WO2015074637A1 - Cellule d'électrolyse électrochimique et son procédé de fonctionnement - Google Patents

Cellule d'électrolyse électrochimique et son procédé de fonctionnement Download PDF

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Publication number
WO2015074637A1
WO2015074637A1 PCT/DE2014/000559 DE2014000559W WO2015074637A1 WO 2015074637 A1 WO2015074637 A1 WO 2015074637A1 DE 2014000559 W DE2014000559 W DE 2014000559W WO 2015074637 A1 WO2015074637 A1 WO 2015074637A1
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Prior art keywords
cathode
electrode
anode
additional
voltage
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PCT/DE2014/000559
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German (de)
English (en)
Inventor
Maximilian SCHALENBACH
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Forschungszentrum Jülich GmbH
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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
    • 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
    • C25B1/02—Hydrogen or oxygen
    • C25B1/04—Hydrogen or oxygen by electrolysis of water
    • 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
    • C25B15/02—Process control or regulation
    • Y—GENERAL TAGGING OF NEW TECHNOLOGICAL DEVELOPMENTS; GENERAL TAGGING OF CROSS-SECTIONAL TECHNOLOGIES SPANNING OVER SEVERAL SECTIONS OF THE IPC; TECHNICAL SUBJECTS COVERED BY FORMER USPC CROSS-REFERENCE ART COLLECTIONS [XRACs] AND DIGESTS
    • Y02—TECHNOLOGIES OR APPLICATIONS FOR MITIGATION OR ADAPTATION AGAINST CLIMATE CHANGE
    • Y02E—REDUCTION OF GREENHOUSE GAS [GHG] EMISSIONS, RELATED TO ENERGY GENERATION, TRANSMISSION OR DISTRIBUTION
    • Y02E60/00—Enabling technologies; Technologies with a potential or indirect contribution to GHG emissions mitigation
    • Y02E60/30—Hydrogen technology
    • Y02E60/36—Hydrogen production from non-carbon containing sources, e.g. by water electrolysis

