, 1967 1 2 3,336,412 tion reaction can be eliminated by the addition of a halogen PRODUCTION OF UNSATURATED HYDROCAR gas to the reaction mixture. In one preferred embodiment BGNS BY PYROLYSIS 0F SATURATED HY it has now been discovered that the addition of chlorine DROCARBONS to a mixture of methane and oxygen increases the yield of Richard Kenneth Lyon, Elizabeth, and William Bartok, acetylene and eliminates the need for preheating‘ the West?eld, N.J., assignors to Esso Research and Engi neering Company, a corporation of Delaware methane and oxygen reactants. While not wishing to be No Drawing. Filed June 29, 1964, Ser. No. 379,031 bound by any particular theory, it is believed that the ad_ 8 Claims. (Cl. 260-679) dition of chlorine promotes the formation of acetylene in the reaction 3H2+C2<:>2CH4 by formation of HCl This invention relates ‘to an improved process for the 10 thereby driving the reaction in accordance with familiar pyrolysis of certain saturated hydrocarbons to obtain un principles of equilibrium reaction. Furthermore, the re saturated hydrocarbons. More particularly, this invention action H2+Cl2—>2HCl is exothermic and therefore adds relates to the production of unsaturated hydrocarbons additional heat to the reaction. The utilization of chlorine by partial combustion of saturated hydrocarbons. In a pre gas with the unsaturated hydrocarbon-oxygen mixture ferred embodiment, this invention relates to the produc 15 possesses a further advantage in that the halogen gas will tion of acetylene by partial combustion of hydrocarbons not react with the unsaturated hydrocarbon as will water, such as methane.
  • Studies of the Temporary Anion States of Unsaturated Hydrocarbons by Electron Transmission Spectroscopy

    Studies of the Temporary Anion States of Unsaturated Hydrocarbons by Electron Transmission Spectroscopy

    University of Nebraska - Lincoln DigitalCommons@University of Nebraska - Lincoln Paul Burrow Publications Research Papers in Physics and Astronomy 1978 Studies of the Temporary Anion States of Unsaturated Hydrocarbons by Electron Transmission Spectroscopy Kenneth D. Jordan Paul Burrow Follow this and additional works at: https://digitalcommons.unl.edu/physicsburrow Part of the Atomic, Molecular and Optical Physics Commons This Article is brought to you for free and open access by the Research Papers in Physics and Astronomy at DigitalCommons@University of Nebraska - Lincoln. It has been accepted for inclusion in Paul Burrow Publications by an authorized administrator of DigitalCommons@University of Nebraska - Lincoln. digitalcommons.unl.edu Studies of the Temporary Anion States of Unsaturated Hydrocarbons by Electron Transmission Spectroscopy Kenneth D. Jordan Mason Laboratory, Department of Engineering and Applied Science, Yale University, New Haven, Connecticut 06520 Paul D. Burrow Behlen Laboratory of Physics, University of Nebraska, Lincoln, Nebraska 68588 The concept of occupied and unoccupied orbitals has provided a useful means for visualizing many of the most important properties of mo- lecular systems. Yet, there is a curious imbalance in our experimen- tal knowledge of the energies of occupied and unoccupied orbitals. Whereas photoelectron spectroscopy has provided a wealth of data on positive ion states and has established that they can be associated, within the context of Koopmans’ theorem, with the occupied orbitals of the neutral molecule, the corresponding information for the neg- ative ion states, associated with the normally unoccupied orbitals, is sparse. In part this reflects the experimental difficulties connected with measuring the electron affinities of molecules which possess sta- ble anions.
  • The Arene–Alkene Photocycloaddition

