Properties of Sulphuric Acid As a Catalyst
Total Page:16
File Type:pdf, Size:1020Kb
Load more
Recommended publications
-
SULFUR TRIOXIDE -- Chemical Fact Sheet
OLEUM/SULFUR TRIOXIDE -- Chemical Fact Sheet 1 What is it? Oleum is a cloudy, gray, fuming, oily, corrosive liquid with a sharp, penetrating odor. When Oleum comes into contact with air following a spill, it releases Sulfur Trioxide. Sulfur Trioxide is a white gas having the appearance of fog. It also has a sharp, penetrating odor that is detectable at low concentrations. Because of the tendency to liberate Sulfur Trioxide on contact with air, Oleum is also known as “fuming Sulfuric Acid”. Where does it Oleum is made by dissolving Sulfur Trioxide into Sulfuric Acid. Sulfur come from? Trioxide is made from Sulfur Dioxide in the presence of a catalyst. What are the It is used in the oil refining process to make crude oil distillates into higher quality materials. common uses for it? Manufacture of soap Manufacture of high purity Sulfuric Acid for the electronic industry Manufacture of catalyst used in production of Sulfuric Acid. How is it Oleum is shipped by truck and pipeline. transported in CCC? How is it stored Oleum is stored in covered tanks. in CCC? Health Hazards from Exposure Exposure Route Symptoms First Aid Inhalation Irritates nose, throat and Remove to fresh air. Seek (low concentrations) lungs medical attention if Burning Sensation symptoms persist. Sneezing, coughing Inhalation Burning sensation Remove to fresh air, get (high concentrations & prolonged exposure) Coughing, gagging medical attention including Chest tightness and pain, oxygen administration. Fluid in lungs Initiate CPR if breathing has Suffocation, death stopped. Eyes Severely irritates eyes Rinse eyes with water for at Burning/discomfort least 5 minutes. -
Sulfuric Acid from Sulfur Updates on Contact Process PEP Review 2018-12 February 2018
` Sulfuric Acid from Sulfur Updates on Contact Process PEP Review 2018-12 February 2018 Rajiv Narang Director Process Economics Program IHS Markit | PEP Review 2018-12 Sulfuric Acid from Sulfur/Updates on Contact Process PEP Review 2018-12 Sulfuric Acid from Sulfur/Updates on Contact Process Rajiv Narang, Director Abstract Sulfuric acid (H2SO4) is the world’s largest consumed chemical, with consumption of around 260 MMT (million metric tons) on a 100% acid basis and a growth rate of around 2%. Traditionally, consumption of this chemical is considered as a barometer of a nation’s GDP. The majority of sulfuric acid production (59%) is from burning of elemental sulfur, in a contact process. The sulfur is sourced mostly from oil and gas processing facilities, in which the sulfur is removed from various petroleum or natural gas products. IHS Markit’s Process Economics Program (PEP) last addressed this production technology in PEP Report 84A, Sulfuric Acid (June 1985), which covered the manufacture of sulfuric acid from sulfur in new versus old, retrofitted plants, as well as from metallurgical offgases. This review specifically updates the contact process for the production of sulfuric acid by burning of elemental sulfur. The review examines the developments in this production technology, including advances in catalyst, material of construction, and heat recovery. The process is simulated using Aspen Plus™ software. It focuses on technology basis, raw material and utility consumptions, equipment list, capital cost, along with capacity exponents, and production costs for a 2,000 STPD (short ton per day) of (100% basis) sulfuric acid product. This review provides insight into sulfuric acid plant process economics, and can be used as a tool for cost estimation for different plant capacities. -
EPA Method 8: Determination of Sulfuric Acid and Sulfur Dioxide
