Electrocatalyst, method for preparing the same, and use thereof

Abstract

The application discloses an electrocatalyst and a preparation method and application thereof. The electrocatalyst comprises a carrier and an active component. The carrier comprises a MOFs material, and the active component comprises Cu and Ce. Cu and Ce are limited by a coordination bond of a formula I ligand. Through atomic limitation and coordination strategy, transition metal copper and rare earth element cerium are anchored on a carbon-nitrogen material. After no metal to containing two metals, CO2 can be effectively reduced to synthesis gas with different proportions. In terms of performance, the CuCe-NC catalyst with a binuclear metal complex as a metal source is similar to a diatomic catalyst and has a synergistic catalytic performance.

Description

Technical Field

[0001] This invention relates to the field of catalysis technology, and in particular to an electrocatalyst, its preparation method, and its application. Background Technology

[0002] Electrocatalysis, which converts CO2 into valuable chemical products, is considered one of the most effective methods for solving environmental pollution and energy shortage problems. Many different types of electrocatalysts have been developed for CO2 reduction, but they typically require noble metal catalysts (such as Pt and Ru). The high cost and low abundance of noble metals limit their large-scale use. To overcome this, inexpensive transition metals (such as Fe, Co, Ni, and Cu) are used as substitutes. Furthermore, due to the readily available raw materials, simple preparation, and good conductivity of carbon and nitrogen materials, using transition metals supported on carbon and nitrogen materials for electrocatalytic CO2 reduction has become a research hotspot in recent years. However, the high production cost, low activity, poor stability, and complex synthesis methods of transition metal catalysts limit the development of this technology. Therefore, developing low-cost, high-activity, high-selectivity, and high-stability catalysts is of great significance for realizing the practical application of CO2 electrochemical reduction. Summary of the Invention

[0003] The present invention aims to at least solve one of the aforementioned technical problems existing in the prior art. Therefore, the object of the present invention is to provide an electrocatalyst, its preparation method, and its application.

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

[0005] In a first aspect, the present invention provides an electrocatalyst comprising a support and an active component, wherein the support comprises a carbon-nitrogen material and the active component comprises Cu and Ce; Cu and Ce are confined by coordination bonds of formula I ligands;

[0006]

[0007] In this invention, a multi-toothed I ligand (CAS No.: 115142-66-0, chemical name: 3-[2-[2-[2-(3-formyl-2-hydroxyphenoxy)ethoxy]ethoxy]ethoxy]-2-hydroxybenzaldehyde) is coordinated with Cu and Ce to confine Cu and Ce, and then anchored to a support to obtain a bimetallic electrocatalyst with higher activity, selectivity and stability, and also has synergistic catalytic performance.

[0008] In some embodiments of the present invention, the raw materials for preparing the electrocatalyst include MOF materials, a nitrogen source, Cu salt, Ce salt and formula I ligand.

[0009] In some embodiments of the present invention, the molar ratio of Cu to Ce in the electrocatalyst is (0.9–1.1):(0.9–1.1).

[0010] In some embodiments of the present invention, the mass ratio of the support to the active ingredient in the electrocatalyst is (497-499):(1-3).

[0011] In some embodiments of the present invention, the electrocatalyst has a rod-shaped structure.

[0012] In some embodiments of the present invention, the diameter of the electrocatalyst is 150 nm to 300 nm.

[0013] In some embodiments of the present invention, the electrocatalyst is a porous nanorod material.

[0014] In some embodiments of the present invention, the surface of the electrocatalytic material is distributed with micropores.

[0015] In some embodiments of the present invention, the MOFs material includes any one of HKUST-1, M2(dobpdc), MIL-100, MIL-101, MIL-53, MOF-74, NU-1000, PCN-222, PCN-224, UiO-66, UiO-67, ZIF-8, ZIFs or derivatives thereof.

[0016] In some embodiments of the present invention, the Cu salt includes at least one of copper nitrate trihydrate, copper chloride, and copper sulfate.

[0017] In some embodiments of the present invention, the Ce salt includes at least one of cerium acetate, cerium chloride, and cerium nitrate.

[0018] In some embodiments of the present invention, the nitrogen source includes at least one of urea, 2-methylimidazole, and dicyandiamide.

[0019] A second aspect of the present invention provides a method for preparing the aforementioned electrocatalyst, comprising the following steps:

[0020] S1: Bimetallic complexes are prepared by coordinating Cu salt, Ce salt and formula I ligand.

[0021] S2: An electrocatalyst is prepared by reacting a bimetallic complex or MOF material with a nitrogen source, followed by freeze-drying, calcination under an inert atmosphere, and acid etching.

