US20050020856A1 - Process for production of acetyl anhydrides and optionally acetic acid from methane and carbon dioxide - Google Patents

Process for production of acetyl anhydrides and optionally acetic acid from methane and carbon dioxide Download PDF

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Publication number
US20050020856A1
US20050020856A1 US10/627,254 US62725403A US2005020856A1 US 20050020856 A1 US20050020856 A1 US 20050020856A1 US 62725403 A US62725403 A US 62725403A US 2005020856 A1 US2005020856 A1 US 2005020856A1
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acid
process according
anhydride
acetyl
product
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US10/627,254
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Alexis Bell
Sudip Mukhopadhyay
Mark Zerella
John Sunley
Sander Gaemers
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BP Chemicals Ltd
University of California
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University of California
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Priority to US10/627,254 priority Critical patent/US20050020856A1/en
Assigned to REGENTS OF THE UNIVERSITY OF CALIFORNIA, THE reassignment REGENTS OF THE UNIVERSITY OF CALIFORNIA, THE ASSIGNMENT OF ASSIGNORS INTEREST (SEE DOCUMENT FOR DETAILS). Assignors: MUKHOPADHYAY, SUDIP, BELL, ALEXIS T., ZERELLA, MARK
Assigned to BP CHEMICALS LIMTIED reassignment BP CHEMICALS LIMTIED ASSIGNMENT OF ASSIGNORS INTEREST (SEE DOCUMENT FOR DETAILS). Assignors: GAEMERS, SANDER, SUNLEY, JOHN GLENN
Priority to US10/897,769 priority patent/US6960682B2/en
Priority to RU2006105510/04A priority patent/RU2006105510A/ru
Priority to JP2006521257A priority patent/JP2006528633A/ja
Priority to CA002533264A priority patent/CA2533264A1/fr
Priority to PCT/US2004/023681 priority patent/WO2005009927A2/fr
Priority to KR1020067001658A priority patent/KR20060065644A/ko
Priority to CNA2004800238781A priority patent/CN1839110A/zh
Priority to BRPI0412244-5A priority patent/BRPI0412244A/pt
Priority to EP04757223A priority patent/EP1651589A4/fr
Publication of US20050020856A1 publication Critical patent/US20050020856A1/en
Priority to NO20060407A priority patent/NO20060407L/no
Abandoned legal-status Critical Current

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    • C—CHEMISTRY; METALLURGY
    • C07—ORGANIC CHEMISTRY
    • C07C—ACYCLIC OR CARBOCYCLIC COMPOUNDS
    • C07C309/00—Sulfonic acids; Halides, esters, or anhydrides thereof
    • C—CHEMISTRY; METALLURGY
    • C07—ORGANIC CHEMISTRY
    • C07C—ACYCLIC OR CARBOCYCLIC COMPOUNDS
    • C07C51/00—Preparation of carboxylic acids or their salts, halides or anhydrides
    • C07C51/15—Preparation of carboxylic acids or their salts, halides or anhydrides by reaction of organic compounds with carbon dioxide, e.g. Kolbe-Schmitt synthesis
    • C—CHEMISTRY; METALLURGY
    • C07—ORGANIC CHEMISTRY
    • C07C—ACYCLIC OR CARBOCYCLIC COMPOUNDS
    • C07C381/00—Compounds containing carbon and sulfur and having functional groups not covered by groups C07C301/00 - C07C337/00
    • C—CHEMISTRY; METALLURGY
    • C07—ORGANIC CHEMISTRY
    • C07C—ACYCLIC OR CARBOCYCLIC COMPOUNDS
    • C07C51/00—Preparation of carboxylic acids or their salts, halides or anhydrides
    • C07C51/54—Preparation of carboxylic acid anhydrides
    • C07C51/56—Preparation of carboxylic acid anhydrides from organic acids, their salts, their esters or their halides, e.g. by carboxylation
    • C—CHEMISTRY; METALLURGY
    • C07—ORGANIC CHEMISTRY
    • C07C—ACYCLIC OR CARBOCYCLIC COMPOUNDS
    • C07C53/00—Saturated compounds having only one carboxyl group bound to an acyclic carbon atom or hydrogen
    • C—CHEMISTRY; METALLURGY
    • C07—ORGANIC CHEMISTRY
    • C07C—ACYCLIC OR CARBOCYCLIC COMPOUNDS
    • C07C67/00—Preparation of carboxylic acid esters
    • C07C67/08—Preparation of carboxylic acid esters by reacting carboxylic acids or symmetrical anhydrides with the hydroxy or O-metal group of organic compounds

