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WO2019023414A1 - Procédé cyclique utilisant des solutions alcalines créées à partir d'eau électrolytiquement décarboxylée en tant que collecteur de co2 atmosphérique suivi d'une récupération électrochimique de co2 répétée avec production simultanée de dihydrogène - Google Patents

Procédé cyclique utilisant des solutions alcalines créées à partir d'eau électrolytiquement décarboxylée en tant que collecteur de co2 atmosphérique suivi d'une récupération électrochimique de co2 répétée avec production simultanée de dihydrogène Download PDF

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Publication number
WO2019023414A1
WO2019023414A1 PCT/US2018/043811 US2018043811W WO2019023414A1 WO 2019023414 A1 WO2019023414 A1 WO 2019023414A1 US 2018043811 W US2018043811 W US 2018043811W WO 2019023414 A1 WO2019023414 A1 WO 2019023414A1
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compartment
effluent
hydroxide
solution
atmosphere
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Heather D. Willauer
Dennis R. Hardy
Felice Dimascio
Frederick Williams
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US Department of Navy
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US Department of Navy
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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
    • C25B1/14—Alkali metal compounds
    • B—PERFORMING OPERATIONS; TRANSPORTING
    • B01—PHYSICAL OR CHEMICAL PROCESSES OR APPARATUS IN GENERAL
    • B01D—SEPARATION
    • B01D53/00—Separation of gases or vapours; Recovering vapours of volatile solvents from gases; Chemical or biological purification of waste gases, e.g. engine exhaust gases, smoke, fumes, flue gases, aerosols
    • B01D53/14—Separation of gases or vapours; Recovering vapours of volatile solvents from gases; Chemical or biological purification of waste gases, e.g. engine exhaust gases, smoke, fumes, flue gases, aerosols by absorption
    • B—PERFORMING OPERATIONS; TRANSPORTING
    • B01—PHYSICAL OR CHEMICAL PROCESSES OR APPARATUS IN GENERAL
    • B01D—SEPARATION
    • B01D53/00—Separation of gases or vapours; Recovering vapours of volatile solvents from gases; Chemical or biological purification of waste gases, e.g. engine exhaust gases, smoke, fumes, flue gases, aerosols
    • B01D53/14—Separation of gases or vapours; Recovering vapours of volatile solvents from gases; Chemical or biological purification of waste gases, e.g. engine exhaust gases, smoke, fumes, flue gases, aerosols by absorption
    • B01D53/1425—Regeneration of liquid absorbents
    • B—PERFORMING OPERATIONS; TRANSPORTING
    • B01—PHYSICAL OR CHEMICAL PROCESSES OR APPARATUS IN GENERAL
    • B01D—SEPARATION
    • B01D53/00—Separation of gases or vapours; Recovering vapours of volatile solvents from gases; Chemical or biological purification of waste gases, e.g. engine exhaust gases, smoke, fumes, flue gases, aerosols
    • B01D53/14—Separation of gases or vapours; Recovering vapours of volatile solvents from gases; Chemical or biological purification of waste gases, e.g. engine exhaust gases, smoke, fumes, flue gases, aerosols by absorption
    • B01D53/1456—Removing acid components
    • B01D53/1475—Removing carbon dioxide
    • B—PERFORMING OPERATIONS; TRANSPORTING
    • B01—PHYSICAL OR CHEMICAL PROCESSES OR APPARATUS IN GENERAL
    • B01D—SEPARATION
    • B01D53/00—Separation of gases or vapours; Recovering vapours of volatile solvents from gases; Chemical or biological purification of waste gases, e.g. engine exhaust gases, smoke, fumes, flue gases, aerosols
    • B01D53/14—Separation of gases or vapours; Recovering vapours of volatile solvents from gases; Chemical or biological purification of waste gases, e.g. engine exhaust gases, smoke, fumes, flue gases, aerosols by absorption
    • B01D53/1493—Selection of liquid materials for use as absorbents
