A catalyst for ozone decomposition, a preparation method and applications thereof

Abstract

The application discloses a catalyst for ozone decomposition, a preparation method and application thereof, and the catalyst is a layered double hydroxide with a hydrotalcite structure, wherein the double metal is nickel element and manganese element respectively; and the catalyst further contains copper element. Synthesis of the catalyst is based on recovery of waste lithium manganate battery, and a waste treatment by waste idea is adopted. When the obtained catalyst is used for degrading ozone, the catalyst has high catalytic efficiency, and under the conditions of an ozone concentration of 50ppm, a test temperature of 27 DEG C, a mass space velocity of 800000 mL.g ‑1 ·h ‑1 After 4h of catalytic reaction, the degradation efficiency is still above 95%. And under the conditions of a relative humidity of 60%, a space velocity of 400000 mL.g ‑1 ·h ‑1 The conversion rate of 4h of catalytic ozone decomposition can still reach 80%, compared with the same kind of nickel-manganese hydrotalcite prepared by pure substance, the performance is improved by 10-20%, and the catalyst has good application prospect.

Description

Technical Field

[0001] This invention relates to a catalyst for ozone decomposition, its preparation method, and its application, belonging to the field of catalyst technology. Background Technology

[0002] The production and consumption of lithium batteries have experienced explosive growth. Simultaneously, the effective disposal of large quantities of waste lithium batteries has become a major problem. Among them, lithium manganese oxide batteries, due to their low cost, good fast-charging performance, and outstanding low-temperature performance, are gaining increasing market share in the electric bicycle sector, resulting in a new "urban mine" of waste lithium batteries. Waste lithium manganese oxide batteries are rich in manganese (Mn) and lithium (Li) and other metallic elements. Effective recycling and utilization of these batteries can avoid heavy metal pollution and bring considerable economic benefits. On the other hand, ozone, as a significant precursor to smog and organic aerosols, seriously pollutes the atmosphere and poses potential harm to human health. Nickel-manganese layered double hydroxides (TLDs), due to their abundant interlayer hydroxyl groups and oxygen vacancies, are considered a potential effective ozone decomposition catalyst. However, the manganese used in the preparation of nickel-manganese LTDs faces certain resource constraints. Based on the above two backgrounds, this patent proposes to prepare nickel-manganese layered double hydroxides for ozone decomposition using cathode materials from waste lithium manganese oxide batteries. This aims to provide a new application for the resource utilization of waste lithium batteries and to provide a new approach for the synthesis of nickel-manganese layered double hydroxides for ozone catalytic oxidation. Summary of the Invention

[0003] The purpose of this invention is to provide a catalyst for ozone decomposition, a preparation method thereof, and its application. This catalyst is prepared using waste lithium manganese oxide battery cathode material, and the resulting catalyst has excellent ozone decomposition conversion rate and good application prospects.

[0004] To achieve the above objectives, the technical solution adopted by the present invention is as follows:

[0005] A catalyst for ozone decomposition, wherein the catalyst is a layered bimetallic hydroxide with a hydrotalcite structure, wherein the bimetals are nickel and manganese; the catalyst also contains copper, and the molar ratio of nickel, manganese and copper in the catalyst is (2.5-3.5):1:(0.02-0.05).

[0006] The catalyst described above has a large number of hydroxyl radicals and / or active sites in its structure, which makes it highly catalytically active during ozone decomposition and has good stability at 400,000 mL·g. -1 ·h -1 At air velocity and 60% relative humidity, it can still maintain a degradation rate of over 80% for 4 hours.