Definitions

  • This invention relates to the production of acetyl anhydrides, and optionally of acetic acid, and particularly to a process for the production of such substances from methane and carbon dioxide.
  • Methane is the lowest molecular weight, and simplest in structure, of the hydrocarbons. Because of the existence of large reserves of methane worldwide it has been considered desirable for some time to develop processes to convert methane to more valuable chemicals. Processes for production of acetic acid from methanol represent an ultimate use of methane, but in current commercial practice, the methane first must be converted to methanol. A process that produces acetic acid directly from methane would be more desirable.
  • PCT application WO 96/05163 of Hoechst A. G. describes a gas phase reaction of methane and carbon dioxide to produce acetic acid, using a catalyst containing one or more Group VIA, VIIA and/or VIIIA metals. Selectivities of 70-95% based on methane are asserted; however the application contains no exemplary data.
  • Kurioka et al. (1995, supra) also reported a liquid phase experiment in which methane was reacted with carbon dioxide in the presence of palladium acetate, cupric acetate, potassium persulfate and trifluoroacetic acid, reportedly producing acetic acid. The yield was said to have been 1650% (based on the palladium). This work was continued and further reported on by Taniguchi et al., Studies in Surface Science and Catalysis 1998, 439-442.
  • TFA trifluoroacetic acid
  • Taniguchi et al. (1998) hypothesized that the acetic acid was produced by reaction of methane and carbon dioxide, but subsequent work by others (and by us) showed that this was not correct; in the Taniguchi et al. work the acetic acid would have been produced primarily if not entirely by reaction of methane and TFA, with concomitant production of one mole of fluoroform for each mole of acetic acid produced by this reaction.
  • TFA is an expensive feedstock for the production of acetic acid.
  • An improved process for the production of acetyl anhydrides also would be desirable.
  • An acetyl anhydride compound can be defined as a compound, which upon reaction with water liberates acetic acid and another non-hydrohalogenoic acid.
  • an acetyl anhydride compound may be described as a compound in which the hydroxy group of acetic acid has been replaced with the anion of a non-hydrohalogenoic acid.
  • Acetyl sulfate is one example of an acetyl anhydride. It typically is produced by reacting acetic anhydride with sulfuric acid and has a number of uses, for instance as a sulfonating agent and as a chemical intermediate.
  • This invention relates to a process for producing an acetyl anhydride comprising:
  • the invention relates to a process for producing a product comprising acetic acid from methane and carbon dioxide comprising producing an acetyl anhydride as above, and then reacting the product of this step with water.
  • the invention in another aspect, relates to a process for producing a product comprising an acetate ester by reacting the acetyl anhydride-containing product with an alcohol.
  • the acetyl anhydride could be hydrogenated to produce products comprising ethanol, ethyl bisulfate, ethyl acetate, etc., depending on the non-acetyl component of the anhydride.
  • Acetyl anhydrides produced as above may be novel compounds and thus form another aspect of this invention.
  • the invention also comprises the step of recovering acetic acid from the reaction product of the acetyl anhydride and water, or recovering the acetate ester from the reaction product of the acetyl anhydride and alcohol.
  • FIG. 1 depicts 1 H NMR analysis of a product obtained by contacting methane, carbon dioxide, trifluoroacetic acid and trifluoroacetic anhydride, then contacting the product with water.
