Carbon dioxide recovery method and firing equipment used in same

Abstract

The invention provides a carbon dioxide recovery method capable of improving marine environment and reducing greenhouse gas. Disclosed is a method for recovering carbon dioxide in which calcium oxide (b) is produced by calcining a raw material of calcium carbonate (a), a heat pump is driven by heat energy generated during the calcination, water (c) is cooled by cold and heat obtained by the heat pump, and carbon dioxide (d) generated during the calcination is recovered in the cooling water. The calcium oxide (b) obtained after calcination is digested to obtain calcium hydroxide (f), the calcium hydroxide (f) is exposed to the atmosphere to recover carbon dioxide (d), and the calcium carbonate (a) obtained again is dispersed on the land side (22) of the high tide line (21) of the coast (2) where carbon dioxide is present during rainfall.

Description

Technical Field

[0001] The present invention relates to a carbon dioxide recovery method for reducing carbon dioxide and a firing apparatus used therefor. Background Art

[0002] At present, in order to prevent global warming, measures are being taken around the world to reduce carbon dioxide emissions. In the prior art, as a technique for reducing the concentration of carbon dioxide in the atmosphere, there is a technique of recovering carbon dioxide discharged from an exhaust gas outlet of a factory or the like and converting the recovered carbon dioxide into a mineral and then fixing it in the ground. Regarding this technique, there is a storage facility for which a verification experiment has been conducted (for example, see Non-Patent Document 1).

[0003] In addition, as another technique, there is also a technique of recovering carbon dioxide from the atmosphere, dissolving the recovered carbon dioxide in water, injecting it into the ground, absorbing it in the ground and fixing it, and then recovering hot spring water (for example, see Patent Document 1).

[0004] However, in the case of recovering carbon dioxide from an exhaust gas outlet, it is impossible to recover carbon dioxide that has been discharged and diffused into the atmosphere.

[0005] In addition, whether recovering carbon dioxide from an exhaust gas outlet or from the atmosphere, ultimately it is converted into a mineral and fixed in the ground. That is, it is considered that calcium oxide contained in basalt forming the earth's crust reacts with carbon dioxide and is fixed in the ground in the form of calcium carbonate. If only considering the reduction of carbon dioxide, directly introducing carbon dioxide from the atmosphere into the ground and fixing it as a mineral may achieve the goal. However, this is very different from the mechanism of the carbon dioxide reduction function originally existing in the natural environment, and thus other problems may occur, and it takes a long time to improve the increasingly deteriorating marine environment due to the increase in carbon dioxide in the atmosphere.

[0006] In addition, an adsorption medium for absorbing carbon dioxide is required. After the adsorption medium adsorbs carbon dioxide, it is necessary to remove carbon dioxide from the adsorption medium and dissolve it in water and inject it into the ground, so the cost of the adsorption medium is high.

[0007]

Non-Patent Document 1

[0008]

Patent Document 1

[0009] In view of the above situation, an object of the present invention is to provide a carbon dioxide recovery method that can both improve the marine environment and easily achieve greenhouse gas reduction.

[0010] The carbon dioxide recovery method of the present invention for solving the above technical problems is: spreading calcium hydroxide and / or calcium carbonate on the land side of the high tide line adjacent to the high tide line on the coast, where the area where the coast is located is an environment where carbon dioxide exists during rainfall.

[0011] The carbon dioxide recovery method of the present invention for solving the above technical problems is: arranging calcium hydroxide and / or calcium carbonate on the surface of the part above the part soaked by seawater at high tide on a reef or on the surface of the part above the part soaked by seawater at high tide on a marine concrete structure, which exists on the land side of the high tide line adjacent to the high tide line on the coast, where the area where the coast is located is an environment where carbon dioxide exists during rainfall.

[0012] The carbon dioxide recovery method of the present invention for solving the above technical problems is: arranging calcium hydroxide and / or calcium carbonate on the surface of the concrete structure of a river or waterway entering the coast, where the coast is an environment where carbon dioxide exists during rainfall, and the concrete structure is located above the planned water level of the river or waterway.

[0013] In the above carbon dioxide recovery method, preferably, the concrete structure is a structure that has been constructed for more than 3 years or a structure in which the internal framework material is exposed on the outside.

[0014] In the above carbon dioxide recovery method, preferably, calcium oxide is made by calcining a calcium carbonate raw material in a closed environment, the carbon dioxide emitted during the calcination process is recovered or used, and the calcium oxide obtained by the calcination is digested to obtain calcium hydroxide, and the calcium hydroxide is exposed to the atmosphere to absorb carbon dioxide to obtain calcium carbonate again, and the calcium hydroxide and / or calcium carbonate thus obtained is used.

[0015] In the above carbon dioxide recovery method, preferably, renewable energy is used for the calcination of calcium carbonate.

[0016] In the above carbon dioxide recovery method, preferably, the calcium carbonate raw material is shellfish.

[0017] In the above carbon dioxide recovery method, preferably, the heat energy generated during the calcination of the calcium carbonate raw material is used to prepare hot water stored in a water heater or for temperature adjustment of a greenhouse.

[0018] In the above carbon dioxide recovery method, preferably, the carbon dioxide generated during the calcination of calcium carbonate raw materials penetrates into the ground and is fixed as minerals; or the carbon dioxide is adsorbed by a carbon dioxide adsorbent for recovery, or directly recovered as carbon dioxide gas, or used as a raw material for synthetic fuels, or discharged into a greenhouse for crop production.

[0019] In the above carbon dioxide recovery method, preferably, the heat generated during the calcination of calcium carbonate raw materials is used to drive a heat pump, and the hot and cold obtained from the heat pump are used to cool water. The cooled water recovers the carbon dioxide generated during the calcination, and the resulting carbonated water penetrates into the ground and is fixed as minerals; or the carbonated water is used for crop production, or used as a raw material for synthetic fuels, or used as a photosynthetic culture solution.

[0020] The firing equipment of the present invention for solving the above technical problems is the firing equipment for calcium carbonate used in the above carbon dioxide recovery method, and is characterized in that: it includes a reaction kettle capable of accommodating calcium carbonate raw materials in a closed state, and a heater using renewable energy for heating is provided in the reaction kettle. The heater can heat the calcium carbonate raw materials placed in the reaction kettle to a temperature at which they decompose into calcium oxide and carbon dioxide. Moreover, a discharge path is provided in the reaction kettle for separating and recovering the carbon dioxide obtained in the reaction kettle from inside the reaction kettle to the outside of the reaction kettle by decomposition pressure and / or pressure feeding.

[0021] In the above firing equipment, preferably, at the discharge point of the discharge path, a gas storage cylinder for filling the carbon dioxide generated in the reaction kettle is provided.

[0022] In the above firing equipment, preferably, a water supply path is provided in the reaction kettle, and the water supply path is used to supply the water required for adding water to the calcium oxide obtained in the reaction kettle for digestion to obtain calcium hydroxide.

[0023] The above firing equipment further includes a heat pump using the heat generated in the reaction kettle, and a carbon dioxide absorption device that cools water using the hot and cold obtained from the heat pump to produce cooled water and allows the cooled water to absorb carbon dioxide. The carbon dioxide absorption device is connected to the discharge point of the discharge path in a state where the carbon dioxide from the discharge path is dissolved in the cooled water of the carbon dioxide absorption device.

[0024] Advantages of the Invention: As described above, according to the present invention, on the coast of an area where there is an environment containing carbon dioxide during rainfall, calcium hydroxide and / or calcium carbonate is disposed on the land side of the high tide line adjacent to the high tide line of the coast, or on the surface of the concrete structure of a river or waterway that enters the coast and is above the design water level. Then, calcium hydroxide absorbs carbon dioxide in rainwater and is converted into calcium carbonate, and calcium carbonate absorbs carbon dioxide in rainwater that causes rainfall to become acid rain and is converted into calcium bicarbonate. Thus, the effect of alleviating acid rain can be exerted, which is beneficial to solving the problem that the pH value of seawater decreases due to acid rain dissolved with carbon dioxide. In addition, calcium ions and bicarbonate ions are easily obtained from calcium bicarbonate after the alleviating effect is exerted. Therefore, bivalve shellfish growing in the sand, shellfish such as conch attached to reefs, foraminifera, and corals can easily obtain calcium carbonate required for bone growth, and seaweeds can easily obtain carbon dioxide required for photosynthesis, thereby improving their growth environment. As a result, the number of fish that feed on them will also increase, and a good marine environment beneficial to fishery can be obtained. In addition, as described above, calcium bicarbonate can be decomposed in the sea into calcium carbonate that forms the shells of shellfish and carbon dioxide consumed in the photosynthesis of seaweeds and can be reused. The calcium bicarbonate flowing into the crust side will ultimately penetrate into the basalt layer that constitutes the crust and be converted into minerals and fixed.

