WO2024258224A1 - Procédé de production d'hydroxyde de calcium à partir de calcaire ou d'un composé de calcium - Google Patents

Procédé de production d'hydroxyde de calcium à partir de calcaire ou d'un composé de calcium Download PDF

Info

Publication number
WO2024258224A1
WO2024258224A1 PCT/KR2024/008175 KR2024008175W WO2024258224A1 WO 2024258224 A1 WO2024258224 A1 WO 2024258224A1 KR 2024008175 W KR2024008175 W KR 2024008175W WO 2024258224 A1 WO2024258224 A1 WO 2024258224A1
Authority
WO
WIPO (PCT)
Prior art keywords
calcium hydroxide
weight
parts
producing calcium
paragraph
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/KR2024/008175
Other languages
English (en)
Korean (ko)
Inventor
허남회
박희선
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.)
Sogang University Research Foundation
Original Assignee
Sogang University Research Foundation
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 Sogang University Research Foundation filed Critical Sogang University Research Foundation
Publication of WO2024258224A1 publication Critical patent/WO2024258224A1/fr
Anticipated expiration legal-status Critical
Ceased legal-status Critical Current

Links

Images

Classifications

    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01F—COMPOUNDS OF THE METALS BERYLLIUM, MAGNESIUM, ALUMINIUM, CALCIUM, STRONTIUM, BARIUM, RADIUM, THORIUM, OR OF THE RARE-EARTH METALS
    • C01F11/00—Compounds of calcium, strontium, or barium
    • C01F11/02—Oxides or hydroxides
    • B—PERFORMING OPERATIONS; TRANSPORTING
    • B01—PHYSICAL OR CHEMICAL PROCESSES OR APPARATUS IN GENERAL
    • B01J—CHEMICAL OR PHYSICAL PROCESSES, e.g. CATALYSIS OR COLLOID CHEMISTRY; THEIR RELEVANT APPARATUS
    • B01J23/00—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00
    • B01J23/38—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00 of noble metals
    • B01J23/40—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00 of noble metals of the platinum group metals
    • B01J23/46—Ruthenium, rhodium, osmium or iridium
    • B—PERFORMING OPERATIONS; TRANSPORTING
    • B01—PHYSICAL OR CHEMICAL PROCESSES OR APPARATUS IN GENERAL
    • B01J—CHEMICAL OR PHYSICAL PROCESSES, e.g. CATALYSIS OR COLLOID CHEMISTRY; THEIR RELEVANT APPARATUS
    • B01J23/00—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00
    • B01J23/38—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00 of noble metals
    • B01J23/40—Catalysts comprising metals or metal oxides or hydroxides, not provided for in group B01J21/00 of noble metals of the platinum group metals
    • B01J23/46—Ruthenium, rhodium, osmium or iridium
    • B01J23/462—Ruthenium

