[go: up one dir, main page]

WO2011073621A1 - Système de pile à combustible - Google Patents

Système de pile à combustible Download PDF

Info

Publication number
WO2011073621A1
WO2011073621A1 PCT/GB2010/002277 GB2010002277W WO2011073621A1 WO 2011073621 A1 WO2011073621 A1 WO 2011073621A1 GB 2010002277 W GB2010002277 W GB 2010002277W WO 2011073621 A1 WO2011073621 A1 WO 2011073621A1
Authority
WO
WIPO (PCT)
Prior art keywords
fuel cell
liquid
fuel
cell system
carbonate
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.)
Ceased
Application number
PCT/GB2010/002277
Other languages
English (en)
Inventor
Michael Alexander Priestnall
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.)
Individual
Original Assignee
Individual
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 Individual filed Critical Individual
Publication of WO2011073621A1 publication Critical patent/WO2011073621A1/fr
Anticipated expiration legal-status Critical
Ceased legal-status Critical Current

Links

Classifications

    • 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
    • H01M8/06—Combination of fuel cells with means for production of reactants or for treatment of residues
    • H01M8/0693—Treatment of the electrolyte residue, e.g. reconcentrating
    • 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
    • H01M8/06—Combination of fuel cells with means for production of reactants or for treatment of residues
    • H01M8/0662—Treatment of gaseous reactants or gaseous residues, e.g. cleaning
    • H01M8/0668—Removal of carbon monoxide or carbon dioxide
    • 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
    • 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
    • H01M8/10—Fuel cells with solid electrolytes
    • H01M8/1009—Fuel cells with solid electrolytes with one of the reactants being liquid, solid or liquid-charged
    • 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
    • H01M8/10—Fuel cells with solid electrolytes
    • H01M2008/1095—Fuel cells with polymeric electrolytes
    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M2300/00—Electrolytes
    • H01M2300/0002—Aqueous electrolytes
    • H01M2300/0014—Alkaline electrolytes
    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M2300/00—Electrolytes
    • H01M2300/0017—Non-aqueous electrolytes
    • H01M2300/0048—Molten electrolytes used at high temperature
    • H01M2300/0051—Carbonates
    • 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
    • H01M8/10—Fuel cells with solid electrolytes
    • H01M8/1009—Fuel cells with solid electrolytes with one of the reactants being liquid, solid or liquid-charged
    • H01M8/1011—Direct alcohol fuel cells [DAFC], e.g. direct methanol fuel cells [DMFC]
    • 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
    • H01M8/10—Fuel cells with solid electrolytes
    • H01M8/1009—Fuel cells with solid electrolytes with one of the reactants being liquid, solid or liquid-charged
    • H01M8/1011—Direct alcohol fuel cells [DAFC], e.g. direct methanol fuel cells [DMFC]
    • H01M8/1013—Other direct alcohol fuel cells [DAFC]
    • 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
    • Y02E60/50—Fuel cells