[0025] In addition, 1 mole of carbon dioxide generated when 1 mole of calcium carbonate raw material is calcined is directly fixed in the ground after being converted into carbonated water, or is recovered or used by being adsorbed by an adsorbent, used in the production of crops, used as a culture solution, used as a raw material for synthetic fuels, etc. At the same time, the obtained calcium oxide is converted into calcium hydroxide after digestion. By exposing the calcium hydroxide to the atmosphere, 1 mole of carbon dioxide can be recovered, and 2 moles of carbon dioxide can be recovered from 1 mole of calcium carbonate. In addition, 1 mole of carbon dioxide can be further recovered from the 1 mole of calcium carbonate to form calcium bicarbonate. Therefore, a total of 3 moles of carbon dioxide can be recovered from 1 mole of calcium carbonate raw material.

[0026] Among them, 1 mole of carbon dioxide is originally obtained by discharging the carbon dioxide fixed in the calcium carbonate raw material. The discharged carbon dioxide can be directly fixed in the ground after being converted into carbonated water, or can be utilized by being adsorbed by an adsorbent, used in the production of crops, used as a culture solution, used as a raw material for synthetic fuels, recovered and used as carbon dioxide gas, etc., and will not be discharged into the atmosphere. By exposing the calcium hydroxide obtained after digestion of the calcium oxide obtained after discharge to the expected atmosphere, the carbon dioxide discharged into the atmosphere can be recovered, and thus efficient carbon dioxide recovery can be achieved. BRIEF DESCRIPTION OF THE DRAWINGS

[0027] Figure 1It is a part of the overall composition of the carbon dioxide recovery method involved in the present invention, that is, a diagram of the treatment process from recovering carbon dioxide from calcium carbonate to obtaining calcium hydroxide.

[0028] Figure 2 It is a part of the overall composition of the carbon dioxide recovery method involved in the present invention, that is, a diagram of the treatment process from recovering carbon dioxide from calcium hydroxide to obtaining calcium carbonate.

[0029] Figure 3 It is a part of the overall composition of the carbon dioxide recovery method involved in the present invention, that is, a diagram of the treatment process from recovering carbon dioxide from calcium carbonate to obtaining and using calcium bicarbonate.

[0030] Figure 4 It is a structural diagram schematically showing the overall structure of the firing equipment used for recovering carbon dioxide from calcium carbonate in the carbon dioxide recovery method involved in the present invention.

[0031] Figure 5 It is a schematic diagram schematically showing an example of the utilization method of the carbonic acid water obtained in the carbon dioxide recovery method involved in the present invention.

[0032] Figure 6 It is a schematic diagram schematically showing another example of the utilization method of the carbonic acid water obtained in the carbon dioxide recovery method involved in the present invention.

[0033] Figure 7 It is a schematic diagram schematically showing still another example of the utilization method of the carbonic acid water obtained in the carbon dioxide recovery method involved in the present invention.

[0034] Figure 8 It is a structural diagram showing another embodiment of the firing equipment used for recovering carbon dioxide from calcium carbonate in the carbon dioxide recovery method involved in the present invention.

[0035] Figure 9 It is used to illustrate a part of the overall composition of the carbon dioxide recovery method involved in the present invention, that is, a diagram of the treatment process from recovering carbon dioxide from calcium carbonate to obtaining and using calcium bicarbonate through reefs.

[0036] Figure 10 It is used to illustrate a part of the overall composition of the carbon dioxide recovery method involved in the present invention, that is, a diagram of the treatment process from recovering carbon dioxide from calcium carbonate to obtaining and using calcium bicarbonate through a revetment wall.

[0037] Figure 11It is a part of the overall configuration of the carbon dioxide recovery method according to the present invention, that is, a diagram showing the treatment process from recovering carbon dioxide from calcium carbonate to obtaining and utilizing calcium bicarbonate through a breakwater and wave dissipating blocks.

[0038] Figure 12 It is a photo of the roadside gutter cover plate shortly after ion exchange and the roadside gutter cover plate with the skeleton material exposed due to aging in the carbon dioxide recovery method according to the present invention. Detailed implementation manners

[0039] Figures 1 to 3 It shows the outline of the overall configuration of the carbon dioxide recovery method according to the present invention. Figure 4 It shows the outline of the overall structure of the firing device 1 used in this carbon dioxide recovery method.

[0040] As Figure 1 shown, the carbon dioxide recovery method of the present invention is as follows: calcium oxide b is manufactured by calcining the raw material of calcium carbonate a. At the same time, the heat energy generated during this calcination is used to drive the heat pump 16 (refer to Figure 4 ), the water c is cooled by the cold and heat obtained by this heat pump 16, and the cooled water recovers the carbon dioxide d generated during the above calcination to obtain carbonated water e. And, water c is added to the calcium oxide b obtained by the above calcination for digestion to obtain calcium hydroxide f. Then, as Figure 2 shown, the calcium hydroxide f is exposed to the atmosphere to recover carbon dioxide d, and the calcium carbonate a obtained again is, as Figure 3 shown, scattered on the back beach 25a on the land side 22 of the high tide line 21 of the coast 2 that becomes an acidic environment during rainfall.

[0041] As the raw material of calcium carbonate a, limestone can be used, or shells can be used. In the case of using shells, since organic substances such as seaweeds are attached to the surface of the shells, the shells can be dried in the sun to decompose the organic substances by ultraviolet rays and then used. Additionally, preferably, the raw material of calcium carbonate a is crushed into granular form before use, and more preferably, it is crushed into powder form before use. In the case of using shells, they can also be used directly.

[0042] Calcium oxide b is obtained by calcining the above-mentioned calcium carbonate a at 800 to 900 °C. In this case, fossil fuels can be used for calcination. However, if fossil fuels are used for calcination, excess carbon dioxide d will be generated during combustion. Therefore, it is preferably calcined by electric heating using the electric energy charged by renewable energy such as solar power generation. As the electric heating, a heater 11a can be used, or a device using electromagnetic induction heating can also be used. In addition, instead of converting sunlight into electric energy, sunlight can be directly concentrated for calcination. Through this calcination, calcium carbonate a decomposes into calcium oxide b and carbon dioxide d. At this time, for example, by carrying out the calcination in a reaction kettle 11 which is a closed system, the carbon dioxide d generated in the reaction kettle 11 can be recovered. In addition, by adding water c to the obtained calcium oxide b for digestion, calcium hydroxide f can be obtained. In addition, in addition to solar power generation, as renewable energy power generation, hydropower, wind power, geothermal power, biomass power generation, waste heat power generation, etc. can also be considered. From the perspective of easy utilization, solar power generation is preferably used. As waste heat, the waste heat of an incinerator or thermal power generation can be utilized.

[0043] There is no particular limitation on the recovery method of carbon dioxide d generated during the calcination of calcium oxide b. From the viewpoint of the lowest recovery cost and easy recovery, it is preferably absorbed by water c. The lower the water temperature, the higher the absorption efficiency. Therefore, it is preferably recovered by absorbing with cooling water. This recovery can be carried out, for example, by driving a heat pump 16 using the heat generated during the calcination of the above-mentioned calcium carbonate a, cooling water c with the heat pump 16, and then using the obtained cooling water.