Definitions

  • Calcium hydroxide (Ca(OH) 2 ) is a strong alkaline substance that is environmentally friendly and harmless to the human body, and is therefore widely used in various industries such as construction, iron and steel, water treatment, agriculture, and food.
  • calcium hydroxide is used to safely treat industrial waste, and since direct landfill of acidic industrial waste can cause fatal environmental disasters by contaminating the soil, calcium hydroxide is used as a neutralizing agent in the treatment process of large amounts of waste acid generated in steelmaking and metal refining processes. Recently, it has been used as a neutralizing agent in high-concentration acidic waste water containing phosphoric acid ( H3PO4 ) or hydrofluoric acid (HF) in the treatment of semiconductor process waste water.
  • H3PO4 phosphoric acid
  • HF hydrofluoric acid
  • Calcium hydroxide with low purity is used as a neutralizing agent for acid wastewater, an inorganic coagulant in water and sewage treatment, and a purifying agent in improving the water quality of lakes and rivers. Meanwhile, calcium hydroxide fine particles with a purity of 90% or higher are used to reduce air pollution and play a significant role in reducing pollutants such as sulfur oxides (SO x ), nitrogen oxides (NO x ), and carbon monoxide, which are environmental pollutants.
  • High-grade calcium hydroxide with a purity of 95% or higher and good color and powder shape is used as a food additive; or for refining sugar or raw sugar.
  • the conventional method for manufacturing calcium hydroxide is a relatively easy process of reacting calcium oxide (CaO) and water, as shown in the following reaction formula 1.
  • CaO calcium oxide
  • the raw material for manufacturing calcium hydroxide is manufactured by heat-treating limestone (CaCO 3 ) at a high temperature of 900°C or higher, the energy cost is high.
  • the conventional method for manufacturing calcium hydroxide is a process that emits a large amount of carbon dioxide, as shown in the following reaction formula 2, and thus has the problem of large greenhouse gas emissions.
  • limestone the raw material ore of calcium hydroxide
  • Patent Document 1 Republic of Korea Patent Publication No. 10-2013-7025562.
  • the present invention provides a method for producing calcium hydroxide from limestone or a calcium compound.
  • the first aspect of the present invention provides a method for producing calcium hydroxide, comprising catalytically reacting limestone or a calcium compound; nitric acid; and hydrogen to obtain calcium hydroxide and an ammonia compound.
  • the second aspect of the present invention provides a ruthenium oxide catalyst, which is represented by the following chemical formula I and has a monoclinic crystal structure, and is used in the method for producing calcium hydroxide according to the first aspect:
  • the method for producing calcium hydroxide according to the embodiments of the present invention does not require a high-temperature heat treatment process to produce calcium oxide (CaO), and thus can be performed at a lower temperature than conventional calcium hydroxide production methods, thereby realizing an economical process with lower energy costs.
  • the method for producing calcium hydroxide according to the embodiments of the present invention can implement an environmentally friendly process that does not emit carbon dioxide compared to conventional methods.
  • the method for producing calcium hydroxide according to the embodiments of the present invention may produce expensive ammonia compounds as a side effect.
  • the yield of calcium hydroxide obtainable using the method for producing calcium hydroxide according to the embodiments of the present invention may be about 60% or more, about 70% or more, about 80% or more, about 85% or more, about 90% or more, about 95% or more, about 96% or more, or about 97% or more.
  • the catalyst used in the method for producing calcium hydroxide according to the embodiments of the present invention is economical because it does not melt or lose its structure during the reaction, so the reaction can be performed for a long time, and can be separated and recovered after the reaction and reused.
  • the catalyst used in the method for producing calcium hydroxide according to the embodiments of the present invention has excellent reaction activity and can produce calcium hydroxide in a high yield.