Definitions

  • This invention relates to a fuel cell in which Carbon Dioxide (C0 2 ) is captured and sequestered as a solid mineral during fuel cell operation.
  • Carbon capture and storage encompasses a range of approaches by which the C0 2 that would otherwise be emitted during oxidation of hydrocarbon fuels is prevented from release to the atmosphere.
  • Near-term adoption of such technologies is generally considered to be essential if fossil fuels are to continue to be widely used while at the same time global emissions of C0 2 are to be reduced.
  • Economic considerations dictate that only those effective CCS processes that add the least cost to total cost of electrical energy generated are likely to be adopted.
  • At present one of the lowest cost processes involves capturing pure C0 2 from combustion exhaust gases; liquefaction of the C0 2 ; transport and transfer of the liquid C0 2 to a suitable high-pressure, high- integrity underground or undersea repository; and long-term geological storage of the liquid C0 2 .
  • CCS complex chemical reaction of captured C0 2 with metal ions (e.g. magnesium and calcium) to form stable solid carbonate minerals which can be readily stored long-term without risk of C0 2 release and may even have value as industrial materials.
  • metal ions e.g. magnesium and calcium
  • C0 2 -mineralisation processes are also generally considered as only being appropriate to large scale, point sources of C0 2 where, typically >0.1 million-tonnes C0 2 per year is produced, these sources generally being considered to account for ⁇ 60% of global C0 2 emissions.
  • Alkaline fuel cells have been established since 1910 (Teitelbaum) as being an efficient means of converting the chemical energy in hydrocarbon fuels, even gasoline or coal, directly to electrical energy.
  • the ability to operate alkaline fuel cells on non-precious metal electrocatalysts also offers a cost advantage over other low-temperature fuel cell types, such as proton-exchange membrane (PEM) fuel cells, that require platinum-based anode and cathode electrocatalysts.
  • PEM proton-exchange membrane
  • AFCs which currently operate using liquid aqueous hydroxide electrolytes, such as potassium and sodium hydroxides, are sensitive to carbonation by both C0 2 in the ambient air used as oxidant at the cathode of the AFC and any C0 2 generated at the anode of the AFC by electrochemical oxidation of carbon-containing fuels. Partial dissolution of C0 2 in the hydroxide electrolyte and reaction with it forms carbonates which, at sufficient concentration, can precipitate out and form unwanted and potentially damaging deposits. The reduction in hydroxide concentration can reduce electrolyte conductivity and cell efficiency.
  • AFCs are generally operated on high-purity hydrogen and often incorporate some C0 2 scrubbing system to remove C0 2 from inlet air fed to the cathode.
  • This situation is summarised by Prof. Elton Cairns in Ch.17 vol.1 pp.301 of The Handbook of Fuel Cells (ISBN 0471499269): "Sodium or potassium electrolytes cannot be used directly with ambient air or with organic fuels, since they react with C0 2 to yield carbonate, eventually converting the hydroxide electrolyte to a carbonate electrolyte. At the concentrations normally used, this results in the precipitation of sodium or potassium carbonate and/or bicarbonate, damaging the electrodes and rendering the cell useless.”
  • GB1213777 Efforts have been made to address the problem of carbonation of electrolyte in alkaline fuel cells, one example of which is described in GB1213777.
  • the system described in GB1213777 forces potassium carbonate out of solution in potassium hydroxide by adding additional hydroxide to the solution in a separate chamber outside the fuel cell.
  • the system exploits the reduced solubility of the carbonate in highly concentrated hydroxide so that solid carbonate is separated out.
  • a problem with this approach is that it consumes the hydroxide electrolyte. Fresh hydroxide must be continually added for the system to keep operating. This is economically unattractive.
  • the system described in GB1213777 also fails to sequester the carbon dioxide into a geologically stable carbonate, as potassium and sodium carbonates will readily dissolve in rainwater.
  • the invention aims to address problems associated with the costs, scale and risks of carbon capture and storage (CCS) technologies.
  • CCS carbon capture and storage
  • the invention also aims to address the costs and electrolyte-carbonation of fuel cells, and the efficiency of conversion of hydrocarbon fuels to electrical energy.
  • the present invention is defined in the appended independent claims, to which reference should be made. Preferred features are set out in the dependent claims.
  • the invention may thus relate to a fuel cell in which C0 2 is produced as a reaction product and/or in which C0 2 enters the cell, for example mixed with air being used as an oxidant or contained in flue gases from a fossil fuel power station or other reactor.
  • the C0 2 dissolves in or reacts with a liquid in the fuel cell, which may be a carrier liquid for a fuel supplied to the cell, a carrier liquid for an oxidant supplied to the cell, and/or the electrolyte of the cell.
  • the liquid may serve one, two or all of these functions, as described below.
  • the C0 2 dissolved in or reacted with the liquid in the fuel cell may then be sequestered or converted into an insoluble carbonate, by reaction with group II metal ions or another suitable reagent such as Fe.
  • the invention comprises a fuel cell, consisting of an anode, a cathode and an electrolyte, operating on fuel and oxidant reactants, either or both of which contain carbon.
  • a fuel cell consisting of an anode, a cathode and an electrolyte, operating on fuel and oxidant reactants, either or both of which contain carbon.
  • the same or different liquids may be used for electrolyte and for dispersion/dissolution of oxidant and fuel.
  • the electrolyte may be a solid.
  • C0 2 (which may be contained in a fluid, such as ambient air, entering the fuel cell or may be generated within the fuel cell as a result of electrochemical oxidation of fuel) is at least partially prevented from release to the atmosphere from the exhaust of the fuel cell by dissolution in or reaction with one or more of the liquid or liquids.
  • the C0 2 captured in this way is concurrently or subsequently converted into a solid carbonate or bicarbonate that is geologically stable.
  • Group II metal ions typically calcium ions or magnesium ions or both calcium and magnesium ions, can be used to react with the dissolved or reacted C0 2 to form these stable carbonates. It is also or alternatively possible to use other means to react with the dissolved or reacted C0 2 to form the stable carbonates, such as iron.
  • the fuel cell system is able to capture and sequester C0 2 in the air or other fluids fed to the fuel cell, or C0 2 or other carbon-containing oxidation products that are produced by electrochemical oxidation of a carbon-containing fuel, or any combination of these.
  • a fuel cell in which the carbon-containing reactant is dispersed in the liquid electrolyte and the C0 2 is initially captured by reaction with or dissolution in the liquid electrolyte; a solid-membrane-type fuel cell in which the reactant is supplied to the fuel cell dispersed in a carrier liquid which reacts with or dissolves the C0 2 ; a fuel cell in which C0 2 supplied to or generated at one electrode is transported through the electrolyte as a carbonate or bicarbonate ion to react with or dissolve in a carrier liquid at the other electrode.