[0044] The carbonated water e obtained by absorbing carbon dioxide d with water c can be, for example, Figure 5 As shown, instead of the carbon dioxide gas used in the greenhouse 3, it is sprayed onto the crops 32 and the soil 33 through a pipeline 31 provided in the greenhouse 3 for the cultivation of the crops 32; or, it can be as Figure 6 shown, directly injected into the soil 33 for cultivating the crops 32 through the provided pipeline 31, and the crops 32 absorb it from the roots for photosynthesis; or, it can be as Figure 7As shown, it is placed in the water tank 30 for hydroponics and circulated in the cultivation tank 34 of the crop 32 by the water pump 35, and is used as the nutrient solution for hydroponics. In addition, in addition to the crop 32, it can also be used as the nutrient solution for various plants that reproduce by photosynthesis. Specifically, it can be used as the nutrient solution for the reproduction of chlorella, which is a raw material for synthetic fuel. Here, the device configuration in the case of hydroponics is not particularly limited. In addition, carbonated water e can also be used as a raw material for synthesizing synthetic fuels such as synthetic alcohol, and can also be used as a beverage after filtration treatment. In addition, as another example of a raw material for synthetic fuel, it is utilized when synthesizing synthetic petroleum by reacting free radical water, seed oil h, and carbon dioxide (for example, WO2016 / 103762, Edelweiss Chemical Science Journal Research Article ISSN: 2641 - 7383 Chemical Synthesis of Fuel Hydrocarbon From CO2 and Activated Water, and Purification of Commercial Light oil for Dream Oil).

[0045] Here, there may be a concern that if the carbon dioxide d in the carbonated water e spilled into the soil 33 or directly injected into the soil 33 is not completely consumed, it will be emitted from the soil 33 and discharged into the atmosphere again, becoming the carbon dioxide d in the atmosphere. However, the molecular weight of carbon dioxide d is 44g, which is heavier than nitrogen, oxygen, etc. that make up the air, so it can stay in the soil 33 for a long time. In the case where the amount of carbon dioxide d is excessive due to the supply of carbonated water e, as long as the closed - system soil 33 such as the greenhouse 3 is adopted as described above, the amount of carbon dioxide d used can be controlled by using carbonated water e and water c together. Even if the closed - system soil 33 such as the greenhouse 3 is not adopted, the excess carbon dioxide d can be absorbed by spreading calcium hydroxide f and / or calcium carbonate a in the soil 33. In this way, calcium hydroxide f will be converted into calcium carbonate a, and calcium carbonate a will be converted into liquid calcium bicarbonate g, so that the excess carbon dioxide d will be converted into calcium bicarbonate g and infiltrate into the soil 33, and finally be fixed in the form of calcium carbonate a in the basalt that makes up the earth's crust.

[0046] On the other hand, when the calcium hydroxide f obtained by digestion after calcination is exposed to the atmosphere, it can absorb carbon dioxide d. After the calcium hydroxide f absorbs carbon dioxide d in the atmosphere, it is transformed into calcium carbonate a. In this case, by exposing the calcium hydroxide f to the desired location, the carbon dioxide d emitted into the atmosphere can be recovered. Additionally, by using this calcium hydroxide f in a location where carbon dioxide d is known to be generated, the carbon dioxide d can be recovered efficiently. Alternatively, the calcium carbonate a described below can be arranged at the location where carbon dioxide d is recovered, and the carbon dioxide d can be recovered using this calcium carbonate a as well.

[0047] Figure 4 An example of a specific firing device 1 is shown. The firing device 1 is configured such that a pipe 12 provided in a reaction kettle 11 that is a closed system branches into two pipes, and on-off valves 13 are provided in each pipe. By switching the on-off valves 13, the reaction kettle 11 can be evacuated by a vacuum water pump 14, or the carbon dioxide d generated in the reaction kettle 11 can be sent to a carbon dioxide absorption device 15. In the reaction kettle 11, a heater 11a is provided, and the heater 11a is heated using electric energy obtained by charging a battery 110 with a solar panel 100. The heater 11a can heat the inside of the reaction kettle 11 to 800 to 900 °C. A heat exchanger 16a of a heat pump 16 is connected to the reaction kettle 11 so that the heat energy generated in the reaction kettle 11 can be utilized. The cold and heat exchanger 16b of the heat pump 16 and the carbon dioxide recovery device 15 are connected such that the cold and heat generated by the heat pump 16 can cool the water c of the carbon dioxide absorption device 15 through the cold and heat exchanger 16b to produce cooling water. The water c is connected to the reaction kettle 11 and the carbon dioxide absorption device 15 via a supply path 17 branched from a water pump 18, and on-off valves 19 are provided respectively. By switching the on-off valves 19, the water c from the water pump 18 can be supplied to the carbon dioxide absorption device 15 or the reaction kettle 11 via the supply path 17. In the reaction kettle 11, by adding water c to the calcium oxide b generated after being heated to 800 to 900 °C as described above for digestion, the calcium oxide b can be transformed into calcium hydroxide f. Additionally, when the water pump 18 utilizes the water pressure of a water pipe, it can be controlled by the on-off valve 19, and thus can be omitted.

[0048] The firing device 1 is equipped with a control unit 120 that controls the start of processing when sufficient electric energy required for processing calcium carbonate a corresponding to the capacity of the reaction kettle 11 is obtained by charging the battery 110 using the solar panel 100. The firing device 1 adopts a batch processing method, that is, it starts running when the charging amount required for one-time processing is obtained. This firing device 1 first puts the raw material of calcium carbonate a into the reaction kettle 11 and closes the reaction kettle 11, then reduces the pressure with a vacuum water pump 14, and then heats it to 800 - 900 °C with a heater 11a. Since carbon dioxide d is generated when calcium carbonate a decomposes into calcium oxide b and carbon dioxide d, the generated carbon dioxide d is transported through the pipeline 12 to the water c in the carbon dioxide absorption device 15, and the water c absorbs the carbon dioxide d and becomes carbonated water e. Due to the supply of this carbon dioxide d, the water c supplied to the carbon dioxide absorption device 15 becomes a high-temperature state, but in the carbon dioxide absorption device 15, the water c is cooled by the heat pump 16, so carbonated water e that has sufficiently absorbed carbon dioxide d can be obtained. According to the amount of calcium carbonate a raw material put into the reaction kettle 11, the amount of generated carbon dioxide d can be calculated. Therefore, when a specified amount of carbon dioxide d is sent to the carbon dioxide absorption device 15, the path is closed, and then water c is added to the calcium oxide b generated in the reaction kettle 11 for digestion, and calcium hydroxide f can be obtained. The calcium hydroxide f obtained in this way does not use fossil fuels, so it is substantially possible to obtain the calcium hydroxide f without emitting carbon dioxide d. The length of the pipeline 12 from the reaction kettle 11 to the vacuum water pump 14 is set to a length that can be sufficiently cooled, and it is preferably cooled by air cooling or water cooling. In addition, in order to prevent the high-temperature carbon dioxide d from passing directly through the vacuum water pump 14, it is preferably that the pipeline 12 is connected in parallel with the vacuum water pump 14, and each pipeline 12 can be opened and closed by an on-off valve (not shown). In this case, it is preferably that the high-temperature carbon dioxide d does not pass through the vacuum water pump 14 but passes through the parallel pipeline 12. During the generation of carbon dioxide d, the carbon dioxide d passes through the pipeline 12. After the generation of carbon dioxide d ends, the pipeline 12 provided with the vacuum water pump 14 is switched, and the carbon dioxide d in the reaction kettle 11 is sent to the carbon dioxide absorption device 15 side by the vacuum water pump 14. Of course, if sufficient cooling can be obtained in the pipeline 12 from the reaction kettle 11 to the vacuum water pump 14, the carbon dioxide d can also be sent to the carbon dioxide absorption device 15 side by the vacuum water pump 14.