  • Figure 1 is a schematic diagram of a reaction in which nitric acid and hydrogen containing calcium carbonate (CaCO 3 ) are catalytically reacted to obtain calcium hydroxide (Ca(OH) 2 ) and an ammonia compound, in one embodiment of the present invention.
  • FIG. 2 is a powder X-ray diffraction (PXRD) graph of Ca(OH) 2 manufactured according to Example 1 of the present application.
  • Figure 3 is a powder X-ray diffraction analysis graph of NH 4 NO 3 manufactured according to Example 1 of the present invention.
  • Figure 4 is a powder X-ray diffraction analysis graph of limestone, a reactant of Example 5 of the present invention.
  • Figure 5 is a powder X-ray diffraction analysis graph of Ca(OH) 2 manufactured according to Example 5 of the present invention.
  • step of ⁇ or “step of ⁇ ” as used throughout this specification do not mean “step for ⁇ .”
  • the term "combination(s) thereof" included in the expressions in the Makushi format means one or more mixtures or combinations selected from the group consisting of the components described in the Makushi format, and means including one or more selected from the group consisting of said components.
  • references to “A and/or B” mean “A or B, or A and B.”
  • the first aspect of the present invention provides a method for producing calcium hydroxide, comprising catalytically reacting limestone or a calcium compound; nitric acid; and hydrogen to obtain calcium hydroxide and an ammonia compound.
  • the limestone is an ore containing calcium carbonate (CaCO 3 ) as its main component, and may contain other components, and the scope to which the present invention can be applied may be expanded.
  • the limestone may contain marble, calcite, feldspar, limestone, chalk, glacierite, seashells, egg shells, and coral containing calcium carbonate.
  • the calcium compound may include one or more selected from process by-products, wastes and salts containing calcium.
  • the process by-product or the waste may include at least one selected from slag and waste concrete.
  • the salt means a salt containing calcium, and may not be limited.
  • the salt may include at least one selected from a chloride, an oxide, a sulfate, a carbonate, a nitrate, a phosphate, a sulfate, a silicate, and a hydrate thereof containing calcium, and non-limiting examples thereof include a chloride (e.g., CaCl 2 ), a nitrate (e.g., Ca(NO 3 ) 2 ), an oxide (e.g., CaO), a silicate (e.g., calcium silicate), or a sulfur oxide (e.g., CaSO 4 ).
  • the concentration of the nitric acid may be from about 0.1 M to about 16 M, but may not be limited thereto. In one embodiment of the present invention, the concentration of the nitric acid is from about 0.1 M to about 16 M, from about 0.1 M to about 14 M, from about 0.1 M to about 12 M, from about 0.1 M to about 10 M, from about 0.1 M to about 8 M, from about 0.1 M to about 6 M, from about 0.1 M to about 5 M, from about 0.1 M to about 4 M, from about 0.1 M to about 3 M, from about 0.1 M to about 2 M, from about 0.1 M to about 1 M, from about 1 M to about 16 M, from about 1 M to about 14 M, from about 1 M to about 12 M, from about 1 M to about 10 M, from about 1 M to about 8 M, from about 1 M to about 6 M, from about 1 M to about 5 M, from about 1 M to about 4 M, from about 1 M to about 3 M, about 1 M to about 2 M, about
  • the concentration of the nitric acid when the concentration of the nitric acid is less than about 0.1 M, the production rate of calcium hydroxide may be slowed, and when the concentration of the nitric acid is more than about 16 M, the yield ratio of calcium hydroxide may be decreased due to the high acidity.
  • the catalyst may be selected from a metal, alloy or oxide including at least one selected from titanium (Ti), vanadium (V), chromium (Cr), manganese (Mn), iron (Fe), cobalt (Co), nickel (Ni), copper (Cu), zinc (Zn), molybdenum (Mo), indium (In), tin (Sn), phosphorus (P), aluminum (Al), silicon (Si), ruthenium (Ru), rhodium (Rh), palladium (Pd), silver (Ag), tungsten (W), rhenium (Re), osmium (Os), iridium (Ir), platinum (Pt), and gold (Au).
  • the catalyst may include ruthenium oxide represented by the following chemical formula I:
  • the reaction activity may be enhanced, but may not be limited thereto.
  • the diameter of the particles of the catalyst may be about 10 nm or less, about 8 nm or less, about 6 nm or less, or about 4 nm or less.
  • the catalyst does not melt or its structure collapse during the reaction, so the reaction can be performed for a long period of time.
  • the catalyst can be separated and recovered after the reaction is completed and reused.