  • the invention uses a liquid electrolyte (such as the hydroxide electrolyte of an alkaline fuel cell, or the carbonate electrolyte of an aqueous or molten carbonate fuel cell) to capture and convert into carbonate the majority of the carbon dioxide or other carbon-containing oxidation products that are generated from electrochemical oxidation of a carbon-containing fuel and C0 2 that is present with the oxygen in the air that is fed to the fuel cell to oxidise the fuel.
  • a liquid electrolyte such as the hydroxide electrolyte of an alkaline fuel cell, or the carbonate electrolyte of an aqueous or molten carbonate fuel cell
  • a liquid electrolyte such as the hydroxide electrolyte of an alkaline fuel cell, or the carbonate electrolyte of an aqueous or molten carbonate fuel cell
  • Sequestration of product C0 2 as a solid may be used to increase the Gibbs free energy of the fuel cell reaction and thereby increase the electrical conversion efficiency of the fuel cell.
  • Electrochemical reaction of C0 2 within the fuel cell to form carbonates may be used to extract useful electrical energy from the mineralisation process, for example by supplying C0 2 to one electrode and metal ions or mineral species to the other electrode. Continuous removal of the reaction product C0 2 (e.g. by reaction with a metallic species to form a solid carbonate precipitate) in a fuel cell shifts the equilibrium of the fuel oxidation half-cell reaction further to the right, in accordance with Le Chatelier's principle. This increases the free energy of the reaction and the overall cell potential. This results in an increase in electrical conversion efficiency, a reduction in the proportion of C0 2 generated per unit of electrical energy and an improvement in the cost effectiveness of a fuel cell system.
  • Exemplar reactions include:
  • carbonate fuel cell where carbonate or bicarbonate (herein referred to as carbonate) species are formed electrochemically, it is possible to extract additional electrical energy from the reactions of C0 2 with the electrolyte, or with additives to the electrolyte, or with reactants supplied to the electrodes. In principle, this enables C0 2 to be used as a reactant for the fuel cell in which the Gibbs free energy of reaction to form carbonates is partially converted to electrical energy. Suitable reactants for such a fuel cell could include the exhaust gases of fossil-fuelled power stations and the C0 2 that forms part of ambient air.
  • a fuel cell with at least one selective electrocatalyst can be fed with ambient air where the C0 2 component of the air is one reactant and oxygen or mineral species supplied to the fuel cell is another reactant.
  • Such a fuel cell could be used to sequester carbon dioxide directly from the atmosphere while producing useful electricity.
  • Continual removal of product C0 2 and continual regeneration of hydroxide electrolyte enables an alkaline fuel cell to operate continuously and efficiently with carbon-containing fuels and ambient air, reducing fuel cell operating costs, reducing risks of damage by electrolyte carbonation and increasing operating time between servicing. Further, it enables C0 2 to be captured and
  • the use of a fuel cell as a means to capture C0 2 offers an advantage in the inherent separation of product C0 2 from the air used in the electrochemical oxidation. This avoids energy being expended in separating or concentrating the C0 2 as is required in conventional CCS processes.
  • Inherent dissolution of C0 2 in the electrolyte of an AFC offers an advantage in that additional processes, materials or energy are not required to separate or dissolve the C0 2 from exhaust gases. This advantage is enhanced if the carbon-containing fuel is dissolved or dispersed in the electrolyte and the C0 2 generated is released directly into the electrolyte.
  • the process is particularly suited to a mixed- reactant or single-chamber type fuel cell in which fuel and oxidant (and, optionally, electrolyte) are combined together in one mixture. Additionally, the temperature, pH and composition of the electrolyte of the fuel cell can be selected to optimise the dissolution and/or reaction of C0 2 and the precipitation of mineral carbonate.
  • (Bi)carbonate precipitates in the electrolyte can also be separated and reacted with suitable minerals to regenerate hydroxide and to form stable carbonates through reactions such as:
  • Finely-divided waste mineral materials are available from a variety of industrial processes such as spoil materials from metals mining, ashes from combustion processes, slags from metal refining and cement and concrete wastes. Many of these materials are available at low or negative cost and with suitably small particle sizes that will enable them to react rapidly with C0 2 to form stable carbonates. Use of such waste feedstock materials in conjunction with a fuel cell system may improve the overall economic case for CCS. Likewise the chemistry of the CCS mineralisation process may be selected to produce mineral carbonate species that have industrial utility and value.
  • the invention provides a fuel cell system comprising:
  • a fuel cell comprising an anode, a cathode, fuel, oxidant reactant, at least one of the fuel and oxidant reactant containing carbon, and a liquid, wherein C0 2 or a carbon-containing oxidation product in the fuel cell reacts or dissolves in the liquid; and a means for regenerating the liquid by converting the reacted or dissolved C0 2 or carbon-containing oxidation product to a geologically stable carbonate.
  • the invention provides a fuel cell system comprising: a fuel cell comprising an anode, a cathode, fuel, oxidant reactant, at least one of the fuel and oxidant reactant containing carbon, and a liquid, wherein C0 2 or a carbon-containing oxidation product in the fuel cell reacts or dissolves in the liquid; and a means for sequestering the reacted or dissolved C0 2 or carbon- containing oxidation product and regenerating the liquid.
  • Figure 1 is a schematic diagram of a fuel cell system in accordance with a first embodiment of the invention
  • Figure 2 is a schematic diagram illustrating the industrial application of a fuel cell as shown in Figure 1 , for producing power;
  • FIG. 3 is a schematic diagram of a fuel cell system in accordance with a second embodiment of the invention.
  • FIG. 4 is a schematic diagram of a fuel cell system in accordance with a third embodiment of the invention.
  • FIG. 5 is a schematic diagram of a fuel cell system in accordance with a fourth embodiment of the invention.
  • Figure 1 shows a generic schematic of a first aspect of the invention.
  • Figure 1 shows a fuel cell operated with carbon-containing reactants and fabricated according to the current art, which consists of an electrically-conductive anode electrode 1 and an electrically-conductive cathode electrode 2, separated by, and in contact with an electrolyte 3.
  • the electrolyte may be a solid membrane but in this example is a liquid, which may be constrained within a solid matrix or may be free-flowing and circulated through the fuel cell via an entry port 11 and an exit port 14 (e.g. for cooling purposes or to prevent crossover of fuel from anode to cathode).
  • a carbon-containing liquid or gaseous fuel 9 is supplied to the anode electrode 1 , via an anode chamber 4, and an oxidant 10, typically air containing ⁇ 0.04% C0 2 , is supplied to the cathode 2, via a cathode chamber 5.
  • the anode electrode 1 includes an electrically-conductive substrate 8, typically a porous mesh, cloth or paper of carbon or metal, to which is bonded an electrocatalyst 7, active towards the electro-oxidation of fuel, and in contact with both the fuel 9 and electrolyte 3.
  • the cathode contains an electrically-conductive substrate 8, typically a porous mesh, cloth or paper of carbon or metal, to which is bonded an electrocatalyst 7, active towards the electro-oxidation of fuel, and in contact with both the fuel 9 and electrolyte 3.
