EP2643489A1 - Extraction de métaux alcalins et/ou de métaux alcalino-terreux pour utilisation dans la séquestration du carbone - Google Patents

Extraction de métaux alcalins et/ou de métaux alcalino-terreux pour utilisation dans la séquestration du carbone

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Publication number
EP2643489A1
EP2643489A1 EP11843209.5A EP11843209A EP2643489A1 EP 2643489 A1 EP2643489 A1 EP 2643489A1 EP 11843209 A EP11843209 A EP 11843209A EP 2643489 A1 EP2643489 A1 EP 2643489A1
Authority
EP
European Patent Office
Prior art keywords
mineral
alkaline earth
earth metal
formic acid
dissolution
Prior art date
Legal status (The legal status is an assumption and is not a legal conclusion. Google has not performed a legal analysis and makes no representation as to the accuracy of the status listed.)
Withdrawn
Application number
EP11843209.5A
Other languages
German (de)
English (en)
Inventor
Bogdan Z Dlugogorski
Manisha Ghoorah
Eric M Kennedy
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.)
Newcastle Innovation Ltd
Original Assignee
Newcastle Innovation Ltd
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
Priority claimed from AU2010905241A external-priority patent/AU2010905241A0/en
Application filed by Newcastle Innovation Ltd filed Critical Newcastle Innovation Ltd
Publication of EP2643489A1 publication Critical patent/EP2643489A1/fr
Withdrawn legal-status Critical Current