  • a catalyst comprising ruthenium oxide represented by the chemical formula I for the reaction, but another metal or metal salt may be additionally used as an auxiliary catalyst.
  • the catalyst may be used in an amount of about 0.1 to about 10 parts by weight based on 100 parts by weight of the limestone or the calcium compound. In one embodiment of the present invention, the catalyst is present in an amount of from about 0.1 part by weight to about 10 parts by weight, from about 0.1 part by weight to about 9 parts by weight, from about 0.1 part by weight to about 8 parts by weight, from about 0.1 part by weight to about 7 parts by weight, from about 0.1 part by weight to about 6 parts by weight, from about 0.1 part by weight to about 5 parts by weight, from about 0.1 part by weight to about 4 parts by weight, from about 0.1 part by weight to about 3 parts by weight, from about 0.1 part by weight to about 2 parts by weight, from about 0.1 part by weight to about 1 part by weight, from about 1 part by weight to about 10 parts by weight, from about 1 part by weight to about 9 parts by weight, from about 1 part by weight to about 8 parts by weight, from about 1 part by weight to about 7 parts by weight, from about 1 part by weight
  • the reaction time of the hydrogenation reaction may become longer and/or the reaction may not be completed, and when the catalyst is used in an amount of about 10 parts by weight or more with respect to 100 parts by weight of the limestone or the calcium compound, the speed of the hydrogenation reaction may become faster, but the separation efficiency may decrease in the process of separating the product and the catalyst.
  • the catalytic reaction may be performed at a temperature range of about 20°C to about 200°C. In one embodiment of the present invention, the catalytic reaction is performed at a temperature of about 20°C to about 200°C, about 20°C to about 190°C, about 20°C to about 180°C, about 20°C to about 170°C, about 20°C to about 160°C, about 20°C to about 150°C, about 20°C to about 140°C, about 20°C to about 130°C, about 30°C to about 200°C, about 30°C to about 190°C, about 30°C to about 180°C, about 30°C to about 170°C, about 30°C to about 160°C, about 30°C to about 150°C, about 30°C to about 140°C, about 30°C to about 130°C, about 40°C to about 200°C, about 40°C to about The catalytic reaction may be performed at a temperature range of about 190°C, about 40°C, about a temperature range
  • the catalytic reaction may be performed in a hydrothermal reactor.
  • the pressure of the hydrogen may be from about 0.1 MPa to about 10 MPa. In one embodiment of the present invention, the pressure of the hydrogen is from about 0.1 MPa to about 10 MPa, from about 0.1 MPa to about 9 MPa, from about 0.1 MPa to about 8 MPa, from about 0.1 MPa to about 7 MPa, from about 0.1 MPa to about 6 MPa, from about 0.1 MPa to about 5 MPa, from about 0.1 MPa to about 4 MPa, from about 0.1 MPa to about 3 MPa, from about 1 MPa to about 10 MPa, from about 1 MPa to about 9 MPa, from about 1 MPa to about 8 MPa, from about 1 MPa to about 7 MPa, from about 1 MPa to about 6 MPa, from about 1 MPa to about 5 MPa, from about 1 MPa to about 4 MPa, from about 1 MPa to about 3 MPa, from about 1.5 MPa to about 10 MPa, from about 1.5 MPa to about 9 MPa, about 1.5 MPa to about 8 MP
  • the reaction progress rate when the pressure of the hydrogen is about 0.1 MPa or lower, the reaction progress rate may be very slow, and when the pressure of the hydrogen is about 10 MPa or higher, the reaction may not progress smoothly. In one embodiment of the present disclosure, the pressure of the hydrogen may be most preferably about 2 MPa.
  • the calcium hydroxide may be obtained as a precipitate of the solution through filtration, but is not limited thereto.
  • the ammonia may be obtained in the form of an ammonia compound by adding carbon dioxide or an acid to the solution, but is not limited thereto.
  • separating the catalyst may be further included.
  • separating a precipitate including the catalyst and the calcium hydroxide may be further included.
  • the method may further include adding an inorganic acid to the product of the hydrogenation reaction to obtain an ammonium salt.
  • the inorganic acid may be, but is not limited to, sulfuric acid, nitric acid, hydrochloric acid, or acetic acid.
  • the ammonium salt may be ammonium sulfate ((NH 4 ) 2 SO 4 ), ammonium hydrogen sulfate (NH 4 HSO 4 ), ammonium nitrate (NH 4 NO 3 ), ammonium hydrochloride (NH 4 Cl), or ammonium acetate (NH 4 CH 3 CO 2 ), and the ammonium salt may vary depending on the type of the inorganic acid.
