EP2038212A1 - Procédé d'oxydation d'un gaz contenant du chlorure d'hydrogène - Google Patents

Procédé d'oxydation d'un gaz contenant du chlorure d'hydrogène

Info

Publication number
EP2038212A1
EP2038212A1 EP07725288A EP07725288A EP2038212A1 EP 2038212 A1 EP2038212 A1 EP 2038212A1 EP 07725288 A EP07725288 A EP 07725288A EP 07725288 A EP07725288 A EP 07725288A EP 2038212 A1 EP2038212 A1 EP 2038212A1
Authority
EP
European Patent Office
Prior art keywords
hydrogen chloride
carbon monoxide
oxidation
reactor
oxygen
Prior art date
Legal status (The legal status is an assumption and is not a legal conclusion. Google has not performed a legal analysis and makes no representation as to the accuracy of the status listed.)
Withdrawn
Application number
EP07725288A
Other languages
German (de)
English (en)
Inventor
Michael Haas
Markus Dugal
Knud Werner
Current Assignee (The listed assignees may be inaccurate. Google has not performed a legal analysis and makes no representation or warranty as to the accuracy of the list.)
Covestro Deutschland AG
Original Assignee
Bayer MaterialScience AG
Priority date (The priority date is an assumption and is not a legal conclusion. Google has not performed a legal analysis and makes no representation as to the accuracy of the date listed.)
Filing date
Publication date
Application filed by Bayer MaterialScience AG filed Critical Bayer MaterialScience AG
Publication of EP2038212A1 publication Critical patent/EP2038212A1/fr
Withdrawn legal-status Critical Current

Links

Classifications

    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
    • C01B7/00—Halogens; Halogen acids
    • C01B7/01—Chlorine; Hydrogen chloride
    • C01B7/07—Purification ; Separation
    • C01B7/0706—Purification ; Separation of hydrogen chloride
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
    • C01B32/00—Carbon; Compounds thereof
    • C01B32/50—Carbon dioxide
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
    • C01B7/00—Halogens; Halogen acids
    • C01B7/01—Chlorine; Hydrogen chloride
    • C01B7/03—Preparation from chlorides
    • C01B7/04—Preparation of chlorine from hydrogen chloride