  • the cathode contains an electrically-conductive substrate 8, typically a porous mesh, cloth or paper of carbon or metal, to which is bonded an electrocatalyst 7, active towards the electro-oxidation of fuel,
  • the fuel cell system of Figure 1 incorporates a liquid 17, supplied with any combination of the fuel 9 or the oxidant 10 or the electrolyte 11 , or supplied as the electrolyte, that reacts with C0 2 within the fuel cell and exits the fuel cell, in substantially carbonated form 18, via ports 12 and/or 13 and/or 14; and, secondly, a reaction chamber 19 in which the carbonated liquid 18 is reacted with a group II metal ion 20 to form a solid group II metal carbonate precipitate 21 and to regenerate liquid 17.
  • the cathode 2 typically contains an active oxygen-reduction catalyst such as silver, platinum, nickel, manganese dioxide or transition metal carbide (and combinations thereof) and the anode 1 typically contains a fuel oxidation electrocatalyst, such as a transition metal oxide decorated with precious metal particles, nickel, palladium or platinum alloy (or combinations thereof).
  • the electrolyte 3 is preferably an alkaline liquid aqueous hydroxide, such as sodium or potassium hydroxide, or other ionically-conducting fluid which will dissolve or react with C0 2 .
  • Alternative electrolytes are possible such as aqueous or molten salts including carbonates.
  • the fuel is preferably carbon-containing and a liquid, such as methanol.
  • the fuel may be dissolved or dispersed in the electrolyte.
  • the fuel or electrolyte-fuel mixture is supplied to the anode 1 of the fuel cell and the electrolyte 3 or fuel-electrolyte mixture is circulated between and past the anode 1 and cathode 2, so that the anode and cathode have a continuous ionic connection between them.
  • Air or other appropriate oxidant 10 is supplied to the cathode.
  • the anode and cathode of the cell are connected electrically to an external circuit and electricity is generated when fuel is electrochemicaiiy oxidised at the anode and oxidant is electrochemicaiiy reduced at the cathode.
  • liquid 17 may be sodium hydroxide and the C0 2 reacts with flowing sodium hydroxide to generate dissolved or dispersed sodium carbonate and/or sodium bicarbonate.
  • fuel such as methanol can react electrochemicaiiy with carbonate or
  • bicarbonate ion at the anode to generate product carbon dioxide which can dissolve in the electrolyte to form (bi)carbonate ions and/or further react with dissolved carbonate to form bicarbonate ions.
  • Hydroxide ions formed at the cathode of the fuel cell from electrochemical reduction of oxygen can react with bicarbonate to form carbonate ions or oxygen may react directly with C0 2 at the cathode to form carbonate ions. Reactions occurring at electrodes and within the electrolyte may include:
  • particles of magnesium or calcium silicates dispersed in the electrolyte react with the dissolved or dispersed C0 2 or (bi)carbonate to form a solid precipitate of magnesium or calcium carbonates and silica and to regenerate hydroxide ions. These precipitates are continuously or periodically settled and separated from the electrolyte.
  • the electrolyte containing dissolved/dispersed C0 2 or (bi)carbonates and/or depleted in hydroxide ions is replaced or topped-up with a fresh source of hydroxide or other appropriate ions.
  • the electrolyte is then reacted with an appropriate source of metal ions to form a stable carbonate precipitate.
  • the electrolyte containing dissolved/dispersed CO2 or carbonates is circulated through a bed of metal silicates or other appropriate oxide, hydroxide, silicate or other species which are capable of reacting with the dissolved carbonates to form solid carbonates and to regenerate hydroxide ions.
  • a direct-oxidation fuel cell operating on a carbon-based fuel generates carbon dioxide as a reaction product.
  • the fuel preferably a (first) liquid
  • a (second) liquid preferably an alkaline electrolyte
  • the (second or carrier) liquid dissolves and/or reacts with the product C0 2 .
  • Product C0 2 is captured as a solid mineral precipitate through reaction with a metal ionic species, preferably a magnesium, and/or calcium ionic species, which is preferably in solution and preferably in a solution formed of the (second) liquid.
  • the solid carbonate precipitate is removed and the (second) liquid, to which additional fuel is added, is recirculated to the anode of the fuel cell.
  • the purpose of the process and system is to prevent gaseous C0 2 from being released to the atmosphere during the electrochemical oxidation of a carbon-containing fuel and the simultaneous sequestration of the CO2 in a mineral precipitate.
  • a carbon containing fuel such as methanol or particles of coal
  • a carrier liquid(s) such as sodium hydroxide or an amine
  • the membrane electrolyte is ionically conducting to hydroxide ions and/or to protons and/or to carbonate ions and/or to oxide ions.
  • C0 2 generated by the electrochemical oxidation of the fuel at the anode dissolves in the carrier liquid(s) or reacts with carrier liquid(s) to form carbonate species.
  • Mineral solids such as metal carbonates, oxides, hydroxides and/or silicates
  • C0 2 reacting at one electrode is transported through the electrolyte in the form of carbonate or bicarbonate ions to the other electrode, where it reacts again to form a solid carbonate precipitate. Electrical energy is generated as a consequence of the transport of (bi)carbonate ions from one electrode to the other.
  • a first example is a direct-methanol alkaline fuel cell of the type shown in Figure 1 in which aqueous KOH is used both as the liquid to react with the product C0 2 in the fuel cell and also as the fuel cell electrolyte.
  • CaO is used as the source of group II metal ions to precipitate calcium carbonate from the carbonated electrolyte (K 2 C0 3 and KHC0 3 ) and to regenerate KOH.
  • Anode and cathode electrodes 1 ,2 are formed from a conductive porous carbon cloth laminated to a PTFE-bonded mixture of carbon black and nanoparticulate platinum (such as "BiPlex PlaXC” anode material available from Gaskatel GmbH).
  • the fuel 9 is an aqueous methanol solution (CH 3 OH), typically industrially synthesised from coal or natural gas.
  • the oxidant 10 is simply air and in particular oxygen found in air.
  • the electrolyte 3 is 3 molar potassium hydroxide (KOH) in water.
  • Electrolyte and fuel are each supplied to the fuel cell at a rate of at least 1 mole (56g) of KOH per mole (32g) of CH 3 OH that is oxidised. Any methanol that is supplied to, but not consumed (oxidised) in, the fuel cell is recycled for subsequent supply to the fuel cell.
  • Oxygen (in air) is supplied to the fuel cell at a rate at least three moles (96g) of 0 2 per two moles (64g) of CH 3 OH that is oxidised. Excess air (or air partially depleted of oxygen and C0 2 ) is exhausted to atmosphere. Products of the fuel cell reactions are exhausted from the fuel cell in solution with the electrolyte.
  • methanol is oxidised to form water (H 2 0) and carbonate ions (C0 3 2 ) and/or bicarbonate ions (HC0 3 ⁇ ) in the electrolyte according to the following reactions:
  • Bicarbonate ion formation is favoured at low rates of electrolyte supply (low ratio of KOH: CH 3 OH), while carbonate ion formation is favoured at high rates of KOH supply.
  • the electrons released at the anode 1 by the electro-oxidation of the methanol are transferred through an external electrical circuit, doing useful work as electricity, before returning to the cathode 2 where they take part in the electro- reduction of the oxygen.
  • the exhaust carbonated electrolyte from the fuel cell containing dissolved product carbonate and/or bicarbonate ions is reacted with lime (calcium oxide, CaO) in at least the proportion of 1 mole (56g) of CaO per mole (60g) of dissolved (bi)carbonate ion.