[0007] The above-mentioned method for preparing the catalyst for ozone decomposition includes the following steps:

[0008] S1: Obtain the positive electrode sheet of the waste lithium manganese oxide battery and crush it to obtain positive electrode active powder;

[0009] Specifically, the waste MLB cells are immersed in a NaCl solution of a certain concentration to ensure complete discharge and safety during subsequent disassembly. The battery casing is then cut open with tools, and the battery is disassembled and sorted into positive electrode material and remaining parts (negative electrode material, iron shell, separator, and electrolyte). The positive electrode material is air-dried, then cut into small square pieces and roasted in a muffle furnace to remove PVDF. The roasted positive electrode pieces are then crushed and sieved to finally obtain positive electrode active powder.

[0010] S2: The positive electrode active powder is treated with leaching solution and then filtered. Nickel metal salt is added to the filtrate to obtain a mixed metal solution.

[0011] S3: Add H2O2 solution and urea to the mixed metal solution, heat to react, and then sequentially separate the solid and liquid, wash, dry and grind to obtain the catalyst.

[0012] Preferably, in step S2, the leachate includes a leaching agent and a reducing agent, wherein the leaching agent is one or more of nitric acid, sulfuric acid, hydrochloric acid, and phosphoric acid; and the reducing agent is one or more of hydrogen peroxide, sodium bisulfite, and glucose.

[0013] Preferably, in step S2, the volume ratio of leaching agent to reducing agent in the leachate is (90-110):(4-6).

[0014] Preferably, in step S2, the leaching conditions for the positive electrode active powder are: 60-80℃, 1-5h, and solid-liquid ratio of (15-25)g:1L.

[0015] Preferably, in step S2, before adding nickel metal salt to the filtrate, deionized water is added to the filtrate first, and then the pH of the filtrate is adjusted to 3-4 by sodium hydroxide or potassium hydroxide.

[0016] The added nickel metal salt is one or more of nickel nitrate, nickel chloride, and nickel sulfate; exemplary examples include combinations of nickel nitrate and nickel chloride, nickel nitrate and nickel sulfate, and nickel chloride and nickel sulfate.

[0017] Preferably, in step S2, the molar ratio of nickel to manganese in the mixed metal solution is (2.5-3.5):1.

[0018] Preferably, in step S3, the molar ratio of H2O2 in the H2O2 solution to manganese in the mixed metal solution is (0.5-3):1, and the role of H2O2 is to remove the Mn in the lithium manganese oxide battery leaching solution in S1. 2+ Oxidized to Mn3+ Furthermore, this molar ratio is beneficial for synthesizing highly crystalline hydrotalcite. When the amount of H2O2 solution added is too small, the content of high-valence manganese is too low, which is insufficient to form a complete hydrotalcite structure, resulting in significantly lower crystallinity and poor crystallization.

[0019] The molar ratio of urea to nickel and manganese in the mixed metal solution is (3-3.5):1. The role of urea is to provide an alkaline environment after heating and to form NH₂COO during the reaction. - Intercalation, followed by hydrothermal treatment to convert into CO3 2 Furthermore, this molar ratio provides an alkaline environment for the synthesis of hydrotalcite to form a certain proportion of layered hydrotalcite structure, and also provides carbonate ions to enter the interlayer and combine with nickel and manganese. When the urea content is too low, the solution alkalinity is too low, and the hydroxide and carbonate ions it provides are insufficient to form a complete hydrotalcite structure. When the urea content is too high, the solution alkalinity is too high, and the hydroxide and carbonate ions are excessive, which easily leads to the formation of hydroxide impurities.

[0020] Preferably, in step S3, the reaction conditions are: 110-130℃, 11-13h; the drying conditions are: 55-65℃, 6-12h.

[0021] Preferably, in step S3, the solid-liquid separation method includes vacuum filtration.

[0022] Preferably, in step S3, the washing solution includes anhydrous ethanol and deionized water.

[0023] Preferably, in step S3, the washing solution is neutral at the end of the washing process.

[0024] Preferably, in step S3, the drying method is vacuum drying.

[0025] Preferably, in step S3, the vacuum drying is carried out in a vacuum drying oven.