[0049] In addition, the above-mentioned firing device 1 is configured such that the heat energy during calcination is converted between cold and heat by the heat pump 16, and the cooling water obtained by using this cold and heat absorbs carbon dioxide d and becomes carbonated water e. However, the firing device 1 is not limited to the above structure, and it can also be configured to replace the carbon dioxide absorption device 15 and the heat pump 16 and be equipped with Figure 8The firing device 1 of the water heater 6 that utilizes the heat energy during firing to store hot water. The following describes the differences from Figure 4 the shown firing device 1. The reaction kettle 11 is the same, so the same markings as Figure 1 are used. Through the heat exchanger 61 provided in the reaction kettle 11, a part of the heat obtained in the reaction kettle 11 can be utilized to heat the water c stored in the water heater 6 to achieve hot water preparation. The water c is supplied to the water heater 6 from the water inlet path 64 via the water pump 62 and the water inlet valve 63. Similar to a general water heater 6, the hot water heated by the water heater 6 can be used for hot water supply. Additionally, this hot water can be supplied to the reaction kettle 11 via the supply path 67 provided with the water pump 65 and the on-off valve 66. For the calcium oxide b obtained after calcination in the reaction kettle 11, this hot water or steam can be added for digestion. Moreover, if water c is used instead of hot water or steam for digestion, the water pump 65 can be omitted, the water supply path 64 downstream of the water pump 62 can be branched, and a supply path 67 via the on-off valve 66 can be provided in the reaction kettle 11. A part of the heat obtained from the hot water of the water heater 6 can be used for temperature regulation of the greenhouse 3, or the heat obtained from the heat exchanger 61 can be directly discharged into the greenhouse 3 for temperature regulation of the greenhouse 3.

[0050] On the other hand, in the Figure 4 shown firing device 1, a carbon dioxide absorption device 15 and a heat pump 16 are provided, which absorb the carbon dioxide d generated during firing with cooling water to form carbonated water e. And Figure 8In the firing apparatus 1 shown, the carbon dioxide d obtained by calcination can be directly taken out from the pipe 12 by using the vacuum water pump 14 and the on-off valve 13 and then infiltrated into the ground to be fixed as a mineral. In this case, as the ground into which the carbon dioxide d is infiltrated, it is preferably directly below land such as a forest or farmland that can consume carbon dioxide through photosynthesis. That is, in the case of a forest or farmland, sufficient water will be accumulated in the ground directly below the forest or farmland due to rain or the like, and thus the water in the ground is likely to become a solvent in which the carbon dioxide d is dissolved. Therefore, if the carbon dioxide d infiltrated into the ground infiltrates into the basalt layer that constitutes the earth's crust, it will be fixed as calcium carbonate a and transformed into a mineral. In addition, even if the carbon dioxide d infiltrated into the ground is saturated, the plants in the forest or farmland can consume the carbon dioxide d through photosynthesis, so it is difficult for the carbon dioxide d infiltrated into the ground to diffuse back into the atmosphere again. Moreover, the ground varies depending on the region, and generally, when the depth is 8 m to 10 m or more, the overall annual temperature is approximately stable at 10°C to 17°C, so the infiltrated carbon dioxide d can be stably absorbed regardless of the season. When infiltrating the carbon dioxide d into the ground, the generated carbon dioxide d can be directly sent to an appropriate depth in the ground through the pipe 12 or the like, and the depth is preferably 8 to 10 m. When the water c that becomes the absorption solvent in the ground is insufficient, it is preferably to supply the water c that becomes the absorption solvent while supplying the carbon dioxide d. When the water c is supplied to the ground as the absorption solvent, after absorbing the carbon dioxide d, it will become carbonated water e, and this carbonated water e can also be drawn out and utilized. In addition, as other absorption solvents, calcium carbonate a can also be added. In the case of calcium carbonate a, after absorbing a small amount of carbon dioxide d, it becomes liquid calcium bicarbonate g, so it is easy to infiltrate deeper into the earth's crust. For use in photosynthesis, the introduction depth does not have to exceed 8 to 10 m and can be less than 8 m. In addition, it can also be introduced into the basalt layer that constitutes the earth's crust. In this case, the carbon dioxide is fixed in the calcium oxide that constitutes the basalt component and can be fixed as calcium carbonate in the earth's crust.

[0051] In addition, instead of the above-mentioned carbon dioxide absorption device 15, ammonia-based carbon dioxide adsorbents such as ammonia or solid amine, porous carbon dioxide adsorbents, or other carbon dioxide adsorbents can be used to adsorb and recover the carbon dioxide d generated by calcination. In addition, it can also be directly recovered into a gas cylinder (only Figure 4Part of the carbon dioxide recovery device 15 connected to the pipeline 12 therein is replaced with a gas cylinder (the illustration is omitted). However, if it is directly recovered into the gas cylinder (the illustration is omitted), since the raw material of calcium carbonate a is calcined to 800 - 900 °C and then decomposed into calcium oxide b and carbon dioxide d to produce carbon dioxide d, it is necessary to recover the high-temperature carbon dioxide d. Therefore, it can also be configured that by making the length of the pipeline 12 from the reaction kettle 11 to the gas cylinder (the illustration is omitted) longer, or by performing air cooling or water cooling on the outside of the pipeline 12, etc., the heat is dissipated to the outside of the pipeline 12, and then the cooled carbon dioxide d is recovered into the gas cylinder (the illustration is omitted).

[0052] In addition, the carbon dioxide d generated by calcination can also be utilized as the carbon dioxide d for the growth of crops 32 discharged into an enclosed space such as the greenhouse 3. The technologies of converting carbon dioxide d into carbonated water e for the foundation to absorb, adsorbing with a carbon dioxide adsorbent, discharging into the greenhouse 3 for the growth of crops 32, and using as a raw material for synthetic fuel as described above can be used in combination in multiple ways.

[0053] Furthermore, the above-mentioned firing equipment 1 is configured to charge the battery 110 using the solar panel 100 and can perform batch processing that starts running when the required charging amount for one-time processing is obtained. However, the battery 110 can also be removed and only the solar panel 100 can be used. In this case, the calcination depends on the electric energy that can be obtained by the solar panel 100 during the day. Therefore, the amount of calcium carbonate a that can be processed at one time can be determined by reverse calculation based on the electric energy that can be obtained by the solar panel 100, or the temperature can be raised over several days for calcination. However, in the case of raising the temperature over several days, it is necessary to improve the heat preservation performance so that the temperature of the reaction kettle 11 does not decrease compared with the previous day.

[0054] The calcium hydroxide f obtained in this way can be used directly in the form of powder or granules. Or, if it is a shell, it can be used in the state after the shell is calcined or after it is crushed into powder or granules later. In addition, water c can be added to the calcium hydroxide f to make a paste-like coating, and then coated on a certain object, which can increase the specific surface area and thus make it easier to recover carbon dioxide d. In this case, in addition to mixing the calcium hydroxide f and water c to make a paste for use, glue or the like can also be added to the paste to be formulated into a so-called plaster for use. In this case, as the plaster, a substance obtained by mixing and kneading water c and glue in the calcium hydroxide f can be used. Various skeletal materials or straws, etc. can also be added to the plaster. As the glue, it can be a natural glue extracted from seaweed commonly used in plaster, or a synthetic glue such as an aqueous acrylic resin. In addition, nanofibers, etc. can be added to replace straw and glue. The calcium hydroxide f in the plaster will absorb carbon dioxide d to generate calcium carbonate a and water c.

[0055] However, since glue, straw, or nanofibers have strong water retention capacity, when calcium hydroxide f absorbs carbon dioxide d and turns into calcium carbonate a, it will simultaneously absorb the generated water c, making it difficult to dry and potentially causing mildew or other problems. In this case, it is preferable not to add glue, straw, or nanofibers, or to limit the usage amount to the minimum, or to add photocatalysts such as titanium oxide for preventing mildew.

[0056] When recovering carbon dioxide d from calcium hydroxide f, it can be used in a form that can be applied, such as the above-mentioned plaster or paste, or directly used in powder form. As the place for application, for example, it can be applied to the rails, sleepers, or utility poles at the part of the railway track that does not come into contact with the locomotive wheels; the power control towers of transmission lines or their bases; the pipes or storage tanks of various factories; the infrastructure (foundation facilities) that supports various living facilities such as bridges or piers. Among them, when applying to the surface of steel components, in order to prevent the steel components from being corroded by calcium hydroxide f, a protective layer can be formed on the surface of the steel components by coating epoxy resin or various inorganic fibers such as basalt fiber, glass fiber, mineral fiber, rock fiber, artificial mineral fiber, or ceramic fiber, and then applying it on the protected surface. In addition, when applying to the surface of concrete or the like, since the concrete itself is alkaline, it can be directly applied to the surface. When directly using the powder, it can be placed in the exhaust path such as a chimney where carbon dioxide d is easily generated by means of a breathable filter container (not shown) or the like, or directly scattered on the ground or the like.