[0022] In some embodiments of the present invention, S1 specifically involves: dissolving the ligand of formula I in an organic solvent, adding ethylenediamine and Ce salt to react, then adding Cu salt to react, and evaporating to obtain a bimetallic complex.

[0023] In some embodiments of the present invention, S1 specifically involves: dissolving the ligand of formula I in an organic solvent, adding ethylenediamine and Ce salt and reacting for 1 to 4 hours, then adding Cu salt and reacting for 1 to 4 hours, and finally evaporating to obtain a bimetallic complex.

[0024] In some embodiments of the present invention, the organic solvent includes at least one of methanol, acetonitrile, and ethanol.

[0025] In some embodiments of the present invention, in S2, the calcination temperature is 800℃~1000℃ and the time is 1h~4h.

[0026] In some embodiments of the present invention, S2 specifically involves: reacting the bimetallic complex, MOF material, and nitrogen source for 3-8 hours, freeze-drying for 24-48 hours, calcining at 800-1000°C for 1-4 hours under an inert atmosphere, and then etching with acid to obtain the electrocatalyst.

[0027] In some embodiments of the present invention, in S2, the mass ratio of the bimetallic complex to the MOFs material is (3-4):(24-26).

[0028] In some embodiments of the present invention, in S2, the mass ratio of the nitrogen source to the bimetallic complex is (10-15):(1-2).

[0029] A third aspect of the invention provides a battery electrode comprising a current collector and an electrode material coated on the current collector, the electrode material comprising the electrocatalyst.

[0030] The beneficial effects of this invention are: by anchoring transition metal copper and rare earth element cerium onto carbon and nitrogen materials through atomic confinement and coordination strategies, the CO2 can be effectively reduced to syngas with different proportions after the absence of metals is eliminated and the two metals are added. In terms of performance, the CuCe-NC catalyst with binuclear metal complex as the metal source is similar to a diatomic catalyst and has synergistic catalytic performance. It has a higher Faraday efficiency for CO in electrocatalytic carbon dioxide reduction and can regulate the ratio of CO to H2 from at least 0.6 to 1.5. Attached Figure Description

[0031] Figure 1 The images show the XRD patterns of the PCN-222 and Cu-PCN-222 materials of this invention.

[0032] Figure 2 This is a crystal structure diagram of Co2-abpt in Comparative Example 2 of the present invention.

[0033] Figure 3This is a crystal structure diagram of [Cu2(μ-adenine)4Cl2]Cl2 in Comparative Example 3 of the present invention.

[0034] Figure 4 These are TEM images of the CuCe-NC electrocatalyst (a) in Example 1 of the present invention, the Cu-Ce-NC electrocatalyst (b) in Comparative Example 1, and the Cu-NC catalyst (c) in Comparative Example 4.

[0035] Figure 5 This is a linear sweep voltammetry (LSV) chromatogram of the electrocatalytic carbon dioxide reduction of the CuCe-NC catalyst of this invention.

[0036] Figure 6 This is a linear sweep voltammetry (LSV) chromatogram of the electrocatalytic carbon dioxide reduction of the Cu-Ce-NC catalyst of this invention.

[0037] Figure 7 This is a linear sweep voltammetry (LSV) chromatogram of the electrocatalytic carbon dioxide reduction of the Cu-NC catalyst of this invention.

[0038] Figure 8 This is a linear sweep voltammetry (LSV) chromatogram of the electrocatalytic carbon dioxide reduction of the Ce-NC catalyst of this invention.

[0039] Figure 9 This is a linear sweep voltammetry (LSV) chromatogram of the electrocatalytic carbon dioxide reduction of the Co2-NC catalyst of this invention.

[0040] Figure 10 This is a linear sweep voltammetry (LSV) chromatogram of the electrocatalytic carbon dioxide reduction of the Cu2-NC catalyst of this invention.

[0041] Figure 11 This is a Faraday efficiency diagram of the electrocatalytic carbon dioxide reduction of the CuCe-NC catalyst of this invention.

[0042] Figure 12 This is a Faraday efficiency diagram of the electrocatalytic carbon dioxide reduction of the Cu-Ce-NC catalyst of the present invention.

[0043] Figure 13 This is a Faraday efficiency diagram of the electrocatalytic carbon dioxide reduction of the Cu-NC catalyst of the present invention.

[0044] Figure 14 This is a Faraday efficiency diagram of the electrocatalytic carbon dioxide reduction of the Ce-NC catalyst of the present invention. Detailed Implementation

[0045] The present invention will be further described in detail below through specific embodiments. Unless otherwise specified, the raw materials, reagents, or apparatus used in the embodiments and comparative examples are all available from conventional commercial sources or can be obtained by existing technical methods. Unless otherwise specified, the test or experimental methods are conventional methods in the art.