  • the solids are separated from the solution (e.g. by filtration or settling), excess product water from the fuel cell reaction is removed as hydration water in the solid carbonate (or by evaporation) and the regenerated electrolyte is recycled for use again as input to the fuel cell.
  • thermodynamically favourable oxidation of carbon to aqueous carbonate and regeneration of the alkaline capture liquid (carrier liquid) by precipitation of solid carbonates can be represented as:
  • Figure 2 illustrates how the fuel cell chemistry described in Example 1 can be utilised for a 500MW power station.
  • the group II metal ions can be provided from a number of economically viable sources, such as olivines, serpentines, industrial waste materials, mine and quarry fines, oil drilling cuttings or combustion ash. As shown in Figure 2, a proportion, typically between 5 and 30% of energy output from the power station, may be needed to process the source of metal ions.
  • Figure 2 shows the approximate quantities of raw material required and generated by the power station. Figure 2 also illustrates that the system provided savings in treating waste material.
  • the methanol fuel 9 is supplied to the fuel cell dissolved in the aqueous KOH electrolyte 3, rather than as a separate supply to the anode, in a similar mode to that described in US5004424.
  • the platinum is replaced with an electrocatalyst such as silver or manganese oxide that is inactive toward methanol oxidation.
  • a suitable cathode is a conductive porous nickel mesh laminated to a PTFE-bonded mixture of carbon black and nanoparticulate silver (such as "BiPlex Oxag" cathode material available from Gaskatel GmbH).
  • Reaction sequences are the same as in Example 1. Any excess, unreacted methanol fuel that exits the fuel cell in the electrolyte exhaust stream may be directly recycled or recovered by distillation when the carbonated electrolyte is regenerated and excess product water removed.
  • an impermeable anion-conducting solid polymer electrolyte membrane (PEM) 30, is used instead of KOH as electrolyte.
  • PEM solid polymer electrolyte membrane
  • Figure 3 which is otherwise of the same layout as the system of Figure 1.
  • Ethanol, rather than methanol, is used as fuel 9 and the ethanol is dissolved in a carrier fluid 17 consisting of an aqueous solution of ammonia/ammonium hydroxide (NH 4 OH) where the molar ratio of ammonium hydroxide to ethanol is at least 2:1.
  • carrier fluid 17 consisting of an aqueous solution of ammonia/ammonium hydroxide (NH 4 OH) where the molar ratio of ammonium hydroxide to ethanol is at least 2:1.
  • Anode and cathode electrodes 1 ,2 are bonded directly to either side of the alkaline PEM 30.
  • Electro-oxidation of ethanol at the anode 1 by hydroxide ions conducted through the PEM generates carbon dioxide which reacts with the NH 4 OH in the carrier liquid to form ammonium bicarbonate, thereby avoiding C0 2 release to the atmosphere:
  • a further example of the invention uses a mixed-reactant, single-feed fuel cell with a porous flow-through polymer membrane electrolyte, as shown in Figure 4 (which is of the type described in US2003165727).
  • a low-grade oxygen- contaminated reformate gas is used as fuel
  • exhaust gases from an air-rich combustion process are used as oxidant
  • aqueous ammonia are used as the liquid to be carbonated
  • a suspension of magnesium hydroxide particles is used as an integral source of group II ions.
  • the fuel 9, oxidant 10, carrier liquid 17 and group II ion source 20 are introduced into the fuel cell in a single feed, and spent oxidant and depleted fuel exits together with carrier liquid and a carbonate precipitate 21.
  • the carbonate precipitate is separated from the carrier liquid in a chamber 19 and the carrier liquid is returned to the fuel cell together with fresh fuel and oxidant.
  • An anion-conducting polymer electrolyte membrane 3 is used (such as available commercially from Solvay, Fumatec, Dupont or Tokayama), which is multiply perforated to allow a fluid with entrained particles to pass through it with minimal pressure drop.
  • a flow-through fuel cell is constructed using membrane electrode assemblies formed by bonding porous anode and cathode electrodes 1 ,2 to each side of the perforated membrane.
  • the anode contains an electrocatalyst 7 such as tungsten oxide that is selective toward oxidation of fuel while the cathode contains an electrocatalyst such as silver that is selective toward reduction of oxygen.
  • the fuel cell contains a single chamber with the membrane electrode assembly or assemblies arranged across it.
  • the single-feed for the fuel cell is prepared consisting of a three-phase mixture of bubbles of reformate gases (containing hydrogen, carbon monoxide, oxygen, nitrogen and carbon dioxide), air and exhaust combustion gases in a liquid aqueous ammonia solution with suspended solid particles of magnesium hydroxide.
  • the mixture is pumped through the single chamber of the fuel cell where the fuel components of the mixed feed are electro-oxidised at the anode and the oxygen is electro-reduced at the cathode. Electricity is generated by these electrochemical reactions and used in an external circuit.
  • perforations and porosity of the membrane electrode assemblies are large enough, and the flow-rates high enough, to avoid clogging of the electrode and electrolyte pores by the suspended particles in the feed mixture.
  • the ammonium carbonate reacts with the suspended particles of magnesium hydroxide and with any magnesium ions in solution to form suspended particles of solid magnesium carbonate and to regenerate ammonium hydroxide solution.
  • C0 2 may also react directly with the suspended magnesium hydroxide particles to form magnesium carbonate and hydroxide ions. Little or no gaseous CO 2 exits the fuel cell.
  • the solid, gaseous and liquid phases of the mixture are separated and the ammonium solution returned for re-use in the fuel cell. Any unreacted fuel may be recycled to the fuel cell or combusted.
  • the solid carbonate product phases can be filtered and consolidated and used as construction materials.
  • example 1 Another variant of example 1 is a fuel cell in which C0 2 is supplied to one electrode and is transported through the electrolyte as a carbonate or bicarbonate ion to react with a liquid at the other electrode.
  • the cathode 2 of the fuel cell is supplied with a gas mixture 50 containing C0 2 and 0 2 , such as air or a flue gas.
  • the anode 1 is supplied with limewater, a solution containing calcium hydroxide, which, in this example, is liquid 17 and fuel 51 and source of group II ion 20, i.e. all one and the same, so that the anode chamber inside the fuel cell is also the reaction chamber where regeneration of the liquid 17 and precipitation of solid calcium carbonate 21 takes place.
  • a separate electrolyte 3 such as aqueous caesium carbonate is provided to separate the cathode and anode compartments and to conduct carbonate ions between them.
  • Anodes, cathodes and their respective electrocatalysts, such as carbon-supported platinum dispersed on carbon cloth, are chosen as suitable for the alkaline environment and to accelerate the reactions at each electrode. Oxygen is electrochemically reduced at the cathode electrode to form carbonate ion in combination with the C02:
  • the fuel cell of this example is able to extract electrical energy directly from the exothermic oxidation of carbon dioxide to carbonate.
  • the direct formation of a solid carbonate also has advantages of driving the electrochemical reaction and increasing electrical conversion efficiency according to le Chatelier's principle, i.e. through removal of a reaction product.
  • Chemistries for C0 2 sequestration other than those described as examples herein are possible such as those described in WO2009139813,

