EP3440241A1 - Difunctional electrode and electrolysis device for chlor-alkali electrolysis - Google Patents
Difunctional electrode and electrolysis device for chlor-alkali electrolysisInfo
- Publication number
- EP3440241A1 EP3440241A1 EP17714804.6A EP17714804A EP3440241A1 EP 3440241 A1 EP3440241 A1 EP 3440241A1 EP 17714804 A EP17714804 A EP 17714804A EP 3440241 A1 EP3440241 A1 EP 3440241A1
- Authority
- EP
- European Patent Office
- Prior art keywords
- cathode
- electrode
- silver
- cell
- catalyst
- 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- Withdrawn
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Classifications
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- C—CHEMISTRY; METALLURGY
- C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
- C25B—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES FOR THE PRODUCTION OF COMPOUNDS OR NON-METALS; APPARATUS THEREFOR
- C25B11/00—Electrodes; Manufacture thereof not otherwise provided for
- C25B11/04—Electrodes; Manufacture thereof not otherwise provided for characterised by the material
- C25B11/051—Electrodes formed of electrocatalysts on a substrate or carrier
- C25B11/073—Electrodes formed of electrocatalysts on a substrate or carrier characterised by the electrocatalyst material
- C25B11/091—Electrodes formed of electrocatalysts on a substrate or carrier characterised by the electrocatalyst material consisting of at least one catalytic element and at least one catalytic compound; consisting of two or more catalytic elements or catalytic compounds
- C25B11/097—Electrodes formed of electrocatalysts on a substrate or carrier characterised by the electrocatalyst material consisting of at least one catalytic element and at least one catalytic compound; consisting of two or more catalytic elements or catalytic compounds comprising two or more noble metals or noble metal alloys
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- C—CHEMISTRY; METALLURGY
- C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
- C25B—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES FOR THE PRODUCTION OF COMPOUNDS OR NON-METALS; APPARATUS THEREFOR
- C25B1/00—Electrolytic production of inorganic compounds or non-metals
- C25B1/01—Products
- C25B1/34—Simultaneous production of alkali metal hydroxides and chlorine, oxyacids or salts of chlorine, e.g. by chlor-alkali electrolysis
- C25B1/46—Simultaneous production of alkali metal hydroxides and chlorine, oxyacids or salts of chlorine, e.g. by chlor-alkali electrolysis in diaphragm cells
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- C—CHEMISTRY; METALLURGY
- C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
- C25B—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES FOR THE PRODUCTION OF COMPOUNDS OR NON-METALS; APPARATUS THEREFOR
- C25B11/00—Electrodes; Manufacture thereof not otherwise provided for
- C25B11/04—Electrodes; Manufacture thereof not otherwise provided for characterised by the material
- C25B11/051—Electrodes formed of electrocatalysts on a substrate or carrier
- C25B11/073—Electrodes formed of electrocatalysts on a substrate or carrier characterised by the electrocatalyst material
- C25B11/091—Electrodes formed of electrocatalysts on a substrate or carrier characterised by the electrocatalyst material consisting of at least one catalytic element and at least one catalytic compound; consisting of two or more catalytic elements or catalytic compounds
- C25B11/095—Electrodes formed of electrocatalysts on a substrate or carrier characterised by the electrocatalyst material consisting of at least one catalytic element and at least one catalytic compound; consisting of two or more catalytic elements or catalytic compounds at least one of the compounds being organic
-
- C—CHEMISTRY; METALLURGY
- C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
- C25B—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES FOR THE PRODUCTION OF COMPOUNDS OR NON-METALS; APPARATUS THEREFOR
- C25B15/00—Operating or servicing cells
- C25B15/08—Supplying or removing reactants or electrolytes; Regeneration of electrolytes
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- C—CHEMISTRY; METALLURGY