[0057] As Figure 3As shown, calcium hydroxide f and / or calcium carbonate a obtained again after carbon dioxide d is recovered from the calcium hydroxide f are spread on the back beach 25a of the land side 22 of the high tide line 21 adjacent to the high tide line 21 of the coast 2 where carbon dioxide d exists during rainfall. Here, the environment where carbon dioxide d exists during rainfall refers to rainfall in which the rainwater absorbs carbon dioxide d. The key point here is that calcium hydroxide f and / or calcium carbonate a are not spread in the seawater 20 of the coast 2 where carbon dioxide d exists during rainfall, but are spread on the back beach 25a of the land side 22 of the high tide line 21 adjacent to the high tide line 21 of the coast 2. At present, the concentration of carbon dioxide d in the atmosphere is rising, and rainwater becomes acidic with a pH value of 5 to 6, so shallow waters and sea surfaces in the marine environment are being attacked by acid rain. Therefore, the pH value of seawater 20, which was about 8.17 before the Industrial Revolution, has dropped to about 8.06. In places such as estuaries where rainwater easily flows in and harbors with small currents, seawater 20 cannot maintain alkalinity and becomes acidic. This not only causes the pH value of seawater 20 to drop, but also leads to a decrease in fish catch. If this phenomenon is solved from a chemical perspective through reverse engineering, it will be found that after bivalves and other shellfish, foraminifera, etc. are eaten by organisms such as sea bream, grouper, pufferfish, pufferfish, and octopus, these shells are crushed and excreted as feces and then piled up on the seabed foundation 23 to form part of the sand 24. The main component of the crushed shells that become these feces is calcium carbonate a, which is insoluble in alkaline seawater 20. It is accumulated in the sandy soil 24 on the seabed foundation 23 through the above-mentioned ingestion behavior. The calcium carbonate a deposited in the sandy soil 24 of the seabed foundation 23 is washed onto the land by the waves together with the sandy soil 24 to form a beach 25. For example, the beach 25 formed after the foraminifera shells of calcium carbonate a as main component are washed up on land is called the beach 25 of star sand. For example, this calcium carbonate a is insoluble in alkaline environment, but can be dissolved in a trace amount in water c, and can be dissolved in the acid rain containing carbon dioxide d. Therefore, in the beach 25, the calcium carbonate a of the back beach 25a not submerged by seawater plays the effect of alleviating acid rain, and finally converts into liquid calcium bicarbonate g after further absorbing carbon dioxide d. After the water c evaporates after the rain, this calcium bicarbonate g is transferred back to carbon dioxide d and calcium carbonate a again, and is deposited on the back beach 25a with good drainage, thereby, the calcium bicarbonate g that infiltrates into the depths of the back beach 25a can infiltrate into the sandy soil 24 with the state of liquid, and merges into the sea in the ground. Therefore, the concentration of calcium bicarbonate g inside the sandy soil 24 in the sea area near the boundary with the land becomes high, which is an environment rich in calcium bicarbonate g for oyster larvae to easily obtain calcium carbonate a to form skeletons, and an environment rich in calcium bicarbonate g for seaweed to easily obtain carbon dioxide d consumed during photosynthesis, thereby promoting the growth of seaweed and shellfish and increasing the number of fish that feed on them.It can be considered that the calcium carbonate a that reaches the beach 25a in such a way that it is ingested by fish and then discharged onto the beach as feces is converted into calcium bicarbonate g, and a mechanism has been formed to neutralize acid rain and then flow into the sea to stabilize the pH value of the seawater 20. Moreover, the sandy soil 24 that serves as the basis for forming such a calcium carbonate a circulation (Circulation Cycle) is replenished by sediments flowing in from rivers or estuaries. In addition, the calcium oxide contained in the basalt that makes up the earth's crust absorbs rainwater and is converted into calcium hydroxide. Subsequently, it dissolves in acid rain containing carbon dioxide and turns into calcium carbonate. After further playing a role in alleviating acid rain, it becomes calcium bicarbonate g in the same way as the above process and plays the same role as the above effect. In addition, if the calcium oxide contained in the basalt that makes up the earth's crust neutralizes acid rain and then continues to come into contact with the rainwater seeping into the foundation, it will turn into lime water via calcium hydroxide f, seep into the sandy soil 24 through rivers or underground aquifers, or flow into the sea from estuaries or underground. In this case, unlike the situation where calcium carbonate absorbs carbon dioxide and turns into calcium bicarbonate g and flows into the sea, the lime water is alkaline lime water after calcium hydroxide f dissolves in water, and it can flow into the sea without absorbing carbon dioxide. While this lime water plays a role in promoting the restoration of the ocean acidified by absorbing carbon dioxide, it can also provide calcium ions, thus facilitating the formation of an environment in which marine organisms can easily obtain the calcium ions required for growth.

[0058] However, in the current situation, through human fishing, for example, sea bream, grouper, puffer fish, octopus, etc. are caught, and shellfish are also caught by humans. After being eaten by humans, the shells, which are the source of calcium carbonate a, are disposed of as garbage. As a result, the amount of calcium carbonate a accumulated in the sandy soil 24 of the seabed foundation 23 is rapidly decreasing. Therefore, the growth of shellfish and seaweeds is reduced, and the fish that feed on them also decrease. Moreover, acid rain also reduces the pH value of the seawater 20, and the back beach 25a of the beach 25, which could originally alleviate acid rain, is also reduced due to coastal development and construction, etc., making the situation even more serious. In addition, the calcium oxide contained in basalt and the like that makes up the earth's crust is only a little over 10%. Therefore, even if it is possible to form an aqueous solution of calcium bicarbonate g or lime water as described above, it is impossible to continue forming it forever. Usually, under the action of natural phenomena such as landslides and crustal movements caused by weathering, etc., rainwater will renew the water veins through new sediments. However, due to urban development and the construction of sand control dams, etc., the water channels are modified so that rainwater drains from the modified or fixed water channels, and thus it is no longer possible to obtain new replenishment of calcium bicarbonate solution or lime water. These aqueous solutions of calcium bicarbonate g or lime water can only flow through the modified water channels and flow into the sea from specific estuaries with drainage channels. In this way, calcium ions will only accumulate at these specific estuaries, resulting in abnormal growth of oysters and other shellfish in some places.

[0059] Therefore, only by restoring the cycle of the above-mentioned calcium carbonate a can carbon dioxide d be effectively absorbed, leading to an increase in shellfish, seaweeds, and fish. It is considered that the most effective and important thing is to return the liquid calcium bicarbonate g formed by dissolving calcium carbonate a in acid rain to the sea. That is, if only calcium carbonate a enters the sea, the calcium carbonate a will not dissolve in the alkaline seawater 20, so the pH value of the seawater 20 cannot be improved, and it can only relieve the acid rain directly entering the seawater 20. In addition, there are also sea areas that become acidic due to the influence of acid rain. In such places, calcium carbonate a will be converted into calcium bicarbonate g, but the efficiency is not high. The most effective way is to supply calcium carbonate a to the back beach 25a of the well-drained beach 25 in the area facing the boundary line dividing from the coast 2. In this way, calcium carbonate a plays a role in relieving acid rain, absorbs carbon dioxide d, is converted into liquid calcium bicarbonate g, seeps into the sandy soil 24 from the back beach 25a, and then flows into the sea. As a result, not only can the reduction of carbon dioxide d be achieved and the pH value of the seawater 20 be stabilized, but also an environment rich in calcium bicarbonate g, which is conducive to the formation of the skeletons of young shellfish and easy to obtain calcium carbonate a, can be formed through the sandy soil 24. For seaweeds, it becomes an environment rich in calcium bicarbonate g, which is easy to obtain the carbon dioxide d consumed in photosynthesis, thus promoting the growth of seaweeds and shellfish and increasing the fish that feed on them. In addition, it is considered that if the rainfall time is long, the concentration of carbon dioxide d dissolved in the rainwater of acid rain will also gradually change, and calcium carbonate a may not be converted into calcium bicarbonate g. However, the molecular weight of carbon dioxide d dissolved in the acid rain is 44g, which is heavier than the molecular weights of oxygen and nitrogen that make up the air. Therefore, it will be pressed to the ground or the sea surface by rainfall and seep into the ground or the sea surface, increasing the concentration of carbon dioxide d on the ground or the sea surface. However, when the rain stops and dries, the carbon dioxide d on the ground surface or the sea surface is easy to diffuse outdoors because of the wind. However, the carbon dioxide d seeping into the sea surface or the ground is not easy to dissipate because the molecular weight of carbon dioxide d is heavier than the molecular weights of oxygen and nitrogen that make up the air as described above. Among them, the carbon dioxide d on the sea surface will be dispersed by the seawater 20. At the same time, because the seawater 20 itself is alkaline, it is difficult for calcium carbonate a to absorb carbon dioxide d. The carbon dioxide d on the ground is easy to accumulate on the ground surface, so calcium carbonate a is easy to absorb carbon dioxide d. In particular, in a well-drained place like the beach 25, after the rain stops, the water c is easy to quickly recede or evaporate, and the carbon dioxide d is easy to stay on the trace left after the water c disappears, thus easily forming an environment where calcium carbonate a is easy to absorb carbon dioxide d. In the beach 25, the back beach 25a on the land side 22 of the high tide line 21 adjacent to the high tide line 21 is not easily affected by the seawater 20, that is, it is difficult to become alkaline, so calcium carbonate a is easy to absorb carbon dioxide d.