    The Arene–Alkene Photocycloaddition

    The arene–alkene photocycloaddition Ursula Streit and Christian G. Bochet* Review Open Access Address: Beilstein J. Org. Chem. 2011, 7, 525–542. Department of Chemistry, University of Fribourg, Chemin du Musée 9, doi:10.3762/bjoc.7.61 CH-1700 Fribourg, Switzerland Received: 07 January 2011 Email: Accepted: 23 March 2011 Ursula Streit - [email protected]; Christian G. Bochet* - Published: 28 April 2011 [email protected] This article is part of the Thematic Series "Photocycloadditions and * Corresponding author photorearrangements". Keywords: Guest Editor: A. G. Griesbeck benzene derivatives; cycloadditions; Diels–Alder; photochemistry © 2011 Streit and Bochet; licensee Beilstein-Institut. License and terms: see end of document. Abstract In the presence of an alkene, three different modes of photocycloaddition with benzene derivatives can occur; the [2 + 2] or ortho, the [3 + 2] or meta, and the [4 + 2] or para photocycloaddition. This short review aims to demonstrate the synthetic power of these photocycloadditions. Introduction Photocycloadditions occur in a variety of modes [1]. The best In the presence of an alkene, three different modes of photo- known representatives are undoubtedly the [2 + 2] photocyclo- cycloaddition with benzene derivatives can occur, viz. the addition, forming either cyclobutanes or four-membered hetero- [2 + 2] or ortho, the [3 + 2] or meta, and the [4 + 2] or para cycles (as in the Paternò–Büchi reaction), whilst excited-state photocycloaddition (Scheme 2). The descriptors ortho, meta [4 + 4] cycloadditions can also occur to afford cyclooctadiene and para only indicate the connectivity to the aromatic ring, and compounds. On the other hand, the well-known thermal [4 + 2] do not have any implication with regard to the reaction mecha- cycloaddition (Diels–Alder reaction) is only very rarely nism.
  • MODULE 11: GLOSSARY and CONVERSIONS Cell Engines

    MODULE 11: GLOSSARY and CONVERSIONS Cell Engines

    Hydrogen Fuel MODULE 11: GLOSSARY AND CONVERSIONS Cell Engines CONTENTS 11.1 GLOSSARY.......................................................................................................... 11-1 11.2 MEASUREMENT SYSTEMS .................................................................................. 11-31 11.3 CONVERSION TABLE .......................................................................................... 11-33 Hydrogen Fuel Cell Engines and Related Technologies: Rev 0, December 2001 Hydrogen Fuel MODULE 11: GLOSSARY AND CONVERSIONS Cell Engines OBJECTIVES This module is for reference only. Hydrogen Fuel Cell Engines and Related Technologies: Rev 0, December 2001 PAGE 11-1 Hydrogen Fuel Cell Engines MODULE 11: GLOSSARY AND CONVERSIONS 11.1 Glossary This glossary covers words, phrases, and acronyms that are used with fuel cell engines and hydrogen fueled vehicles. Some words may have different meanings when used in other contexts. There are variations in the use of periods and capitalization for abbrevia- tions, acronyms and standard measures. The terms in this glossary are pre- sented without periods. ABNORMAL COMBUSTION – Combustion in which knock, pre-ignition, run- on or surface ignition occurs; combustion that does not proceed in the nor- mal way (where the flame front is initiated by the spark and proceeds throughout the combustion chamber smoothly and without detonation). ABSOLUTE PRESSURE – Pressure shown on the pressure gauge plus at- mospheric pressure (psia). At sea level atmospheric pressure is 14.7 psia. Use absolute pressure in compressor calculations and when using the ideal gas law. See also psi and psig. ABSOLUTE TEMPERATURE – Temperature scale with absolute zero as the zero of the scale. In standard, the absolute temperature is the temperature in ºF plus 460, or in metric it is the temperature in ºC plus 273. Absolute zero is referred to as Rankine or r, and in metric as Kelvin or K.
  • Aromatic Compounds

    Aromatic Compounds

    OCR Chemistry A Aromatic Compounds Aromatic Compounds Naming Aromatic compounds contain one or more benzene rings (while aliphatic compounds do not contain benzene rings). Another term for a compound containing a benzene ring is arene. The basic benzene ring, C6H6 is commonly represented as a hexagon with a ring inside. You should be aware that there is a hydrogen at each corner although this is not normally shown. N.B. it is OK to use benzene in this form in structural formulae too! Arenes occur naturally in many substances, and are present in coal and crude oil. Aspirin, for example, is an aromatic compound, an arene: HO O O CH 3 O Naming of substances based on benzene follows familiar rules: CH Br NO 3 2 benzene methylbenzene bromobenzene nitrobenzene Numbers are needed to identify the positions of substituents. The carbons around the ring are numbered from 1-6 consecutively and the name which gives the lowest number(s) is chosen: CH3 CH3 Cl Br Cl Br 2-bromomethylbenzene 4-bromomethylbenzene 1,2-dichlorobenzene Cl Cl Cl 1,3,5-trichlorobenzene Page 1 OCR Chemistry A Aromatic Compounds Determining the structure of benzene (historical) 1825 – substance first isolated by Michael Faraday, who also determined its empirical formula as CH 1834 – RFM of 78 and molecular formula of C6H6 determined H H H C C C Much speculation over the structure. Many suggested structures like: C C C H H H 1865 – Kekulé publishes suggestion of a ring with alternating double and single bonds: H H C H C C displayed C C skeletal H C H H This model persisted until 1922, but not all chemists accepted the structure because it failed to explain the chemical and physical properties of benzene fully: if C=C bonds were present as Kekulé proposed, then benzene would react like alkenes.
  • &EPA Ambient Water Quality Criteria for Toluene