733 METHOD 8 - DETERMINATION OF SULFURIC ACID AND SULFUR DIOXIDE EMISSIONS FROM STATIONARY SOURCES NOTE: This method does not include all of the specifications (e.g., equipment and supplies) and procedures (e.g., sampling and analytical) essential to its performance. Some material is incorporated by reference from other methods in this part. Therefore, to obtain reliable results, persons using this method should have a thorough knowledge of at least the following additional test methods: Method 1, Method 2, Method 3, Method 5, and Method 6. 1.0 Scope and Application. 1.1 Analytes. Analyte CAS No. Sensitivity Sulfuric acid, including: 0.05 mg/m3 Sulfuric acid 7664-93-9 (0.03 × 10-7 3 (H2SO4) mist 7449-11-9 lb/ft ) Sulfur trioxide (SO3) 3 Sulfur dioxide (SO2) 7449-09-5 1.2 mg/m (3 x 10-9 lb/ft3) 1.2 Applicability. This method is applicable for the determination of H2SO4 (including H2SO4 mist and SO3) and gaseous SO2 emissions from stationary sources. NOTE: Filterable particulate matter may be determined along with H2SO4 and SO2 (subject to the approval of the Administrator) by inserting a heated glass fiber filter 734 between the probe and isopropanol impinger (see Section 6.1.1 of Method 6). If this option is chosen, particulate analysis is gravimetric only; sulfuric acid is not determined separately. 1.3 Data Quality Objectives. Adherence to the requirements of this method will enhance the quality of the data obtained from air pollutant sampling methods. 2.0 Summary of Method. A gas sample is extracted isokinetically from the stack. -
Source Test Method ST-20 SULFUR DIOXIDE, SULFUR TRIOXIDE
Source Test Method ST-20 SULFUR DIOXIDE, SULFUR TRIOXIDE, SULFURIC ACID MIST (Adopted January 20, 1982) REF: Regulations 6-320, 6-330, 9-1-302, 9-1-304 thru 310, 10-1-301, 12-6-301 1. APPLICABILITY 1.1 This method is used to quantify emissions of s ulfur dioxide, sulfur trioxide and sulfuric acid mist. It determines compliance with Regulations 6-320 and 6-330 for SULFUR TRIOXIDE and SULFURIC ACID MIST, and 9-1-302, 9- 1-304 thru 310 and 10-1-301 and 12-6-301 for SULFUR DIOXIDE. 1.2 This method, modified with a glass fiber disc filter as the back-up SO 3 filter, has been given alternate status by the EPA to EPA Method 8. It may be used to determine compliance with oxides of sulfur regulations under Regulation 9. 2. PRINCIPLE 2.1 Sulfuric acid mist, sulfur trioxide and sulfur dioxide are collected in a single extractive sampling train. Acid mist is trapped in a quartz wool plug in the sample probe and is subsequently analyzed with an acid-base titration. Sulfur trioxide is absorbed in an 80% isopropyl alcohol (IPA)/water solution with a quartz wool back-up filter and is analyzed using analytical procedure Lab-12. Sulfur dioxide is absorbed in an aqueous hydrogen peroxide solution and is analyzed using analytical procedure Lab-12. 3. RANGE 3.1 The minimum measurable concentration using this method listed below are: 3 3.1.1 Acid mist - 0.0002 gr/ft as H2SO4 3.1.2 Sulfur trioxide - 7 ppm 3.1.3 Sulfur dioxide - 7 ppm 3.2 The maximum measurable concentrations using this method listed below are: 3.2.1 Acid mist - undetermined 3.2.2 Sulfur trioxide - 350 ppm 3.2.3 Sulfur dioxide - 2.5 % 4. -
Catalyst Precursors for Hydrodesulfurization Synthesized in Supercritical Fluids Manuel Théodet
New generation of ”bulk” catalyst precursors for hydrodesulfurization synthesized in supercritical fluids Manuel Théodet To cite this version: Manuel Théodet. New generation of ”bulk” catalyst precursors for hydrodesulfurization synthesized in supercritical fluids. Material chemistry. Université Sciences et Technologies - Bordeaux I,2010. English. NNT : 2010BOR14092. tel-00559113 HAL Id: tel-00559113 https://tel.archives-ouvertes.fr/tel-00559113 Submitted on 24 Jan 2011 HAL is a multi-disciplinary open access L’archive ouverte pluridisciplinaire HAL, est archive for the deposit and dissemination of sci- destinée au dépôt et à la diffusion de documents entific research documents, whether they are pub- scientifiques de niveau recherche, publiés ou non, lished or not. The documents may come from émanant des établissements d’enseignement et de teaching and research institutions in France