[0046] In this embodiment of the invention, the preparation method of PCN-222 is as follows:

[0047] In a 20 mL hydrothermal reactor, 108.6 mg of zirconium oxychloride octahydrate, 30 mg of tetrakis(4-carboxyphenyl)porphyrin and 0.45 mL of trifluoroacetic acid were added to 10 mL of N,N-dimethylformamide to dissolve them. The solution was then transferred to a 20 mL hydrothermal reactor and heated in an oven at 120 °C for 18 hours. After cooling to room temperature, the solution was washed and dried.

[0048] In this embodiment of the invention, the preparation method of Formula I ligand is as follows:

[0049]

[0050] 2.19 g of sodium hydride was added to 10 mL of dimethyl sulfoxide (DMSO), and a solution of 5.72 g of 2,3-dihydroxybenzaldehyde in DMSO (20 mL) was added dropwise over 2 h. Then, 9.72 g of triethylene glycol di(p-toluenesulfonate) was added, and the mixture was stirred under N2 conditions for 48 h. Water (300 mL) was added, and the mixture was washed with 10 mL of chloroform (CHCl3), retaining the aqueous layer. The aqueous layer was then acidified to pH 1 and extracted with CHCl3. The organic layer was washed with hydrochloric acid, dried over anhydrous magnesium sulfate, and rotary evaporated to obtain the crude product. The crude product was purified by column chromatography to obtain a pale yellow solid, which is the ligand of formula I.

[0051] Example 1

[0052] This embodiment prepares an electrocatalyst, and the specific process is as follows:

[0053] S1: Preparation of bimetallic complex: 50 mg of Formula I ligand was dissolved in 5 mL of methanol, 9 μ L of ethylenediamine and 40 mg of cerium acetate were added and reacted for 2 h, then copper nitrate trihydrate was added and reacted for 2 h; the bimetallic complex was obtained by rotary evaporation.

[0054] S2: Preparation of CuCe-NC electrocatalyst: 120 mg PCN-222 was added to an aqueous solution of 20 mg bimetallic complex prepared by S1 and 200 mg urea and stirred for 6 h. The mixture was filtered, washed three times with water, and freeze-dried for 36 h. The mixture was then calcined at 900 °C in an argon atmosphere for 2 h. Finally, it was acid-etched, washed, and dried to obtain the CuCe-NC electrocatalyst.

[0055] Comparative Example 1

[0056] This comparative example prepared an electrocatalyst, which differs from Example 1 in that it did not use Formula I ligand. The specific process is as follows:

[0057] Preparation of S1: Cu-PCN-222: 55 mg zirconium oxychloride, 4 mg tetrakis(4-carboxyphenyl)porphyrin copper, 12 mg tetrakis(4-carboxyphenyl)porphyrin and 220 μL trifluoroacetic acid were dissolved in 5 mL N,N-dimethylformamide, placed in a hydrothermal reactor, and heated at 120 °C for 18 h; finally, the mixture was washed and dried.

[0058] S2: Preparation of Cu-Ce-NC electrocatalyst: 120 mg Cu-PCN-222 was added to an aqueous solution of 12 mg cerium acetate and 200 mg urea and stirred for 6 h. The solution was filtered, washed three times with water, and freeze-dried for 36 h. The solution was then calcined at 900 °C in an argon atmosphere for 2 h, and finally acid etched, washed, and dried.

[0059] Comparative Example 2

[0060] This comparative example prepared an electrocatalyst, which differs from Example 1 in that it uses a different ligand. The specific process is as follows:

[0061] Co(NO3)2 (0.08 mM) was dissolved in anhydrous ethanol (4 mL), and then 2,2,3,5-bis(2-pyridyl)-4-amino-1,2,4-triazole (abpt) ligand (0.08 mM) was dissolved in dichloromethane (4 mL). Finally, the cobalt-containing ethanol solution was slowly added dropwise to the dichloromethane solution of the ligand. The two were immiscible and separated into layers. The mixture was sealed and left at room temperature for 2 days to obtain orange-red crystals, which were the [Co2(abpt)2(H2O)2(NO3)2]·2NO3 catalyst, referred to as Co2-abpt catalyst.

[0062] Comparative Example 3

[0063] This comparative example prepared an electrocatalyst, which differs from Example 1 in that it uses a different ligand. The specific process is as follows:

[0064] Copper chloride dihydrate (17.1 mg) was dissolved in 15 mL of methanol and slowly added dropwise to a methanol solution of adenine (27.3 mg) in 15 mL. The mixture was heated at 50 °C, and a blue precipitate appeared. After washing and drying, the precipitate was obtained as a catalyst for [Cu2(μ-adenine)4Cl2]Cl2.