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Classifications

    • C—CHEMISTRY; METALLURGY
    • C22—METALLURGY; FERROUS OR NON-FERROUS ALLOYS; TREATMENT OF ALLOYS OR NON-FERROUS METALS
    • C22B—PRODUCTION AND REFINING OF METALS; PRETREATMENT OF RAW MATERIALS
    • C22B26/00—Obtaining alkali, alkaline earth metals or magnesium
    • C22B26/20—Obtaining alkaline earth metals or magnesium
    • 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
    • B01D53/34—Chemical or biological purification of waste gases
    • B01D53/46—Removing components of defined structure
    • B01D53/62—Carbon oxides
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
    • C01B32/00—Carbon; Compounds thereof
    • C01B32/60—Preparation of carbonates or bicarbonates in general
    • C—CHEMISTRY; METALLURGY
    • C22—METALLURGY; FERROUS OR NON-FERROUS ALLOYS; TREATMENT OF ALLOYS OR NON-FERROUS METALS
    • C22B—PRODUCTION AND REFINING OF METALS; PRETREATMENT OF RAW MATERIALS
    • C22B26/00—Obtaining alkali, alkaline earth metals or magnesium
    • C22B26/10—Obtaining alkali metals
    • C—CHEMISTRY; METALLURGY
    • C22—METALLURGY; FERROUS OR NON-FERROUS ALLOYS; TREATMENT OF ALLOYS OR NON-FERROUS METALS
    • C22B—PRODUCTION AND REFINING OF METALS; PRETREATMENT OF RAW MATERIALS
    • C22B3/00—Extraction of metal compounds from ores or concentrates by wet processes
    • C22B3/04—Extraction of metal compounds from ores or concentrates by wet processes by leaching
    • C22B3/16—Extraction of metal compounds from ores or concentrates by wet processes by leaching in organic solutions
    • C22B3/1608—Leaching with acyclic or carbocyclic agents
    • C22B3/1616—Leaching with acyclic or carbocyclic agents of a single type
    • C22B3/165—Leaching with acyclic or carbocyclic agents of a single type with organic acids
    • 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
    • B01D2251/30—Alkali metal compounds
    • B01D2251/306—Alkali metal compounds of potassium
    • B—PERFORMING OPERATIONS; TRANSPORTING
    • B01—PHYSICAL OR CHEMICAL PROCESSES OR APPARATUS IN GENERAL
    • B01D—SEPARATION
    • B01D2251/00—Reactants
    • B01D2251/40—Alkaline earth metal or magnesium compounds
    • B01D2251/402—Alkaline earth metal or magnesium compounds of magnesium
    • B—PERFORMING OPERATIONS; TRANSPORTING
    • B01—PHYSICAL OR CHEMICAL PROCESSES OR APPARATUS IN GENERAL
    • B01D—SEPARATION
    • B01D2251/00—Reactants
    • B01D2251/40—Alkaline earth metal or magnesium compounds
    • B01D2251/404—Alkaline earth metal or magnesium compounds of calcium
    • 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
    • B—PERFORMING OPERATIONS; TRANSPORTING
    • B01—PHYSICAL OR CHEMICAL PROCESSES OR APPARATUS IN GENERAL
    • B01D—SEPARATION
    • B01D2257/00—Components to be removed
    • B01D2257/50—Carbon oxides
    • B01D2257/504—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
    • B01D53/34—Chemical or biological purification of waste gases
    • B01D53/74—General processes for purification of waste gases; Apparatus or devices specially adapted therefor
    • B01D53/77—Liquid phase processes
    • B01D53/78—Liquid phase processes with gas-liquid contact
    • 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
    • Y02P—CLIMATE CHANGE MITIGATION TECHNOLOGIES IN THE PRODUCTION OR PROCESSING OF GOODS
    • Y02P10/00—Technologies related to metal processing
    • Y02P10/10—Reduction of greenhouse gas [GHG] emissions
    • Y02P10/146—Perfluorocarbons [PFC]; Hydrofluorocarbons [HFC]; Sulfur hexafluoride [SF6]
    • 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
    • Y02P10/00—Technologies related to metal processing
    • Y02P10/20—Recycling
    • 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 the extraction of alkali metals and/or alkaline earth metals from minerals, and rocks containing same, and to their, use in carbon sequestration.
  • Reaction rates for carbonation may be accelerated by decreasing the particle size of the minerals through pulverisation, raising reaction temperature and pressure, changing solution chemistry and using catalysts/additives.
  • One such attempt to increase reaction rates found that serpentine minerals are activated by heating to between 600 and 750 °C which removes part of the hydroxyl groups and amorphises the mineral structure, significantly increasing their reactivity to C0 2 (Balucan et al., 2010).
  • the most comprehensive studies so far Outline two thermodynamically feasible aqueous mineral carbonation approaches.
  • the first process developed by the Albany Research Centre, involves direct carbonation in aqueous solutions of 0.64 M NaHC0 3 and 1 M NaCl conducted at 150 bar C0 2 and 155 °C and 185 °C for heat pre-treated serpentine and olivine respectively (O'Connor et al., 2000, 2001).