or recherche français ou étrangers, des laboratoires abroad, or from public or private research centers. publics ou privés. Distributed under a Creative Commons Attribution - NonCommercial - NoDerivatives| 4.0 International License N° d’ordre : 4092 THÈSE présentée à L’UNIVERSITÉ BORDEAUX I ÉCOLE DOCTORALE DES SCIENCES CHIMIQUES Par Manuel THEODET Ingénieur ENSCPB POUR OBTENIR LE GRADE DE DOCTEUR SPÉCIALITÉ : Physico-Chimie de la Matière Condensée ___________________ NOUVELLE GENERATION DE PRECURSEURS « BULK » DE CATALYSEUR D’HYDRODESULFURATION SYNTHETISES EN MILIEU FLUIDE SUPERCRITIQUE ___________________ NEW GENERATION OF « BULK » CATALYST PRECURSORS FOR HYDRODESULFURIZATION SYNTHESIZED IN SUPERCRITICAL FLUIDS ___________________ Co-superviseurs de recherche : Cristina Martínez & Cyril Aymonier Soutenue le 03 Novembre 2010 Après avis favorable de : M. E. PALOMARES, Professor, UPV, Valencia, Spain Rapporteurs M. M. TÜRK, Professor, KIT, Karlsruhe, Germany Devant la commission d’examen formée de : M. -
PROCESS MODELING and ANALYSIS of CO2 PURIFICATION for OXY-COAL COMBUSTION MASSACHUSETTS INS E by of TECHNOLOGY
PROCESS MODELING AND ANALYSIS OF CO2 PURIFICATION FOR OXY-COAL COMBUSTION MASSACHUSETTS INS E By OF TECHNOLOGY Chukwunwike Ogbonnia Iloeje MAY 18 2011 B.Eng. Mechanical Engineering LIBRRIES University of Nigeria, Nsukka, 2004 SUBMITTED TO THE DEPARTMENT OF MECHANICAL ENGINEERING IN AR(MES PARTIAL FULFILLMENT OF THE REQUIREMENTS FOR THE DEGREE OF MASTER OF SCIENCE IN MECHANICAL ENGINEERING AT THE MASSACHUSETTS INSTITUTE OF TECHNOLOGY JANUARY 2011 0 2011 Massachusetts Institute of Technology. All rights reserved. The author hereby grants to MIT permission to reproduce and to distribute publicly paper and electronic copies of this thesis document in whole or in part in any medium now known or hereafter created. Signature of Author........... ............................... Department of Mechanical Engineering January 14, 2011 Certified by.............. Ahmed F. Ghoniem Ronald C. Crane Professor Thacic Cunanwicnr Accepted by.................................. .... ................. Dave E.Hardt Chairman, Department Committee on Graduate Students *r PROCESS MODELING AND ANALYSIS OF CO2 PURIFICATION FOR OXY-COAL COMBUSTION By Chukwunwike Ogbonnia Iloeje Submitted to the Department of Mechanical Engineering on January 14, 2011 in Partial Fulfillment of the Requirements for the degree of Master of Science in Mechanical Engineering ABSTRACT Oxy-coal combustion technology has great potential as one of the major CO2 capture technologies for power generation from coal. The distinguishing feature of oxy-coal combustion is that the oxygen source is a high concentration oxygen stream and the product flue gas consists primarily of CO2 and H20 with contaminants like NOx, SOx, and non-condensable gases like argon, oxygen and nitrogen. For carbon sequestration and Enhanced Oil Recovery (EOR) applications, pipeline transport standards as well as storage specifications impose concentration limits on these contaminants. -
(VI) and Chromium (V) Oxide Fluorides
Portland State University PDXScholar Dissertations and Theses Dissertations and Theses 1976 The chemistry of chromium (VI) and chromium (V) oxide fluorides Patrick Jay Green Portland State University Follow this and additional works at: https://pdxscholar.library.pdx.edu/open_access_etds Part of the Chemistry Commons Let us know how access to this document benefits ou.y Recommended Citation Green, Patrick Jay, "The chemistry of chromium (VI) and chromium (V) oxide fluorides" (1976). Dissertations and Theses. Paper 4039. https://doi.org/10.15760/etd.5923 This Thesis is brought to you for free and open access. It has been accepted for inclusion in Dissertations and Theses by an authorized administrator of PDXScholar. Please contact us if we can make this document more accessible: [email protected]. All ABSTRACT OF THE TllESIS OF Patrick Jay Green for the Master of Science in Chemistry presented