- C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
- C25B—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES FOR THE PRODUCTION OF COMPOUNDS OR NON-METALS; APPARATUS THEREFOR
- C25B9/00—Cells or assemblies of cells; Constructional parts of cells; Assemblies of constructional parts, e.g. electrode-diaphragm assemblies; Process-related cell features
- C25B9/17—Cells comprising dimensionally-stable non-movable electrodes; Assemblies of constructional parts thereof
- C25B9/19—Cells comprising dimensionally-stable non-movable electrodes; Assemblies of constructional parts thereof with diaphragms
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- H—ELECTRICITY
- H01—ELECTRIC ELEMENTS
- H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
- H01M8/00—Fuel cells; Manufacture thereof
- H01M8/08—Fuel cells with aqueous electrolytes
- H01M8/083—Alkaline fuel cells
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- B—PERFORMING OPERATIONS; TRANSPORTING
- B01—PHYSICAL OR CHEMICAL PROCESSES OR APPARATUS IN GENERAL
- B01J—CHEMICAL OR PHYSICAL PROCESSES, e.g. CATALYSIS OR COLLOID CHEMISTRY; THEIR RELEVANT APPARATUS
- B01J23/00—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00
- B01J23/38—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00 of noble metals
- B01J23/40—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00 of noble metals of the platinum group metals
- B01J23/46—Ruthenium, rhodium, osmium or iridium
- B01J23/462—Ruthenium
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- B—PERFORMING OPERATIONS; TRANSPORTING
- B01—PHYSICAL OR CHEMICAL PROCESSES OR APPARATUS IN GENERAL
- B01J—CHEMICAL OR PHYSICAL PROCESSES, e.g. CATALYSIS OR COLLOID CHEMISTRY; THEIR RELEVANT APPARATUS
- B01J23/00—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00
- B01J23/38—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00 of noble metals
- B01J23/40—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00 of noble metals of the platinum group metals
- B01J23/46—Ruthenium, rhodium, osmium or iridium
- B01J23/468—Iridium
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- B—PERFORMING OPERATIONS; TRANSPORTING
- B01—PHYSICAL OR CHEMICAL PROCESSES OR APPARATUS IN GENERAL
- B01J—CHEMICAL OR PHYSICAL PROCESSES, e.g. CATALYSIS OR COLLOID CHEMISTRY; THEIR RELEVANT APPARATUS
- B01J23/00—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00
- B01J23/38—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00 of noble metals
- B01J23/48—Silver or gold
- B01J23/50—Silver
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- C—CHEMISTRY; METALLURGY
- C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
- C25B—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES FOR THE PRODUCTION OF COMPOUNDS OR NON-METALS; APPARATUS THEREFOR
- C25B11/00—Electrodes; Manufacture thereof not otherwise provided for
- C25B11/02—Electrodes; Manufacture thereof not otherwise provided for characterised by shape or form
Definitions
- the invention relates to an electrode for chlorine-alkali electrolysis, which, if necessary, either develop hydrogen or can consume oxygen.
- the appropriately equipped chlor-alkali electrolysis plant can be used for example for grid stabilization of power grids.
- the invention is based on known per se oxygen-consuming electrodes for the chloralkali electrolysis.
- CAEL chlor-alkali electrolysis
- the CAEL uses a noble metal oxide coated hydrogen evolving cathode in modern membrane electrolysis.
- the energy consumption in the prior art is typically about 2300 kWh / t chlorine (Cl 2 ).
- SVK oxygen-consuming cathodes
- the electrolysis is carried out in the hydrogen-producing mode, with no energy surplus in the oxygen reduction mode.
- the hydrogen from the CAEL is utilized, one part is used for chemical syntheses, another part is thermally utilized, i. Burned in the power plant to produce electricity.
- the chemical industry has an immense demand for hydrogen, which is mainly sourced from reforming processes.
- the share of hydrogen from the CAEL is only 2% of the hydrogen produced or required by the chemical industry (http://www.hvdrogeit.de/wasserstoff.htm).