  • the yield of ammonium ion can be calculated through the weight of the ammonium salt obtained by additionally adding an inorganic acid, but this may be an additional value experimentally confirmed in the process of obtaining an ammonium salt for actual separation and use of ammonium ion after generating ammonia from nitrate ion.
  • the second aspect of the present invention provides a ruthenium oxide catalyst, which is represented by the following chemical formula I and has a monoclinic crystal structure, and is used in the method for producing calcium hydroxide according to the first aspect:
  • x (atomic ratio of hydrogen) is greater than 0 and less than or equal to 4, greater than 0 and less than or equal to about 3.5, greater than 0 and less than or equal to about 3, greater than 0 and less than or equal to about 2.5, greater than 0 and less than or equal to about 2, greater than 0 and less than or equal to about 1.5, greater than 0 and less than or equal to about 1.2, from about 0.1 to about 4, from about 0.1 to about 3.5, from about 0.1 to about 3, from about 0.1 to about 2.5, from about 0.1 to about 2, from about 0.1 to about 1.5, from about 0.1 to about 1.2, from about 0.2 to about 3.5, from about 0.2 to about 3, from about 0.2 to about 2.5, from about 0.2 to about 2, from about 0.2 to about 1.5, from about 0.2 to about 1.2, from about 0.3 to about 3.5, about 0.3 to about 3, about 0.3 to about 2.5, about 0.3 to about 2, about 0.3 to about 1.5, about 0.3 to about 0.3 to about 3.5, about 0.3 to about 3,
  • the ratio of hydrogen when the ratio of hydrogen is from about 0.6 to about 1.4, the monoclinic ruthenium oxide may be easier to produce.
  • x in the chemical formula I when x in the chemical formula I is 0, a structural transition into a tetragonal rutile structure ruthenium oxide may occur, so it is preferable to maintain the hydrogen content.
  • the atomic ratio of hydrogen included in the chemical formula I can be calculated by thermo-gravimetric analysis (TGA). Specifically, in the analysis using the thermo-gravimetric analysis, a solid sample can be placed in a platinum container and the weight change can be measured while increasing the temperature. All hydrogen included in the monoclinic ruthenium oxide (H x RuO 2 ) is removed and converted to tetragonal ruthenium oxide (RuO 2 ). The amount of hydrogen can be quantitatively analyzed from the weight change according to the temperature.
  • TGA thermo-gravimetric analysis
  • the ruthenium oxide catalyst has an incident angle (2 ⁇ ) determined by X-ray powder diffraction measurement (Cu K ⁇ line) of 18.38° ⁇ 2 ⁇ ⁇ 18.42°, 25.45° ⁇ 2 ⁇ ⁇ 25.51°, 26.26° ⁇ 2 ⁇ ⁇ 26.32°, 33.45° ⁇ 2 ⁇ ⁇ 33.51°, 35.28° ⁇ 2 ⁇ ⁇ 35.34°, 36.24° ⁇ 2 ⁇ ⁇ 36.30°, 37.32° ⁇ 2 ⁇ ⁇ 37.38°, 39.55° ⁇ 2 ⁇ ⁇ 39.61°, 40.61° ⁇ 2 ⁇ ⁇ 40.67°, 41.46° ⁇ 2 ⁇ ⁇ 41.52°, 49.17° ⁇ 2 ⁇ Diffraction peaks can be observed at each position of ⁇ 49.23°, 52.31° ⁇ 2 ⁇ ⁇ 52.37°, 54.03° ⁇ 2 ⁇ ⁇ 54.09°, 54.70° ⁇ 2 ⁇ ⁇ 54.76°, 55.95° ⁇ 2 ⁇
  • the ruthenium oxide catalyst may have diffraction peaks observed at positions where the incident angles (2 ⁇ ) determined by X-ray powder diffraction measurement (Cu K ⁇ line) are 18.40°, 25.48°, 26.29°, 33.48°, 35.31°, 36.27°, 37.35°, 39.58°, 40.64°, 41.49°, 49.20°, 52.34°, 54.06°, 54.73°, 55.98°, 58.00°, 60.43°, 61.95°, 63.97°, 65.82°, and 69.16°, respectively.
  • the ruthenium oxide catalyst may have a structure of a monoclinic space group P2 1 /c, C2/m, P2/c, C2/c, P2/m, or P2 1 /m, but may not be limited thereto.
  • the unit cell of the monoclinic crystal structure of the ruthenium oxide catalyst can be defined by lattice constants a to c and edge angle beta ( ⁇ ).
  • 5 ⁇ a ⁇ 6 ⁇ , 5 ⁇ b ⁇ 6 ⁇ , and 5 ⁇ c ⁇ 6 ⁇ , and the beta ( ⁇ ) angle may be about 110° to about 120°.
  • a to c are each about 5 ⁇ to about 6 ⁇ , about 5.1 ⁇ to about 6 ⁇ , about 5.2 ⁇ to about 6 ⁇ , about 5.3 ⁇ to about 6 ⁇ , about 5 ⁇ to about 5.8 ⁇ , about 5.1 ⁇ to about 5.8 ⁇ , about 5.2 ⁇ to about 5.8 ⁇ , about 5.3 ⁇ to about 5.8 ⁇ , about 5 ⁇ to about 5.6 ⁇ , about 5.1 ⁇ to about 5.6 ⁇ , about 5.2 ⁇ to about 5.6 ⁇ , about 5.3 ⁇ to about 5.6 ⁇ , about 5 ⁇ to about 5.4 ⁇ , about 5.1 ⁇ to about 5.4 ⁇ , about 5.2 ⁇ to about 5.4 ⁇ , about 5.3 ⁇ to about 5.4 ⁇ or about 5.35 ⁇ to about 5.4 ⁇ , wherein b can be about 5 ⁇ to about 6 ⁇ , about 5 ⁇ to about 5.8 ⁇ , about 5 ⁇ to about 5.6 ⁇ , about 5 ⁇ to about 5.4 ⁇ , about 5