    • C—CHEMISTRY; METALLURGY
    • C10—PETROLEUM, GAS OR COKE INDUSTRIES; TECHNICAL GASES CONTAINING CARBON MONOXIDE; FUELS; LUBRICANTS; PEAT
    • C10G—CRACKING HYDROCARBON OILS; PRODUCTION OF LIQUID HYDROCARBON MIXTURES, e.g. BY DESTRUCTIVE HYDROGENATION, OLIGOMERISATION, POLYMERISATION; RECOVERY OF HYDROCARBON OILS FROM OIL-SHALE, OIL-SAND, OR GASES; REFINING MIXTURES MAINLY CONSISTING OF HYDROCARBONS; REFORMING OF NAPHTHA; MINERAL WAXES
    • C10G2/00—Production of liquid hydrocarbon mixtures of undefined composition from oxides of carbon
    • C10G2/50—Production of liquid hydrocarbon mixtures of undefined composition from oxides of carbon from carbon dioxide with hydrogen
    • 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
    • C25B1/00—Electrolytic production of inorganic compounds or non-metals
    • C25B1/01—Products
    • C25B1/14—Alkali metal compounds
    • C25B1/16—Hydroxides
    • 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
    • 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
    • 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
    • C25B9/70—Assemblies comprising two or more cells
    • C25B9/73—Assemblies comprising two or more cells of the filter-press type
    • B—PERFORMING OPERATIONS; TRANSPORTING
    • B01—PHYSICAL OR CHEMICAL PROCESSES OR APPARATUS IN GENERAL
    • B01D—SEPARATION
    • B01D2251/00—Reactants
    • B01D2251/30—Alkali metal compounds
    • B01D2251/304—Alkali metal compounds of sodium
    • B—PERFORMING OPERATIONS; TRANSPORTING
    • B01—PHYSICAL OR CHEMICAL PROCESSES OR APPARATUS IN GENERAL
    • B01D—SEPARATION
    • B01D2251/00—Reactants
    • B01D2251/60—Inorganic bases or salts
    • B01D2251/606—Carbonates
    • B—PERFORMING OPERATIONS; TRANSPORTING
    • B01—PHYSICAL OR CHEMICAL PROCESSES OR APPARATUS IN GENERAL
    • B01D—SEPARATION
    • B01D2252/00—Absorbents, i.e. solvents and liquid materials for gas absorption
    • B01D2252/10—Inorganic absorbents
    • B01D2252/103—Water
    • B01D2252/1035—Sea water
    • B—PERFORMING OPERATIONS; TRANSPORTING
    • B01—PHYSICAL OR CHEMICAL PROCESSES OR APPARATUS IN GENERAL
    • B01D—SEPARATION
    • B01D2258/00—Sources of waste gases
    • B01D2258/06—Polluted air
    • 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
    • Y02C—CAPTURE, STORAGE, SEQUESTRATION OR DISPOSAL OF GREENHOUSE GASES [GHG]
    • Y02C20/00—Capture or disposal of greenhouse gases
    • Y02C20/40—Capture or disposal of greenhouse gases of CO2
    • 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
    • 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
    • Y02P—CLIMATE CHANGE MITIGATION TECHNOLOGIES IN THE PRODUCTION OR PROCESSING OF GOODS
    • Y02P20/00—Technologies relating to chemical industry
    • Y02P20/151—Reduction of greenhouse gas [GHG] emissions, e.g. CO2

Definitions

  • the present invention relates to processing seawater or alkaline solutions for repeated recovery of CO2 to be used as feedstock to synthesize fuel.
  • Carbon dioxide (CO2) is reported to be a cause of climate change and responsible for ocean acidification as the world's oceans uptake CO2 by hydrolysis. Ocean acidification and decline in the oceans' carbonate-ion concentration is deteriorating coral reefs and impacting shell-forming marine organisms. (Orr et al., "Anthropogenic ocean acidification over the twenty-first century and its impact ion calcifying organisms, Nature, 437, 681-686 (2005) and Hoegh-Guldbergo Mumby et al, "Coral Reefs Under Rapid climate Change and Ocean Acidification,” Science, 318, 1737-1742 (2007)).
  • Patent 9,303,323 to DiMascio et al. (April 5, 2016); Willauer et al, "Development of an Electrolytic Cation Exchange Module for the Simultaneous Extraction of Carbon Dioxide and Hydrogen Gas from Natural Seawater,” Energy Fuels, 31, 1723-1730 (2017); and U.S. Patent 9,719,178 to DiMascio et al. (August 1, 2017)).