Landscapes

  • Life Sciences & Earth Sciences (AREA)
  • Engineering & Computer Science (AREA)
  • Manufacturing & Machinery (AREA)
  • Sustainable Development (AREA)
  • Sustainable Energy (AREA)
  • Chemical & Material Sciences (AREA)
  • Chemical Kinetics & Catalysis (AREA)
  • Electrochemistry (AREA)
  • General Chemical & Material Sciences (AREA)
  • Fuel Cell (AREA)

Abstract

La présente invention a pour objet un système de pile à combustible et de capture du carbone intégré, fonctionnant sur des réactifs carbonés comprenant un liquide, le CO2 dans la pile à combustible réagissant ou se dissolvant dans le liquide; et un moyen de séquestration du CO2 ayant réagi ou dissous dans le liquide par la formation d'un composé carbonate stable et la régénération du liquide. Le moyen de séquestration du CO2 ayant réagi ou dissous peut être une source d'ions métalliques du groupe II, communément trouvée sous la forme de matériaux minéraux usés finement divisés.
PCT/GB2010/002277 2009-12-15 2010-12-15 Système de pile à combustible Ceased WO2011073621A1 (fr)

Applications Claiming Priority (4)

Application Number Priority Date Filing Date Title
GB0921881.9 2009-12-15
GBGB0921881.9A GB0921881D0 (en) 2009-12-15 2009-12-15 Carbonate fuel cell
GB1010672.2 2010-06-24
GBGB1010672.2A GB201010672D0 (en) 2009-12-15 2010-06-24 Fuel cell system

Publications (1)

Publication Number Publication Date
WO2011073621A1 true WO2011073621A1 (fr) 2011-06-23

Family

ID=41667112

Family Applications (1)

Application Number Title Priority Date Filing Date
PCT/GB2010/002277 Ceased WO2011073621A1 (fr) 2009-12-15 2010-12-15 Système de pile à combustible

Country Status (2)

Country Link
GB (2) GB0921881D0 (fr)
WO (1) WO2011073621A1 (fr)

Cited By (11)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
EP2525896A4 (fr) * 2010-01-22 2014-02-19 Univ Rutgers Séquestration d'un gaz émis par une usine industrielle
US9187835B2 (en) 2011-05-19 2015-11-17 Calera Corporation Electrochemical systems and methods using metal and ligand
US9200375B2 (en) 2011-05-19 2015-12-01 Calera Corporation Systems and methods for preparation and separation of products
US9828313B2 (en) 2013-07-31 2017-11-28 Calera Corporation Systems and methods for separation and purification of products
US9957621B2 (en) 2014-09-15 2018-05-01 Calera Corporation Electrochemical systems and methods using metal halide to form products
US10266954B2 (en) 2015-10-28 2019-04-23 Calera Corporation Electrochemical, halogenation, and oxyhalogenation systems and methods
US10556848B2 (en) 2017-09-19 2020-02-11 Calera Corporation Systems and methods using lanthanide halide
US10590054B2 (en) 2018-05-30 2020-03-17 Calera Corporation Methods and systems to form propylene chlorohydrin from dichloropropane using Lewis acid
US10619254B2 (en) 2016-10-28 2020-04-14 Calera Corporation Electrochemical, chlorination, and oxychlorination systems and methods to form propylene oxide or ethylene oxide
WO2024218758A1 (fr) * 2023-04-20 2024-10-24 Karsten Schibsbye Système de génération d'électricité et de capture de dioxyde de carbone dans l'air
WO2025248508A1 (fr) 2024-05-31 2025-12-04 Karsten Schibsbye Pile à combustible industrialisée