  • FIG. 2 depicts 1 H NMR analysis of a product produced by contacting methane, carbon dioxide and fuming sulfuric acid, then contacting the product with water.
  • FIG. 3 depicts 1 H NMR analysis of a product obtained by contacting methane, carbon dioxide and fuming sulfuric acid, before addition of water.
  • This invention comprises a process for producing an acetyl anhydride comprising contacting methane and carbon dioxide in an anhydrous environment in the presence of effective amounts of a transition metal catalyst and a reaction promoter, and an acid anhydride compound, and optionally an acid, to produce a product comprising the acetyl anhydride.
  • the invention further comprises a process for producing a product comprising acetic acid in two steps, comprising:
  • the invention also comprises the step of:
  • the invention also comprises a process as above, and additionally:
  • methane and carbon dioxide are contacted, in the presence of a transition metal catalyst, a reaction promoter and an acid anhydride compound, and optionally an acid.
  • a transition metal catalyst e.g., platinum, palladium, platinum, palladium, platinum, palladium, platinum, palladium, platinum, palladium, platinum, palladium, palladium, calcium, magnesium, magnesium, magnesium, magnesium, magnesium, magnesium, magnesium, magnesium, magnesium, magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium magnesium
  • Acid anhydrides suitable for use in the processes of this invention include, for example, sulfur trioxide, sulfur dioxide, trifluoroacetic acid anhydride, trifluoromethanesulfonic acid anhydride, anhydrides of other sulfonic acids such as fluorosulfonic acid anhydride, fluoromethanesulfonic acid anhydride, methanesulfonic acid anhydride, etc., NO, NO 2 , N 2 O 5 , P 2 O 5 , SeO 3 , As 2 O 5 , TeO 3 , and B 2 O 3 .
  • Some acid anhydrides, such as anhydrides of longer chain carboxylic acids might not be suitable for use in the processes of this invention, however, as they contain secondary methylene groups that could interact with the reaction promoter.
  • the methane, carbon dioxide, and other materials preferably are contacted in the presence of an acid that one the one hand acts as a solvent but that may also participate as a reagent in the process.
  • Suitable acids include organic acids such as trifluoroacetic, fluorosulfonic, methanesulfonic, fluoromethanesulfonic, and trifluoromethanesulfonic acids, and inorganic acids such as sulfuric, sulfurous, nitric, nitrous, phosphoric, phosphorous, superphosphoric, and boric acids, as well as selenium- and tellurium-containing analogs of the sulfur-containing acids.
  • the acid is the corresponding acid of the acid anhydride compound used, e.g., when the acid anhydride compound is trifluoroacetic acid anhydride the reaction is conducted in the presence of trifluoroacetic acid, and when the acid anhydride compound is sulfur trioxide the acid is sulfuric acid, or in that case, more preferably fuming sulfuric acid is used to supply both the acid and the anhydride.
  • the acid anhydride compound is trifluoroacetic acid anhydride the reaction is conducted in the presence of trifluoroacetic acid, and when the acid anhydride compound is sulfur trioxide the acid is sulfuric acid, or in that case, more preferably fuming sulfuric acid is used to supply both the acid and the anhydride.
  • Mixtures of acid anhydride compounds or of acids may be used, if desired.
  • the molar ratios of the three substances are from about 0.5:1:1 to about 1:6:10, preferably from about 1:1:1 to about 1: 2:2 respectively.
  • the amount of methane generally ranges from about 10 to about 50 mmol (from about 1 to about 5 mol/dm 3 , assuming all the methane enters the liquid phase).
  • the amount of carbon dioxide generally ranges from about 5 to about 60 mmol (from about 0.5 to about 6 mol/dm 3 , assuming all the CO 2 enters the liquid phase).