April 16, 1976. Title: Chemistry of Chromium(VI) and Chromium(V) Oxide Fluorides. APPROVEO BY MEMBERS OF THE THESIS CO'"o\l TIEE: y . • Ii . ' I : • • • • • New preparative routes to chromyl fluoride were sought. It was found that chlorine ironofluoride reacts with chromium trioxide and chromyl chlo ride to produce chromyl fluoride. Attempts were ~ade to define a mechan ism for the reaction of ClF and Cr0 in light of by-products observed 3 and previous investigations. Carbonyl fluoride and chromium trioxide react to fom chro·yl fluoride and carbo:i dioxide. A mechanism was also proposed for this react10n. Chromium trioxide 11itl\ l~F6 or WF5 reacts to produce chromyl fluoride and the respective oxide tetrafluoride. 2 Sulfur hexafluoride did not react with Cr03. -
Oxidation of Sulfur Dioxide to Sulfur Trioxide Over Supported Vanadia Catalysts
Applied Catalysis B: Environmental 19 (1998) 103±117 Oxidation of sulfur dioxide to sulfur trioxide over supported vanadia catalysts Joseph P. Dunn, Prashanth R. Koppula, Harvey G. Stenger, Israel E. Wachs* Zettlemoyer Center for Surface Studies, Department of Chemical Engineering, Lehigh University, Bethlehem, PA 18015, USA Accepted 2 June 1998 Abstract The objectives of this research are to establish the fundamental kinetics and mechanism of sulfur dioxide oxidation over supported vanadia catalysts and use these insights to facilitate the design of SCR DeNOx catalysts with minimal sulfur dioxide oxidation activity. A series of supported vanadia catalysts were prepared on various metal-oxide supports: ceria, zirconia, titania, alumina and silica. Raman spectroscopy was used to determine the coordination of surface species. At low vanadia 5 loadings, vanadia preferentially exists on oxide support surfaces as isolated tetrahedrally coordinated (M±O)3V O species. 5 At higher vanadia loadings, the isolated (M±O)3V O species polymerize on the oxide support surface breaking two V±O±M bonds and forming two V±O±V bridging bonds. The turnover frequency for sulfur dioxide oxidation was very low, 104 to 106 s1 at 4008C, and was independent of vanadia coverage suggesting that only one vanadia site is required for the oxidation reaction. As the support was varied, sulfur dioxide oxidation activity of the supported vanadia catalysts varied by one order of magnitude (Ce>Zr, Ti>Al>Si). The basicity of the bridging V±O±M oxygen appears to be responsible for in¯uencing the adsorption and subsequent oxidation of the acidic sulfur dioxide molecule. Over the range of conditions studied, the rate of sulfur dioxide oxidation is zero-order in oxygen, ®rst-order in sulfur dioxide and inhibited by sulfur trioxide. -
Chemical Reactions
INTRODUCTION:- Sulfuric acid (alternative spelling sulphuric acid) is a highly corrosive strong mineral acid with the molecular formula H2SO4. It is a pungent-ethereal, colorless to slightly yellow viscous liquid which is soluble in water at all concentrations.Sometimes, it is dyed dark brown during production to alert people to its hazards.The historical name of this acid is oil of vitriol. Pure sulfuric acid is not encountered naturally on Earth in anhydrous form, due to its great affinity for water. Dilute sulfuric acid is a constituent of acid rain, which is formed by atmospheric oxidation of sulfur dioxide in the presence of water – i.e., oxidation of sulfurous acid. Sulfur dioxide is the main byproduct produced when sulfur-containing fuels such as coal or oil are burned. Sulfuric acid is formed naturally by the oxidation of sulfide minerals, such as iron sulfide. The resulting water can be highly acidic and is called acid mine drainage (AMD) or acid rock drainage (ARD). This acidic water is capable of dissolving metals present in sulfide ores, which results in brightly colored, toxic streams. Alternative Names:- 1. Oil of vitriol 2. Sulfuric acid 3. Vitriol 4. Battery acid 5. Electrolyte acid PHYSICAL PROPERTIES:- Appearance colourless, oily, corrosive liquid Melting point 10 deg C Molecular Formula H2O4S 337 deg C Boiling point 1mm of Hg at 145.8 deg C Vapor pressure 1.840 g/mL Density <0.3 (25 °C, vs air) vapor density 1.01 pH of 10 % of solution Non flammable Flammability limits 98.07848 g/mol Molar weight CHEMICAL PROPERTIES :- Attacks most metals. -