    &EPA Ambient Water Quality Criteria for Toluene

    United States Cffice of Water EPA 440/5-80-075 Environmental Protection Regula.ions and Standards O,:tober 1980 Agency Criteria and Standards Division Washington DC 20480 c.). & EPA Ambient Water Quality Criteria for Toluene tz r AMBIENT WATER QUALITY CRITERIA FOR TOLUENE Prepared By U.S. ENVIRONMENTAL PROTECTION AGENCY Office of Water Regulations and Standards Criteria and Standards Division Washington, D.C. Office of Research and Development Environmental Criteria and Assessment Office Cincinnati, Ohio Carcinogen Assessment Group Washington, D.C. Environmental Research Laboratories Corvalis, Oregon Duluth, Minnesota Gulf Breeze, Florida Narragansett, Rhode Island DISCLAIMER This report has been reviewed by the Environmental Criteria and Assessment Office, U.S. Environmental Protection Agency, and approved for publication. Mention of trade names or commercial products does not constitute endorsement or recommendation for use. AVAILABILITY NOTICE This document is available to the public through the National Technical Information Service, (NTIS), Springfield, Virginia 22161. El~TAL l'R~e1'!tjf A~ ii FOREWORD Section 304 (a)(1) of the Clear Water Act of 1977 (P.L. 95-217), requires the Administrator of the Environmental Protection Agency to publish criteria for water quality accurately reflecting the latest scientific knowledge on the kind and extent of all identifiable effects on health and welfare which may be expected from the presence of pollutants in any body of water, including ground water. Proposed water quality criteria for the 65 toxic pollutants listed under section 307 (a) (1) of the Cl ean Water Act were deve loped and a notice of thei r availability was published for public comment on March 15, 1979 (44 FR 15926), July 25, 1979 (44 FR 43660), and October 1, 1979 (44 FR 56628).
  • Introduction to Alkenes and Alkynes in an Alkane, All Covalent Bonds

    Introduction to Alkenes and Alkynes in an Alkane, All Covalent Bonds

    Introduction to Alkenes and Alkynes In an alkane, all covalent bonds between carbon were σ (σ bonds are defined as bonds where the electron density is symmetric about the internuclear axis) In an alkene, however, only three σ bonds are formed from the alkene carbon -the carbon thus adopts an sp2 hybridization Ethene (common name ethylene) has a molecular formula of CH2CH2 Each carbon is sp2 hybridized with a σ bond to two hydrogens and the other carbon Hybridized orbital allows stronger bonds due to more overlap H H C C H H Structure of Ethylene In addition to the σ framework of ethylene, each carbon has an atomic p orbital not used in hybridization The two p orbitals (each with one electron) overlap to form a π bond (p bonds are not symmetric about the internuclear axis) π bonds are not as strong as σ bonds (in ethylene, the σ bond is ~90 Kcal/mol and the π bond is ~66 Kcal/mol) Thus while σ bonds are stable and very few reactions occur with C-C bonds, π bonds are much more reactive and many reactions occur with C=C π bonds Nomenclature of Alkenes August Wilhelm Hofmann’s attempt for systematic hydrocarbon nomenclature (1866) Attempted to use a systematic name by naming all possible structures with 4 carbons Quartane a alkane C4H10 Quartyl C4H9 Quartene e alkene C4H8 Quartenyl C4H7 Quartine i alkine → alkyne C4H6 Quartinyl C4H5 Quartone o C4H4 Quartonyl C4H3 Quartune u C4H2 Quartunyl C4H1 Wanted to use Quart from the Latin for 4 – this method was not embraced and BUT has remained Used English order of vowels, however, to name the groups
  • Reactions of Aromatic Compounds Just Like an Alkene, Benzene Has Clouds of  Electrons Above and Below Its Sigma Bond Framework

    Reactions of Aromatic Compounds Just Like an Alkene, Benzene Has Clouds of  Electrons Above and Below Its Sigma Bond Framework