  • the second approach (known as indirect carbonation) is based on two principal steps namely dissolution of the alkali metal or alkaline earth metal mineral to obtain the alkali metal or alkaline earth metal ions in solution, and subsequent carbonate precipitation (Oelkers and Scott, 2005). Since the former mechanism is generally assumed to be rate- limiting with respect to the overall carbonation process, many studies have focused on the extraction of calcium or magnesium from native minerals (Park and Fan, 2004; Carroll and Knauss, 2005; Hanchen et al., 2006).
  • Acid-aided dissolution where hydrochloric acid was used to leach out magnesium ions, was initially investigated by Lackner et al. (1995), This scenario was highly energy intensive and was thus phased out by a different process using acetic acid as an accelerating medium for the artificial weathering of wollastonite.
  • This acid was selected based on the thermodynamic consideration that the extraction acid must not only be stronger than silicic acid but also weaker than carbonic acid, such that the precipitation of carbonates occurs spontaneously (Kakizawa et al., 2001).
  • the present invention seeks to provide an alternative method of extracting alkali metals and alkaline earth metals from minerals and/or rocks containing same.
  • the present invention provides a method of extracting an alkali metal and/or an alkaline earth metal from a mineral including an alkali metal and/or an alkaline earth metal, or a rock containing the mineral, the method including contacting the mineral, with an aqueous composition including formic acid.
  • the mineral is a naturally occurring mineral.
  • the alkali metal is chosen from sodium or potassium. In one form the alkaline earth metal is chosen from calcium or magnesium.
  • the mineral is a silicate.
  • the mineral is chosen from an aluminosilicate or an alkaline earth metal silicate.
  • the aluminosilicate is a feldspar and includes sodium, potassium and/or calcium.
  • the alkaline earth metal silicate is chosen from olivine, enstatite, forsterite, serpentine and/or wollastonite.
  • the mineral, or the rock containing the mineral is crushed prior to contact with the aqueous composition including formic acid.
  • the mineral, or the rock containing the mineral is ground prior to contact with the aqueous composition including formic acid.
  • the mineral, or the rock containing the mineral has an average particle size of between 1 um to 250 um.
  • the composition including formic acid has a pH of between 1 and 1.8.
  • the aqueous composition is at a temperature of between about 20°C and about 95°C.
  • the aqueous composition is at a temperature of between about 75°C to about 85°C.
  • the present invention provides a process for the indirect carbonation of carbon dioxide the process including the following steps:
  • the carbonate is chosen from an alkaline earth metal carbonate and/or an alkali metal aluminium carbonate.
  • the present invention provides a use of formic acid for the extraction of an alkali metal or an alkaline earth metal from a mineral, or a rock containing the mineral.
  • Figure 1 illustrates the cumulative particle size distribution of wollastonite particles before and after acid dissolution before and after reaction at 80 °C, within 3 h and without pH control;
  • Figure 2 depicts X-ray diffraction (XRD) results confirming the presence of wollastonite as the major phase
  • Figure 3 illustrates the pH profile for dissolution in 0.1 formic acid
  • Figure 4 illustrates the pH profile for dissolution in 0.1 M acetic acid
  • Figure 5 illustrates the Extent of Ca extraction with increasing temperature in 3 h (pH 2.0-4.5;
  • Figure 6 illustrates the Concentration of aqueous species as calculated at thermodynamic equilibrium, at 80 °C and 1 atm (OLI Analyzer Studio 3.0); symbols are used only to identify each plot;
  • Figure 7 illustrates the Solid phase, composition and pH profile for the results presented in Figure 6(OLI Analyzer Studio 3.0); symbols are used only to identify each plot;
  • Figure 8 illustrates the Dissolution in formic acid at 80 °C and pH 1.04;
  • Figure 9 illustrates the Dissolution in acetic acid at 80 °C and pH 1.61 ;
  • Figure 10 illustrates the Dissolution in DL-lactic acid at 80 °C and pH 1.19.
  • Figure 1 1 is an Arrhenius plot of the initial dissolution rates. Description of Embodiments, Examples and the Accompanying Figures
  • 'formic acid' (also referred to in literature as methanioc acid) is used to denote the carboxylic acid of the chemical formula HCOOH.
  • the term 'indirect carbonation' refers to the two step process of extracting a reactive compound in a first step and subsequently carbonating the reactive compound in a second step.
  • the term 'a rock containing the mineral' includes any type of rock which may contain a mineral which includes an alkali metal or an alkaline earth metal such as for example peridotites, basalts, harzburgites and limburgites.