  • this reaction is conducted at a temperature of from about 10 to about 200° C., preferably from about 60 to about 100° C., and for a time of from about 2 to about 48 hours, preferably from about 10 to about 20 hours.
  • the process can be either a batch or continuous process, but is preferably a continuous process.
  • the total pressure of the reaction is suitably in the range 5 barg to 200 barg.
  • the partial pressure of methane is suitably in the range 2.5 barg to 100 barg, and the partial pressure of carbon dioxide is suitably in the range 2.5 barg to 100 barg.
  • the liquid phase initially comprises the acid anhydride compound and optionally the acid.
  • the acid anhydride compound is present in an amount constituting from about 1% to about 100% of the liquid reaction composition, excluding catalysts and reaction promoters (i.e., if no acid is present, the anhydride is the sole initial liquid component in the process, not including catalyst and reaction promoter).
  • an acid is used in the process, it is present in the liquid reaction composition in an amount of from about 0.1% to about 99% by weight, preferably from about 1% to about 80% by weight.
  • the acid concentration range is suitably chosen depending on the acid and acid anhydride compound used in the processes. The use of a higher amount of acid may be desirable in order to improve solubility of a particular catalyst and/or promoter in the liquid reaction composition.
  • the acid should be used in as dry a state as practicable.
  • Also present at this stage are a catalyst and a reaction promoter.
  • Catalysts suitable for use in this process are transition metal catalysts, particularly compounds of vanadium, chromium, tantalum and niobium.
  • the transition metal catalyst is a vanadium-containing catalyst such as those known in the art to catalyze reactions between methane and carbon dioxide.
  • a preferred catalyst is vanadyl acetylacetonate, VO(acac) 2 , where “acac” represents the group CH 3 COCHCOCH 3 .
  • vanadium-containing catalysts include sodium metavanadate, NaVO 3 , vanadium trioxide, vanadium pentoxide, and heteropolyacid catalysts containing vanadium and other metallic and/or non-metallic elements such as phosphorus, silicon, molybdenum and tungsten.
  • heteropolyacid catalysts are disclosed in Taniguchi et al (1998) and Piao et al. (1999), both supra.
  • Still other suitable catalysts are the vanadium-containing catalysts disclosed in Reis et al. (2003), supra, i.e.:
  • the catalyst is used in an amount of from about 0.05 mmol to about 0.5 mmol (from about 0.005 to about 0.05 mol/dm 3 ).
  • the molar ratio of methane to catalyst is about 150:1.
  • reaction initiator that is, a compound that assists in commencement of the reaction through free-radical initiation or other mechanism.
  • reaction initiators Most of the well-known and commonly used reaction initiators may be employed in this process, providing they do not react with other components to form side products or are otherwise undesirable.
  • the preferred initiator is potassium peroxysulfate, K 2 S 2 O 8 .
  • suitable initiators include K 4 P 2 O 8 , calcium dioxide, urea-hydrogen peroxide and m-chloroperbenzoic acid.
  • the initiator is used in an amount of from about 0.5 to about 20 mmol (from about 0.05 to about 2 mol/dm 3 ), preferably from about 3.5 to about 3.7 mmol (from about 0.35 to about 0.37 mol/dm 3 ).
  • the overall reaction taking place in this process can generally be depicted as CH 4 +CO 2 +XO n ⁇ CH 3 C(O)—O—XO n H where XO n is a binary acid anhydride compound, for example SO 3 , and where the acid form of the binary anhydride is optionally used as the solvent for the reaction, or it can be depicted as CH 4 +CO 2 +Z 2 O ⁇ CH 3 C(O)—O-Z+ZOH where Z 2 O is an acid anhydride compound and where ZOH is an oxygen-containing acid compound, which is optionally used as the solvent for the reaction.