  • Johnson, et al. demonstrated that when the pH of seawater is decreased to 6 or less, carbonate and bicarbonate in the seawater are re-equilibrated to CC gas (equation 2).
  • Johnson et al "Coulometric TCC Analyses for Marine Studies: An
  • the O2 gas is flushed from the anode compartment with the flow of the anolyte water.
  • the H + ions are driven from the surface of the anode, through the cation-permeable membrane, and into the center compartment where they replace the Na + in the flowing seawater. This causes the effluent seawater to be acidified without the need for any additional chemicals.
  • the bicarbonate and carbonate in the seawater are re- equilibrated to carbonic acid (equation 4).
  • the industrial state of the art is to use strong alkaline solutions for the chemical absorption of CO2 from air or stack gas into amine-based solvents such as mono-ethanol-amine (MEA).
  • MEA is highly volatile, highly corrosive, and degrades over time.
  • alkaline solutions are very energy intensive because they cannot be regenerated from carbonate and bicarbonate solution created by chemical absorption of CO2. (Yoo et al, J. Envi. Mang , 53, 512-219 (2013); Mahmoudkhani et al, Inter. J. Green Gas. Cant. , 3, 376-384 (2009); and Baciocchi et al, Chem. Eng. Pro , 1047-1058 (2006)).
  • the present invention provides controlled removal of bicarbonate and carbonate (in the form of a weak acid, H2CO3) from either natural or synthetic alkaline water solutions and its replacement with a strong base containing hydroxide (e.g. sodium hydroxide) that is capable of rapidly chemically absorbing CO2 from the atmosphere as, e.g., NaHC03 solution.
  • a strong base containing hydroxide e.g. sodium hydroxide
  • NaHC03 solution can then be reprocessed by the electrolytic cation exchange module (E-CEM) to take advantage of the removal of CO2 from the air, as an energetic by-product of E-CEM dihydrogen production. This process is cyclical in nature, and no chemicals are needed except the initial alkaline water solution.
  • Carbon serves as one of the principle building blocks needed to synthesize hydrocarbon fuel.
  • inorganic carbon (CO2) from alkaline water sources is removed, a much stronger alkaline solution is formed that is capable of re-equilibrating with CO2 from the atmosphere by chemical absorption to the alkaline water that can be subsequently electrolytically reprocessed for CO2 recovery.
  • the controlled removal of bicarbonate from alkaline water and replacement with hydroxide that promotes the formation of carbonates upon chemical adsorption of CO2 is a potential solution to ocean acidification.
  • the feedstocks will produce renewable hydrocarbons that are superior in performance to fossil derived hydrocarbons and are drop in replacements for all current engines.
  • Alkaline solutions can be defined in this disclosure to include artificial solutions of carbonate, bicarbonate, and hydroxide produced from, e.g., sodium hydroxide, sodium carbonate, and sodium bicarbonate to be processed by the E-CEM for CO2 harvesting.
  • FIG. 1 is a diagram of an electrolytic cation exchange module (E-CEM).
  • FIGS. 2A and 2B show CO2 absorption in 0.05 molar NaOH as a function of time (open circles stirred).
  • FIG. 2A shows how the pH decreased as a function of time.
  • FIG. 2B shows the measured CO2 absorbed in mg/L by coulometry as a function of time.
  • FIG. 3 is a carbonate species equilibrium diagram.
  • FIGS. 4 A and 4B show CO2 absorption in an electrolytic cation exchange module (E- CEM) effluent on a laboratory scale.
  • FIG. 4A shows how the pH decreased as a function of time.
  • FIG. 4B shows the measured CO2 absorbed in mg/L as a function of time.
  • FIGS. 5 A and 5B show CO2 absorption in an E-CEM effluent on a laboratory scale using a larger scale E-CEM.
  • FIG. 5A shows how the pH decreased as a function of time.
  • FIG. 5B shows the measured CO2 absorbed in mg/L as a function of time.
  • the present invention provides a cyclic process using alkaline solutions created from electrolytically decarboxylated water as an atmospheric CO2 collector followed by repeated electrochemical recovery of CO2 with simultaneous production of dihydrogen for liquid hydrocarbon synthesis as stored energy.
  • inorganic carbon ([C02]T) from alkaline water sources is removed, a much stronger alkaline solution is formed that is capable of re- equilibrating with CO2 from the atmosphere by chemical absorption so that the alkaline water can be reprocessed electrochemically.