Definitions

  • Electrochemical electrolysis cell and method for operating the same
  • the invention relates to an electrochemical cell, in particular an electrolysis cell.
  • the invention further relates to a method for operating the aforementioned electrolytic cell.
  • An electrolyzer is understood to be an electrochemical cell in which the application of an electrical current through a conductive electrolyte to separate electrodes forces a non-voluntary redox reaction. At the cathode, the reduction reaction takes place, at the anode, the oxidation reaction. The products of electrolysis arise at the phase boundary of the electrodes to the electrolyte.
  • an acidic or alkaline medium is used.
  • protons are involved in the reaction, in the basic medium, they are hydroxide ions.
  • the products can be separated from each other, but the ionic conductivity of the electrolyte must be preserved.
  • a liquid electrolyte usually a caustic
  • a solid alkaline or acidic electrolyte such as a polymer electrolyte membrane
  • the alkaline polymer electrolyte membranes are still in the experimental stage and have not been able to show any long-term stability.
  • the voltage which must at least be applied for electrolysis is called the decomposition voltage (U z or E z ).
  • U z or E z The voltage which must at least be applied for electrolysis.
  • E z The voltage which must at least be applied for electrolysis.
  • U z or E z The voltage which must at least be applied for electrolysis.
  • E z The voltage which must at least be applied for electrolysis.
  • the cations which have a more positive (weaker negative) potential in the redox series (voltage series) are first of all reduced.
  • the cations which have a more positive (weaker negative) potential in the redox series (voltage series) are first of all reduced.
  • the oxidizable anions first those are oxidized which are as close as possible to the voltage zero point in the redox series, ie have a weaker positive redox potential.
  • the decomposition voltage (deposition potential) can thus be determined on the basis of the respective redox potential.
  • the electrode potentials can be calculated using the Nernst equation.
  • the voltage to be applied is greater than the thermodynamically necessary potential difference of the electrodes. These additional voltages are called overvoltage or overpotential.
  • a disadvantage of an electrolysis with gaseous products may be that the gases initially formed at the electrodes migrate through the electrolyte to the counter electrode (permeate).
  • the permeation of the resulting gases in the electrolysis of water for example, lead to the formation of explosive gases, which represents a safety risk.
  • the lower explosion limit is 4 mol% H 2 in 0 2 .
  • Countermeasures are catalyst-coated current collectors which are intended to catalytically react with the permeated hydrogen together with oxygen to form water on the anode side.
  • the efficiency of the electrolysis is reduced by the unwanted permeation of already formed hydrogen as product gas to the counterelectrode.
  • KOH alkaline electrolytes
  • PEM polymer electrolyte membranes
  • PEM proto exchange membrane
  • the energy efficiency of the electrolysis depends on the load absorption, temperature and operating pressures. Plant manufacturers such as Electrolyser Corp., Brown Boveri, Lurgi, De Nora or Epoch Energy Technology Corp. already offer large electroly- ses with an efficiency of more than 70% according to the manufacturer.
  • the overvoltage can be reduced by about 80 mV.
  • a disadvantage of alkaline electrolysis is the use of potassium hydroxide, which is an extremely corrosive hazardous substance, and the complex subsequent purification of the hydrogen produced.
  • a diaphragm is used which, however, is slightly gas-permeable. The permeation of the two product gases to the counter electrode reduces the efficiency. The diaphragm has an adverse effect on the proton conductivity and thus the efficiency.
  • a polymer electrolyte membrane In the case of acid electrolysis, a polymer electrolyte membrane (PEM) is generally used.
  • PEM polymer electrolyte membrane
  • this gas is permeable to gas and a reduction in the gas permeability is in the current state of the art always only with a disadvantageous reduction of the proton conductivity of the membrane. Again, this would lead to a reduction in the overall efficiency.
  • platinum By using platinum as the catalyst at the cathode, highly pure (> 99.999%) hydrogen can be generated since oxygen at the cathode is catalytically burned or electrochemically reduced.
  • electrolysis with a polymer electrolyte membrane is currently more promising due to its higher efficiency, better gas purity, more variable current density and dynamic current range.
  • the hydrogen formed can already be advantageously compressed during the electrolysis, since the membrane is only slightly gas-permeable and has a particularly high mechanical stability.
  • the polymer electrolyte membrane used was Nafion®, the cathode comprised platinum-supported carbon and the anode iridium oxide as catalysts. Both electrodes have an adjustable water circuit.
  • the hydrogen content in the oxygen on the anode side was determined in-situ. It could be shown that the hydrogen present on the anode side is not electrochemically converted by the iridium oxide catalyst and thus lost.
  • the object of the invention is to reduce more effectively in the electrolysis the permeation of liquid or gaseous products through the electrolyte to the counter electrode, as it is known from the prior art, and thus the overall efficiency of the system by a lower loss of products increase and reduce product contamination.
  • Another object of the invention is to provide an electrolytic cell, with the aid of which the aforementioned procedural advantage can be realized.
  • the invention provides a known electrolysis device with an anode and a cathode, which are connected to a DC voltage source, as well as an electrolyte in which now according to the invention within the electrolyte between the anode and cathode at least one further electrode is arranged.