  • a 5.3533 ⁇
  • b 5.0770 ⁇
  • c 5.3532 ⁇
  • the beta ( ⁇ ) angle may be 115.9074°, but may not be limited thereto.
  • the residual solution was analyzed by ultraviolet-visible spectroscopy, and nitrogen oxide ions (NO 3 - and NO 2 - ) were not detected, confirming that all nitrate ions were reduced to ammonia or nitrogen.
  • Nitric acid was added to the residual solution and evaporated to obtain crystals, which were confirmed to be ammonium nitrate (NH 4 NO 3 ) through X-ray powder diffraction (Fig. 3).
  • the mass of the obtained NH 4 NO 3 is 0.301 g (3.76 mmol), and the yield calculated based on HNO 3 is 94.1%.
  • the hydrogenation reaction was performed in the same manner as in Example 1, except that the reaction was performed under a hydrogen pressure of 5.0 MPa.
  • the precipitate formed after the reaction was dried and confirmed to be Ca(OH) 2 through X-ray powder diffraction analysis.
  • the mass of the obtained Ca(OH) 2 was 0.139 g (1.88 mmol), and the yield of Ca(OH) 2 calculated based on CaCO 3 was 93.8%.
  • nitric acid was added to the residual solution and evaporated to obtain crystals, which were identified as ammonium nitrate (NH 4 NO 3 ) through X-ray powder diffraction.
  • the mass of the obtained NH 4 NO 3 was 0.313 g (3.91 mmol), and the yield calculated based on HNO 3 was 97.8%.
  • the hydrogenation reaction was performed in the same manner as in Example 1, except that 2 mL of distilled water was additionally added and the reaction was performed.
  • the precipitate formed after the reaction was dried and confirmed to be Ca(OH) 2 through X-ray powder diffraction analysis.
  • the mass of the obtained Ca(OH) 2 was 0.125 g (1.69 mmol), and the yield of Ca(OH) 2 calculated based on CaCO 3 was 84.3%.
  • nitric acid was added to the residual solution and evaporated to obtain crystals, which were identified as ammonium nitrate (NH 4 NO 3 ) through X-ray powder diffraction.
  • the mass of the obtained NH 4 NO 3 was 0.294 g (3.67 mmol), and the yield calculated based on HNO 3 was 91.9%.
  • the hydrogenation reaction was performed in the same manner as in Example 1, except that the reaction was performed at 60°C.
  • the precipitate formed after the reaction was dried and confirmed to be Ca(OH) 2 through X-ray powder diffraction analysis.
  • the mass of the obtained Ca(OH) 2 was 0.087 g (1.17 mmol), and the yield of Ca(OH) 2 calculated based on CaCO 3 was 58.7%.
  • nitric acid was added to the residual solution and evaporated to obtain crystals, which were identified as ammonium nitrate (NH 4 NO 3 ) through X-ray powder diffraction.
  • the mass of the obtained NH 4 NO 3 was 0.183 g (2.29 mmol), and the yield calculated based on HNO 3 was 57.2%.
  • the hydrogenation reaction was performed in the same manner as in Example 1, except that 0.2 g of commercial limestone (Fig. 4) was dissolved in nitric acid instead of calcium carbonate as a reactant, and the undissolved solid was separated and used for the reaction.
  • the precipitate formed after the reaction was dried and confirmed to be Ca(OH) 2 by X-ray powder diffraction analysis (Fig. 5).
  • the mass of the obtained Ca(OH) 2 is 0.107 g (1.44 mmol).
  • the reaction was carried out in the same manner as in Example 1, except that ruthenium powder (7.6 mg, 0.075 mmol) was used as a catalyst. After the reaction was completed, the yield of the obtained Ca(OH) 2 was less than 5%, so a very small amount was obtained.
  • the reaction was performed in the same manner as in Example 1, except that platinum powder (14.6 mg, 0.075 mmol) was used as a catalyst. After completion of the reaction, the mass of the obtained Ca(OH) 2 was 0.115 g (1.55 mmol), and the yield of Ca(OH) 2 calculated based on CaCO 3 was 77.6%. The mass of the obtained NH 4 NO 3 was 0.232 g (2.88 mmol), and the yield calculated based on HNO 3 was 72.5%.
  • the reaction was performed in the same manner as in Example 1, except that palladium powder (8.0 mg, 0.075 mmol) was used as a catalyst. After completion of the reaction, the mass of the obtained Ca(OH) 2 was 0.120 g (1.62 mmol), and the yield of Ca(OH) 2 calculated based on CaCO 3 was 81.0%. The mass of the obtained NH 4 NO 3 was 0.256 g (3.20 mmol), and the yield calculated based on HNO 3 was 80.0%.
  • the reaction was carried out in the same manner as in Example 1, except that nickel powder (7.1 mg, 0.075 mmol) was used as a catalyst. After the reaction was completed, the yield of the obtained Ca(OH) 2 was less than 5%, so a very small amount was obtained.