[0026] Preferably, in step S3, the temperature of the vacuum drying is 50-70°C, for example, 50°C, 60°C or 70°C.

[0027] Preferably, the vacuum drying time is 6-24 hours, such as 6 hours, 10 hours, 12 hours, 15 hours, 18 hours, 20 hours, or 24 hours.

[0028] The above-mentioned catalysts are used in the catalytic decomposition of ozone.

[0029] Preferably, the catalyst is used for the decomposition of ozone in the air at room temperature.

[0030] Preferably, the catalyst is used to remove ozone from the atmosphere on the exterior surfaces of buildings and in motor vehicle radiators.

[0031] Preferably, the catalyst is used to remove ozone from confined spaces, both indoors and in high-altitude aircraft.

[0032] Preferably, the catalyst is used for the removal of ozone from water treatment exhaust gas.

[0033] The operational steps for the ozone conversion rate experiment are as follows:

[0034] (1) Compress the catalyst into tablets, grind it, sieve it, take 40-60 mesh particles, weigh the sample with an electronic balance, and fill it into a cylindrical quartz reaction tube with an inner diameter of φ7.0mm and a bed height of 60cm.

[0035] (2) Turn on the air source and the ozone generator, control the final flow rate to 0.5-1.5L / min, so that the ozone concentration after gas mixing is 100ppb-100ppm, and connect the cylindrical quartz reaction tube to the detection system for testing.

[0036] (3) Detect the concentration change before and after the reaction. The concentration before the reaction should reach [O3]in; under the above experimental conditions, the concentration after the reaction is [O3]out.

[0037] (4) Calculate the ozone conversion rate according to the following formula, and retain two significant figures in the result;

[0038] C={([O3]in-[O3]out) / [O3]in}*100;

[0039] C represents the ozone conversion rate, expressed as a percentage.

[0040] [O3]in----Ozone concentration at the reaction inlet, in ppm;

[0041] [O3]out --- Ozone concentration at the reaction outlet, in ppm.

[0042] The beneficial effects of this invention are as follows:

[0043] The catalyst was synthesized based on the recycling of spent lithium manganese oxide batteries, employing a waste-to-waste approach. This resulted in a layered bimetallic hydroxide catalyst with a nickel-manganese hydrotalcite structure, also containing copper. This catalyst exhibited high catalytic efficiency in ozone degradation at an ozone concentration of 50 ppm, a test temperature of 27°C, and a mass hourly space velocity of 800,000 mL·g. -1 ·h -1 Under these conditions, the degradation efficiency remained above 95% after 4 hours of catalytic reaction. Furthermore, at a relative humidity of 60% and a space velocity of 400,000 mL·g⁻¹, the degradation efficiency was maintained. -1 ·h -1Under certain conditions, its conversion rate of catalytic ozone decomposition can still reach up to 80% after 4 hours. Compared with similar nickel-manganese hydrotalcite prepared from pure materials, its performance is improved by 10-20%, showing good application prospects. Attached Figure Description

[0044] Figure 1 These are X-ray diffraction patterns of the catalysts prepared in Examples 1, 2, 3, 4, and 5 of this invention.

[0045] Figure 2 This is the Fourier transform infrared spectrum of the catalyst prepared in Example 1 of this invention;

[0046] Figure 3 These are scanning electron microscope images of the catalyst prepared in Example 1 of this invention;

[0047] Figure 4 The catalysts prepared in Examples 1, 2, 3, 4, 5 and Comparative Example 1 of this invention have a mass hourly space velocity (MSV) of 800,000 mL·g⁻¹. -1 ·h -1 The following performance graph;

[0048] Figure 5 The catalysts prepared in Examples 1, 2, 3, 4, 5 and Comparative Example 1 of this invention have a mass hourly space velocity (MSV) of 400,000 mL·g⁻¹. -1 ·h -1 Performance diagram under 60% relative humidity conditions;