  • the additional electrode or electrodes are connected to either the anode or the cathode by means of another DC voltage source.
  • This additional electrode which is connected via a DC voltage source to one of the electrodes, does not have the function of a reference electrode. With a reference electrode.
  • the potential difference between an electrode and the reference electrode is determined by connecting it via an ion conductor and via an electrical conductor to a suitable measuring device, for example a high-impedance voltmeter or a potentiometer circuit. In this case, no voltage is applied, but a voltage is measured.
  • a suitable measuring device for example a high-impedance voltmeter or a potentiometer circuit. In this case, no voltage is applied, but a voltage is measured.
  • the reverse reaction to the cathode can take place at this, if the additional electrode is connected together with the cathode to an additional DC voltage source. However, if the additional electrode is connected to an additional DC voltage source together with the anode, the reverse reaction to the anode takes place there.
  • a further electrode is usually connected together with the cathode, the other additional electrode together with the anode in each case to a further DC voltage source.
  • the additional electrodes also include the ionic conductivity of the electrolyte as well as an electron-conducting material provided with a catalyst on which the desired electro-chemical reaction takes place.
  • a catalyst on which the desired electro-chemical reaction takes place.
  • a platinum-supported carbon is suitable when acidic water electrolysis is performed, and a nickel-based catalyst when alkaline water electrolysis is performed.
  • the additional fourth electrode could be constructed analogously to the additional third electrode.
  • the additional third and the additional fourth electrode can also be realized by a single electrode, at which then both reversal reactions take place.
  • resistors could be used between the additional electrode as well as the anode and the cathode. In this case, the resistances should be much greater than the resistance of the electrolyte in order to avoid parasitic currents through a direct connection of anode and cathode.
  • this configuration will not be further elaborated below because it is considered to be less efficient than the other constellations of the invention.
  • the device according to the invention provides that at least one additional electrode (third electrode) are connected together with the cathode or the anode via a DC voltage source.
  • the additional third electrode is connected together with the cathode via a DC voltage source. This means that this extra voltage has its positive pole at the third electrode and the negative pole at the cathode. If the third electrode is connected to the anode, the negative pole of the DC voltage source is to be applied to it and the corresponding positive pole to the anode.
  • a DC voltage can also be applied between this fourth electrode and the anode.
  • the negative pole of the further voltage source must be regularly connected to the fourth electrode for this purpose.
  • the electrolysis cell according to the invention is suitable for electrolysis reactions in which during the electrolysis at least one reaction product in the liquid or gaseous state is formed, which can permeate through the electrolyte.
  • this technique can be used for alkaline and acidic electrolytic electrolysis with liquid electrolyte, polymer electrolyte membrane electrolysis (PEM-WE) and chlor-alkali electrolysis.
  • each hydrogen is developed at the cathode.
  • the permeation of the hydrogen formed by the electrolyte takes place due to the thermal diffusion and pressure differences. With increasing temperatures and in particular higher pressures, the permeation through the electrolyte increases. Due to the permeation of the hydrogen through the electrolyte to the counter electrode can form an explosive mixture with the generated oxidizing agent at the anode. Furthermore, so far there is a reduction in the efficiency by the hydrogen permeation through the membrane.
  • an electrolytic cell comprises on the one hand the application of a DC voltage between anode and cathode and additionally the application of at least one further DC voltage between a further additional electrode with the cathode or the anode.
  • the DC voltage is applied to the cathode and the additional electrode.
  • the permeation of the hydrogen formed at the cathode through the electrolyte to the counterelectrode can advantageously be prevented or reduced in the case of water electropolysis.
  • the diffusion of the product formed during the electrolysis at the cathode gas or liquid
  • the electrolyte to the counter electrode anode
  • an additional electrode e.g. B. the third electrode, connected together with the cathode to a DC voltage source, while the additional additional electrode, for. B. the fourth electrode, are connected together with the anode to a DC voltage source.
  • the additional additional electrode for. B. the fourth electrode
  • the fourth electrode therefor are used, in addition, the diffusion of the product formed at the anode, z.
  • oxygen through the electrolyte to the counter electrode (cathode) to reduce.
  • thermodynamically necessary reversible voltage for the electrolysis reaction is applied for the electrochemical reaction between the cathode and the anode.
  • a water electrolysis for example, 1, 23 V.
  • the device according to the invention is used with a cationic or anionic conducting electrolyte.
  • the electrolysis of water can be carried out both with an acidic electrolyte and in a basic medium.
  • an acid or a lye can be used as the liquid electrolyte as the acidic and basic electrolyte.
  • a polymer electrolyte membrane (PEM) as a solid electrolyte.
  • PEM polymer electrolyte membrane
  • the anode and the cathode are connected to a DC voltage source and supplied with a DC voltage which corresponds at least to the decomposition voltage required for the electrolysis.