  • the resulting aqueous solution may pass to the second step of an indirect carbonation process where the aqueous solution including the alkali metal ions or the alkaline earth metal ions (eg, K + , Na + , Ca 2+ and Mg 2+ ) are contacted with carbon dioxide (typically in gaseous form) which then results in the precipitation of carbonates.
  • the alkali metal ions or the alkaline earth metal ions eg, K + , Na + , Ca 2+ and Mg 2+
  • carbon dioxide typically in gaseous form
  • These carbonates may be in the form of alkaline earth metal carbonates and/or an alkali metal aluminium carbonate as examples.
  • the temperature of the extraction reaction may be between 20°C and 95°C. The highest dissolution reaction rates were found when the temperature of the extraction reaction was maintained at about 80°C.
  • the pH of the aqueous composition including formic acid may be between 1 and 1.8. It was also found to be advantageous to crush the mineral, or the rock containing the mineral, prior to being contacted with the aqueous composition including formic acid. In addition to crushing the mineral, or the rock containing the mineral, an additional processing step of grinding the mineral, or the rock containing the mineral, may also be used to break the particles of the alkaline earth metal silicate down to a particle size of between 1 and 250 ⁇ and preferably a particle size of between 10 and 80 um.
  • VMD volume mean diameter
  • Figure 1 illustrates the cumulative particle size distribution of wollastonite particles before and after acid dissolution.
  • the average density of the starting material was 2.86 g/cm 3 while its specific surface area was determined to be 0.1 m 2 /g based on a low temperature N 2 adsorption BET method (Micromeritics Gemini).
  • X-ray diffraction (XRD) results confirmed the presence of wollastonite as the major phase ( Figure 2).
  • Diopside and pectolite, appearing as minor phases, are both metasilicates like wollastonite and crystallise in the monoclinic and triclinic systems respectively.
  • Table 1 lists the elemental composition derived from X-ray fluorescence (X F). Distributing the elemental abundances among minerals leads to approximate contents of 81.8% wollastonite (CaSi0 3 ), 9.2% diopside (MgCaSi 2 06), 4.6% silica (Si0 2 ), 1.9% pectolite CNaCa 2 Si 3 Og(OH)), and possibly 0.7% hedenbergite (FeCaSi 2 0 6 ); possibly with diopside and hedenbergite end members forming a solid solution. The remainder of about 0.5%, after accounting for the loss on ignition, seems to include mostly the aluminosilicate minerals.
  • Loss on ignition Wollastonite (CaSi0 3 ) dissolution experiments were performed in a three-neck glass reactor, immersed in a temperature-controlled water bath, equipped with a condenser to minimise solution losses due to evaporation. Two series of experiments were carried out in non-pH controlled and pH controlled systems to determine the extent of calcium extraction and the rates of dissolution, respectively.
  • the first set of experiments were conducted at temperatures ranging from 22 °C to 80 °C in an acidic leaching medium with a concentration of 0.1 M, for a total reaction time of 3 hours.
  • the analytical reagent grade formic and DL-lactic acids were purchased from Sigma Aldrich (Australia) while acetic acid was obtained from Ajax Finechem Pty Ltd (Australia). Acid solutions were prepared, in ultrapure deionised water with electrical resistivity of 18.2 ⁇ /cm, by standard volumetric dilution techniques. In-situ pH measurements, with an accuracy of ⁇ 0.01 , were taken by a Hanna pH probe and meter. Temperature control was achieved by using a water bath. Dispersion of the particles was accomplished through continuous stirring of the slurry by a magnetic stirrer.
  • Equations 1 - 3 illustrate the extraction of calcium from CaSi0 3 using formic acid (HCOOH - pK a 3.75), acetic acid (CH 3 COOH - pK a 4.76) and DL-lactic acid (CH 3 CHOHCOOH - pK, 3.86).
  • Reactions constitute an overall description of the dissolution process.
  • other ions will also exist, such as, for Reaction 1 , calcium monoformate Ca(HCOO)" and calcium formate Ca(HCOO) 2 , and, Reaction 2, calcium monoacetate Ca(CH 3 COO) ⁇ and calcium acetate Ca(CH 3 COO) 2 .
  • OLI Analyzer Studio 3.0 predicted only calcium ion (Ca ) for Reaction 3, due to the absence of thermodynamic data for calcium monolactate and calcium lactate in the database of the software.
  • the suspension was filtered through a 0.45 um PVDF membrane.
  • the filter cake was also analysed for its calcium content. Volumes of 4.5 mL of 65% HN0 3 , 4.5 mL of 37% HC1 and 3 mL of 50% HBF were added to 0.1 g of the dried solid residue prior to digestion in a Milestone start D microwave unit. Complete digestion was achieved after 1 h at 160 °C. The liquid was then analysed by ICP-OES.