- the comparatively smaller amount of hydrogen that is involved in the network stabilization by a bifunctional electrolysis process either optionally either easily stored or replaced by the existing hydrogen production processes.
- the subject matter of the invention is a bifunctional electrode for operation as a cathode in a chlor-alkali electrolysis in which hydrogen is selectively generated at the cathode or if oxygen is supplied to the cathode, which consumes it at the cathode is, comprising at least one planar, electrically conductive support and an applied on the support gas diffusion layer and electrocatalyst based on silver and / or silver oxide (silver catalyst), characterized in that as additional electrocatalyst, a ruthenium catalyst based on ruthenium and / or ruthenium and / or an iridium catalyst based on iridium and / or iridium oxide, preferably ruthenium catalyst is provided, wherein the carrier has a catalytic coating with additional electrocatalyst and / or the additional electrocatalyst present in admixture with the silver catalyst t.
- a bifunctional electrode for the CAEL of the aforementioned type is not yet known.
- water is electrochemically reduced to hydrogen and hydroxide ions at the cathode.
- an electrode is used, which consists for example of nickel and is equipped with a coating based on platinum or other precious metals or noble metal oxides. These electrodes are characterized by a particularly low overvoltage for hydrogen evolution.
- This optimized coating has at least three different layers.
- the bottom layer contains platinum and is in direct contact with the nickel carrier.
- the middle layer contains a mixture of noble metal oxides (at least 60% rhodium by weight).
- the outer layer directly in contact with the electrolyte is based on ruthenium oxide.
- Electrodes whose coating is constructed in this way show a much higher stability to the reverse polarization than electrodes whose coating consists of only a single catalytically active layer.
- Such known electrodes are not suitable as a gas diffusion electrode and are thus not usable as a bifunctional electrode.
- Such electrodes set basic standards for the effectiveness of hydrogen-producing electrodes.
- Electrodes that consume oxygen, i. Reacting oxygen with water to hydroxide ions are also known in principle.
- DE102005023615A describes an electrode for the reduction of oxygen to hydroxide ions, which is based on a compressed powder mixture of silver oxide, PTFE and silver.
- electrodes of this type are well suited as a gas diffusion electrode for oxygen reduction. On the other hand, these electrodes do not show good performance in hydrogen evolution and thus can not be operated economically in the hydrogen evolution mode. With the bifunctional electrode according to the invention, it is now possible to solve the aforementioned objects of the invention.
- the bifunctional electrode according to the invention consists inter alia of a carrier element, for example a nickel fabric. On this carrier is the oxygen-reducing catalyst applied containing gas diffusion layer. This can be done by dry or wet production processes known in principle (see eg DE102005023615A1).
- the gas diffusion layer consists at least of a mixture of fluoropolymer and silver catalyst and ruthenium catalyst.
- the catalytic coating of the support with ruthenium and / or optionally iridium catalyst in an amount of 0.05 to 2.5 wt .-%, preferably 0.1 to 1.5 wt .-%, based on the total content Silver catalyst, ruthenium catalyst and / or optionally iridium catalyst and fluoropolymer before.
- the new electrode is formed by applying and compacting a mixture of fluoropolymer and silver catalyst and optionally ruthenium catalyst in powder form on the electrically conductive support.
- a particularly preferred embodiment of the new bifunctional electrode is characterized in that the content of fluoropolymer in the electrode, in particular PTFE as a fluoropolymer, 1 to 15 wt .-%, preferably 2 to 13 wt .-%, particularly preferably 3 to 12 wt. % Fluoropolymer and 99-85% by weight, preferably 98-87% by weight, particularly preferably 97-88% by weight silver catalyst based on the sum of the contents of fluoropolymer and silver catalyst.
- PTFE as a fluoropolymer
- the weight ratio of ruthenium catalyst and optionally iridium catalyst to the silver catalyst in a preferred embodiment of the new electrode is from 0.05 to 100 to 3 to 100, in particular from 0.06 to 100 to 0.9 to 100.