Definitions

  • the present invention relates to a process for the production of chlorine from a gas containing hydrogen chloride and carbon monoxide, which comprises the step of catalysed oxidation of carbon monoxide and optionally other oxidizable constituents to carbon dioxide with oxygen in an upstream reactor under adiabatic conditions.
  • CO carbon monoxide
  • a greater amount of carbon monoxide (CO) may be present as an impurity in the HCl exhaust.
  • CO contents in the range from 0 to 3% by volume are generally found in the HCl offgas of the phosgene wash-off column.
  • pioneering gas phase phosgenation DE 42 17 019 Al, DE 103 07 141 Al
  • higher CO amounts (0 to more than 5%) are to be expected because in this method preferably no condensation of phosgene, and a related extensive Separation of the unreacted carbon monoxide, before the phosgenation is carried out.
  • a wide variety of catalysts is used, for example based on ruthenium, chromium, copper, etc.
  • Such catalysts are described, for example, in DE 1 567 788 A1, EP 251 731 A2, EP 936 184 A2, EP 761 593 Al, EP 711 599 Al and DE 102 50 131 Al.
  • these can simultaneously act as oxidation catalysts for any secondary components such as carbon monoxide or organic compounds.
  • the catalytic carbon monoxide oxidation to carbon dioxide is extremely exothermic and causes uncontrolled local temperature increases at the surface of the heterogeneous catalyst (hot spot) in the way that deactivation of the catalyst can take place with respect to the HCl oxidation.
  • metal carbonyls can be reversible or irreversible and thus be in direct competition with HCl oxidation.
  • carbon monoxide may be mixed with some elements, e.g. Osmium, rhenium, ruthenium (see Chem. Rev. 103, 3707-3732, 2003), even at high temperatures very stable bonds and thus cause an inhibition of the desired target reaction.
  • Osmium, rhenium, ruthenium see Chem. Rev. 103, 3707-3732, 2003
  • Another disadvantage could arise from the volatility of these metal carbonyls (see Chem. Rev., 21, 3-38, 1937), whereby not inconsiderable amounts of catalyst are lost and, in addition, depending on the application, require a complicated purification step of the reaction product.
  • catalyst deactivation can be caused by both destruction of the catalyst and by limitation of stability. Competition between hydrogen chloride and carbon monoxide can also lead to inhibition of the desired HCl oxidation reaction. For an optimal operation of the Deacon process is therefore a very low content of carbon monoxide in the HCl gas necessary to ensure a long life of the catalyst used.
  • JP-2005289800-A describe the attempt to stabilize the catalytic phase for the HCl oxidation to the simultaneous oxidation of hydrogen chloride and carbon monoxide, and other minor components (eg phosgene, hydrogen and organic Connections).
  • this procedure is limited to small amounts of secondary constituents, preferably less than 0.5% by volume in the HCl gas stream.
  • the present invention thus relates to a process for the production of chlorine from a hydrogen chloride and carbon monoxide-containing gas comprising the steps:
  • the hydrogen chloride and carbon monoxide containing gas used in the process of the invention is generally the offgas of a phosgenation reaction to form organic isocyanates. It may also be exhaust gases from chlorination reactions of hydrocarbons.
  • the hydrogen chloride and carbon monoxide-containing gas according to the invention may comprise further oxidisable constituents, in particular hydrocarbons. These are generally also oxidized in step a) to form CO 2 .
  • the content of hydrogen chloride in the hydrogen chloride and carbon monoxide-containing gas entering the pre-reactor of step a) is, for example, in the range of 20 to 99.5% by volume.
  • the content of carbon monoxide in the hydrogen chloride and carbon monoxide-containing gas entering the pre-reactor of step a) is, for example, in the range of 0.5 up to 15% by volume.
  • the process according to the invention makes it possible to tolerate considerably higher amounts of carbon monoxide in the exhaust gas of the phosgenation process when coupled with an isocyanate process.
  • step a) The oxidation of carbon monoxide and the optionally present further oxidizable constituents in step a) is expedient by the addition of oxygen, oxygen-enriched
  • oxygen or oxygen-containing gas can be stoichiometric based on the carbon monoxide content or operated with an excess of oxygen. By adjusting the oxygen excess and optionally an optional
  • Addition of inert gas, preferably nitrogen, optionally, the heat removal from the catalyst in step a) and the outlet temperature of the process gases can be controlled.
  • the inlet temperature of the hydrogen chloride and carbon monoxide-containing gas at the inlet of the pre-reactor in step a) is preferably 0 to 300 ° C., in particular 0 to 150 ° C., preferably 0 to 100 ° C. and more suitably 20 to 100 ° C.
  • the outlet temperature of the gas containing hydrogen chloride at the outlet of the prereactor of step a) is, for example, 100 to 600 ° C., preferably 150 to 400 ° C.
  • the average operating temperature of the prereactor in step a) is generally about 50 to 400 ° C. These comparatively low temperatures enable more economical operation under increased safety conditions.
  • the pre-reactor is operated adiabatically in step a), i. there is no heat to or from the outside.
  • the adiabatic operation of the reactor is ensured by a suitable isolation of the reactor.
  • the heat of reaction released can be used for the adiabatic heating of the starting materials in order to be conducted in the subsequent step to HCl oxidation.
  • This effect was calculated for different CO contents, as well as different ratios of oxygen, at an entrance temperature of 5O 0 C ( Figure 1).
  • step a) of the process according to the invention preference is given to using at least one catalyst which contains at least one element from the group consisting of: chromium, Ruthenium, palladium, platinum, nickel, rhodium, iridium, gold iron, copper, manganese, cobalt, zirconium. These elements may be used alone or in combination, and may be in the form of their oxides. The catalysts may optionally also be supported.
  • catalysts in step a) are those based on palladium, platinum, ruthenium, rhodium or iridium with a promoter (nickel, manganese, copper, silver, lanthanum,...) (See US Pat. No. 4,639,432).
  • Supported gold particles are also suitable for low temperature CO oxidation (J. Catal., 144, 175-192, 1993; Appl. Catal. A: General, 299, 266-273, 2006; Catal. Today, 112, 126-129, 2006), as well as cobalt compounds, eg in the form of cobalt spinels (Appl. Catal.
  • Cerium nanoparticles can also be used for CO oxidation (Phys. Chem. Chem. Phys., 7, 2936-2941, 2005).
  • the step a) is preferably carried out under such pressure conditions which correspond to the operating pressure of the HCl oxidation in step b).