  • This cyclical direct CO2 capture and recovery from air and simultaneous production of dihydrogen is the central feature of this invention.
  • Re-equilibrated cathodic alkaline solutions can be repeatedly reprocessed for CCh recovery from the atmosphere.
  • the entire process requires only a source of electricity (no chemicals) and alkaline water to produce the alkaline hydroxide absorbent solutions for recovery of CCh from the atmosphere.
  • FIG. 1 shows a diagram of the E-CEM, which comprises an anode, an anode
  • a cation membrane separating the anode compartment and a center compartment, another cation membrane separating the center compartment and a cathode compartment, and a cathode adjacent to the cathode compartment.
  • An alkaline solution is fed to the center compartment, water is fed to both the anode compartment and the cathode compartment, and a source of electricity is applied to the anode.
  • Ch is formed in the anode compartment
  • CCh is formed in the center compartment
  • H2 and NaOH are formed in the cathode compartment.
  • the CO2 formed in center compartment and the H2 formed in the cathode compartment are removed to be used as a feedstock to synthesize fuel.
  • the effluent from the cathode compartment comprising NaOH is collected. This effluent absorbs CCh from the atmosphere to form a re-equilibrated solution that can be fed back into the center compartment of the E-CEM.
  • Faraday's constant is defined as the amount of electricity associated with one mole of unit charge or electron, having the value 96,487 ampere-second/equivalent.
  • 96,487 A sec will produce 1 ⁇ 4 mole O2 gas and 1 mole H +
  • 96,487 A sec will produce 1 ⁇ 2 mole H2 gas and 1 mole OH " .
  • seawater with a HCO3 " concentration of 142 ppm (0.0023 M) and a flow rate of 1900 milliliters per minute will require a theoretical applied minimum current of 7.0 A to lower the pH to less than 6.0 and convert HCCb " to H2CO3 (equation 12).
  • the theoretical amount of CO2 that can be removed from the acidified seawater is 0.0023 moles per liter.
  • the theoretical amount of H2 gas generated at 7.0 A is
  • Equations 8-13 describe the ability to control the removal of a weak base (HCO3 " ) in the form of a weak acid H2CO3 (equations 4 and 5) from seawater and its replacement with a strong base using applied current.
  • the strong base is produced by the primary ionized species in the cathode effluent water (equation 6) that consists of OH " and Na + .
  • the Na + comes from the seawater or alkaline solution processed in the center compartment of the E-CEM.
  • the Na + ion is 8 to 10 times more concentrated in seawater than the other ions present Mg 2+ , Ca 2+ , and K + on a mole per liter basis.
  • FIGS. 2A and 2B demonstrate the absorption of CO2 into 0.05 molar NaOH solutions left open to the atmosphere in a five gallon bucket (11.25" in diameter by 14.25" high) for 385 hours.
  • FIG. 2A shows how the pH of both 2 liter solutions decreased as a function of time and the effect of stirring the solution (open circles) on absorption was minimal.
  • FIG. 2B provides the measured CO2 absorbed in mg/L by coulometry as a function of time in both 0.05 molar solutions.
  • the simple NaOH solutions provide a timeframe for CO2 absorption from the atmosphere that contains only 0.7 to 0.8 mg of CO2 per liter of air. These solutions provide a means of concentrating over 1000 times that of the atmosphere as shown in FIG. 2B.
  • the speciation diagram shown in FIG. 3 suggests that Na2C03 is the primary product formed above pH 10.3. (Fleischer et al, "Detailed Modeling of The Chemisorption of CO2 Into NaOH In A Bubble Column,” Chemical Engineering Science, 51, 1715-1724 (1996)). As CO2 is absorbed and the pH of the solution begins to fall, bicarbonate is the primary product.
  • FIGS. 4 A and 4B demonstrate CO2 absorption into combined effluent from the E-CEM process.
  • Key West seawater was processed through a laboratory E-CEM unit at a flow rate of 140 mL/min and deionized water flowrate to the anode and cathode of 14 mL/min and 12 mL/min.
  • the initial pH of the seawater was 8.03 and was reduced to 3.6.
  • the effluent solutions were collected at a pH of 3.6 for approximately 20 minutes.
  • the acidified seawater was sparged with nitrogen.