  • the overall reaction taking place in this process can be depicted as CH 4 +CO 2 +H 2 S 2 O 7 ⁇ CH 3 C(O)—O—SO 3 H+H 2 SO 4 where fuming sulfuric acid (H 2 S 2 O 7 ) is used in the process, which may be alternatively written as CH 4 +CO 2 +SO 3 ⁇ CH 3 C(O)—O—SO 3 H (i.e.
  • the product of this process is a mixed anhydride of acetic acid and the acid anhydride compound and/or a mixed anhydride of acetic acid and the acid, if an acid is also used in the process.
  • this mixed anhydride an “acetyl anhydride”.
  • the product of the reaction is generally also known as acetyl sulfate, which typically is used as a sulfonating agent or as a chemical intermediate. For example, it can be hydrogenated to provide ethanol, ethyl acetate or ethyl bisulfate. Reaction of acetyl sulfate with alcohols produces alkyl acetates and sulfuric acid. Acetyl sulfate is generally produced by reacting acetic anhydride with sulfuric acid; consequently step (a) of the process may serve as an alternate process for producing acetyl sulfate.
  • acetyl anhydride resulting from a process in which trifluoromethanesulfonic acid is used, or its anhydride is used without the acid is a novel compound, having the formula CH 3 C(O)—O—SO 2 CF 3 , and forms an aspect of this invention. Subsequent reaction of it with water produces acetic acid and trifluoromethanesulfonic acid.
  • the addition of water to the acetyl anhydride is generally performed at a temperature of from about 0 to about 100° C., preferably from about 30 to about 60° C., and is exothermic.
  • the resulting product is a mixture of acetic acid and the acid used in the acetyl anhydride production, or of acetic acid and the acid anhydride compound, if no acid is employed.
  • the product may also contain small amounts of by-products such as the methyl ester of the starting acid.
  • the acetic acid may readily be separated from the reaction products by techniques such as azeotropic distillation or membrane separation. The other acid may conveniently be recycled to the acetyl anhydride production step.
  • the ester similarly may be recovered from the reaction products by techniques such as azeotropic distillation or membrane separation.
  • the products of such a reaction usually also include acetic acid and/or esters of the other acid component of the acetyl anhydride (e.g. trfluoroacetates, trifluoromethanesulfonates, etc.).
  • acetic acid and/or esters of the other acid could also be recovered from the products of this step, if desired.
  • acetic acid using a combination of trifluoroacetic acid and its anhydride
  • the amounts used were 3.7 mmol K 2 S 2 O 8 , 0.16 mmol VO(acac) 2 , 10.0 g trifluoroacetic acid and 3.0 g of its anhydride.
  • the solvent was chilled to 5-8° C. during these additions to minimize the thermal decomposition of K 2 S 2 O 8 .
  • the reactor was then purged with N 2 to expel the air out of the system. It was then pressurized first with 120 psig CO 2 and then finally with 80 psig methane from adjacent connecting cylinders.
  • the reactor was heated to 85° C. under stirring and maintained for 16-17 h.
  • Table 1 shows the effect of the starting acid on the conversion of CH 4 to acetic acid. The highest conversion (16%) was obtained with trifluoroacetic anhydride and trifluoroacetic acid. Approximately 7% conversion of CH 4 to acetic acid was obtained when fuming sulfuric acid was used, and 13% conversion when trifluoromethanesulfonic acid anhydride and trifluoromethanesulfonic acid were used. Small amounts of methyl esters of the starting acids were produced as byproducts in each reaction. To ensure that any CO or CO 2 produced by the oxidation of CH 4 by K 2 S 2 O 8 under the reaction conditions was not responsible for acetic acid formation, a blank reaction was performed in the absence of CO 2 . 1 H NMR analysis of the product is shown in FIG.