  • FIGS 3 and 4 illustrate typical pH profiles as wollastonite dissolution proceeds in acidic medium.
  • the pH was found to vary in the range of 2.0 to 4.5. This process is characterised by the consumption of protons and the release of cations from the silicate mineral, resulting in the alkalisation of the reaction mixture thus increasing solution pH. Since dissolution is incongruent at such low pH (Schott et al, 2002), the concentration of calcium is expected to be much higher compared to other ions that could leach out, hence allowing an initial monitoring of the reaction course via the pH of the system.
  • the following equilibrium aqueous phase composition was predicted: 0.1 g Ca 2+ , 0.14 g calcium monoformate equivalent to 0.07 g Ca and 0.06 g calcium formate equivalent to 0.02 g Ca 2+ .
  • the total mass of calcium in solution amounts to 0.19 g, which represents 95% of the input mass.
  • a solid phase consisting of only silicon dioxide and pH range of 2.5-5 were also predicted.
  • Experimental data was found to be compatable with results from the simulation, except for the measurements of pH, which appear to be significantly lower in the experimental measurements than in thermodynamic predictions. The difference is as high as 1 pH unit at the end of an experiment.
  • the dissolution may proceed via the following steps, where -O-Ca-OH denotes surface calcium atoms terminated with hydroxyl groups:
  • Reactions 4 and 6 are pH dependent.
  • the ligands themselves may assist in the dissolution of wollastonite, say, via the following reaction
  • ligands The effectiveness of ligands depends both on the nature of their functional groups, molecular structure and thermodynamic stability of the transitional surface complexes they form (Pokrovsky et al, 2009).
  • Organic ligands such as acetate, lactate and formate are known to form monodentate complexes on oxides, which upon polarisation, labilise the Ca-0 bonds thereby facilitating the removal of calcium atoms from the crystal lattice (Swaddle, 1997).
  • the calcium-ligand complexes detach the surface, the underlying layers are exposed to further contact with the solvent.
  • the kinetic behaviour of the dissolution reactions displays an initial fast rate during the first 10 min followed by a slowdown, observed in all cases.
  • the dissolution rates can be considered to be surface controlled (i.e., film-diffusion or reaction- rate controlled) but the levelling off of calcium concentration in filtrates indicates a diffusion limitation (i.e., pore/crack-diffusion controlled) at the later part of the process (Park et al., 2003, Alexander et al., 2006).
  • a sixth degree polynomial to all measurements and applied that polynomial to estimate the rates at t - 0 min.
  • Table 3 summarises the rates of dissolution, which have been normalised to the specific surface area at the investigated temperatures. The highest initial rate has been recorded for formic acid at 80 °C.
  • the calculations are based on an estimate of the mineral surface area which is equal to the total mass of reacting material multiplied by the specific surface area per unit mass of material, as determined by the BET method. While some researchers have assumed that the surface area of the leached layer grew linearly with time (Stillings and Brantley, 1 95), others found that the surface area of their reacted wollastonite grains increased according • to a power law function (Weissbart and Rimstidt, 2000). The surface area certainly changes as the reaction proceeds but for this study, during the very onset of the reactions, when we made our measurements, it is the same as the BET surface area of the fresh particles.
  • A refers to a pre-exponential factor in mol m '2 s “1 (which is here a function of pH) and E a represents the activation energy, in kJ mol "1 , defined by
  • FIG. 1 1 illustrates an Arrhenius plot with the logarithm of the measured wollastonite dissolution rates on the ordinate and the reciprocal of temperature on the abscissa.
  • the activation energies are derived from the slopes of the straight lines that best fit the points, given by -£ a /2.303 R.
  • the calculated activation energies and pre-exponential factors are presented in Table 4. It should be noted that the term for temperature dependence denotes an apparent global activation energy because the dissolution of minerals is not a single elementary reaction but rather involves a complex series of reactions, each carrying their own activation energy (Lasaga, 1995).
  • the low activation energy for the formic acid implies mass transfer control for diffusion of H + and HCOO " in the aqueous film surrounding the reacting particles.
  • the ligand (HCOO " ) provides an effective, low activation energy pathway for solubilising Ca 2+ , as suggested by reaction 8.