Landscapes

  • Chemical & Material Sciences (AREA)
  • Organic Chemistry (AREA)
  • Engineering & Computer Science (AREA)
  • Materials Engineering (AREA)
  • Chemical Kinetics & Catalysis (AREA)
  • Life Sciences & Earth Sciences (AREA)
  • Geology (AREA)
  • Inorganic Chemistry (AREA)
  • Catalysts (AREA)

Abstract

La présente demande concerne un procédé de production d'hydroxyde de calcium à partir de calcaire ou d'un composé de calcium. Le procédé de production d'hydroxyde de calcium selon des modes de réalisation de la présente demande peut mettre en œuvre un procédé respectueux de l'environnement qui n'évacue pas de dioxyde de carbone par rapport à un procédé classique. Le procédé peut également mettre en œuvre un procédé économique doté de faibles coûts énergétiques puisque le procédé n'utilise pas de procédé de traitement thermique à haute température pour la production d'oxyde de calcium (CaO) et est ainsi réalisé à basse température par rapport à un procédé classique de production d'hydroxyde de calcium.
PCT/KR2024/008175 2023-06-16 2024-06-14 Procédé de production d'hydroxyde de calcium à partir de calcaire ou d'un composé de calcium Ceased WO2024258224A1 (fr)

Applications Claiming Priority (2)

Application Number Priority Date Filing Date Title
KR10-2023-0077530 2023-06-16
KR1020230077530A KR20240176637A (ko) 2023-06-16 2023-06-16 석회석 또는 칼슘 화합물로부터 수산화 칼슘을 제조하는 방법

Publications (1)

Publication Number Publication Date
WO2024258224A1 true WO2024258224A1 (fr) 2024-12-19

Family

ID=93852452

Family Applications (1)

Application Number Title Priority Date Filing Date
PCT/KR2024/008175 Ceased WO2024258224A1 (fr) 2023-06-16 2024-06-14 Procédé de production d'hydroxyde de calcium à partir de calcaire ou d'un composé de calcium

Country Status (2)

Country Link
KR (1) KR20240176637A (fr)
WO (1) WO2024258224A1 (fr)

