Method for fixing nitrogen, fixing carbon dioxide or synthesizing organic matter by supplying various energy in presence of air and in presence of water, or mixture of water and salts, and metals or natural materials

Abstract

To provide means for synthesizing nitrogen and carbon compounds by supplying water, air, and any energy including heat.SOLUTION: A method for synthesizing nitrogen and carbon compounds comprises supplying energy such as heat, light, or electricity in a container in the presence of air, in which water alone, or water and salts, and metals or other natural materials coexist.SELECTED DRAWING: Figure 1

Description

[Technical field]

[0001] The present invention relates to a method for nitrogen fixation, carbon dioxide fixation, or organic synthesis in the presence of air and water, or a mixture of water and salts, metals, or naturally occurring materials, by providing various types of energy such as heating, ultrasonic irradiation, or electrical current. [Background technology]

[0002] The inventors have previously discovered that nitrogen fixation, carbon dioxide fixation, or organic synthesis can be achieved by irradiating ultraviolet light onto water or a mixture of water and salts, metals, or naturally occurring materials (Patent Document 1). Ultraviolet light has strong energy, and it is believed that irradiation can destroy intermolecular bonds, ionize, or put molecules into a higher energy state. When water is irradiated with ultraviolet light, the water decomposes and simultaneously reacts with nitrogen and carbon dioxide in the air, which is believed to cause nitrogen fixation, carbon dioxide fixation, or organic synthesis. The inventors believed that similar reactions could be caused by applying energy other than ultraviolet light to water, and focused on the temperature at which energy can be most easily applied. Details are provided below. [Patent documents] 1. Patent application 2023-132168

[0003] 1. Effect of temperature The effect of temperature was investigated by sealing water in a sealed container and using a thermostatic bath to examine nitrogen fixation, carbon dioxide fixation, and organic synthesis at various temperatures. 20 mL of ion-exchanged water was placed in a 100 mL sealed container (DO bottle), sealed with a lid, and left to stand in a thermostatic bath set to 6°C, 20°C, 40°C, 50°C, 60°C, 70°C, and 80°C for approximately 20 hours. The pH, ammonium, nitrite, nitrate, amino acids, and sugars were investigated and compared with the initial values ​​or concentrations. In the nitrogen system, the ammonium ion (NH4 + For the detection of nitrite ions (NO2), the indophenol method (Non-Patent Document 1), the thymol primary chlorite method (Non-Patent Document 2), or the Nessler method (Non-Patent Document 3) are used. -) uses the naphthylethylenediamine method (Non-Patent Document 4) and nitrate ion (NO3 - For sugar-based compounds, the Park-Johnson method (Non-Patent Document 7), sulfate-silver nitrate method (Non-Patent Document 8), phenol-sulfuric acid method (Non-Patent Document 9), Somogyi method (Non-Patent Document 10), and Selivanoff method (Non-Patent Document 11) were used. For amines and amino acids, the ninhydrin method (Non-Patent Document 12) was used. [Non-patent literature] 1.JIS K 0102, Testing Methods for Industrial Wastewater, Japan Standards Association 148-149 (2008) 2.W.Kh.Klibus,'TN Nazarchuk:J.Anal.Chem USSR,16,80(1961) 3.Japanese Industrial Standards JIS G 1228(1969) 4.Japanese Industrial Standards JIS K 0102, Testing Methods for Industrial Wastewater (2008)43.1.1 5.Kato, Okinaka, Sakai Analytical Chemistry 3:231(1954) 6.Langenfeld,NJ,Payne,LE and Bugbee,B.(2021)PLoS ONE 16(11):e029760 7.Park,JTet al.J.Biol.Chem.,181,149(1949). 8. Kazuhiko Niwa, ed., Chemistry Encyclopedia Editorial Committee (ed.), Vol. 1 (Condensed Edition 26th Edition), Kyoritsu, 1981 10 9. Dubois, M. et al.: Anal. Chem., 28, 350 (1956). 10. Somogyi, M.: J. Biol. Chem., 125, 399 (1938) 11. Francisco, Sanchez-Viesca, and Reina Gomez. Modern Chemistry 6.1 (2018): 1-5 12. S. Lie. 1nst. Brew. vo. 179, p. 37-41 (1973) The results are shown in Figure 1. In both cases, the higher the temperature, the higher the pH, and the more active the production of ammonium, nitrite ions, nitrate ions, amines or amino acids, and sugars. That is, nitrogen fixation, carbon dioxide fixation, amino acid synthesis, and sugar synthesis are promoted. This was the same as when ultraviolet light was irradiated (Patent Document 1). In addition, in the display of the measurement results, only amines or amino acids are shown as optical density (OD) rather than concentration, due to the detection sensitivity. Since a low OD exceeds the detection sensitivity and causes a large error, it is shown as OD without conversion. [Figure 1]