[0049] Figure 6 The catalysts prepared in Comparative Examples 1, 2, 3, and 4 of this invention were used at an initial ozone concentration of 50 ppm and a mass hourly space velocity of 400,000 mL·g. -1 ·h -1 Performance diagram under 60% relative humidity conditions;

[0050] Figure 7 The catalysts prepared in Comparative Examples 1, 5, 6, and 7 of this invention were used at an initial ozone concentration of 50 ppm and a mass hourly space velocity of 400,000 mL·g. -1 ·h -1 Performance diagram under 60% relative humidity conditions. Detailed Implementation

[0051] The present invention will now be described in detail with reference to the accompanying drawings and embodiments.

[0052] In the following examples and comparative examples, the operating procedures for the ozone conversion rate experiment are as follows:

[0053] (1) Compress the catalyst into tablets, grind it, sieve it, take 40-60 mesh particles, weigh the sample with an electronic balance, and fill it into a cylindrical quartz reaction tube with an inner diameter of φ7.0mm and a bed height of 60cm.

[0054] (2) Turn on the air source and the ozone generator, control the final flow rate to 0.5-1.5L / min, so that the ozone concentration after gas mixing is 100ppb-100ppm, and connect the cylindrical quartz reaction tube to the detection system for testing.

[0055] (3) Detect the concentration change before and after the reaction. The concentration before the reaction should reach [O3]in; under the above experimental conditions, the concentration after the reaction is [O3]out.

[0056] (4) Calculate the ozone conversion rate according to the following formula, and retain two significant figures in the result;

[0057] C={([O3]in-[O3]out) / [O3]in}*100;

[0058] C represents the ozone conversion rate, expressed as a percentage.

[0059] [O3]in----Ozone concentration at the reaction inlet, in ppm;

[0060] [O3]out --- Ozone concentration at the reaction outlet, in ppm.

[0061] Example 1

[0062] The catalyst preparation method provided in this embodiment includes the following steps:

[0063] (1) Soak the waste MLBs cells in a 5% (v%) NaCl solution until they are fully discharged.

[0064] (2) The battery casing was sawed open, and the battery was disassembled and sorted into positive electrode material and remaining parts (negative electrode material, iron shell, separator, and electrolyte). The positive electrode material was air-dried in a fume hood, then cut into small square pieces, and calcined in a muffle furnace at 600°C to remove PVDF. The calcined positive electrode pieces were then pulverized and sieved to finally obtain positive electrode active powder.

[0065] (3) Place the above positive electrode active powder in 100 ml of 4 mol·L⁻¹ -1 The mixture was prepared by leaching H2SO4 and 5 ml of 5% (v%) H2O2 at a solid-liquid ratio of 20:1 (g / L); the leaching temperature was 70℃ and the leaching time was 2 hours. After leaching, the mixture was filtered through a filter membrane to obtain a clear leachate.

[0066] (4) Take 23.28 mL of lithium manganese oxide battery leaching solution and place it in 126.72 mL of deionized water. Add 7.1 g of NaOH solid to it and stir vigorously to make the pH value of the solution 3. Then add 4.3618 g of nickel nitrate hexahydrate solid to the mixed solution to obtain solution A.

[0067] (5) Add 1 mL of 30% H2O2 solution and 3.964 g of urea to solution A, stir vigorously for 30 minutes to obtain solution B.

[0068] (6) Pour solution B into a high-pressure reactor with a polytetrafluoroethylene liner, place the reactor in a forced-air drying oven, react at 120°C for 12 hours, then filter the precipitate, wash the precipitate with 1000 mL of anhydrous ethanol and 2000 mL of deionized water until neutral, and dry it under vacuum at 60°C for 8 hours to obtain the catalyst, denoted as Ni-MLB-LDH.