Citations (28)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
FR1272625A (fr) * 1960-09-02 1961-09-29 Nat Res Dev élément de pile à gaz ou d'électrolyseur
FR1446698A (fr) * 1965-09-09 1966-07-22 Gen Electric Perfectionnements aux piles à combustibles
US3300345A (en) * 1964-09-03 1967-01-24 Jr Ernest H Lyons Electrolytic cell for producing electricity and method of operating the cell
US3338667A (en) 1963-12-02 1967-08-29 Johns Manville Recovery of silica, iron oxide and magnesium carbonate from the treatment of serpentine with ammonium bisulfate
GB1213777A (en) 1968-05-14 1970-11-25 Varta Ag Process for separating carbonate compounds from the alkaline electrolytes of fuel cells
US3826686A (en) * 1969-07-24 1974-07-30 Brunswick Corp Electrochemical electrodes
US4160856A (en) * 1974-01-25 1979-07-10 Societe Generale De Constructions Electriques Et Mecaniques"Alsthom Et Cie Novel fuel cell containing novel means for removal of carbonates
WO1990014694A1 (fr) * 1989-05-16 1990-11-29 Ab Olle Lindström Cellule electrochimique muni d'un recipient a combustible
US5004424A (en) 1987-10-20 1991-04-02 Johnson Matthey Public Limited Company Apparatus for demonstrating and studying the operation of a fuel cell
DE19921816C1 (de) * 1999-05-11 2000-10-26 Andre Peine Brennstoffzellen-System und Brennstoffzelle für derartiges System
US20030124408A1 (en) * 2001-12-28 2003-07-03 Matsushita Electric Industrial Co., Ltd. Fuel cell system
US20030165727A1 (en) 2000-03-24 2003-09-04 Priestnall Michael Alexander Mixed reactant fuel cells with flow through porous electrodes
US20040213705A1 (en) 2003-04-23 2004-10-28 Blencoe James G. Carbonation of metal silicates for long-term CO2 sequestration
US20040219090A1 (en) 2003-05-02 2004-11-04 Daniel Dziedzic Sequestration of carbon dioxide
US20050002847A1 (en) 2003-05-02 2005-01-06 The Penn State Research Foundation Process for sequestering carbon dioxide and sulfur dioxide
US20050180910A1 (en) 2003-12-31 2005-08-18 Ah-Hyung Park Carbon dioxide sequestration using alkaline earth metal-bearing minerals
US20060185985A1 (en) 2004-09-23 2006-08-24 Jones Joe D Removing carbon dioxide from waste streams through co-generation of carbonate and/or bicarbonate minerals
US20060210867A1 (en) * 2005-03-21 2006-09-21 Kenis Paul J Membraneless electrochemical cell and microfluidic device without pH constraint
US20060234098A1 (en) * 2005-04-18 2006-10-19 Clean Coal Energy, Llc Direct carbon fuel cell with molten anode
WO2006108532A1 (fr) 2005-04-08 2006-10-19 Cesarino Salomoni Capture de co2 et utilisation dans la digestion de matiere organique en vue de la production de methane
WO2007106883A2 (fr) 2006-03-15 2007-09-20 Carbon Trap Technologies, L.P. Procédés et systèmes de capture du dioxyde de carbone en utilisant des courants effluents
US20070261947A1 (en) 2005-11-23 2007-11-15 Geerlings Jacobus J C Process for Sequestration of Carbon Dioxide by Mineral Carbonation
WO2008018928A2 (fr) 2006-04-27 2008-02-14 President And Fellows Of Harvard College Capture de dioxyde de carbone et procédés associés
WO2008101293A1 (fr) 2007-02-20 2008-08-28 Hunwick Richard J Système, appareil et procédé de séquestration de dioxyde de carbone
WO2008142017A2 (fr) 2007-05-21 2008-11-27 Shell Internationale Research Maatschappij B.V. Procédé de séquestration de dioxyde de carbone par carbonatation minérale
US20090010827A1 (en) 2005-12-20 2009-01-08 Jacobus Johannes Cornelis Geerlings Process for Sequestration of Carbon Dioxide
US20090214408A1 (en) 2005-07-05 2009-08-27 Greensols Australia Pty Ltd Preparation and use of cationic halides, sequestration of carbon dioxide
WO2009139813A2 (fr) 2008-04-17 2009-11-19 Michigan Technological University Capture et séquestration de dioxyde de carbone dans des gaz de combustion

Patent Citations (29)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
FR1272625A (fr) * 1960-09-02 1961-09-29 Nat Res Dev élément de pile à gaz ou d'électrolyseur
US3338667A (en) 1963-12-02 1967-08-29 Johns Manville Recovery of silica, iron oxide and magnesium carbonate from the treatment of serpentine with ammonium bisulfate
US3300345A (en) * 1964-09-03 1967-01-24 Jr Ernest H Lyons Electrolytic cell for producing electricity and method of operating the cell
FR1446698A (fr) * 1965-09-09 1966-07-22 Gen Electric Perfectionnements aux piles à combustibles
GB1213777A (en) 1968-05-14 1970-11-25 Varta Ag Process for separating carbonate compounds from the alkaline electrolytes of fuel cells
US3826686A (en) * 1969-07-24 1974-07-30 Brunswick Corp Electrochemical electrodes
US4160856A (en) * 1974-01-25 1979-07-10 Societe Generale De Constructions Electriques Et Mecaniques"Alsthom Et Cie Novel fuel cell containing novel means for removal of carbonates
US5004424A (en) 1987-10-20 1991-04-02 Johnson Matthey Public Limited Company Apparatus for demonstrating and studying the operation of a fuel cell
WO1990014694A1 (fr) * 1989-05-16 1990-11-29 Ab Olle Lindström Cellule electrochimique muni d'un recipient a combustible
DE19921816C1 (de) * 1999-05-11 2000-10-26 Andre Peine Brennstoffzellen-System und Brennstoffzelle für derartiges System
US20030165727A1 (en) 2000-03-24 2003-09-04 Priestnall Michael Alexander Mixed reactant fuel cells with flow through porous electrodes
US20030124408A1 (en) * 2001-12-28 2003-07-03 Matsushita Electric Industrial Co., Ltd. Fuel cell system
US20040213705A1 (en) 2003-04-23 2004-10-28 Blencoe James G. Carbonation of metal silicates for long-term CO2 sequestration
US20080112868A1 (en) 2003-04-23 2008-05-15 Ut-Battelle, Llc Carbonation of metal silicates for long-term co2 sequestration
US20050002847A1 (en) 2003-05-02 2005-01-06 The Penn State Research Foundation Process for sequestering carbon dioxide and sulfur dioxide
US20040219090A1 (en) 2003-05-02 2004-11-04 Daniel Dziedzic Sequestration of carbon dioxide
US20050180910A1 (en) 2003-12-31 2005-08-18 Ah-Hyung Park Carbon dioxide sequestration using alkaline earth metal-bearing minerals
US20060185985A1 (en) 2004-09-23 2006-08-24 Jones Joe D Removing carbon dioxide from waste streams through co-generation of carbonate and/or bicarbonate minerals
US20060210867A1 (en) * 2005-03-21 2006-09-21 Kenis Paul J Membraneless electrochemical cell and microfluidic device without pH constraint
WO2006108532A1 (fr) 2005-04-08 2006-10-19 Cesarino Salomoni Capture de co2 et utilisation dans la digestion de matiere organique en vue de la production de methane
US20060234098A1 (en) * 2005-04-18 2006-10-19 Clean Coal Energy, Llc Direct carbon fuel cell with molten anode
US20090214408A1 (en) 2005-07-05 2009-08-27 Greensols Australia Pty Ltd Preparation and use of cationic halides, sequestration of carbon dioxide
US20070261947A1 (en) 2005-11-23 2007-11-15 Geerlings Jacobus J C Process for Sequestration of Carbon Dioxide by Mineral Carbonation
US20090010827A1 (en) 2005-12-20 2009-01-08 Jacobus Johannes Cornelis Geerlings Process for Sequestration of Carbon Dioxide
WO2007106883A2 (fr) 2006-03-15 2007-09-20 Carbon Trap Technologies, L.P. Procédés et systèmes de capture du dioxyde de carbone en utilisant des courants effluents
WO2008018928A2 (fr) 2006-04-27 2008-02-14 President And Fellows Of Harvard College Capture de dioxyde de carbone et procédés associés
WO2008101293A1 (fr) 2007-02-20 2008-08-28 Hunwick Richard J Système, appareil et procédé de séquestration de dioxyde de carbone
WO2008142017A2 (fr) 2007-05-21 2008-11-27 Shell Internationale Research Maatschappij B.V. Procédé de séquestration de dioxyde de carbone par carbonatation minérale
WO2009139813A2 (fr) 2008-04-17 2009-11-19 Michigan Technological University Capture et séquestration de dioxyde de carbone dans des gaz de combustion