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  • Oil, Petroleum & Natural Gas (AREA)
  • Chemical Kinetics & Catalysis (AREA)
  • Geochemistry & Mineralogy (AREA)
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  • Compounds Of Alkaline-Earth Elements, Aluminum Or Rare-Earth Metals (AREA)
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Abstract

L'invention concerne un procédé d'extraction d'un métal alcalin et/ou d'un métal alcalino-terreux à partir d'un minéral comprenant un métal alcalin et/ou un métal alcalino-terreux, ou d'une roche contenant le minéral. Le procédé consiste à mettre en contact le minéral avec une composition aqueuse comprenant de l'acide formique. L'invention concerne également l'utilisation desdits métaux dans la séquestration du carbone.
EP11843209.5A 2010-11-26 2011-11-25 Extraction de métaux alcalins et/ou de métaux alcalino-terreux pour utilisation dans la séquestration du carbone Withdrawn EP2643489A1 (fr)

Applications Claiming Priority (2)

Application Number Priority Date Filing Date Title
AU2010905241A AU2010905241A0 (en) 2010-11-26 Extraction of alkali metals and/or alkaline earth metals for use in carbon sequestration
PCT/AU2011/001537 WO2012068639A1 (fr) 2010-11-26 2011-11-25 Extraction de métaux alcalins et/ou de métaux alcalino-terreux pour utilisation dans la séquestration du carbone

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EP2643489A1 true EP2643489A1 (fr) 2013-10-02

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US (1) US20140065039A1 (fr)
EP (1) EP2643489A1 (fr)
CN (1) CN103415632A (fr)
AU (1) AU2011334545A1 (fr)
MX (1) MX2013005982A (fr)
WO (1) WO2012068639A1 (fr)

Families Citing this family (4)

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Publication number Priority date Publication date Assignee Title
US9963351B2 (en) * 2014-04-10 2018-05-08 Cambridge Carbon Capture Ltd Method and system of activation of mineral silicate minerals
CN109762997B (zh) * 2019-03-12 2021-02-02 中南大学 一种从难处理高硅富钪钨渣中提取钪的方法
DE102021116491A1 (de) 2021-06-25 2022-12-29 Rheinisch-Westfälische Technische Hochschule Aachen, Körperschaft des öffentlichen Rechts Karbonatisierungsverfahren und Karbonatisierungsmischung
AU2022373670A1 (en) 2021-10-18 2024-05-02 Project Vesta, PBC Carbon-removing sand and method and process for design, manufacture, and utilization of the same

Family Cites Families (8)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
CN1283581C (zh) * 2003-01-17 2006-11-08 中国地质大学（北京） 利用钾长石生产矿物聚合材料的方法
US20040213705A1 (en) * 2003-04-23 2004-10-28 Blencoe James G. Carbonation of metal silicates for long-term CO2 sequestration
US7722842B2 (en) * 2003-12-31 2010-05-25 The Ohio State University Carbon dioxide sequestration using alkaline earth metal-bearing minerals
KR101464010B1 (ko) * 2006-11-22 2014-11-20 오리카 익스플로시브스 테크놀로지 피티와이 리미티드 통합 화학 공정
CN101636224B (zh) * 2006-11-22 2012-11-14 澳瑞凯炸药技术有限公司 集成化学方法
CN101020577A (zh) * 2007-01-19 2007-08-22 华中科技大学 一种二氧化碳矿物化的方法
US7749476B2 (en) * 2007-12-28 2010-07-06 Calera Corporation Production of carbonate-containing compositions from material comprising metal silicates
CN101302010B (zh) * 2008-06-27 2011-10-26 刘启波 菱镁矿加工中副产二氧化碳联产碳酸盐及在污水处理中的应用方法

Non-Patent Citations (1)

* Cited by examiner, † Cited by third party
Title
See references of WO2012068639A1 *

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AU2011334545A1 (en) 2013-07-11
WO2012068639A1 (fr) 2012-05-31
MX2013005982A (es) 2014-07-28
CN103415632A (zh) 2013-11-27

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