[0060] In addition, in the case of the foreshore 25b or the outer beach 26 of such a shore 2, after supplying calcium carbonate a, the calcium carbonate a accumulates on the seabed foundation 23 and is then washed by waves to the backshore 25a, exerting the same effect as in the case of supplying calcium carbonate a to the backshore 25a described above. Therefore, calcium carbonate a can also be supplied to such an area.

[0061] However, since it takes a long time to be washed from the seabed foundation 23 to the backshore 25a by the action of waves, it is optimal to supply calcium carbonate a to the well-drained backshore 25a on the land side 22 of the high tide line 21 of the shore 2 as described above.

[0062] In addition, in recent years, concrete has been used more frequently to maintain rivers and estuaries to prevent sediment from flowing in. In such places, since there is no supply of new sandy soil 24, a beach 25 cannot be formed. Instead, the sandy soil of the backshore 25a is scraped away, resulting in the disappearance of the beach 25. Therefore, even if calcium carbonate a is supplied to the foreshore 25b or the outer beach 26 in such places, it will not be washed by waves to the backshore 25a. Thus, it is necessary to supply calcium carbonate a directly to the well-drained backshore 25a on the land side 22 of the high tide line 21 of the shore 2 as described above.

[0063] In addition, during rainfall, supplying calcium hydroxide f and / or calcium carbonate a to the backshore 25a on the land side 22 of the high tide line 21 of the shore 2 as described above can improve the marine environment. However, in addition to this, acid rain also flows into the sea from rivers or waterways, and this acid rain flowing into the sea from rivers or waterways causes the pH value of the seawater 20 to decrease. Therefore, in the sea area near the estuary, if the pH value is acidic, calcium hydroxide f and / or calcium carbonate a can be supplied to this sea area to prevent the pH value from decreasing; calcium hydroxide f and / or calcium carbonate a can also be supplied to such areas near the estuary or near the riverbed to prevent the pH value from decreasing.

[0064] In addition, calcium hydroxide f and / or calcium carbonate a can also be supplied to these rivers or waterways to reduce their pH value before flowing into the sea. Specifically, calcium hydroxide f and / or calcium carbonate a can be directly put into the rivers or waterways, or calcium hydroxide f and / or calcium carbonate a can be made into a paste and applied or scattered in a powder state to artificial concrete structures 5 such as river embankments, weirs, waterways built to maintain rivers flowing into the sea, or road drainage ditches used to guide rainwater into waterways (for example Figure 12The surfaces of the covers 5a, 5b) of the roadside drainage ditches shown. Of course, since there is water flowing in rivers or waterways, for the surface of the concrete structure 5 below the design water level, it can only be directly sprinkled; but for the surface of the concrete structure 5 above the design water level, it can be made into a paste for coating or sprinkled in powder form. In addition, for places that are below the design water level but where the water dries up on sunny days, it can also be supplied after the water dries up. For example, for places such as road drainage ditches, their covers (5a, 5b), L-shaped side ditches, or catch basins that are dry on sunny days, calcium hydroxide f and / or calcium carbonate a can be easily coated on their surfaces.

[0065] In addition, such places can also be places where powder is directly scattered instead of being coated on the surface. That is, acid rain needs to flow a relatively long distance from such places until it flows into the sea. Therefore, even if powdered calcium hydroxide f and / or calcium carbonate a are directly supplied, during their flow in the waterway, they will absorb carbon dioxide d in the acid rain, neutralize the acid rain and turn it into calcium bicarbonate g. Thus, the time until it flows into the sea can be utilized to make it play a role in alleviating acid rain and prevent the pH value of the seawater 20 from decreasing. If the water dries up due to the rain stopping on the way in the waterway before flowing into the sea, calcium bicarbonate g will be restored to calcium carbonate a due to the separation of water c and carbon dioxide d, but it can absorb carbon dioxide d in the acid rain and turn into calcium bicarbonate g when the next rainfall occurs. Therefore, the situation of being restored to calcium carbonate a on the way in the waterway is the same as the situation of scattering calcium carbonate a on the way in the waterway. In addition, after calcium hydroxide f absorbs carbon dioxide d, it turns into calcium carbonate a, and after further absorbing carbon dioxide d, it turns into calcium bicarbonate g. If calcium hydroxide f is directly contacted with rainwater, after this rainwater flows into the sea, since this rainwater is alkaline lime water, this lime water can absorb carbon dioxide and improve the acidified ocean, and at the same time can supply calcium ions, thus being conducive to forming an environment in which marine organisms can obtain calcium ions and grow easily.

[0066] In addition, even if carbon dioxide d in calcium bicarbonate g separates again after the rain stops in such side ditches or waterways, since the molecular weight of carbon dioxide d is heavier than the molecular weights of nitrogen and oxygen that make up the air, and if it is a closed system path such as a covered side ditch, catch basin, or waterway, carbon dioxide d is likely to stay. Therefore, it is also easy to maintain the state of calcium bicarbonate g after the rain stops. Even if it is restored to carbon dioxide d, it will stay in such a closed system path and turn into the state of calcium bicarbonate g after neutralizing the acid rain when the next rainfall occurs and then flow into the sea.

[0067] In addition, in the case where natural structures 4 such as the reefs 41 shown in the backshore 25a as described above cannot be formed, Figure 9 the natural structures 4 such as the reefs 41 shown, Figure 10 the revetment walls 51 shown, or Figure 11In the case of the artificial concrete structure 5 such as the breakwater 52 or the wave dissipating block 53 shown, there is no land at the backshore 25a to which the powdery calcium carbonate a is supplied, and even if it is supplied to the reef 41, the seawall 51, the breakwater 52, or the wave dissipating block 53, it will be quickly washed away by the seawater 20. Therefore, for such natural structures 4 or concrete structures 5, it is preferably arranged by coating after making calcium hydroxide f and / or calcium carbonate a into plaster or paste as described above. Originally, the reef 41 as the natural structure 4 is usually composed of basalt or limestone to block the alkaline seawater 20, and the seawall 51, the breakwater 52, or the wave dissipating block 53 of the concrete structure 5 is composed of alkaline concrete. These basalt, limestone, or concrete (in addition to the seawall 51, the breakwater 52, and the wave dissipating block 53, also including the concrete structure 5 of the above-mentioned river) all contain calcium oxide b and calcium carbonate a, but these basalt, limestone, or concrete themselves also play a role in alleviating acid rain and are converted into calcium bicarbonate g and penetrate into the foundation, or dissolve in the seawater 20 and are lost. After a long time, the surface concrete of the concrete structures 5 such as the artificial seawall 51, the breakwater 52, or the wave dissipating block 53 will deteriorate, resulting in the exposure of the internal skeleton materials. Therefore, it is obvious that calcium hydroxide f and calcium carbonate a are lost due to the role of alleviating acid rain. As an example, Figure 12 The cover plate 5a of the roadside drainage ditch and the cover plate 5b of the aged roadside drainage ditch are shown. The aged cover plate 5b consumed calcium hydroxide f and calcium carbonate a in the concrete during the process of alleviating acid rain, resulting in the exposure and deterioration of the internal skeleton materials. The degree of this deterioration varies depending on the location and region. In the early stage, the skeleton materials will be exposed in about 3 years and gradually develop to the inside, leading to complete damage. Therefore, by coating plaster or paste of calcium hydroxide f and / or calcium carbonate a on the surfaces of such concrete structures 5 as the reef 41, the seawall 51, the breakwater 52, and the wave dissipating block 53, the role of alleviating acid rain can be played, and at the same time, these natural structures 4 can regain calcium carbonate a, so as to delay the deterioration of the concrete in the concrete structure 5. In addition, the concrete structure 5 coated with calcium hydroxide f and / or calcium carbonate a is not limited to Figure 12 the structure in which the internal skeleton materials of the concrete such as the cover plate 5b of the deteriorated roadside drainage ditch shown are exposed. It can also be the cover plate 5a of the roadside drainage ditch that has just been replaced. However, if it is the cover plate 5a of the roadside drainage ditch that has just been replaced, it can play the role of alleviating acid rain by itself. However, if it is the cover plate 5b of the deteriorated roadside drainage ditch, it is difficult to play the role of alleviating acid rain. Therefore, in the sense of playing the role of alleviating acid rain, it is preferably applied to the cover plate 5b of the deteriorated roadside drainage ditch, so that the effect of preventing acid rain from reducing the pH value of the seawater 20 can be obtained more effectively.