Non-Patent Citations (2)

* Cited by examiner, † Cited by third party
Title
CARBON DIOXIDE STORAGE BY MINERAL CARBONATION
ELTON CAIRNS, HANDBOOK OF FUEL CELLS, vol. 1, pages 301

Cited By (16)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
EP2525896A4 (fr) * 2010-01-22 2014-02-19 Univ Rutgers Séquestration d'un gaz émis par une usine industrielle
US9957623B2 (en) 2011-05-19 2018-05-01 Calera Corporation Systems and methods for preparation and separation of products
US9187835B2 (en) 2011-05-19 2015-11-17 Calera Corporation Electrochemical systems and methods using metal and ligand
US9187834B2 (en) 2011-05-19 2015-11-17 Calera Corporation Electrochemical hydroxide systems and methods using metal oxidation
US9200375B2 (en) 2011-05-19 2015-12-01 Calera Corporation Systems and methods for preparation and separation of products
US10287223B2 (en) 2013-07-31 2019-05-14 Calera Corporation Systems and methods for separation and purification of products
US9828313B2 (en) 2013-07-31 2017-11-28 Calera Corporation Systems and methods for separation and purification of products
US9957621B2 (en) 2014-09-15 2018-05-01 Calera Corporation Electrochemical systems and methods using metal halide to form products
US10266954B2 (en) 2015-10-28 2019-04-23 Calera Corporation Electrochemical, halogenation, and oxyhalogenation systems and methods
US10844496B2 (en) 2015-10-28 2020-11-24 Calera Corporation Electrochemical, halogenation, and oxyhalogenation systems and methods
US10619254B2 (en) 2016-10-28 2020-04-14 Calera Corporation Electrochemical, chlorination, and oxychlorination systems and methods to form propylene oxide or ethylene oxide
US10556848B2 (en) 2017-09-19 2020-02-11 Calera Corporation Systems and methods using lanthanide halide
US10590054B2 (en) 2018-05-30 2020-03-17 Calera Corporation Methods and systems to form propylene chlorohydrin from dichloropropane using Lewis acid
US10807927B2 (en) 2018-05-30 2020-10-20 Calera Corporation Methods and systems to form propylene chlorohydrin from dichloropropane using lewis acid
WO2024218758A1 (fr) * 2023-04-20 2024-10-24 Karsten Schibsbye Système de génération d'électricité et de capture de dioxyde de carbone dans l'air
WO2025248508A1 (fr) 2024-05-31 2025-12-04 Karsten Schibsbye Pile à combustible industrialisée

Also Published As

Publication number Publication date
GB0921881D0 (en) 2010-01-27
GB201010672D0 (en) 2010-08-11

Similar Documents

Publication Publication Date Title
WO2011073621A1 (fr) Système de pile à combustible
EP3978434B1 (fr) Dispositif de production de gaz, système de production de gaz, système de production de fer, système de production de produit chimique et procédé de production de gaz
JP5005664B2 (ja) 二酸化炭素のメチルアルコール及び関連酸素化物又は炭化水素への再生
US8828216B2 (en) Efficient production of fuels
CN101835726B (zh) 制备氮肥的电化学方法
US20230126394A1 (en) Electrochemical system with an electrochemical stack for carbon dioxide capture and regeneration
US20110083968A1 (en) Low-voltage alkaline production using hydrogen and electrocatalytic electrodes
US8444846B2 (en) Method and system for producing hydrogen using sodium ion separation membranes
CN103154323A (zh) 用于制备氮肥的电化学方法
US20150080483A1 (en) Power station-based methanation system
CN114349029B (zh) 一种生产高纯碳酸盐的解耦式二氧化碳矿化膜电解系统
Oarga-Mulec et al. Back to the future with emerging iron technologies
US20250382710A1 (en) Low voltage electrolyzer and methods of using thereof
CN114497668B (zh) 一种解耦式二氧化碳矿化发电系统及其矿化发电的方法
US7955749B2 (en) Carbon-fueled fuel cell
KR102305659B1 (ko) 통합 공정 기반 이산화탄소 광물화 장치 및 방법
Cavaliere Hydrogen from electrolysis
KR102305660B1 (ko) 무기 폐기물을 이용한 통합 공정 기반 이산화탄소 광물화 장치 및 방법
CN110311146B (zh) 一种利用有机物作催化剂的二氧化碳矿化发电方法
JP2023085880A (ja) 二酸化炭素処理装置
Giaconia et al. 5 Development perspective for green hydrogen production
US20240166537A1 (en) Electrochemical hydrogen-looping system for low-cost co2 capture from seawater
KR102744183B1 (ko) 이산화탄소 전환시스템
US20240416275A1 (en) Accelerated co2 removal by electrochemical ocean alkalinity enhancement coupled with direct air capture
EP4534732A1 (fr) Appareil de production de monoxyde de carbone, appareil d'électrolyse de dioxyde de carbone et procédé d'électrolyse de dioxyde de carbone

Legal Events

Date Code Title Description
121 Ep: the epo has been informed by wipo that ep was designated in this application

Ref document number: 10801211

Country of ref document: EP

Kind code of ref document: A1

NENP Non-entry into the national phase

Ref country code: DE

122 Ep: pct application non-entry in european phase

Ref document number: 10801211

Country of ref document: EP

Kind code of ref document: A1