- a bifunctional electrode has proven particularly advantageous which has a thickness of 0.2 to 3 mm, preferably 0.2 to 2 mm, particularly preferably 0.2 to 1 mm.
- a new bifunctional electrode has also proved to be advantageous, in which the surface charge with ruthenium catalyst, calculated as ruthenium metal, is 1 to 55 g / m 2 .
- silver-based catalysts such as silver oxide, in particular silver I-oxide, silver metal powder or mixtures thereof are used.
- a ruthenium and / or iridium compound may be added, e.g. as chloride or dispersed oxide.
- mixed catalysts of, for example, silver oxide with ruthenium oxide or silver with ruthenium oxide can be produced.
- the electrically conductive carrier of the new bifunctional electrode is designed in particular as a net, fleece, foam, woven fabric, mesh or expanded metal, and is particularly preferably designed as a woven fabric.
- Particularly preferred material for the electrically conductive carrier in the new bifunctional electrode are carbon fibers, nickel or silver, nickel is preferably used as the material.
- the bifunctional electrode has a silver catalyst consisting of silver, silver oxide or a mixture of silver and silver oxide, wherein the silver oxide is preferably silver (I) oxide. Most preferably, the silver catalyst is silver.
- the gas diffusion layer can be applied on one or both sides of the outer surfaces of the carrier, preferably, the gas diffusion layer is applied on one side on the carrier.
- electrolytic cells as described in EP 717130 Bl, DE 10108452 C2, DE 3420483 Al, DE 10333853 Al, EP 1882758 Bl, WO 2007080193 A2 or WO 2003042430, can be used after modification.
- these cells may be used but must be modified to additionally install, for example, a suitable cathodic head space purge device for removal of hydrogen prior to continued operation in the oxygen-consuming mode and a device for removing the generated hydrogen.
- the cell structure described in WO 2003042430 A2 can be used to operate the bifunctional electrode according to the invention, but other cell structures, after appropriate modification, for the operation of the bifunctional Electrode be used.
- the invention accordingly also provides a novel electrolysis apparatus for the bifunctional operation of a chlor-alkali electrolysis with a cathode at which hydrogen is selectively generated or oxygen is consumed in a gas diffusion layer of the cathode, at least comprising an electrolytic cell for chlor-alkali electrolysis with an anode half cell, a cathode half cell and a cation exchange membrane separating the anode half cell and the cathode half cell, an anode for developing chlorine disposed in the anode half cell, a cathode disposed in the cathode half cell, and a supply line for selectively supplying an oxygen containing gas into a gas space of the cathode half cell, and Zu - And derivatives for the Edukt- and product streams, characterized in that the above-described bifunctional electrode according to the invention is provided as the cathode.
- the latter has at least one supply line for purging the gas space of the cathode half-cell with inert gas.
- This can be used to prevent hazardous operation of mixing hydrogen from the hydrogen-producing mode with oxygen from the oxygen-consuming mode.
- the electrode according to the invention allows operation of the electrolyzer in both of the above operating modes with high efficiency. That is, the electrolyzer can be operated in the oxygen reduction (ORR) mode and in the hydrogen evolution reaction (HER) mode.
- ORR oxygen reduction
- HER hydrogen evolution reaction
- ORR mode oxygen reduction mode
- ORR mode oxygen and water are converted to hydroxide ions at the cathode.
- the HER mode water reacts at the cathode to form hydroxide ions and hydrogen.
- the invention also provides a bifunctional method for chlor-alkali electrolysis, optionally with a low supply of electric current from the connected to the electrolysis cell power grid of the cathode oxygen-containing gas is supplied to the gas space of the cathode half-cell and at a first cell voltage at the cathode oxygen is reduced or is supplied at a high supply of electricity from the connected to the electrolysis cell power grid of the cathode, no oxygen-containing gas and at a second cell voltage, which is higher than the first cell voltage, is generated at the cathode hydrogen, characterized in that as electrolysis apparatus, an above-described electrolysis apparatus according to the invention with the new bifunctional electrode is used as the cathode.