  • Such operating pressures are generally between 1 and 100 bar, preferably between 1 and 50 bar, more preferably between 1 and 25 bar.
  • a slightly increased pressure is preferably used.
  • the content of carbon monoxide in the prereactor of step a) is expediently reduced to less than 1% by volume, preferably to less than 0.5% by volume, more preferably to less than 0.1% by volume, according to the invention.
  • the gas leaving the prereactor of the step contains essentially HCl, CO2, O2 and other minor components, such as nitrogen.
  • the unreacted oxygen can then be used in the further course for the HCl oxidation in step b).
  • the CO-lean gas leaving the prereactor according to step a) optionally passes via a heat exchanger into the reactor for the oxidation of the hydrogen chloride of step b).
  • the heat exchanger between the reactor of step b) and the prereactor of step a) is expediently coupled via a temperature control to the prereactor of step a).
  • the temperature of the gas, which is forwarded to HCl oxidation in the further course can be set exactly. In this case, heat can be dissipated as needed, if the outlet temperature is too high, for example by steam generation. If the outlet temperature is too low, the process gases can be brought to the desired temperature with a small amount of heat.
  • step b) of the process according to the invention the oxidation of the hydrogen chloride is carried out with oxygen to form chlorine in a conventional manner. It is therefore possible to refer to the prior art (cf., for example, WO04 / 014845-A1), the disclosure content of which belongs to the present invention.
  • step b hydrogen chloride is oxidized to chlorine in an exothermic equilibrium reaction with oxygen to produce water vapor.
  • Typical reaction temperatures are between 150 and 500 0 C, usual reaction pressures are between 1 and 50 bar. Since it is an equilibrium reaction, it is expedient to work at the lowest possible temperatures at which the catalyst still has sufficient activity.
  • oxygen in superstoichiometric amounts. For example, a two- to four-fold excess of oxygen is customary. Since no selectivity losses are to be feared, it may be economically advantageous to work at relatively high pressures and, accordingly, at longer residence times than normal pressure.
  • Suitable catalysts include ruthenium oxide, ruthenium chloride or other ruthenium compounds supported on silica, alumina, titania or zirconia. Suitable catalysts can be obtained, for example, by applying ruthenium chloride to the support and then drying or drying and calcining. Suitable catalysts may further contain chromium (III) oxide.
  • Conventional reactors in which the catalytic hydrogen chloride oxidation is carried out are a fixed bed or fluidized bed reactor. The microreactor technology is also a possible alternative. The hydrogen chloride oxidation can be carried out in several stages.
  • the catalytic hydrogen chloride oxidation may also adiabatically but preferably isothermally or approximately isothermally, discontinuously, preferably continuously or as a fixed bed process, preferably as a fixed bed process, particularly preferably in tube bundle reactors to heterogeneous catalysts at reactor temperatures of 180 to 500 0 C, preferably 200 to 400 0 C. , Particularly preferably 220 to 350 0 C and a pressure of 1 to 30 bar, preferably 1, 2 to 25 bar, more preferably 1.5 to 22 bar and in particular 2.0 to 21 bar are performed.
  • adiabatic, isothermal or approximately isothermal mode of operation it is also possible to use a plurality of reactors with intermediate cooling, that is to say 2 to 10, preferably 2 to 6, more preferably 2 to 5, in particular 2 to 3, reactors connected in series.
  • the oxygen can be added either completely together with the hydrogen chloride before the first reactor or distributed over the various reactors.
  • This series connection of individual reactors can also be combined in one apparatus.
  • a preferred embodiment is that one uses a structured catalyst bed, in which the catalyst activity increases in the flow direction. Such structuring of the catalyst bed can by different impregnation of the catalyst support with active material or by different dilution of the catalyst with an inert material.
  • rings, cylinders or balls of titanium dioxide, zirconium dioxide or mixtures thereof, alumina, steatite, ceramic, glass, graphite or stainless steel can be used.
  • Ruthenium compounds or copper compounds on support materials, which may also be doped, are particularly suitable as heterogeneous catalysts, preference being given to optionally doped ruthenium catalysts.
  • suitable carrier materials are silicon dioxide, graphite, rutile or anatase titanium dioxide, zirconium dioxide, aluminum oxide or mixtures thereof, preferably titanium dioxide, zirconium dioxide, aluminum oxide or mixtures thereof, particularly preferably ⁇ - or ⁇ -aluminum oxide or mixtures thereof.
  • the copper or ruthenium-supported catalysts can be obtained, for example, by impregnation of the support material with aqueous solutions of CuCl 2 or RuCl 3 and optionally a promoter for doping, preferably in the form of their chlorides.
  • the conversion of hydrogen chloride in a single pass can be limited to 15 to 95%, preferably 40 to 95%, particularly preferably 50 to 90%. After conversion, unreacted hydrogen chloride can be partly or completely recycled to the catalytic hydrogen chloride oxidation.
  • the catalytic hydrogen chloride oxidation has the advantage over the generation of chlorine by hydrogen chloride electrolysis on the advantage that no expensive electrical energy is required that no questionable safety issues hydrogen is obtained as by-product and that the supplied hydrogen chloride must not be completely pure.
  • the heat of reaction of the catalytic hydrogen chloride oxidation can be used advantageously for the production of high-pressure steam. This can be used to operate the phosgenation reactor and the isocyanate distillation columns. From the chlorine-containing gas resulting in step b), the chlorine is separated in a conventional manner. Chlorine obtained by the process according to the invention can then be reacted with carbon monoxide to phosgene by the processes known from the prior art, which can be used for the preparation of TDI or MDI from TDA or MDA. The hydrogen chloride which is formed in turn during the phosgenation of TDA and MDA can then be converted into chlorine according to step b) by the processes described.
  • Figure 2 shows the process of the invention, as it can be included in the isocyanate synthesis.
  • the carbon monoxide content is significantly reduced in the HCl stream, whereby a deactivation of the Deacon catalyst is slowed down at the next stage by uncontrolled temperature increase.
  • the HCl gas feed gas is heated to the operating temperature required for HCl oxidation without much external energy input.