[0068] In addition, when applied after being made into a plaster or paste, calcium hydroxide f turns into calcium carbonate a after absorbing carbon dioxide d and drying. However, if the original particles of calcium hydroxide f are fine, the surface of the film after drying is relatively smooth. Therefore, when applied in places where people may walk, such as the revetment wall 51, the breakwater 52, or the wave dissipating block 53, it is preferable to add calcium carbonate a crushed into larger particles as a skeleton material to the plaster or paste, so that the effect that people will not slip when walking on the film after drying can be obtained.

[0069] In addition, in the case of applying the plaster or paste, it is preferable to apply it on the land side 22 of the high tide line 21 of the coast 2, that is, on the upper side than the part immersed in the sea water 20 during high tide. More specifically, it is the part of the reef 41, the revetment wall 51, the breakwater 52, or the wave dissipating block 53 that is exposed to the atmosphere without being immersed in the sea water 20. By applying it to such a part, calcium hydroxide f in the plaster or paste can absorb carbon dioxide d in the atmosphere and turn into calcium carbonate a, and then the calcium carbonate a absorbs carbon dioxide d in the atmosphere or rainwater and turns into liquid calcium bicarbonate g. The calcium bicarbonate g penetrates into the reef 41, the revetment wall 51, the breakwater 52, or the wave dissipating block 53 coated with the plaster or paste, is fixed on the reef 41, the revetment wall 51, the breakwater 52, or the wave dissipating block 53, and at the same time can flow into the sea to stabilize the pH value of the sea water 20 and is conducive to forming an environment that is easy to supply calcium carbonate a to juvenile shells and seaweeds.

[0070] In addition, it is preferable to arrange calcium hydroxide f and / or calcium carbonate a on the land side 22 of the high tide line 21 of the coast 2, especially the backshore 25. However, as long as it is a place where rainwater can seep in and flow into the sea water 20, in addition to the part of the reef 41, the revetment wall 51, the breakwater 52, or the wave dissipating block 53 that is exposed to the atmosphere without being immersed in the sea water 20, as long as it is the land side 22 of the high tide line 21 of the coast 2. If it is a river, a watercourse, or a drainage ditch, as long as the path does not pass through a sewage treatment facility. If it is a place on the coast 2 that is quite far from the high tide line 21, as long as it is a place where rainwater can seep in and flow into the sea water 20. In such a place, it can be, depending on the terrain or the underground aquifer, the land side 22 of the coast 2 that is 1000 m away from the high tide line 21; preferably, the land side 22 of the coast 2 that is 100 m away from the high tide line 21; more preferably, within the range of the above-mentioned backshore 25.

[0071] Based on this carbon dioxide recovery method, 1 mole of carbon dioxide d generated when calcining 1 mole of calcium carbonate a as a raw material can be recovered in a way that it is directly fixed in the ground or after being converted into carbonated water e, adsorbed by an adsorbent, used for the production of crops 32, used as a culture solution, used as a synthetic material, or used as a beverage. At the same time, by digesting the obtained calcium oxide b into calcium hydroxide f and exposing the calcium hydroxide f to the atmosphere, 1 mole of carbon dioxide d can be recovered. Therefore, 2 moles of carbon dioxide d can be recovered from 1 mole of calcium carbonate a. Among them, 1 mole of carbon dioxide d is the carbon dioxide d originally fixed in the raw material of calcium carbonate a being discharged, and this discharged carbon dioxide d is recovered as carbonated water e, so it will not be emitted into the atmosphere; the calcium oxide b obtained after discharge is digested into calcium hydroxide f, and by exposing the calcium hydroxide f to the expected atmosphere, the carbon dioxide d already present in the atmosphere can be recovered. Therefore, by concentrating the recovery of carbon dioxide d in specific areas such as factory areas where carbon dioxide d is likely to be generated in large quantities, efficient carbon dioxide reduction can be achieved.

[0072] In addition, since it is to first recover the carbon dioxide d originally fixed in the raw material of calcium carbonate a, then digest the obtained calcium oxide b into calcium hydroxide f, and expose the calcium hydroxide f to the atmosphere to recover carbon dioxide d. Therefore, there is no need to specifically absorb carbon dioxide d with an adsorption medium while the existing device is operating, and the recovery of carbon dioxide d can be achieved naturally.

[0073] Furthermore, if the calcium carbonate a obtained by recovering the carbon dioxide d is placed on the land side 22 of the high tide line 21 of the coast 2 which becomes an acidic environment during rainfall, or on the surface of the concrete structure 5 of the river or waterway which flows into the coast 2 in the area which becomes an acidic environment during rainfall, the carbon dioxide d in the rainwater which causes the rain to become acid rain can be further recovered by the mitigation effect of the calcium carbonate a per 1 mol of carbon dioxide d, and the carbon dioxide d can also solve the problem of the decrease in the pH value of the seawater 20. In this case, the calcium carbonate a plays a role in mitigating acid rain and then converts into liquid calcium bicarbonate g, which infiltrates into the sandy soil 24, the reef 41, or the concrete structure 5 from the land side 22, not only stabilizing the pH value of the seawater 20, but also forming an environment rich in calcium bicarbonate g, which is easy for young shellfish to obtain calcium carbonate a required for skeleton formation, and an environment rich in calcium bicarbonate g, which is easy for seaweed to obtain carbon dioxide d consumed by photosynthesis, thereby promoting the growth of seaweed and shellfish and increasing the number of fish that feed on them. In addition, the remaining calcium bicarbonate g will eventually penetrate into the basalt constituting the seabed foundation 23 and be fixed as a mineral. In addition, even if calcium bicarbonate g does not flow into the sea, but arrives at the basalt constituting the earth's crust, it will be equally absorbed by the calcium oxide b constituting the basalt and converted into a mineral and fixed. Therefore, even if the land side 22 far away from the high tide line 21 of the coast 2 in the area of ​​acidic environment when being located at rain, and calcium bicarbonate g cannot be merged into the sea, this calcium bicarbonate g can also be fixed in the earth's crust as a mineral, and carbon dioxide d can still be recovered in the end. However, the mode of making calcium bicarbonate g flow into the sea can promote the growth of marine algae and shellfish, increase the fish that take them as food, and thus is more advantageous from the meaning of improving the marine environment. In addition, when calcium hydroxide f does not absorb carbon dioxide d and is transformed into calcium carbonate a, if directly exposed to rainwater, river water, groundwater, etc. with the form of calcium hydroxide f, the lime water formed thereby is alkaline, and thus can absorb carbon dioxide and play the role of improving the marine environment of acidification.

[0074] In addition, for the carbon dioxide d generated when calcining the raw material of calcium carbonate a, the heat energy during the calcination can be used to drive the heat pump 16, and then the cold heat obtained by the heat pump 16 can be used to cool the water c, and the carbon dioxide d can be recovered with the cooled water c and converted into carbonic acid water e, so that the carbon dioxide d can be recovered at a low cost.