  • the solutions were combined and measured at an initial pH of 10.5 (FIG. 4A) and CO2 content of 9.66 mg/L (FIG. 4B). Samples were collected over twenty two hours and it was found that the pH of the combined effluents reduced to as low as 9.5 (FIG. 4A) and the [C02]T measured as high as 33.41 mg/L.
  • West seawater was processed through a larger scale E-CEM at 0.5 gpm and electrode flowrates up to 0.042 gpm.
  • the effluent solutions were collected and combined under three separate experimental conditions.
  • the initial pH of the seawater before processing was 8.3.
  • the E-CEM effluent streams were collected for 160 minutes. This equates to five thirty-minute polarity cycles.
  • a polarity cycle is defined by the length of time an electrode is functioning as an anode/or cathode before the polarity in the module is switched and the electrode acting as the anode/or cathode becomes the cathode/or anode.
  • Polarity switching is a common practice in the Electrodialysis Reversal (EDR) process to desalinate brackish ground and surface waters and it is designed into this system to provide electrode regeneration at regular intervals called polarity cycles. (Dermentzis, "Continuous electrodeionization through electrostatic shielding," Electrochim. Acta, 53, 2953-2962 (2008)).
  • FIGS. 5A and 5B show that the pH and % CO2 of the combined processed water measured 9.3 and 19.0% (Large Pool filled black circles). After sixty-nine hours the [C02]T content increased to 55% and the pH dropped to 9.0.
  • FIGS. 5A and 5B show the combined effluent pH initially measured approximately 9 for each pool.
  • the third experiment collected effluent from the E-CEM for two polarity cycles in a 32 gallon bucket that was 1.6 feet in diameter. This container had the smallest surface to volume ratio of all three experiments.
  • the initial pH and % CC of the combined effluents from the E- CEM measured 9.2 and 7.7 %.
  • the final pH and % CCh measured 8.5 and 29.1% after 219 hours.
  • Table 2 shows the final pH of the catholyte solution measured an average of 13.5 which equates to 0.5 mol/L of NaOH available for absorption of CO2 from the atmosphere. At these lower electrode flowrates the catholyte solution is more concentrated causing an increase in pH by approximately 1 pH unit. At these flowrates the catholyte was passed through a PVC column and treated with air at a flow rate of 4 1pm at a space time of 16 minutes. The pH of the catholyte dropped to an average of 13.2.

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  • Engineering & Computer Science (AREA)
  • Organic Chemistry (AREA)
  • Electrochemistry (AREA)
  • Materials Engineering (AREA)
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  • Oil, Petroleum & Natural Gas (AREA)
  • General Chemical & Material Sciences (AREA)
  • Analytical Chemistry (AREA)
  • Inorganic Chemistry (AREA)
  • Electrolytic Production Of Non-Metals, Compounds, Apparatuses Therefor (AREA)
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Abstract

La présente invention concerne un procédé d'élimination contrôlée de bicarbonate à partir d'eau alcaline et de son remplacement par une base forte qui est capable d'absorber chimiquement du CO2 à partir de l'atmosphère sous la forme d'une solution de carbonate et de bicarbonate. Cette solution de bicarbonate et de carbonate est retraitée dans le compartiment central d'un module d'échange de cations électrolytique (E-CEM) pour tirer profit de l'élimination de CO2 à partir de l'air, et en tant que sous-produit énergétique de production de dihydrogène par E-CEM, et pour régénérer la solution absorbante de base forte initiale. Par conséquent, ce procédé est de nature cyclique, et aucun produit chimique n'est nécessaire à l'exception d'une source initiale d'eau alcaline.
PCT/US2018/043811 2017-07-26 2018-07-26 Procédé cyclique utilisant des solutions alcalines créées à partir d'eau électrolytiquement décarboxylée en tant que collecteur de co2 atmosphérique suivi d'une récupération électrochimique de co2 répétée avec production simultanée de dihydrogène Ceased WO2019023414A1 (fr)

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US10717044B1 (en) * 2019-09-09 2020-07-21 Saudi Arabian Oil Company Multi-pollutant exhaust treatment using seawater for marine applications
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CN117165956A (zh) * 2022-05-25 2023-12-05 势加透博（北京）科技有限公司 二氧化碳捕集与纯化的方法及系统
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