- the bifunctional electrode according to the invention may preferably be operated such that, with a slightly elevated pressure on the liquid side of the electrode, the hydrogen produced is not released into the gap between the electrode and the membrane, but is emitted above the side of the bifunctional electrode facing the gas side , This prevents hydrogen gas bubbles from accumulating in the gap and disrupting the electrolysis process.
- the direction in which the hydrogen is released can be achieved both by the electrode properties per se and by the operation with higher pressure on the side of the liquor in relation to the gas pressure on the gas side.
- alkali is understood here and hereinafter to mean alkali metal hydroxide, preferably sodium hydroxide solution or potassium hydroxide solution, particularly preferably sodium hydroxide solution.
- the operation of the bifunctional electrode in a preferred embodiment of the new electrolysis process at a differential pressure between the pressure on the side of the liquor to the gas pressure on the other side of the electrode of greater than 0.1 mbar but less than 100 mbar.
- the absolute pressure on the side of the liquor is fundamentally dependent on 1. the height of the electrode, 2. the density of the liquor and 3. the gas pressure above the liquor. If the pressure is given on the side of the liquor, this refers to the pressure of the liquor at the lowest point of the electrode in the cell, to a liquor with a concentration of 32% by weight or the respectively specified concentration and last on the atmospheric gas pressure above the liquor liquid level. Since the pressure on the side of the gas is independent of the height, this is assumed to be constant over the height seen.
- Another object of the invention is the use of the new electrolysis apparatus for chlor-alkali electrolysis associated with a flexible use of electricity for optional storage of electrical energy as hydrogen.
- hydrogen can be produced regeneratively only by water electrolysis by means of regenerative electricity. This produces at the anode, the co-product oxygen, which often finds no economic use and must be delivered to the atmosphere.
- separate plant for water electrolysis must be built, which means a high investment cost.
- these systems can only be operated with a comparatively low overall utilization, ie only when sufficient regenerative energy is available. As a result, the wear in these systems is very high, which affects the economic use, that is so that the hydrogen produced is extremely expensive.
- the advantage of the new bifunctional electrolysis is that the hydrogen production can be carried out in existing plants, which only need to be changed slightly and which are operated all year under full load, since the products chlorine and caustic soda are also required year-round.
- Hydrogen management can be carried out in many existing infrastructure. If, for example, the state of North Rhine-Westphalia is considered in Germany, there already exists a hydrogen-gas composite system that can be used as a storage facility for hydrogen, meaning that no further investments in hydrogen storage infrastructures need to be made here. Description of cell structure and method of measurement:
- the characterization of the electrodes from the following examples was carried out in a commercially available half-cell (FlexCell, Fa. GASKATEL) with a 3-electrode arrangement.
- the counter electrode was platinum.
- the reference electrode used was a reversible hydrogen electrode (RHE, HydroFlex, GASKATEL).
- the third electrode was the respective electrode to be characterized, the test electrode.
- ORR mode oxygen reduction mode
- the gas space on the back of the test electrode was purged with an excess of oxygen, with a gas pressure of 0.5-5 mbar was set. This was achieved by passing the gas from the headspace through a dip with water.
- the gas space behind the test electrode was purged with nitrogen.
- the gas pressure of nitrogen was also 0.5 - 5mbar.
- the gas phase of the electrolyte compartment was purged with nitrogen during the HER mode to prevent a detonating gas reaction.
- the projected active area was 3.14 cm 2 and the concentration of caustic soda was 32% by weight.
- the temperature of the caustic soda was 80 ° C and the current density measured 4 kA / m 2 . Due to the interference of the hydrogen gas bubbles on the potential measurement, the electrode was investigated in the HER mode at a caustic soda temperature of about 63 ° C and a current density of 1.5 kA / m 2 .