[0069] The X-ray diffraction pattern of the catalyst prepared in this embodiment is as follows: Figure 1 As shown. Crystal planes (003), (006), and (009) are observed at 2θ values ​​of 11°, 23°, and 34.5°, corresponding to the layered structure of LDH. Crystal planes (015), (018), (110), and (113) are observed at 2θ values ​​of 39°, 46°, 60°, and 61°, attributed to the hydrotalcite properties of the nanostructure. The Fourier transform infrared spectrum of the catalyst prepared in this example is shown below. Figure 2 As shown, the peaks at 676, 832, 1077, 1375, 1604, and 3365 cm⁻¹ are attributed to MO and NO₃, respectively. - SO4 2- CO3 2- , H2O and OH bonds or species. XRD and FT-IR results confirmed that the obtained catalyst was LDH, NO3 - SO4 2- CO3 2- These are interlayer anions. The scanning SEM image of the catalyst prepared in this example is shown below. Figure 3 As shown in region a, the image indicates that the obtained catalyst is a flower-like structure formed by the stacking of two-dimensional nanosheets. (mapping image) Figure 3 The bd region shows that the elements on the sample surface are evenly distributed.

[0070] Example 2

[0071] The difference between this embodiment and embodiment 1 is that in step (5), the amount of H2O2 added is 0.5 mL, while the other conditions are exactly the same as in embodiment 1.

[0072] Depend on Figure 1The X-ray diffraction pattern of the catalyst prepared in this embodiment shows that the catalyst is similar to that in Example 1, belonging to the nickel-manganese hydrotalcite structure, and its crystallinity is significantly weaker than that in Example 1.

[0073] Example 3

[0074] The difference between this embodiment and embodiment 1 is that in step (5), the amount of H2O2 added is 1.5 mL, while the other conditions are exactly the same as in embodiment 1.

[0075] The X-ray diffraction pattern of the catalyst prepared in this embodiment shows that the catalyst is similar to that in Example 1, belonging to the nickel-manganese hydrotalcite structure, and the crystallinity is significantly weaker than that in Example 1.

[0076] Example 4

[0077] The difference between this embodiment and embodiment 1 is that in step (5), the amount of urea added is 3.694g, while the other conditions are exactly the same as in embodiment 1.

[0078] Depend on Figure 1 The X-ray diffraction pattern of the catalyst prepared in this embodiment shows that the catalyst is similar to that in Example 1, belonging to the nickel-manganese hydrotalcite structure, and the crystallinity is slightly weaker than that in Example 1.

[0079] Example 5

[0080] The difference between this embodiment and embodiment 1 is that in step (5), the amount of urea added is 4.264g, while the other conditions are exactly the same as in embodiment 1.

[0081] Depend on Figure 1 The X-ray diffraction pattern of the catalyst prepared in this embodiment shows that the catalyst is similar to that in Example 1, belonging to the nickel-manganese hydrotalcite structure, and its crystallinity is significantly weaker than that in Example 1.

[0082] Comparative Example 1

[0083] The catalyst preparation method provided in this comparative example includes the following steps:

[0084] Add 4.3618g of nickel nitrate hexahydrate and 1.16mL of manganese nitrate solution to 150mL of deionized water and stir until homogeneous to obtain solution A;

[0085] Add 1 mL of 30% H2O2 solution and 3.964 g of urea to solution A, stir at room temperature for 30 min to obtain solution B;

[0086] Solution B was poured into a reaction vessel with a polytetrafluoroethylene liner and reacted at 120°C for 12 hours. The reaction vessel was then placed in a forced-air drying oven and reacted at 120°C for 12 hours. After that, the precipitate was filtered and washed with 1000 mL of anhydrous ethanol and 2000 mL of deionized water until neutral. The precipitate was then dried under vacuum at 60°C for 8 hours to obtain the catalyst, denoted as NiMn-LDH.

[0087] Comparative Example 2

[0088] The difference between this comparative example and Comparative Example 1 is that in step (1), 0.0062g Cu(NO3)2·3H2O is added again, while the other conditions are exactly the same as those in Example 1.