  • the cathode and the third electrode are connected to another DC voltage source, the voltage applied here being smaller than that applied between the anode and the cathode.
  • the third electrode is the positive pole of this additional voltage.
  • the hydrogen produced at the cathode (product gas) is partly tapped off as product gas.
  • a not inconsiderable part migrates disadvantageously in the electrolyte to the counter electrode and therefore leads to losses. Part of this permeating hydrogen will be according to the invention again electro-chemically oxidized at the third electrode.
  • the protons thus formed migrate back to the cathode in the electric field, where they are again reduced and converted into the product gas.
  • the permeation of the hydrogen to the anode side is advantageously reduced.
  • a DC voltage between the third electrode and the cathode is applied, which is smaller than the DC voltage between the cathode and anode, but greater than the decomposition voltage for the product gas to be produced, for. B. hydrogen.
  • the advantageous hydrogen recovery can be advantageously enhanced by a large pressure difference between the anode and cathode side, since at high pressures on the cathode side and the adverse hydrogen permeation is increased by the electrolyte to the counter electrode. Accordingly, the method is particularly effective when high pressures are set on the cathode side, such as 30 bar or even up to 200 bar.
  • high pressures are set on the cathode side, such as 30 bar or even up to 200 bar.
  • catalyst layers can be used, in which a proton and electron-conducting phase occurs, and which are produced by the mixing of a proton-conducting polymer with an electron-conducting supported catalyst.
  • iridium oxide is used as a catalyst on the anode, at which hydrogen can not be oxidized.
  • platinum is used as a catalyst, which can be used in analogy to the fuel cell for hydrogen oxidation at the third electrode.
  • nickel can be used both as anode and as cathode catalyst and also for the third and fourth electrode.
  • the oxygen can be pumped back to the anode.
  • the hydrogen produced can only be consumed at an additional electrode, which at least reduces the safety problem of anodic hydrogen.
  • an alkali or a basic polymer can be used, as they are already known from the prior art for electrolysis purposes.
  • the additional electrode should, in principle, be located between the two other standard electrodes, namely the anode and the cathode.
  • the optimum position of the additional electrode with respect to the anode and the cathode can easily be determined experimentally by a person skilled in the art.
  • the additional third electrode is connected to a DC voltage source together with the cathode, and positioned very close to the cathode, the hydrogen concentration is particularly high in the case where hydrogen is produced at the cathode in the acidic electrolyte , In this case, it would require a high current for the transport of hydrogen from the additional third electrode to the cathode.
  • the additional third electrode is too close to the anode, the concentration of the cathodic product (hydrogen) would initially decrease. However, the concentration of product gas from the anode (oxygen) would be high at the additional third electrode. In the event oxygen were generated at the anode, catalytic recombination of oxygen and hydrogen could occur at the catalyst surface of the additional third electrode. However, this would lead to a loss of hydrogen, which is equivalent to a reduction in the overall efficiency of this electrolysis cell.
  • thermodynamically necessary reversible voltage of 1, 23 V must be used. In practice, however, voltages between 1, 5 and 2.5 V are realistically set due to losses. For the chlor-alkali electrolysis according to the voltage series even higher voltages are applied.
  • the electrolyzer according to the invention with an acidic electrolyte should - if the additional electrode is connected to the cathode to a DC voltage source - the voltage between the cathode and the third electrode at least the overvoltage at the cathode, so that the protons coming from the anode not can already be reduced at the additional third electrode.
  • Overvoltages occur when at least one single step of the electrolysis reaction is kinetically inhibited, ie slowed down, and are typical of reactions in which gaseous reaction products such as hydrogen, oxygen or halogens occur. This means that the electrochemical absolute potential of the additional third electrode must be greater than that necessary for hydrogen reduction at the cathode. For an acidic water electrolysis that would be, for example, 0 V.
  • the overvoltage at the cathode is approximately constant and depends on the electrode material and the quality of the catalyst.
  • the overvoltage of the cathode is negative and increases with the electrolysis current. According to the prior art, these overvoltages are in the range of a maximum of 0.2 V at the cathode.
  • this must at least be applied to achieve the thermodynamic potential for the oxidation of the cathodic product.
  • an overvoltage for the oxidation of the cathodic product must be applied to the third electrode, as well as the ohmic losses due to the ion transport through the electrolyte.
  • the overvoltage to this oxidation should be less than the overvoltage of the cathode, since the currents between the third electrode and the cathode are smaller than the currents between the anode and the cathode. Accordingly, depending on the electrolysis current and the quality of the catalysts, voltages of about 0 V to a maximum of 0.6 V with respect to the cathode at the third electrode are to be expected.
  • the reverse reaction at the additional third electrode which is connected to a DC voltage source with the cathode, is to be regarded as advantageous, since the desired product hydrogen, which is lost by the permeation through the membrane, by means of a small amount of energy can be recovered.
  • the reaction at the third electrode leads to a slight reduction of the cathodic overvoltage and thus slightly increases the voltage to be applied for the electrolysis of water.