[0004] 2. Comparison of tap water and water purified with ion exchange resin From the results of 1., it is thought that these synthesis events have already occurred in water stored at normal temperatures, so a comparison was made between tap water before it was passed through the ion exchange resin and ion exchanged water that had just passed through the resin. The water temperature at this time was 16°C. The results are shown in Figure 2. As is clear from the figure, in the tap water, although only a small amount of ammonium was produced, the presence of nitrate ions was noticeable. From this, it is assumed that water that has passed through a temperature difference will have a history of mainly the presence of nitrate ions. Therefore, the water that had just passed through the ion exchange resin was immediately cooled, sealed to prevent air from entering, and stored in a cool, dark place, and this was used as the test water for future studies. [Figure 2]

[0005] 3. Heating when the air is removed from the sealed container and air is sealed in To investigate the temperature-dependent reaction of water with components in air (nitrogen, oxygen, and carbon dioxide), 100 mL of water was placed in a sealed flask and degassed with an aspirator for at least 45 minutes. Then, 1) the flask was left degassed, 2) nitrogen was sealed in, 3) carbon dioxide was sealed in, and 4) air was sealed in. 2) to 4) were kept at room temperature and 1 atm, and each flask was heated at 80°C for 4 hours. The results are shown in Figure 3. The pH of the degassed sample was 7, exactly neutral. This was due to the loss of carbon dioxide from the air. When heated in a degassed state, no ammonium synthesis was observed, and no nitrite ions, nitrate ions, amines or amino acids, or sugars were observed. This is natural, since there is no substrate to react with water. When nitrogen was sealed in, there was a slight increase in ammonium, nitrite ions, nitrate ions, amines or amino acids, but no sugars were observed. Again, since only nitrogen, the substrate, was provided, it seemed natural that reduced ammonium and oxidized nitrite ions and nitrate ions were produced. The hydrogen and oxygen used for reduction and oxidation were thought to be due to the decomposition of water. In the case where carbon dioxide was enclosed, the pH was acidic because the dissolved carbon dioxide was converted to carbonic acid. There was no increase in nitrogen compounds such as ammonium, nitrite ions, or nitrate ions, but there was a large increase in sugar. On the other hand, in the case where air was enclosed, all compounds increased significantly. From these results, it is believed that water was decomposed by heat, and the nitrogen, oxygen, and carbon dioxide in the air combined, causing nitrogen fixation, carbon dioxide fixation, amine or amino acid synthesis, and sugar synthesis. [Figure 3] From the above, it was shown that the addition of thermal energy causes water to react with air, resulting in nitrogen fixation, carbon dioxide fixation, amine or amino acid synthesis, and sugar synthesis, just as with ultraviolet light.

[0006] 4. Ultrasonic irradiation Next, we tried to apply ultrasound to provide energy. In order to verify only the effect of ultrasound, we used an intermittent method in which the exposure time was short and the time of standing was extended while cooling was used to suppress heat generation due to ultrasound. 100 mL of ion-exchanged water was placed in a beaker and immersed in a tray filled with ice. Using an ultrasonic homogenizer (Yamato Chemical LUH300), we repeatedly applied 20 kHz, 40 W for 2 seconds and then stood still for 15 seconds, and examined the pH, ammonium, nitrite ion, nitrate ion, amines or amino acids, and sugars over a period of 80 minutes. The results are shown in Figure 4. As shown in the figure, it can be seen that the reaction rate increases with time for all samples. It is believed that these reactions are caused by the action of ultrasound, regardless of temperature. [Figure 4]