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US10/627,254 2003-07-24 2003-07-24 Process for production of acetyl anhydrides and optionally acetic acid from methane and carbon dioxide Abandoned US20050020856A1 (en)

Priority Applications (11)

Application Number Priority Date Filing Date Title
US10/627,254 US20050020856A1 (en) 2003-07-24 2003-07-24 Process for production of acetyl anhydrides and optionally acetic acid from methane and carbon dioxide
US10/897,769 US6960682B2 (en) 2003-07-24 2004-07-22 Process for production of acetyl anhydrides and optionally acetic acid from methane and carbon dioxide
EP04757223A EP1651589A4 (fr) 2003-07-24 2004-07-23 Methode de production d'anhydrides acetiques et eventuellement d'acide acetique a partir du methane et du dioxyde de carbone
BRPI0412244-5A BRPI0412244A (pt) 2003-07-24 2004-07-23 processo para produção de acetil anidridos e opcionalmente ácido acético a partir de metano e dióxido de carbono
PCT/US2004/023681 WO2005009927A2 (fr) 2003-07-24 2004-07-23 Methode de production d'anhydrides acetiques et eventuellement d'acide acetique a partir du methane et du dioxyde de carbone
JP2006521257A JP2006528633A (ja) 2003-07-24 2004-07-23 メタン及び二酸化炭素からアセチル無水物及び随意選択的な酢酸の生成法
CA002533264A CA2533264A1 (fr) 2003-07-24 2004-07-23 Methode de production d'anhydrides acetiques et eventuellement d'acide acetique a partir du methane et du dioxyde de carbone
RU2006105510/04A RU2006105510A (ru) 2003-07-24 2004-07-23 Способ получения ангидридов уксусной кислоты и необязательно уксусной кислоты из метана и диоксида углерода
KR1020067001658A KR20060065644A (ko) 2003-07-24 2004-07-23 메탄 및 이산화탄소로부터 아세틸 무수물 및 임의로아세트산을 제조하는 방법
CNA2004800238781A CN1839110A (zh) 2003-07-24 2004-07-23 从甲烷和二氧化碳生产乙酰基酸酐和任选地生产乙酸的方法
NO20060407A NO20060407L (no) 2003-07-24 2006-01-25 Metode for fremstilling av acetyl-anhydrider og eventuelt eddiksyre fra metan og karbondioksid

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US10/897,769 Expired - Lifetime US6960682B2 (en) 2003-07-24 2004-07-22 Process for production of acetyl anhydrides and optionally acetic acid from methane and carbon dioxide

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US (2) US20050020856A1 (fr)
EP (1) EP1651589A4 (fr)
JP (1) JP2006528633A (fr)
KR (1) KR20060065644A (fr)
CN (1) CN1839110A (fr)
BR (1) BRPI0412244A (fr)
CA (1) CA2533264A1 (fr)
NO (1) NO20060407L (fr)
RU (1) RU2006105510A (fr)
WO (1) WO2005009927A2 (fr)

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* Cited by examiner, † Cited by third party
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WO2007018679A1 (fr) * 2005-07-26 2007-02-15 Lyondell Chemical Technology, L.P. Préparation d'acétate d'alkyle tertiaire
US20090325388A1 (en) * 2008-06-30 2009-12-31 Hitachi High-Technologies Corporation Method of semiconductor processing
US10882874B2 (en) * 2016-06-22 2021-01-05 Adeka Corporation Vanadium compound
CN113003548A (zh) * 2021-04-02 2021-06-22 昆明鼎邦科技股份有限公司 一种除去粗硒中碲制备高纯硒的方法

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MX2015010722A (es) * 2013-02-25 2016-01-14 Scripps Research Inst Procesos selectivos, directos para la oxidacion de alcanos de gas natural para alcoholes.
CN104177256B (zh) * 2014-08-04 2016-05-25 山西农业大学 一种梨小食心虫性信息素(z/e)-8-十二碳烯醋酸酯的合成方法
CN105218361A (zh) * 2015-10-19 2016-01-06 石家庄中硕药业有限公司 一种十二碳烯醇乙酸酯的合成方法
KR102629665B1 (ko) * 2017-05-30 2024-01-25 바스프 에스이 알칸설폰산의 제조 방법
RU2654982C1 (ru) * 2017-08-10 2018-05-23 ФЕДЕРАЛЬНОЕ ГОСУДАРСТВЕННОЕ БЮДЖЕТНОЕ УЧРЕЖДЕНИЕ НАУКИ ИНСТИТУТ ОРГАНИЧЕСКОЙ ХИМИИ им. Н.Д. ЗЕЛИНСКОГО РОССИЙСКОЙ АКАДЕМИИ НАУК (ИОХ РАН) Тетранитратоборат нитрония и способ его получения
KR102391903B1 (ko) * 2020-02-07 2022-04-28 한국과학기술연구원 메탄으로부터 메탄올 전구체, 메탄올 또는 메틸에스테르 제조방법