Landscapes

  • Chemical & Material Sciences (AREA)
  • Organic Chemistry (AREA)
  • Inorganic Chemistry (AREA)
  • Chemical Kinetics & Catalysis (AREA)
  • Catalysts (AREA)
  • Organic Low-Molecular-Weight Compounds And Preparation Thereof (AREA)

Abstract

La présente invention concerne un procédé de fabrication de chlore à partir d'un gaz contenant du chlorure d'hydrogène et du monoxyde de carbone, ledit procédé comprenant une étape d'oxydation catalysée du monoxyde de carbone, ainsi qu'éventuellement d'autres composants oxydables en dioxyde de carbone avec de l'oxygène dans un réacteur en aval dans des conditions adiabatiques.
EP07725288A 2006-05-23 2007-05-16 Procédé d'oxydation d'un gaz contenant du chlorure d'hydrogène Withdrawn EP2038212A1 (fr)

Applications Claiming Priority (2)

Application Number Priority Date Filing Date Title
DE102006024548A DE102006024548A1 (de) 2006-05-23 2006-05-23 Verfahren zur Oxidation eines Chlorwasserstoff-enthaltenden Gases
PCT/EP2007/004372 WO2007134775A1 (fr) 2006-05-23 2007-05-16 Procédé d'oxydation d'un gaz contenant du chlorure d'hydrogène

Publications (1)

Publication Number Publication Date
EP2038212A1 true EP2038212A1 (fr) 2009-03-25

Family

ID=38326284

Family Applications (1)

Application Number Title Priority Date Filing Date
EP07725288A Withdrawn EP2038212A1 (fr) 2006-05-23 2007-05-16 Procédé d'oxydation d'un gaz contenant du chlorure d'hydrogène

Country Status (9)

Country Link
US (1) US20100266481A1 (fr)
EP (1) EP2038212A1 (fr)
JP (1) JP2009537451A (fr)
KR (1) KR20090015982A (fr)
CN (1) CN101448736A (fr)
DE (1) DE102006024548A1 (fr)
RU (1) RU2008150589A (fr)
TW (1) TW200808654A (fr)
WO (1) WO2007134775A1 (fr)