[0007] 5. Energy supply by electrolysis It is well known that passing electricity through water will split it into hydrogen and oxygen. This is the most well-known method of providing energy. We investigated whether nitrogen fixation, carbon dioxide fixation, and organic synthesis were occurring during this process, as seen with heating. A horizontal electrophoresis apparatus (Toyobo Agarose Electrophoresis Apparatus Gelmate) was used, and 150 mL of water was placed in each of the cathode and anode tanks, and both electrodes were connected with filter paper. The filter paper was covered with food packaging film to prevent drying. Joule heat was generated by the application of electricity, which caused heat generation, so the entire tank was placed in a tray and ice water was poured into the tray to cool it. In addition, the filter paper part to which the electricity was applied had a large resistance, and heat generation was expected here as well, so ice-cold ice packs were placed there to cool it. This prevented the temperature rise during the application of electricity. Therefore, it was thought that there would be no effect from the temperature rise. A DC power supply (Jookoo Co., Ltd., Tokyo, Japan, Power Supply Type-PAV-50) was connected to both electrodes, and electricity was applied at 400 V (40 mA) for 80 minutes. Changes in pH, ammonium, nitrite ion, nitrate ion, amines or amino acids, and sugars were recorded over time. The results are shown in Figure 5. H + However, the anode has OH - The cathode became acidic and the anode became alkaline. Compared to the cathode, everything increased on the anode. The reduction and oxidation reactions were - ) occurs on the anode side where OH - It was shown that the application of electricity provides energy to the water, and nitrogen fixation, carbon dioxide fixation, and organic matter synthesis occur in the same way as temperature. [Figure 5]

[0008] 6. Visible light effects Furthermore, although the inventor has already reported that energy is given by ultraviolet irradiation (Patent Document 1), we investigated whether visible light, in addition to ultraviolet light, would work. 20 mL of ion-exchanged water was placed in a beaker and exposed to sunlight on a sunny day (48,000 lx). One was left as it was, and the other was placed with an ultraviolet shielding plate on top, and irradiated for 5 hours under sunny conditions. The ultraviolet shielding plate has the ability to block ultraviolet light with a wavelength of 400 nm or less. After irradiation, the beaker was weighed to match the initial weight, the evaporated water was replenished, and each product was examined. The results are shown in Figure 6. As expected, the one without the shielding filter, that is, the one irradiated with light including ultraviolet light, showed higher values ​​in all cases, but the one with the ultraviolet shielding filter and only visible light showed smaller values. However, even with visible light, the values ​​of ammonium, nitrite ions, nitrate ions, amines or amino acids, and sugars were higher than those of untreated water, indicating that these synthesis occurs even under visible light. [Figure 6] From the above, it was found that by supplying some kind of energy to water, ammonium, nitrite ions, nitrate ions, amines or amino acids, sugars, etc. are produced. DISCLOSURE OF THEINVENTION [Problem to be solved by the invention]

[0009] An object of the present invention is to produce nitrogen compounds and carbonate compounds by providing energy to water. [Means for solving the problem]

[0010] As a result of extensive research into achieving the above-mentioned object, the inventors have discovered that the above-mentioned problems can be solved by placing water in a container and applying energy such as heat, pressure, microwaves, ultrasound, electricity, etc. to the water. Based on this finding, the present invention provides 1. A method for synthesizing nitrogen compounds and carbon compounds, which comprises providing energy to water in the presence of air to synthesize nitrogen compounds and carbon compounds; 2. The method for synthesizing a nitrogen compound or a carbon compound according to 1., wherein the energy supply is heat. 3. The method for synthesizing nitrogen compounds and carbon compounds according to 1., characterized in that the water is ion-exchanged water, or a solution or suspension containing salts, metals, natural rocks or gravel, or naturally occurring materials. 4. The method for synthesizing nitrogen compounds and carbon compounds according to 1., wherein the naturally occurring material is silica gel, zeolite, talc, alumina, activated clay, florisil, or a processed version of these. 5. The method for synthesizing a nitrogen compound or a carbon compound according to 1., wherein the energy supply is microwave. 6. The method for synthesizing a nitrogen compound or a carbon compound according to 1., wherein the energy supply is ultrasonic. 7. The method for synthesizing a nitrogen compound or a carbon compound according to 1., wherein the energy supply is a direct current. 8. The method for synthesizing a nitrogen compound or a carbon compound according to 1., wherein the energy is provided by light. This provides: The present invention is characterized by the following points that are different from the conventional techniques. In other words, energy is provided to water alone, or to water containing salts, metals, natural gravel, rocks, or naturally occurring materials, and the energy source is something readily available, such as heat. The process can proceed in any way, including at room temperature and pressure. DETAILED DESCRIPTION OF THE PREFERRED EMBODIMENTS