    Reactions of Aromatic Compounds Just like an alkene, benzene has clouds of electrons above and below its sigma bond framework. Although the electrons are in a stable aromatic system, they are still available for reaction with strong electrophiles. This generates a carbocation which is resonance stabilized (but not aromatic). This cation is called a sigma complex because the electrophile is joined to the benzene ring through a new sigma bond. The sigma complex (also called an arenium ion) is not aromatic since it contains an sp3 carbon (which disrupts the required loop of p orbitals). Ch17 Reactions of Aromatic Compounds (landscape).docx Page1 The loss of aromaticity required to form the sigma complex explains the highly endothermic nature of the first step. (That is why we require strong electrophiles for reaction). The sigma complex wishes to regain its aromaticity, and it may do so by either a reversal of the first step (i.e. regenerate the starting material) or by loss of the proton on the sp3 carbon (leading to a substitution product). When a reaction proceeds this way, it is electrophilic aromatic substitution. There are a wide variety of electrophiles that can be introduced into a benzene ring in this way, and so electrophilic aromatic substitution is a very important method for the synthesis of substituted aromatic compounds. Ch17 Reactions of Aromatic Compounds (landscape).docx Page2 Bromination of Benzene Bromination follows the same general mechanism for the electrophilic aromatic substitution (EAS). Bromine itself is not electrophilic enough to react with benzene. But the addition of a strong Lewis acid (electron pair acceptor), such as FeBr3, catalyses the reaction, and leads to the substitution product.
  • Chapter 7 - Alkenes and Alkynes I

    Chapter 7 - Alkenes and Alkynes I

    Andrew Rosen Chapter 7 - Alkenes and Alkynes I 7.1 - Introduction - The simplest member of the alkenes has the common name of ethylene while the simplest member of the alkyne family has the common name of acetylene 7.2 - The (E)-(Z) System for Designating Alkene Diastereomers - To determine E or Z, look at the two groups attached to one carbon atom of the double bond and decide which has higher priority. Then, repeat this at the other carbon atom. This system is not used for cycloalkenes - If the two groups of higher priority are on the same side of the double bond, the alkene is designated Z. If the two groups of higher priority are on opposite sides of the double bond, the alkene is designated E - Hydrogenation is a syn/cis addition 7.3 - Relative Stabilities of Alkenes - The trans isomer is generally more stable than the cis isomer due to electron repulsions - The addition of hydrogen to an alkene, hydrogenation, is exothermic (heat of hydrogenation) - The greater number of attached alkyl groups, the greater the stability of an alkene 7.5 - Synthesis of Alkenes via Elimination Reactions, 7.6 - Dehydrohalogenation of Alkyl Halides How to Favor E2: - Reaction conditions that favor elimination by E1 should be avoided due to the highly competitive SN 1 mechanism - To favor E2, a secondary or tertiary alkyl halide should be used - If there is only a possibility for a primary alkyl halide, use a bulky base - Use a higher concentration of a strong and nonpolarizable base, like an alkoxide - EtONa=EtOH favors the more substituted double bond
  • Reactions of Alkenes and Alkynes

    Reactions of Alkenes and Alkynes

    05 Reactions of Alkenes and Alkynes Polyethylene is the most widely used plastic, making up items such as packing foam, plastic bottles, and plastic utensils (top: © Jon Larson/iStockphoto; middle: GNL Media/Digital Vision/Getty Images, Inc.; bottom: © Lakhesis/iStockphoto). Inset: A model of ethylene. KEY QUESTIONS 5.1 What Are the Characteristic Reactions of Alkenes? 5.8 How Can Alkynes Be Reduced to Alkenes and 5.2 What Is a Reaction Mechanism? Alkanes? 5.3 What Are the Mechanisms of Electrophilic Additions HOW TO to Alkenes? 5.1 How to Draw Mechanisms 5.4 What Are Carbocation Rearrangements? 5.5 What Is Hydroboration–Oxidation of an Alkene? CHEMICAL CONNECTIONS 5.6 How Can an Alkene Be Reduced to an Alkane? 5A Catalytic Cracking and the Importance of Alkenes 5.7 How Can an Acetylide Anion Be Used to Create a New Carbon–Carbon Bond? IN THIS CHAPTER, we begin our systematic study of organic reactions and their mecha- nisms. Reaction mechanisms are step-by-step descriptions of how reactions proceed and are one of the most important unifying concepts in organic chemistry. We use the reactions of alkenes as the vehicle to introduce this concept. 129 130 CHAPTER 5 Reactions of Alkenes and Alkynes 5.1 What Are the Characteristic Reactions of Alkenes? The most characteristic reaction of alkenes is addition to the carbon–carbon double bond in such a way that the pi bond is broken and, in its place, sigma bonds are formed to two new atoms or groups of atoms. Several examples of reactions at the carbon–carbon double bond are shown in Table 5.1, along with the descriptive name(s) associated with each.
  • INVESTIGATION of POLYCYCLIC AROMATIC HYDROCARBONS (Pahs) on DRY FLUE GAS DESULFURIZATION (FGD) BY-PRODUCTS