Nitration of Naphthalene and Remarks on the Mechanism of Electrophilic Aromatic Nitration* (Two-Step Mechanism) GEORGE A
Proc. Nati. Acad. Sci. USA Vol. 78, No. 6, pp. 3298-3300, June 1981 Chemistry Nitration of naphthalene and remarks on the mechanism of electrophilic aromatic nitration* (two-step mechanism) GEORGE A. OLAH, SUBHASH C. NARANG, AND JUDITH A. OLAH Institute of Hydrocarbon Chemistry, Department of Chemistry, University of Southern California, Los Angeles, California 90007 Contributed by George A. Olah, March 2, 1981 ABSTRACT Naphthalene was nitrated with a variety of ni- Table 1. Nitration of naphthalene with various nitrating agents trating agents. Comparison of data with Perrin's electrochemical nitration [Perrin, C. L. (1977)J. Am. Chem. Soc. 99, 5516-5518] a/p shows that nitration of naphthalene gives an a-nitronaphthalene Temp, isomer to fi-nitronaphthalene ratio that varies between 9 and 29 and is Reagent Solvent OC ratio Ref. thus not constant. Perrin's data, therefore, are considered to be NO2BF4 Sulfolane 25 10 * inconclusive evidence for the proposed one-electron transfer NO2BF4 Nitromethane 25 12 mechanism for the nitration of naphthalene and other reactive HNO3 Nitromethane 25 29 1 aromatics. Moodie and Schoefield [Hoggett, J. G., Moodie, R. B., HNO3 Acetic acid 25 21 1 Penton, J. R. & Schoefield, K. (1971) Nitration andAromatic Reac- HNO3 Acetic acid 50 16 1 tivity (Cambridge Univ. Press, London)], as well as Perrin, in- HNO3 Sulfuric acid 70 22 1 dependently concluded that, in the general scheme of nitration of HNO3 Acetic 25 9 reactive aromatics, there is the necessity to introduce into the clas- anhydride sical Ingold mechanism an additional step involving a distinct in- CH30NOjCH3OSO2F Acetonitrile 25 13 * termediate preceding the formation ofthe Wheland intermediate AgNO3/CH3COCI Acetonitrile 25 12 * (o complexes). -
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. -
Dissociation Constants and Ph-Titration Curves at Constant Ionic Strength from Electrometric Titrations in Cells Without Liquid
U. S. DEPARTMENT OF COMMERCE NATIONAL BUREAU OF STANDARDS RESEARCH PAPER RP1537 Part of Journal of Research of the N.ational Bureau of Standards, Volume 30, May 1943 DISSOCIATION CONSTANTS AND pH-TITRATION CURVES AT CONSTANT IONIC STRENGTH FROM ELECTRO METRIC TITRATIONS IN CELLS WITHOUT LIQUID JUNCTION : TITRATIONS OF FORMIC ACID AND ACETIC ACID By Roger G. Bates, Gerda L. Siegel, and S. F. Acree ABSTRACT An improved method for obtaining the titration curves of monobasic acids is outlined. The sample, 0.005 mole of the sodium salt of the weak acid, is dissolver! in 100 ml of a 0.05-m solution of sodium chloride and titrated electrometrically with an acid-salt mixture in a hydrogen-silver-chloride cell without liquid junction. The acid-salt mixture has the composition: nitric acid, 0.1 m; pot assium nitrate, 0.05 m; sodium chloride, 0.05 m. The titration therefore is performed in a. medium of constant chloride concentration and of practically unchanging ionic strength (1'=0.1) . The calculations of pH values and of dissociation constants from the emf values are outlined. The tit ration curves and dissociation constants of formic acid and of acetic acid at 25 0 C were obtained by this method. The pK values (negative logarithms of the dissociation constants) were found to be 3.742 and 4. 754, respectively. CONTENTS Page I . Tntroduction __ _____ ~ __ _______ . ______ __ ______ ____ ________________ 347 II. Discussion of the titrat ion metbod __ __ ___ ______ _______ ______ ______ _ 348 1. Ti t;at~on. clU,:es at constant ionic strength from cells without ltqUld JunctlOlL - - - _ - __ _ - __ __ ____ ____ _____ __ _____ ____ __ _ 349 2.