[0011] Next, examples and comparative examples of the present invention will be described. Note that the examples shown below are for the purpose of facilitating understanding of the present invention, and the present invention is not limited to these examples. In other words, other examples or modifications based on the technical concept of the present invention are naturally included in the present invention. EXAMPLES

[0012] Recovery of ammonia evaporated by heating Ammonium and ammonia are in equilibrium, but the equilibrium changes greatly depending on the pH. On the acidic side, it exists mostly as ammonium, but on the alkaline side, it becomes ammonia, which gradually evaporates as a gas, but when heated, it evaporates rapidly. In the experiment shown in 1, a sealed container was used, so there was no need to consider this volatilization, but in an open state, the amount of ammonium synthesis cannot be accurately determined even if the evaporated water is supplemented. Therefore, a reflux condenser (Graham condenser) is connected to the round flask, heated to boil, and when it passes through the spiral conduit of the condenser, it is cooled by the running water passing through the outside of the conduit, so it returns to water halfway through the spiral, and then returns to its original state by descending the spiral. In other words, the volume of water does not decrease even when it is heated to boil. In addition, a Muencke gas washing bottle is connected to the condenser. It is filled with water, and the ammonia gas that evaporates and flows in is dissolved and supplemented as it passes through the water. This is because ammonia is easily soluble in water. The overall configuration is shown in Figure 7. [Figure 7] This device is ventilated from the outside with an air pump. This is because the air in the flask is expelled by heating and the flask becomes filled with water vapor, resulting in a shortage of air. This is set up so that the reaction between water and air can proceed sufficiently. 100 mL of ion-exchanged water was placed in a round flask and heated. The same amount of ion-exchanged water was also placed in a Muenke Gas bottle. The bottom of the round flask was heated to boiling by applying a flame directly to it. As the flask was heated, gas spewed out into the Muenke Gas bottle and bubbles rose. However, the generation of bubbles stopped over time. This was due to the air in the round flask expanding and escaping during the initial heating period. As heating continued, bubbles stopped appearing, but this is because only water vapor was rising from the round flask, and the water vapor was cooled by the Graham condenser and returned to water. Once the initial bubbling stopped, an air pump was turned on and adjusted so that a constant amount of bubbles were constantly generated from the Muenke Gas bottle. Heating was continued for 4 hours. If ammonium was synthesized by heating, the ammonia that evaporated would be captured in the Muenke flask and could be detected. The results are shown in Figure 8. Ammonium was detected in both the round flask and the Muenke washing bottle. This shows that ammonium was synthesized by heating, some of which became ammonia and evaporated, and was captured in the Muenke washing bottle. It was also found that nitrate ions evaporated and were captured in the Muenke washing bottle. [Figure 8] EXAMPLES

[0013] Microwave irradiation Microwaves are widely used as a heating tool in the form of a microwave oven. We used this to verify whether there was any difference depending on the heating method. Deionized water in a 20 mL beaker was irradiated with microwaves at 80 W for 4 minutes, and the products were measured over time. The results are shown in Figure 9. As a result, it was shown that the amount of ammonium, nitrite ions, nitrate ions, amines or amino acids, and sugars increased with irradiation time. Therefore, it was confirmed that temperature-dependent production occurs even when the heating method is changed. [Figure 9] EXAMPLES

[0014] Autoclave heating Next, to investigate whether water can be heated to above 100°C, an autoclave (Sanyo automatic high-pressure steam sterilizer, MLS-2420) was used to pressurize and heat the water. For sterilization purposes, the autoclave is set to 2 atmospheres and 121°C. 20 mL of ion-exchanged water was placed in a beaker and treated for 15 minutes. The results are shown in Figure 10. All of these results indicate that nitrogen fixation, carbon dioxide fixation, and organic matter synthesis occurred as a result of this treatment. However, it is not possible to determine whether the synthesis was due to pressure or temperature in this experiment. [Figure 10] EXAMPLES

[0016] Effects of additives Previously, it was shown that the production rate increases when various substances are mixed into water by UV irradiation (Patent Document 1), but it was found that natural gravel is more effective, so we investigated whether heating when these substances are mixed would have a similar effect. The method was the same as in Figure 3. Gravel was collected from around Hakodate City (Yoshioka fishing port), 20 g of gravel was taken, and after degassing, nitrogen was sealed in, carbon dioxide was sealed in, oxygen was sealed in, and air was sealed in. The flask was heated in a thermostatic bath for 3 hours, and the product was examined. The results are shown in Figure 11. Various substances were mixed into the gravel, and although it was thoroughly washed while being heated in advance, it is thought that the components dissolved due to long-term heating, but in all cases, a higher production was shown compared to the case of water. [Figure 11] Effects of the invention