Citations (8)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
US4221712A (en) * 1979-03-23 1980-09-09 Exxon Research & Engineering Co. Process for forming a metal sulfonate containing EPDM
US4316828A (en) * 1977-11-29 1982-02-23 Exxon Research & Engineering Co. Bulk neutralization
US5401876A (en) * 1992-07-23 1995-03-28 Elf Atochem S.A. Synthesis of chloroacetic acids
US5659077A (en) * 1996-03-22 1997-08-19 Natural Resources Canada Production of acetic acid from methane
US6380426B1 (en) * 2001-09-26 2002-04-30 Council Of Scientific And Industrial Research Process for the preparation of a carboxylic acid
US6383977B1 (en) * 1997-12-24 2002-05-07 Saudi Basic Industries Corporation Catalysts for producing acetic acid from ethane oxidation, processes of making the same and methods of using same
US6399816B1 (en) * 1997-10-17 2002-06-04 Celanese Chemicals Europe Gmbh Method for selectively producing acetic acid through the catalytic oxidation of ethane
US6472558B1 (en) * 1999-11-12 2002-10-29 Bp Chemicals Limited Process for the production of acetic acid

Family Cites Families (3)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
GB226248A (en) 1923-06-22 1924-12-22 Henry Dreyfus Improvements relating to the manufacture of acetic acid, acetaldehyde or acetone or mixtures containing the same
WO1996005163A1 (fr) 1994-08-12 1996-02-22 Hoechst Aktiengesellschaft Procede de preparation d'acide acetique
JPH10226665A (ja) * 1996-12-10 1998-08-25 Sumitomo Chem Co Ltd カルボン酸類の製造方法

Patent Citations (8)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
US4316828A (en) * 1977-11-29 1982-02-23 Exxon Research & Engineering Co. Bulk neutralization
US4221712A (en) * 1979-03-23 1980-09-09 Exxon Research & Engineering Co. Process for forming a metal sulfonate containing EPDM
US5401876A (en) * 1992-07-23 1995-03-28 Elf Atochem S.A. Synthesis of chloroacetic acids
US5659077A (en) * 1996-03-22 1997-08-19 Natural Resources Canada Production of acetic acid from methane
US6399816B1 (en) * 1997-10-17 2002-06-04 Celanese Chemicals Europe Gmbh Method for selectively producing acetic acid through the catalytic oxidation of ethane
US6383977B1 (en) * 1997-12-24 2002-05-07 Saudi Basic Industries Corporation Catalysts for producing acetic acid from ethane oxidation, processes of making the same and methods of using same
US6472558B1 (en) * 1999-11-12 2002-10-29 Bp Chemicals Limited Process for the production of acetic acid
US6380426B1 (en) * 2001-09-26 2002-04-30 Council Of Scientific And Industrial Research Process for the preparation of a carboxylic acid

Cited By (4)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
WO2007018679A1 (fr) * 2005-07-26 2007-02-15 Lyondell Chemical Technology, L.P. Préparation d'acétate d'alkyle tertiaire
US20090325388A1 (en) * 2008-06-30 2009-12-31 Hitachi High-Technologies Corporation Method of semiconductor processing
US10882874B2 (en) * 2016-06-22 2021-01-05 Adeka Corporation Vanadium compound
CN113003548A (zh) * 2021-04-02 2021-06-22 昆明鼎邦科技股份有限公司 一种除去粗硒中碲制备高纯硒的方法

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RU2006105510A (ru) 2006-06-27
CN1839110A (zh) 2006-09-27
WO2005009927A3 (fr) 2005-03-24
WO2005009927A2 (fr) 2005-02-03
KR20060065644A (ko) 2006-06-14
CA2533264A1 (fr) 2005-02-03
EP1651589A2 (fr) 2006-05-03
JP2006528633A (ja) 2006-12-21
US20050065364A1 (en) 2005-03-24

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