[0089] Comparative Example 3

[0090] The difference between this comparative example and comparative example 1 is that in step (1), 0.0124g Cu(NO3)2·3H2O is added, while the other conditions are exactly the same as those in example 1.

[0091] Comparative Example 4

[0092] The difference between this comparative example and comparative example 1 is that in step (1), 0.0248g Cu(NO3)2·3H2O is added again, while the other conditions are exactly the same as those in example 1.

[0093] Comparative Example 5

[0094] The difference between this comparative example and comparative example 1 is that in step (1), 0.0055g of Al(NO3)3·9H2O is added, while the other conditions are exactly the same as those in example 1.

[0095] Comparative Example 6

[0096] The difference between this comparative example and comparative example 1 is that in step (1), 0.011g of Al(NO3)3·9H2O is added, while the other conditions are exactly the same as those in example 1.

[0097] Comparative Example 7

[0098] The difference between this comparative example and comparative example 1 is that in step (1), 0.022g of Al(NO3)3·9H2O is added, while the other conditions are exactly the same as those in example 1.

[0099] Performance testing

[0100] Activity evaluation test: ozone concentration in the reaction gas was 50 ppm, temperature was 27℃, and test space velocity was 800,000 mL·g -1 ·h -1 The test duration is 4 hours; record the ozone conversion rate corresponding to the 4-hour test duration, such as... Figure 4As shown in Table 1.

[0101] Effect of humidity on catalyst activity: ozone concentration in the reaction gas was 50 ppm, temperature was 27℃, and test space velocity was 400,000 mL·g -1 ·h -1 The test humidity was 40%; the ozone conversion rate was recorded after a test time of 4 hours. Figure 5 As shown in Table 2.

[0102] Depend on Figure 4-5 It can be seen that the nickel-iron hydrotalcite catalyst provided in Example 1 has the highest catalytic decomposition ability of ozone at a temperature of 27°C and a mass hourly space velocity of 800,000 mL·g. -1 ·h -1 Under high space velocity conditions, the catalytic efficiency still reached up to 94% after 4 hours of catalytic reaction. This was achieved at a temperature of 27℃, relative humidity of 60%, and a mass hourly space velocity of 400,000 mL·g⁻¹. -1 ·h -1 Under high air velocity conditions, the catalytic efficiency can still reach up to 80% after 4 hours of catalytic reaction.

[0103] Comparing Examples 1, 2, and 3, it can be seen that when the molar ratio of 30% H2O2 to Mn ions is (0.5-3):1, the catalyst exhibits high performance under dry conditions. However, only when the molar ratio of 30% H2O2 to Mn ions is 2:1 does the catalyst show strong resistance to moisture.

[0104] Comparing Examples 1, 4, and 5, it can be seen that under dry conditions, the catalytic performance of the catalyst is significantly reduced when a small amount of urea is added; the catalytic performance does not decrease significantly when a larger amount of urea is added, but the catalytic performance decreases significantly in the humidity test.

[0105] The results of ICP-OES (Table 4) show that the leachate from spent lithium manganese oxide batteries contains not only Mn 2+ There is also a small amount of Cu. 2+ And Al 3+ Therefore, this invention also explores Cu 2+ And Al 3+ The effect of ion doping on the ozone degradation performance of NiMn-LDH. The catalytic decomposition results of catalysts in Comparative Examples 1, 2, 3, and 4 show that Cu doping... 2+ The samples all showed varying degrees of increased ozone degradation efficiency, indicating that Cu doping promotes ozone degradation. The effects of comparative examples 1, 5, 6, and 7 show that Al doping... 3+The samples all showed varying degrees of reduction in ozone degradation efficiency, indicating that Al doping inhibits ozone degradation. Therefore, it can be inferred that one reason for the excellent ozone degradation ability of the catalyst obtained in Example 1 is the presence of Cu recovered from lithium manganese oxide batteries. 2+ Ions (as can be seen from Table 4).