  • a voltage must be applied which compensates for at least the difference between the overvoltages at the cathode and the third electrode, but which is considerably lower than the voltage for electrolysis of water. 2.
  • an additional third, but also an additional fourth electrode is used in the electrolysis cell not only an additional third, but also an additional fourth electrode.
  • the additional third electrode is arranged between the cathode and the fourth electrode.
  • the arrangement of the additional third electrode as far as possible from the cathode and the arrangement of the additional fourth electrode would also be as far away as possible from the anode to the concentrations of the products on the additional electrodes and the currents to be applied small to keep. This arrangement would also prevent the product gases permeating through the electrolyte from recombining. In the case of electrolysis of water, for example, the risk of explosive gas mixtures can be further reduced in this way.
  • the electrochemical cell according to the invention operated as an electrolyzer of water in an acidic medium, advantageously makes it possible to maintain the proton conductivity of the electrolyte while simultaneously reducing the disadvantageous hydrogen permeation, and thus an overall increase in the efficiency of the electrolyzer.
  • FIG. 1 shows schematically an embodiment of the invention, in which water is reacted in an electrolytic cell according to the invention, which has three electrodes and an acidic electrolyte. Between the two electrodes (anode and cathode), at which the electrochemical decomposition of the water usually takes place, an additional third electrode is arranged within the electrolyte between anode and cathode, which together with the cathode is connected to a DC voltage source.
  • iridium oxide was used as the anode catalyst and platinum supported on carbon as the cathode catalyst.
  • platinum supported on carbon As a catalyst of the additional third electrode, carbon supported platinum was also used.
  • the electrolyte used was Nafion® (acidic polymer electrolyte membrane).
  • the voltage required to oxidize the hydrogen in the membrane and to reduce it again at the cathode is designated U H u.
  • the electrolysis voltage was titled U W E.
  • the DC voltage applied between the third electrode and the cathode may be many times lower than that of the electrolysis current due to the low permeation and low overpotential of hydrogen oxidation and reduction.
  • the additional electricity to be applied is more than made up for by the increased efficiency of the electrolysis cell.
  • This embodiment of the invention is particularly advantageous if the electrolysis of water is carried out as a differential pressure method, which means that a significantly higher pressure is set on the hydrogen side than on the oxygen side.
  • a significantly higher pressure is set on the hydrogen side than on the oxygen side.
  • the invention can be particularly effective at this point, and by the forced oxidation at the third electrode significantly reduce the loss of hydrogen.
  • an electrolytic cell which has three electrodes and an acidic electrolyte.
  • an additional third electrode is arranged within the electrolyte between the anode and cathode, which, in contrast to FIG. 1, now together with the anode a DC chip source is connected. While advantageously the 0 2 crossover can be reduced in this embodiment, this is at the expense of efficiency since the electrolysis reaction (formation of oxygen) is partially reversed.
  • the voltage to be applied depends, inter alia, on the catalyst quality of the third electrode.
  • FIG. 3 shows schematically a further embodiment of the invention, in which water is reacted in an electrolysis cell according to the invention, which has four electrodes and an alkaline electrolyte. Between the two electrodes (anode and cathode), at which the electrochemical decomposition of the water usually takes place, both a third and an additional fourth electrode is disposed within the electrolyte between the anode and cathode.
  • the third electrode is made of a material capable of electrochemically oxidizing hydrogen
  • the fourth electrode is made of a material capable of electrochemically reducing oxygen.
  • the voltage needed to oxidize the hydrogen in the membrane is designated U H u.
  • the voltage required to reduce the oxygen in the membrane and to reoxidize it at the anode is designated U 0 u.
  • the electrolysis voltage was titled U WE .
  • the hydrogen is electrochemically oxidized at the third electrode.
  • the oxygen present in the electrolyte and permeating the cathode is electrochemically reacted at the fourth electrode.
  • the hydroxilions produced by the electrolysis are used to reduce the oxygen at this additional electrode.
  • the oxygen can be electrochemically pumped by the DC current between the fourth electrode and the anode through the electrolyte.
  • the basic idea of the invention - the utilization of an electrochemical pump for the recovery and the reduction and oxidation of contaminants of the products among one another - can be used advantageously in electrolyses with gaseous or liquid products. It serves to reduce the permeation of products through the electrolyte, which leads to safety problems, a loss of efficiency and contamination of the products of the electrolysis.
  • at least one additional third electrode is introduced in addition to the anode and cathode necessary for the electrolysis.
  • the product produced at the cathode which is located in the cationic electrolyte, can be electrochemically oxidized and reduced again at the cathode.
  • a low voltage must be applied between the third electrode and the cathode, which can reoxidize the product gas produced at the cathode.
  • the anodic product can be reduced at one of the additional electrodes and thus electrochemically pumped to the anode.
  • the applied voltage can usually due to the low currents of permeation and low overvoltage, z. B. the hydrogen oxidation and - reduction, many times lower than that for the actual electrolysis.