Citations (4)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
JP2000007329A (ja) * 1998-06-29 2000-01-11 Tochigi Prefecture 板状水酸化カルシウムの製造法
US10322940B2 (en) * 2014-12-05 2019-06-18 Japan Science And Technology Agency Composite, method for producing composite, ammonia synthesis catalyst, and ammonia synthesis method
KR102304406B1 (ko) * 2019-11-01 2021-09-23 (주)원익머트리얼즈 루테늄계 암모니아 분해 촉매 및 그 제조방법
KR20220011076A (ko) * 2020-07-20 2022-01-27 서강대학교산학협력단 루테늄 산화물 및 이를 포함하는 촉매

Patent Citations (4)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
JP2000007329A (ja) * 1998-06-29 2000-01-11 Tochigi Prefecture 板状水酸化カルシウムの製造法
US10322940B2 (en) * 2014-12-05 2019-06-18 Japan Science And Technology Agency Composite, method for producing composite, ammonia synthesis catalyst, and ammonia synthesis method
KR102304406B1 (ko) * 2019-11-01 2021-09-23 (주)원익머트리얼즈 루테늄계 암모니아 분해 촉매 및 그 제조방법
KR20220011076A (ko) * 2020-07-20 2022-01-27 서강대학교산학협력단 루테늄 산화물 및 이를 포함하는 촉매

Non-Patent Citations (1)

* Cited by examiner, † Cited by third party
Title
CASTAÑO SARA VALLEJO, LA PLANTE ERIKA CALLAGON, COLLIN MARIE, SANT GAURAV, PILON LAURENT: "A pilot-process for calcium hydroxide production from iron slag by low-temperature precipitation", JOURNAL OF ENVIRONMENTAL CHEMICAL ENGINEERING, ELSEVIER BV, NL, vol. 10, no. 3, 1 June 2022 (2022-06-01), NL , pages 1 - 13, XP093250590, ISSN: 2213-3437, DOI: 10.1016/j.jece.2022.107792 *

Also Published As

Publication number Publication date
KR20240176637A (ko) 2024-12-24

Similar Documents

Publication Publication Date Title
US20150075328A1 (en) Processes for treating fly ashes
CN114555539A (zh) 由含钙岩石和矿物生产氧化钙或普通波特兰水泥的工艺
US9458522B2 (en) Method for recovery of the constituent components of laterites
CN114981208B (zh) 用于商业和工业利用硫酸钙同时从磷酸生产中获得稀土元素的集成方法
CN109554553A (zh) 一种废铑催化剂中铑的回收方法
EP2995702A1 (fr) Procédé de production de zinc
CN102725231B (zh) 用于制备氧化铬(iii)的方法
WO2013165148A1 (fr) Procédé de production de tétraoxyde de trimanganèse de grande pureté et tétraoxyde de trimanganèse de grande pureté produit par le procédé
WO1989000980A1 (fr) Procede permettant le traitement de boue rouge par etapes multiples et sans dechet, afin de recuperer les matieres de base de l'industrie chimique
AU605965B2 (en) Process for the manufacture of zirconium oxide hydrate from granular crystallized zirconium oxide
US3767595A (en) Process for producing copper chromite catalysts
CS219302B2 (en) Method of making the magnesium oxide
US7968066B2 (en) Method for production of alkali metal chromates
WO2001077021A1 (fr) Production de carbonate de strontium a partir de celestite
CN109336177B (zh) 一种用双氧水和氨水清洁生产高纯五氧化二钒的方法
CN113830776B (zh) 从硫化铜镍矿尾矿中回收多金属结晶联产水玻璃的方法
CN108557881B (zh) 一种含铋物料生产高纯氧化铋的方法
CN1168661C (zh) 一种制备碳酸锶的方法
CN1030308C (zh) 钛酸盐的制备方法
CN100519419C (zh) 一种氯化锶的制备方法
WO2016148446A1 (fr) Procédé de fabrication d'un composé de zinc à partir de poussière de four à arc électrique
KR20240176637A (ko) 석회석 또는 칼슘 화합물로부터 수산화 칼슘을 제조하는 방법
KR100424353B1 (ko) 석회용융분해법을 사용한 지르코늄옥시크로라이드의 제조방법
CN118954455B (zh) 一种废旧磷酸锰铁锂正极材料全组分的回收方法
CN101774624B (zh) 一种Sr(NO3)2的制备方法

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: 24823741

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: 24823741

Country of ref document: EP

Kind code of ref document: A1