[0106] Table 1. Ozone conversion efficiency of the catalysts prepared in Examples 1-5 and Comparative Example 1 under dry conditions.

[0107]

[0108]

[0109] Table 2 shows the ozone conversion efficiency of the catalysts prepared in Examples 1-5 and Comparative Example 1 at 60% humidity.

[0110]

[0111] Table 3 shows the ozone conversion efficiency of the catalysts prepared in Comparative Examples 1-7 at 60% humidity.

[0112]

[0113] Table 4. ICP-OES results of the leachate, catalyst prepared in Example 1, and catalyst prepared in Comparative Example 1.

[0114]

[0115] I. The unit is mg·L -1 II. The unit is mass percentage (wt%).

[0116] The above description is only a preferred embodiment of the present invention. It should be noted that for those skilled in the art, several improvements and modifications can be made without departing from the principle of the present invention, and these improvements and modifications should also be considered within the scope of protection of the present invention.

Claims

1. A method for the preparation of a catalyst for the decomposition of ozone, characterized in that, The catalyst is a layered double hydroxide with a hydrotalcite structure, wherein the double metal is nickel element and manganese element respectively; the catalyst further contains copper element, and the molar ratio of nickel element, manganese element and copper element in the catalyst is (2.5-3.5):1:(0.02-0.05); The preparation method comprises the following steps: S1: obtaining a positive plate of a waste lithium manganate battery and crushing the positive plate to obtain a positive active powder; S2: filtering the positive active powder after treatment by a leaching solution, adding a nickel metal salt to the filtrate to obtain a mixed metal solution; S3: adding an H2O2 solution and urea to the mixed metal solution, heating and reacting, and then sequentially performing solid-liquid separation, cleaning, drying and grinding to obtain the catalyst.

2. The method for producing a catalyst for ozone decomposition according to claim 1, characterized by, In step S2, the leaching solution comprises a leaching agent and a reducing agent, wherein the leaching agent is one or more of nitric acid, sulfuric acid, hydrochloric acid and phosphoric acid; and the reducing agent is one or more of hydrogen peroxide, sodium bisulfite and glucose.

3. The method for preparing a catalyst for ozone decomposition according to claim 1, characterized by, In step S2, the volume ratio of the leaching agent to the reducing agent in the leaching solution is (90-110):(4-6).

4. The method for preparing a catalyst for ozone decomposition according to claim 1, characterized by, In step S2, the positive active powder is treated by leaching under the following conditions: 60-80℃, 1-5h, and a solid-liquid ratio of (15-25)g:1L.

5. The method for preparing a catalyst for ozone decomposition according to claim 1, characterized by, In step S2, before the nickel metal salt is added to the filtrate, deionized water is first added to the filtrate, and then the pH of the filtrate is adjusted to 3-4 by sodium hydroxide or potassium hydroxide. The added nickel metal salt is one or more of nickel nitrate, nickel chloride and nickel sulfate.

6. The method for preparing a catalyst for ozone decomposition according to claim 1, characterized by, In step S2, the molar ratio of nickel element to manganese element in the mixed metal solution is (2.5-3.5):

1.

7. The method for preparing a catalyst for ozone decomposition according to claim 1, characterized by, In step S3, the molar ratio of H2O2 in the H2O2 solution to manganese element in the mixed metal solution is (0.5-3):1; and the molar ratio of urea to nickel-manganese elements in the mixed metal solution is (3-3.5):

1.

8. The method for preparing a catalyst for ozone decomposition according to claim 1, characterized by, In step S3, the reaction conditions are 110-130℃, 11-13h; and the drying conditions are 55-65℃, 6-12h.

9. Use of the catalyst prepared by the method of any one of claims 1-8 in catalytic decomposition of ozone.

Images