- the characterization was carried out in the potentiostatic operation at the above-mentioned current density by an electrochemical impedance spectroscopy with a potentiostat type IM6 from Zahner after the CPE model (constant phase phase).
- the measured potential is corrected with the respective current flowing and with the measured so-called R3 resistance, which contains the resistances such as those of the electrolyte, that of the test electrode and that of the connecting cable. This corrected potential served as a benchmark.
- a nickel fabric was used which had a wire thickness of 0.14 mm and a mesh size of 0.5 mm. The coating took place in 5 to 10 coating cycles. It was an approx. 15 wt .-% solution of RuCL used, which was dissolved in n-butanol (76.7 wt .-%) and hydrochloric acid (8.1 wt .-%). The ruthenium content in pure RuCl3 coating solution was 6.1% by weight. After each application, drying was done at 353K and sintering at 743K for 10 minutes each. After the last coat, the fabric was finally sintered at 793K for 60 minutes.
- the applied amounts were determined by weight gain of the nickel fabric by weighing before and after the coating process.
- the order quantity was related to the geometric fabric area.
- the electrode according to the invention has properties which make it possible in ORR mode not to allow harmful amounts of gas to penetrate into the electrolyte and, in the HER mode, to allow the drainage of the hydrogen into the gas space of the cell. This can be done by simple and low pressure differential adjustment.
- the first chamber one consisted of the anode chamber, which was charged with a sodium chloride solution, wherein the feed amount was chosen so that the running concentration of NaCl about 210 g / L and the temperature was about 85 ° C.
- the anode used consisted of an expanded metal, which was equipped with a commercially available ruthenium oxide-based anode coating for chlorine development of the company DENORA.
- the membrane used was a Nafion N982.
- the second chamber was defined by the distance from the membrane to the bifunctional electrode of 3 mm, wherein this second chamber was so bubbled with sodium hydroxide solution that the temperature of the exiting the chamber sodium hydroxide 85 ° C and the concentration was 31.5 wt .-% ,
- the third chamber is used for gas supply and removal.
- O2 was introduced into the chamber.
- the HER mode on the side of the bifunctional electrode facing the gas space, at sufficiently selected pressure level and differential pressure, the hydrogen escaped and did not enter the second chamber.
- the electrode according to the invention was operated at different pressure differences.
- the difference in pressure is the difference that results from the pressure on the side of the electrode facing the liquid and the pressure on the side of the electrode facing the gas side.
- the amount of hydrogen which could be taken from the second chamber was in each case given as follows:
- a Ru02 coated nickel fabric is prepared and used, which will be used as a reference for the HER mode: a 7 cm x 3 cm nickel fabric (wire thickness: 0.15 mesh size: 0.5 mm) was coated with RuC
- the amount of RuC applied was 8.2 g / m 2 (where the area in m 2 is the geometrically projected area, which is the area when the product of electrode length and width, the area corresponding to that facing the anode.)
- This cathode was examined in a half-cell according to the principle described above, see the section "Description of cell structure and method of measurement”.
- the corrected for the R3 resistance potential for the HER mode was -169 mV vs.. RHE (measured at 1.5 kA / m 2 , sodium hydroxide temperature: 63 ° C., NaOH conc .: 32% by weight).
- This type of electrode can not be operated in ORR mode.
- Example 4 Comparative Example: Prior Art SVK (from Example 3) Operated in HER Mode (Hydrogen Development Mode) Since a bifunctional electrode has not been described yet and a hydrogen evolving electrode can not be operated in the oxygen reduction mode, the method described in US Pat the case game operated from the prior art according to DE 10 2005 023 615 AI known SVK operated in the hydrogen evolution mode.
- the electrode was characterized as operated in HER mode in Example 2.
- the corrected for the R3 resistance potential for the HER mode was -413 mV.