Families Citing this family (12)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
DE102007020096A1 (de) * 2007-04-26 2008-10-30 Bayer Materialscience Ag Verfahren zur Oxidation von Kohlenmonoxid in einem HCI enthaltenden Gasstrom
WO2010076262A1 (fr) * 2008-12-30 2010-07-08 Basf Se Catalyseur pour l'oxydation de chlorure d'hydrogène contenant du ruthénium et du nickel
RU2448038C1 (ru) * 2010-11-10 2012-04-20 Учреждение Российской академии наук Институт химии и химической технологии Сибирского отделения РАН (ИХХТ СО РАН) Способ конверсии хлороводорода для получения хлора
CN103717289A (zh) 2011-04-11 2014-04-09 Ada-Es股份有限公司 用于气体组分捕集的流化床方法和系统
CN102602892B (zh) * 2012-04-11 2015-04-01 万华化学集团股份有限公司 通过氯化氢的催化氧化制备氯气的方法
IN2015DN02082A (fr) 2012-09-20 2015-08-14 Ada Es Inc
CN106145039B (zh) * 2015-04-01 2020-09-11 上海氯碱化工股份有限公司 氯化氢制氯工艺中原料预处理的方法
CN107684927B (zh) * 2016-08-03 2020-07-28 万华化学集团股份有限公司 一种用于氯化氢氧化制备氯气的催化剂及其制备方法和用途
CN109453764A (zh) * 2018-11-16 2019-03-12 西安元创化工科技股份有限公司 用于氯化氢氧化制氯气的二氧化钌催化剂及其制备方法
CN109336052A (zh) * 2018-11-23 2019-02-15 宜宾天原集团股份有限公司 用于生产氯化氢的微反应系统及基于该系统的氯化氢生产方法
CN111167468B (zh) * 2020-01-03 2022-09-16 万华化学集团股份有限公司 一种氯化氢氧化制氯的催化剂及其制备方法和应用
KR20220105387A (ko) * 2021-01-20 2022-07-27 한화솔루션 주식회사 염화수소 산화반응을 통한 염소의 고수율 제조방법

Family Cites Families (16)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
US3701822A (en) * 1970-06-11 1972-10-31 Chemical Construction Corp Process and catalyst for treating combustion exhaust gas
FR2424243A1 (fr) * 1978-04-26 1979-11-23 Rhone Poulenc Ind Procede d'oxyhydrochloration non polluant
ZA837689B (en) * 1982-10-18 1984-06-27 Universal Matthey Prod Oxidation catalysts
JPS62270404A (ja) * 1986-05-16 1987-11-24 Mitsui Toatsu Chem Inc 塩素の製造方法
US4774070A (en) * 1986-02-19 1988-09-27 Mitsui Toatsu Chemicals, Incorporated Production process of chlorine
CA1260229A (fr) * 1986-06-30 1989-09-26 Mitsui Chemicals, Inc. Production du chlore
DE4217019A1 (de) * 1992-05-22 1993-11-25 Bayer Ag Verfahren zur Herstellung von aromatischen Diisocyanaten
US5707919A (en) * 1994-11-14 1998-01-13 Mitsui Toatsu Chemicals, Inc. Catalyst for preparing chlorine from hydrogen chloride
US6852667B2 (en) * 1998-02-16 2005-02-08 Sumitomo Chemical Company Limited Process for producing chlorine
JP2002226205A (ja) * 2001-01-29 2002-08-14 Sumitomo Chem Co Ltd 一酸化炭素の酸化方法
JP4081597B2 (ja) * 2001-12-04 2008-04-30 住友化学株式会社 触媒酸化方法
DE10235476A1 (de) * 2002-08-02 2004-02-12 Basf Ag Integriertes Verfahren zur Herstellung von Isocyanaten
DE10242400A1 (de) * 2002-09-12 2004-03-18 Basf Ag Festbettverfahren zur Herstellung von Chlor durch katalytische Gasphasen-Oxidation von Chlorwasserstoff
DE10250131A1 (de) * 2002-10-28 2004-05-06 Basf Ag Verfahren zur Herstellung von Chlor aus Salzsäure
DE10307141A1 (de) * 2003-02-20 2004-09-02 Bayer Ag Verfahren zur Herstellung von (Poly)isocyanaten in der Gasphase
JP2005289800A (ja) * 2004-03-22 2005-10-20 Sumitomo Chemical Co Ltd 塩素の製造方法