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  • Engineering & Computer Science (AREA)
  • Chemical Kinetics & Catalysis (AREA)
  • Electrochemistry (AREA)
  • Materials Engineering (AREA)
  • Metallurgy (AREA)
  • Organic Chemistry (AREA)
  • Automation & Control Theory (AREA)
  • Inorganic Chemistry (AREA)
  • Electrolytic Production Of Non-Metals, Compounds, Apparatuses Therefor (AREA)

Abstract

L'invention concerne un procédé pour faire fonctionner une cellule d'électrolyse selon lequel on applique entre au moins une troisième électrode supplémentaire et l'anode ou entre au moins une troisième électrode supplémentaire et la cathode une autre tension continue inférieure à la première tension continue, nécessaire à l'électrolyse, qui est appliquée entre l'anode et la cathode. Outre une anode et une cathode, la cellule d'électrolyse selon l'invention comporte au moins une autre électrode supplémentaire, disposée entre l'anode et la cathode, qui est reliée soit comme autre cathode à l'anode, soit comme autre anode à la cathode par le biais d'une autre source de tension continue. L'application d'une tension continue entre la cathode et l'électrode supplémentaire a pour effet d'oxyder au niveau de l'électrode supplémentaire, par voie électrochimique, l'hydrogène qui est présent dans l'électrolyte et qui présente l'inconvénient de perméer en direction de l'anode (réaction inverse en direction de la cathode), lequel peut à nouveau être réduit au niveau de la cathode. Ceci permet de réduire notablement la perméation préjudiciable de l'hydrogène en direction de la contre-électrode et donc d'accroître le rendement global du système.
PCT/DE2014/000559 2013-11-20 2014-10-31 Cellule d'électrolyse électrochimique et son procédé de fonctionnement WO2015074637A1 (fr)

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DE102013019341.9 2013-11-20
DE102013019341.9A DE102013019341A1 (de) 2013-11-20 2013-11-20 Elektrochemische Elektrolysezelle sowie Verfahren zum Betreiben derselben

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WO2018115821A1 (fr) * 2016-12-22 2018-06-28 Johnson Matthey Fuel Cells Limited Membrane revêtue de catalyseur dotée d'une structure stratifiée
JP2020507005A (ja) * 2016-12-23 2020-03-05 テクニシュ ユニベルシテイト デルフトＴｅｃｈｎｉｓｃｈｅ Ｕｎｉｖｅｒｓｉｔｅｉｔ Ｄｅｌｆｔ ハイブリッド電池電解槽

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EP4112781A1 (fr) * 2021-06-30 2023-01-04 Siemens Energy Global GmbH & Co. KG Cellule d'électrolyse destinée à l'électrolyse à membrane électrolytique polymère et son procédé de fabrication

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WO2018115821A1 (fr) * 2016-12-22 2018-06-28 Johnson Matthey Fuel Cells Limited Membrane revêtue de catalyseur dotée d'une structure stratifiée
CN110114512A (zh) * 2016-12-22 2019-08-09 庄信万丰燃料电池有限公司 具有层合结构的催化剂涂覆的膜
CN110114512B (zh) * 2016-12-22 2021-08-10 庄信万丰燃料电池有限公司 具有层合结构的催化剂涂覆的膜
CN113529121A (zh) * 2016-12-22 2021-10-22 庄信万丰燃料电池有限公司 具有层合结构的催化剂涂覆的膜
EP3922757A1 (fr) * 2016-12-22 2021-12-15 Johnson Matthey Fuel Cells Limited Membrane enduite de catalyseur ayant une structure stratifiée
US11502308B2 (en) 2016-12-22 2022-11-15 Johnson Matthey Hydrogen Technologies Limited Catalyst-coated membrane having a laminate structure
JP2020507005A (ja) * 2016-12-23 2020-03-05 テクニシュ ユニベルシテイト デルフトＴｅｃｈｎｉｓｃｈｅ Ｕｎｉｖｅｒｓｉｔｅｉｔ Ｄｅｌｆｔ ハイブリッド電池電解槽
US11552352B2 (en) 2016-12-23 2023-01-10 Battolyser Holding B.V. Hybrid battery and electrolyser
JP7252628B2 (ja) 2016-12-23 2023-04-05 テクニシュ ユニベルシテイト デルフト ハイブリッド電池電解槽

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