[0017] The present invention can be carried out using a simple device, and therefore can be verified against various energy supply methods. Therefore, it can be applied to methods not covered here. The nitrogen fixation, carbon dioxide fixation, and organic synthesis methods of the present invention proceed by providing any type of energy to water, and can be realized with only water and air, making them extremely energy-efficient. It is not difficult to imagine that nitrogen compounds and organic matter were being produced by various energies on the primordial Earth from the time when water and air first began to exist. Moreover, they are still being produced today. Naturally occurring water (in puddles, lakes, oceans, etc.) is not only subject to temperature changes due to air temperature fluctuations, but is also exposed to sunlight and, in some cases, lightning strikes, so there is a complex supply of energy. There are also various rocks, and even more complex reactions are occurring. This is not limited to the Earth, but anywhere in the universe, as long as there is air and water, energy is received and the materials that are the basis of life are formed in abundance. In other words, if the conditions are right, life can arise anywhere in the universe. These reactions are inorganic, and unique substances are not formed in one direction. However, it is thought that the catalytic action of metals contained in localized rocks and other materials caused a greater variety of nitrogen compounds and carbon compounds to accumulate over a long period of time, giving rise to life. It was also shown that great care must be taken when handling water. Distilled water is heated to high temperatures, so unless the substances produced are immediately removed, it cannot be used as pure water. It seems that even after distillation, an ion exchange process is still necessary. In addition, when it comes to storage, it should be kept at the lowest possible temperature, avoiding contact with air. It should be noted that not all commercially available water is subject to such considerations. Water stored for a long time at room temperature may contain small amounts of ammonium, nitrite, and nitrate ions, which is not a problem for health, but it can have a significant impact on research and medical use. For the purpose of sterilization, it is recommended to avoid heating and to filter using a membrane filter. Conversely, it may be possible to use these phenomena to learn about the history of water. Although water that has been in contact with air for a long time is out of the question, for example, when examining ice samples that do not melt (such as ice samples from glaciers or the Antarctic), it may be possible to infer the environment at the time the sample froze. [Brief description of the drawings]

[0018] [Figure 1] Effect of temperature The effect on substance generation when the temperature of the thermostatic bath is changed from 6 to 80°C for ion-exchanged water is shown. [Diagram 2] Differences between tap water and ion-exchanged water. This is a comparison of the pH, ammonium, nitrite ion, nitrate ion, amines or amino acids, and sugar production rates of tap water and ion-exchanged water. In order to show everything on the same bar graph, the values ​​are shown side by side as a multiplication factor. The water temperature was 16°C. [Diagram 3] Effects of degassing and sealed gases Ion-exchanged water was placed in a 100 mL flask and degassed with an aspirator for approximately 45 minutes. While still degassed, nitrogen gas, carbon dioxide, oxygen, and air were sealed in. The flasks were then heated at 80°C for 4 hours, and the products produced were examined. The results are shown below. [Figure 4] Ultrasonic irradiation 20 mL of ion-exchanged water was placed in a beaker, cooled, and intermittently ultrasonically treated with a homogenizer. The results of the product were shown. [Diagram 5] Electrolysis method The results of electrolysis of ion-exchanged water are shown below. After electrolysis, the products in each tank connected to the cathode and anode were examined. [Figure 6] Sunlight Irradiation The results are shown below for 20mL of ion-exchanged water irradiated with sunlight on a sunny day. A comparison was made between water with and without a UV shield (visible light only). [Figure 7] FIG. 1 is a block diagram of an ammonia recovery device. FIG. 1 is a block diagram of an apparatus for recovering ammonia volatilized by heating. [Figure 8] Ammonia recovery: Using an apparatus for recovering the volatile components of the product produced by heating, the results of quantifying the amount of ammonia evaporated in the heated water and recovered in the water are shown. [Figure 9] Microwave Irradiation This shows the results of quantifying the products produced over time when ion-exchanged water was irradiated with microwaves using a microwave oven. [Figure 10] Heating in an autoclave The results show the effect of pressurizing and heating ion-exchanged water using an autoclave. [Figure 11] Heating water containing gravel Gravel from around Hakodate City (Yoshioka Fishing Port) was placed in ion-exchange water and heated using the method shown in [Figure 3]. [Explanation of symbols]