[0075] In this case, the obtained carbonated water e also has a wide range of uses. For example, it can be used for sprinkling water to replace the carbon dioxide gas used in the greenhouse 3, can be directly injected into the soil 33 for cultivating crops 32 for photosynthesis, can be used as a culture solution for hydroponics of crops 32, can be used as a culture solution for chlorella, etc. that reproduce by photosynthesis, can be used as drinking water, can be used as a raw material when manufacturing synthetic fuels such as alcohol, etc.

[0076] In the carbon dioxide recovery method of the present invention, 1 mole of carbon dioxide d is recovered from 1 mole of calcium carbonate a as a raw material to obtain calcium oxide b. By exposing calcium hydroxide f obtained after digesting this calcium oxide b to the atmosphere, carbon dioxide d can be recovered (1 mole) in a specific area where carbon dioxide d is easily generated. Then, the calcium bicarbonate g thus obtained can be spread on the land side 22 of the high tide line 21 of the coast 2 that becomes an acidic environment during rainfall to recover carbon dioxide d (1 mole) in rainwater. Thus, 3 moles of carbon dioxide d can be recovered from 1 mole of calcium carbonate a as a raw material. However, instead of converting the raw material of calcium carbonate a into calcium hydroxide f, powdered calcium carbonate a can also be directly spread on the land side 22 of the high tide line 21 of the coast 2 that becomes an acidic environment during rainfall to recover carbon dioxide d (1 mole) in rainwater. In this case, carbonated water e cannot be obtained, and carbon dioxide d in the atmosphere cannot be recovered either. Therefore, 3 moles of carbon dioxide d cannot be recovered from 1 mole of calcium carbonate a as a raw material, but carbon dioxide d in rainwater that causes rainfall to become acid rain can be absorbed, and 1 mole of carbon dioxide d can be recovered from 1 mole of calcium carbonate a, which can neutralize acid rain, thus contributing to solving the problem of the decrease in the pH value of the sea due to acid rain containing carbon dioxide d and realizing the improvement of the marine environment. In addition, in this case, as calcium carbonate a, compared with calcium carbonate a having a calcite structure that is difficult to dissolve, it is preferably calcium carbonate a having an aragonite structure that is easily soluble. Specifically, compared with the shells of foraminifera, sea urchins or scallops, it is preferably calcium carbonate a obtained by crushing the shells of corals, pteropods or clams, etc.

[0077] In addition, the present invention can be implemented in various other ways without departing from its concept or main features. Therefore, the above-described embodiments are merely examples of various aspects and should not be construed in a limiting sense. The scope of the present invention is the scope shown in the claims and is not limited by any content in the specification. Moreover, modifications or changes belonging to the claims are within the scope of the present invention.

[0078] The present invention can utilize existing calcium carbonate raw materials such as shells to reduce carbon dioxide and can improve the acidified marine environment by absorbing carbon dioxide.

[0079] <Explanation of Reference Numerals>

[0080] 1 Firing equipment

[0081] 16 Heat pump

[0082] 2 Coast

[0083] 20 Seawater

[0084] 21 High tide line

[0085] 22 Land side

[0086] 32 Crops

[0087] 41 Reef

[0088] 51 Revetment wall

[0089] 52 Breakwater

[0090] 53 Wave dissipating block

[0091] a Calcium carbonate

[0092] b Calcium oxide

[0093] c Water

[0094] d Carbon dioxide

[0095] e Carbonated water

[0096] f Calcium hydroxide

[0097] g Calcium bicarbonate.

Claims

1. A carbon dioxide recovery method, characterized in that: Calcium hydroxide and / or calcium carbonate are arranged on the land side of the high tide line adjacent to the high tide line on the coast, where the area where the coast is located is an environment where carbon dioxide exists during rainfall.

2. A carbon dioxide recovery method, characterized in that: Calcium hydroxide and / or calcium carbonate are arranged on the surface of the part above the part immersed in seawater at high tide on a reef or on the surface of the part above the part immersed in seawater at high tide on a marine concrete structure, which exists on the land side of the high tide line adjacent to the high tide line on the coast, where the area where the coast is located is an environment where carbon dioxide exists during rainfall.

3. A carbon dioxide recovery method, characterized in that: Calcium hydroxide and / or calcium carbonate are arranged on the surface of the concrete structure of a river or watercourse flowing into the sea, which exists on the land side of the high tide line adjacent to the high tide line on the coast, where the area where the coast is located is an environment where carbon dioxide exists during rainfall.

4. The carbon dioxide recovery method according to claim 2, characterized in that: The concrete structure is a structure that has been more than 3 years after construction or a structure in which the internal framework material is exposed on the outside.

5. The carbon dioxide recovery method according to claim 3, characterized in that: The concrete structure is a structure that has been more than 3 years after construction or a structure in which the internal framework material is exposed on the outside.

6. The carbon dioxide recovery method according to any one of claims 1 to 5, characterized in that: Calcium oxide is made by calcining calcium carbonate raw materials in a closed environment, the carbon dioxide emitted during the calcination process is recovered or used, and the calcium hydroxide obtained by digesting the calcium oxide obtained by the calcination is exposed to the atmosphere to absorb carbon dioxide, and calcium carbonate is obtained again, and the calcium hydroxide and / or calcium carbonate thus obtained are used.

7. The carbon dioxide recovery method according to claim 6, characterized in that: Renewable energy is used for the calcination of calcium carbonate.

8. The carbon dioxide recovery method according to claim 6, characterized in that: The calcium carbonate raw material is shells.

9. The carbon dioxide recovery method according to claim 6, characterized in that: In the above carbon dioxide recovery method, the heat energy generated when calcining calcium carbonate raw materials is used to prepare hot water stored in a water heater or for temperature regulation in a greenhouse.

10. The carbon dioxide recovery method according to claim 6, characterized in that: In the above carbon dioxide recovery method, the carbon dioxide generated when calcining calcium carbonate raw materials is infiltrated into the ground to be converted into minerals and fixed; or the carbon dioxide is adsorbed by a carbon dioxide adsorbent for recovery, or directly recovered as carbon dioxide gas, or used as a raw material for synthetic fuel, or discharged into a greenhouse for crop production.

11. The carbon dioxide recovery method according to claim 6, characterized in that: In the above carbon dioxide recovery method, the heat generated during the calcination of calcium carbonate raw materials is used to drive a heat pump. The cold and heat obtained from the heat pump are used to cool water, and then the cooled water is used to recover the carbon dioxide generated during the calcination. The carbonated water thus obtained is infiltrated into the ground and converted into minerals for fixation; or the carbonated water is used for crop production, or as a raw material for synthetic fuels, or as a photosynthetic culture solution.

12. A firing device, which is a firing device for calcium carbonate used in the carbon dioxide recovery method according to claim 7, characterized in that: It includes a reaction kettle capable of accommodating calcium carbonate raw materials in a closed state. A heater that uses renewable energy for heating is provided in the reaction kettle. The heater can heat the calcium carbonate raw materials placed in the reaction kettle to a temperature at which they decompose into calcium oxide and carbon dioxide. In addition, a discharge path is provided in the reaction kettle. The discharge path is used to separate and recover the carbon dioxide obtained in the reaction kettle from inside the reaction kettle to the outside of the reaction kettle through decomposition pressure and / or pressure feeding.

13. The firing device according to claim 12, characterized in that: At the discharge point of the discharge path, a gas storage cylinder for filling the carbon dioxide generated in the reaction kettle is provided.

14. The firing device according to claim 12, characterized in that: A water supply path is provided in the reaction kettle. The water supply path is used to supply the water required for adding water to the calcium oxide obtained in the reaction kettle for digestion to obtain calcium hydroxide.

15. The firing device according to claim 12, characterized in that: It includes a heat pump that uses the heat generated in the reaction kettle, and a carbon dioxide absorption device that cools water using the cold and heat obtained from the heat pump to produce cooled water and makes the cooled water absorb carbon dioxide. The carbon dioxide absorption device is connected to the discharge point of the discharge path in a state where the carbon dioxide from the discharge path is dissolved in the cooled water of the carbon dioxide absorption device.

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