- RHE 1.5 kA / m 2 , sodium hydroxide solution temperature: 63 ° C, NaOH: 32 wt .-%).
- Hydrogen evolution occurs at a potential that is 244 mV lower than the hydrogen evolution electrode known from the prior art (Example 2).
- Example 5 Inventive bifunctional cathode - Ru02 use of a Ni coat fabric as a support and current distributor in the gas diffusion layer for the inventive bifunctional cathode of the carrier of the electrode of Example 3 was replaced with a Ru0 2 -coated Ni tissue.
- the fabric was made as in Example 2.
- This carrier was used as carrier for the gas diffusion layer analogously to the example described in DE 10 2005 023 615 A1.
- This electrode was incorporated into the half cell and characterized as described above.
- the corrected for the R3 resistance potential for the ORR mode is +785 mV.
- RHE (4.0 kA / m 2 , sodium hydroxide solution temperature: 80 ° C., NaOH: 32% by weight).
- the corrected for the R3 resistance potential for the HER mode was -277 mV vs.. RHE (1.5 kA / m 2 , sodium hydroxide solution temperature: 63 ° C, NaOH: 32 wt .-%).
- the electrode is only 108 mV worse than the hydrogen for the development (HER mode) optimized electrode of the prior art according to Example 2 and at the same time better in the operation of the ORR mode.
- Example 6 Bifunctional Electrode (Inventive): Silver oxide (Ag20) based gas diffusion layer with 1 wt. R11O2 powder additive
- an electrode was produced analogously to the example of DE 10 2005 023 615 Al.
- the composition of the catalyst mixture was as follows: 5% by weight of PTFE, 7% by weight of Ag, 87% by weight of Ag 2 O and 1% by weight of RuO 2 (ACROS: 99.5% anhydride).
- the bifunctional electrode potential for the HER was 60mV better at -109mV vs. RHE than that of the standard electrode (Ru0 2 ) for hydrogen evolution.
- the potential of the bifunctional electrode was 794mV vs ORR mode. RHE by 54 mV better than the SVK known from the prior art (see Example 3) in ORR mode.
- Example 7 Bifunctional electrode with 3% by weight of RuO 2 powder additive (according to the invention)
- an electrode according to DE 10 2005 023 615 Al was manufactured.
- the composition of the catalyst mixture was as follows: 5% by weight PTFE, 7% by weight Ag, 85% by weight
- the potential of the bifunctional electrode for the HER was slightly lower than that of the electrode with 1 wt% Ru0 2 powder at -146 mV vs RHE around 37mV.
- the potential of the bifuntkionellen electrode was in ORR operation was 702mV vs. RHE slightly lower by 92 mV than that of the electrode with 1 wt% Ru0 2 .
- This electrode is also comparatively better in HER mode than the known hydrogen-developing electrode (Example 2).