[0019] [Figure 1] A: pH, B: ammonium, C: nitrite ion, D: nitrate ion, E: amines or amino acids, F: sugars. The horizontal axis represents temperature (℃), and the vertical axis represents pH, concentration (mg / L), or turbidity (OD) for amines or amino acids. [Figure 2] The horizontal axis shows pH and concentration (mg / L), as well as the concentration of amines or amino acids. TIFF2025070913000002.tif10150[Figure 3] A: pH, B: Ammonium, C: Nitrite ion, D: Nitrate ion, E: TIFF2025070913000003.tif24155 shows pH and concentration (mg / L), and for amines or amino acids, it is shown as absorbance (OD). [Figure 4] A: pH (solid line) and temperature (℃) (wavy line), B: ammonium, C: nitrite ion, D: nitrate ion, E: amines or amino acids, F: sugars. The horizontal axis represents time (min), and the vertical axis represents pH, temperature, and concentration (mg / L), and for amines or amino acids, it is expressed as absorbance (OD). [Figure 5] A: pH, B: ammonium, C: nitrite ion, D: nitrate ion, E: amines or amino acids, F: sugars. The solid line indicates the cathode solution, and the wavy line indicates the anode solution. The horizontal axis indicates time (min), and the vertical axis indicates pH, temperature, and concentration (mg / L). For amines or amino acids, the absorbance (OD) is shown. [Figure 6] A: pH, B: ammonium, C: nitrite ion, D: nitrate ion, E: amines or amino acids, F: sugars. The solid line indicates the case where a UV shield is placed, and the wavy line indicates the case where no shield is placed. The horizontal axis indicates time (min), the vertical axis indicates pH, temperature, and concentration (mg / L), and for amines or amino acids, it is indicated by absorbance (OD). [Figure 7] 1: Round-bottom flask, 2: Graham condenser, 3: Muenke gas scrubber Shown is TIFF2025070913000004.tif18154. [Figure 8] A: pH, B: ammonium, C: nitrite ion, D: nitrate ion, E: amines or amino acids, F: sugars. The solid line represents the solution in the round flask, and the wavy line represents the solution in the Muenke gas scrubber. The horizontal axis represents time (min), and the vertical axis represents pH, temperature, and concentration (mg / L), and for amines or amino acids, the absorbance (OD) is shown. [Figure 9] A: pH, B: ammonium, C: nitrite ion, D: nitrate ion, E: amines or amino acids, F: sugars. The horizontal axis represents time (min), and the vertical axis represents pH, temperature, and concentration (mg / L), and for amines or amino acids, it is expressed as absorbance (OD). [Figure 10] A: pH, B: ammonium, C: nitrite ion, D: nitrate ion, E: amines or amino acids, F: sugars. The horizontal axis represents time (min), and the vertical axis represents pH, temperature, and concentration (mg / L), and for amines or amino acids, it is expressed as absorbance (OD). [Figure 11] A: pH, B: Ammonium, C: Nitrite ion, D: Nitrate ion, E: TIFF2025070913000005.tif16155 and air enclosed TIFF2025070913000006.tif10151 represents concentration (mg / L), and for amines or amino acids, it is expressed as optical density (OD).

Claims

1. A method for synthesizing nitrogen compounds and carbon compounds, comprising providing energy to water in the presence of air to synthesize nitrogen compounds and carbon compounds.

2. The method for synthesizing nitrogen compounds and carbon compounds according to claim 1, characterized in that the energy supply is heat.

3. 2. The method for synthesizing nitrogen compounds and carbon compounds according to claim 1, wherein the water is ion-exchanged water, or a solution or suspension containing salts, metals, natural rocks or gravel, or naturally occurring materials.

4. 2. The method for synthesizing nitrogen compounds and carbon compounds according to claim 1, wherein the naturally occurring material is silica gel, zeolite, talc, alumina, activated clay, florisil, or a processed version of these.

5. The method for synthesizing nitrogen compounds and carbon compounds according to claim 1, characterized in that the energy supply is microwave.

6. The method for synthesizing nitrogen compounds and carbon compounds according to claim 1, characterized in that the energy supply is ultrasonic.

7. The method for synthesizing nitrogen compounds and carbon compounds according to claim 1, characterized in that the energy supply is a direct current.

8. 1. The method for synthesizing the nitrogen compound or carbon compound according to claim 1, characterized in that the energy supply is light.

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