    INVESTIGATION of POLYCYCLIC AROMATIC HYDROCARBONS (Pahs) on DRY FLUE GAS DESULFURIZATION (FGD) BY-PRODUCTS

    INVESTIGATION OF POLYCYCLIC AROMATIC HYDROCARBONS (PAHs) ON DRY FLUE GAS DESULFURIZATION (FGD) BY-PRODUCTS DISSERTATION Presented in Partial Fulfillment of the Requirements for the Degree Doctor of Philosophy in the Graduate School of The Ohio State University By Ping Sun, M.S. ***** The Ohio State University 2004 Dissertation Committee: Approved by Professor Linda Weavers, Adviser Professor Harold Walker Professor Patrick Hatcher Adviser Professor Yu-Ping Chin Civil Engineering Graduate Program ABSTRACT The primary goal of this research was to examine polycyclic aromatic hydrocarbons (PAHs) on dry FGD by-products to determine environmentally safe reuse options of this material. Due to the lack of information on the analytical procedures for measuring PAHs on FGD by-products, our initial work focused on analytical method development. Comparison of the traditional Soxhlet extraction, automatic Soxhlet extraction, and ultrasonic extraction was conducted to optimize the extraction of PAHs from lime spray dryer (LSD) ash (a common dry FGD by-product). Due to the short extraction time, ultrasonic extraction was further optimized by testing different organic solvents. Ultrasonic extraction with toluene as the solvent turned out to be a fast and efficient method to extract PAHs from LSD ash. The possible reactions of PAHs under standard ultrasonic extraction conditions were then studied to address concern over the possible degradation of PAHs by ultrasound. By sonicating model PAHs including naphthalene, phenanthrene and pyrene in organic solutions, extraction parameters including solvent type, solute concentration, and sonication time on reactions of PAHs were examined. A hexane: acetone (1:1 V/V) ii mixture resulted in less PAH degradation than a dichloromethane (DCM): acetone (1:1 V/V) mixture.
  • Managing Exposure to Benzene and Total Petroleum Hydrocarbons at Two Oil Refineries 1977–2014

    Managing Exposure to Benzene and Total Petroleum Hydrocarbons at Two Oil Refineries 1977–2014

    International Journal of Environmental Research and Public Health Article Managing Exposure to Benzene and Total Petroleum Hydrocarbons at Two Oil Refineries 1977–2014 Tapani Tuomi *, Henna Veijalainen and Tiina Santonen Finnish Institute of Occupational Health (FIOH), Topeliuksenkatu 41 B, P.O. Box 40, Työterveyslaitos, FI-00032 Helsinki, Finland; henna.veijalainen@ttl.fi (H.V.); tiina.santonen@ttl.fi (T.S.) * Correspondence: tapani.tuomi@ttl.fi; Tel.: +358-9-4747-2926 Received: 15 December 2017; Accepted: 18 January 2018; Published: 24 January 2018 Abstract: Air concentrations of and inhalation exposure to total petroleum hydrocarbons (TPH) and benzene was monitored separately at two oil refineries from 1977 to 2014. Prevention policies and control measures that may explain changes were surveyed. The aim was to evaluate how the application of of Occupational Health and Safety Assessment Series OHSAS 18001.04 principles as well as Environmental protection Agency EPA and European Oil Company Organisation for Environment, Health and Safety CONCAWE practices have influenced air concentrations. Benzene air concentrations declined in 11 of 17 units, six of which were associated with declining exposures. Benzene air concentrations declined across all units on average by 46%. This amounts to an average yearly decline of 1.7%. TPH air concentrations declined in 10 of 17 units, seven of which were associated with declining exposures. The average decline in TPH air concentrations was 49%, corresponding to 1.3% per year. As a result, average working day exposure in 10 of 17 units have declined significantly and today, benzene and TPH exposure in most units are well below 10% of the current Occupational Exposure Limit (OEL8h:s).