Abstract
Description
Claims
Applications Claiming Priority (2)
Application Number | Priority Date | Filing Date | Title |
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EP16164255 | 2016-04-07 | ||
PCT/EP2017/057956 WO2017174563A1 (en) | 2016-04-07 | 2017-04-04 | Difunctional electrode and electrolysis device for chlor-alkali electrolysis |
Publications (1)
Publication Number | Publication Date |
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EP3440241A1 true EP3440241A1 (en) | 2019-02-13 |
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EP17714804.6A Withdrawn EP3440241A1 (en) | 2016-04-07 | 2017-04-04 | Difunctional electrode and electrolysis device for chlor-alkali electrolysis |
Country Status (6)
Country | Link |
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US (1) | US20190112719A1 (en) |
EP (1) | EP3440241A1 (en) |
JP (1) | JP2019510885A (en) |
KR (1) | KR20180128962A (en) |
CN (1) | CN109219676A (en) |
WO (1) | WO2017174563A1 (en) |
Family Cites Families (20)
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GB8501479D0 (en) * | 1985-01-21 | 1985-02-20 | Johnson Matthey Plc | Making polymer-modified electrode |
GB8617325D0 (en) * | 1986-07-16 | 1986-08-20 | Johnson Matthey Plc | Poison-resistant cathodes |
ZA879466B (en) * | 1986-12-19 | 1989-08-30 | Dow Chemical Co | A composite membrane/electrode structure having interconnected roadways of catalytically active particles |
DE4444114C2 (en) | 1994-12-12 | 1997-01-23 | Bayer Ag | Electrochemical half cell with pressure compensation |
DE10108452C2 (en) | 2001-02-22 | 2003-02-20 | Karl Lohrberg | electrolyzer |
ITMI20012379A1 (en) | 2001-11-12 | 2003-05-12 | Uhdenora Technologies Srl | ELECTROLYSIS CELL WITH GAS DIFFUSION ELECTRODES |
DE10333853A1 (en) | 2003-07-24 | 2005-02-24 | Bayer Materialscience Ag | Electrochemical cell |
JP4341838B2 (en) * | 2004-10-01 | 2009-10-14 | ペルメレック電極株式会社 | Electrode cathode |
JP4834329B2 (en) | 2005-05-17 | 2011-12-14 | クロリンエンジニアズ株式会社 | Ion exchange membrane electrolytic cell |
DE102005023615A1 (en) | 2005-05-21 | 2006-11-23 | Bayer Materialscience Ag | Process for the preparation of gas diffusion electrodes |
ITMI20060054A1 (en) | 2006-01-16 | 2007-07-17 | Uhdenora Spa | ELASTIC CURRENT DISTRIBUTOR FOR PERCOLATOR CELLS |
ITMI20061947A1 (en) * | 2006-10-11 | 2008-04-12 | Industrie De Nora Spa | CATHODE FOR ELECTROLYTIC PROCESSES |
ITMI20091719A1 (en) * | 2009-10-08 | 2011-04-09 | Industrie De Nora Spa | CATHODE FOR ELECTROLYTIC PROCESSES |
DE102010039846A1 (en) * | 2010-08-26 | 2012-03-01 | Bayer Materialscience Aktiengesellschaft | Oxygenating electrode and process for its preparation |
DE102010062421A1 (en) * | 2010-12-03 | 2012-06-06 | Bayer Materialscience Aktiengesellschaft | Oxygenating electrode and process for its preparation |
US20130078537A1 (en) * | 2011-09-23 | 2013-03-28 | Bayer Intellectual Property Gmbh | Oxygen-consuming electrode and process for production thereof |
ITMI20122030A1 (en) | 2012-11-29 | 2014-05-30 | Industrie De Nora Spa | CATODO FOR ELECTROLYTIC EVOLUTION OF HYDROGEN |
WO2015082319A1 (en) * | 2013-12-04 | 2015-06-11 | Evonik Industries Ag | Device and method for the flexible use of electricity |
DE102013226414A1 (en) * | 2013-12-18 | 2015-06-18 | Evonik Industries Ag | Apparatus and method for the flexible use of electricity |
-
2017
- 2017-04-04 JP JP2018552156A patent/JP2019510885A/en active Pending
- 2017-04-04 US US16/090,945 patent/US20190112719A1/en not_active Abandoned
- 2017-04-04 KR KR1020187031901A patent/KR20180128962A/en not_active Application Discontinuation
- 2017-04-04 WO PCT/EP2017/057956 patent/WO2017174563A1/en active Application Filing
- 2017-04-04 CN CN201780035687.4A patent/CN109219676A/en active Pending
- 2017-04-04 EP EP17714804.6A patent/EP3440241A1/en not_active Withdrawn
Also Published As
Publication number | Publication date |
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US20190112719A1 (en) | 2019-04-18 |
JP2019510885A (en) | 2019-04-18 |
WO2017174563A1 (en) | 2017-10-12 |
KR20180128962A (en) | 2018-12-04 |
CN109219676A (en) | 2019-01-15 |
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