Non-Patent Citations (1)

* Cited by examiner, † Cited by third party
Title
See references of WO2007134775A1 *

Also Published As

Publication number Publication date
JP2009537451A (ja) 2009-10-29
TW200808654A (en) 2008-02-16
US20100266481A1 (en) 2010-10-21
CN101448736A (zh) 2009-06-03
KR20090015982A (ko) 2009-02-12
RU2008150589A (ru) 2010-06-27
DE102006024548A1 (de) 2007-11-29
WO2007134775A1 (fr) 2007-11-29

Similar Documents

Publication Publication Date Title
EP2038212A1 (fr) Procédé d'oxydation d'un gaz contenant du chlorure d'hydrogène
EP1529033B1 (fr) Procede integre de production d'isocyanates
EP2027063B1 (fr) Procédé de production de chlore par oxydation en phase gazeuse
WO2008131870A1 (fr) Procédé d'oxydation de monoxyde de carbone dans un flux de gaz contenant du chlorure d'hydrogène
EP1542923B1 (fr) Procede a lit fixe pour produire du chlore par oxydation catalytique en phase gazeuse de chlorure d'hydrogene
WO2010076262A1 (fr) Catalyseur pour l'oxydation de chlorure d'hydrogène contenant du ruthénium et du nickel
WO2013060628A1 (fr) Catalyseur et procédé pour produire du chlore par oxydation catalytique en phase gazeuse
EP2139809A1 (fr) Processus d'adsorption pour éliminer des constituants inorganiques d'un flux gazeux contenant du chlorure d'hydrogène
DE102006024549A1 (de) Verfahren zur Herstellung von organischen Isocyanaten
EP1656322A1 (fr) Procede de production de chlore
EP2027066A1 (fr) Procédé pour séparer du monoxyde de carbone d'un gaz contenant du chlorure d'hydrogène
WO2008131869A1 (fr) Procédé de purification et d'oxydation d'un gaz contenant du chlorure d'hydrogène
DE102008051694A1 (de) Verfahren zur Abtrennung von Kohlenmonoxid aus einem HCI-Rohgas
EP1546032A1 (fr) Catalyseur pour l'oxydation catalytique de chlorure d'hydrogene
EP2401072B1 (fr) Catalyseur pour l'oxydation de chlorure d'hydrogène contenant du ruthénium et de l'argent et/ou du calcium
EP3421416A1 (fr) Oxydation photocatalytique de chlorure d'hydrogene à l'aide de monoxyde de carbone
EP2177268A1 (fr) Catalyseur et procédé de fabrication de chlore par oxydation en phase gazeuse
EP1506133B1 (fr) Procede de fabrication de chlore a partir de gaz chlorhydrique
DE102011005897A1 (de) Verfahren zur Bereitstellung von Chlor für chemische Umsetzungen
DE10234908B4 (de) Verfahren zur Herstellung von Chlor aus einem (Chlor)kohlenwasserstoffe enthaltenden Chlorwasserstoffstrom
WO2008131872A1 (fr) Procédé de production de chlore à partir de hcl
DE102008038096A1 (de) Katalytische Oxidation von Chlorwasserstoff mit Ozon

Legal Events

Date Code Title Description
PUAI Public reference made under article 153(3) epc to a published international application that has entered the european phase

Free format text: ORIGINAL CODE: 0009012

17P Request for examination filed

Effective date: 20081223

AK Designated contracting states

Kind code of ref document: A1

Designated state(s): AT BE BG CH CY CZ DE DK EE ES FI FR GB GR HU IE IS IT LI LT LU LV MC MT NL PL PT RO SE SI SK TR

AX Request for extension of the european patent

Extension state: AL BA HR MK RS

STAA Information on the status of an ep patent application or granted ep patent

Free format text: STATUS: THE APPLICATION IS DEEMED TO BE WITHDRAWN

18D Application deemed to be withdrawn

Effective date: 20100201