[0065] Comparative Example 4

[0066] An electrocatalyst was prepared in this comparative example, and the specific process is as follows:

[0067] Preparation of S1: Cu-PCN-222: 55 mg zirconium oxychloride, 4 mg tetrakis(4-carboxyphenyl)porphyrin copper, 12 mg tetrakis(4-carboxyphenyl)porphyrin and 220 μL trifluoroacetic acid were dissolved in 5 mL N,N-dimethylformamide, placed in a hydrothermal reactor, and heated at 120 °C for 18 h; finally, the mixture was washed and dried.

[0068] S2: Preparation of Cu-NC catalyst: 120 mg Cu-PCN-222 was added to an aqueous solution of 200 mg urea and stirred for 6 h. The solution was filtered and washed three times with water, and then freeze-dried for 36 h. The catalyst was then calcined at 900 °C in an argon atmosphere for 2 h, and finally acid etched, washed and dried to obtain Cu-NC catalyst.

[0069] Comparative Example 5

[0070] An electrocatalyst was prepared in this comparative example, and the specific process is as follows:

[0071] 120 mg PCN-222 was added to an aqueous solution of 20 mg Co2-abpt and 200 mg urea and stirred for 6 h. The mixture was then filtered, washed three times with water, and freeze-dried for 36 h. The catalyst was then calcined at 900 °C in an argon atmosphere for 2 h, and finally etched, washed, and dried with acid to obtain the Co2-NC catalyst.

[0072] Comparative Example 6

[0073] An electrocatalyst was prepared in this comparative example, and the specific process is as follows:

[0074] 120 mg of PCN-222 was added to an aqueous solution of 20 mg [Cu2(μ-adenine)4Cl2]Cl2 and 200 mg of urea and stirred for 6 h. The mixture was then filtered, washed three times with water, and freeze-dried for 36 h. The catalyst was then calcined at 900 °C under an argon atmosphere for 2 h, and finally etched, washed, and dried with acid to obtain the Cu2-NC catalyst.

[0075] Comparative Example 7

[0076] An electrocatalyst was prepared in this comparative example, and the specific process is as follows:

[0077] 120 mg of PCN-222 was added to an aqueous solution of 20 mg of cerium acetate and 200 mg of urea and stirred for 6 h. The mixture was then filtered, washed three times with water, and freeze-dried for 36 h. The catalyst was then calcined at 900 °C under an argon atmosphere for 2 h, and finally etched, washed, and dried with acid to obtain the Ce-NC catalyst.

[0078] Experimental Example 1

[0079] This experimental example characterizes the structure of the material.

[0080] Figure 1 XRD patterns of PCN-222 and Cu-PCN-222 materials.

[0081] from Figure 1 It can be seen that both PCN-222 and Cu-PCN-222 were successfully synthesized; the catalyst maintained the structure of the parent PCN.

[0082] Figure 2 and Figure 3 These are the crystal structure diagrams of Co2-abpt and [Cu2(μ-adenine)4Cl2]Cl2, respectively.

[0083] Figure 4 These are transmission electron micrographs (TEM images) of the CuCe-NC electrocatalyst (a) prepared in Example 1, the Cu-Ce-NC electrocatalyst (b) prepared in Comparative Example 1, and the Cu-NC catalyst (c) prepared in Comparative Example 4.

[0084] from Figure 4 As can be seen, the catalyst is in the shape of nanorods, and the surface of the material has many micropores, which may be caused by the gas during the high-temperature volatilization and pyrolysis process. The porous structure can provide more catalytic sites.

[0085] Experimental Example 2

[0086] This experimental example tests the catalytic performance of the material. The specific procedure is as follows:

[0087] 1. The following steps are taken during the testing of the catalyst's electrocatalytic carbon dioxide reduction performance:

[0088] The catalyst was prepared into an electrode solution with a concentration of 2 mg / mL, consisting of 970 μL of ethanol and 30 μL of naphthol solution. 250 μL of the electrode solution was then uniformly dropped onto carbon cloth, resulting in a loading of 0.5 mg / cm³. 2 Cyclic voltammetry (CV), linear sweep voltammetry (LSV), and electrolysis (BE) tests were performed using an H-type electrolytic cell. The electrolyte used was 0.5 mol / L KHCO3, with a platinum sheet electrode as the counter electrode and an Ag / AgCl electrode as the reference electrode. LSV tests were performed under saturated carbon dioxide and saturated argon atmospheres, respectively, at a scan rate of 5 mV / s and a potential window of 0 V to -1.4 V (vs. RHE).

[0089] The results are as follows Figures 5-10 As shown, where, Figure 5 Linear sweep voltammetry (LSV) plot of electrocatalytic carbon dioxide reduction using CuCe-NC catalyst; Figure 6 Linear sweep voltammetry (LSV) plot of electrocatalytic carbon dioxide reduction using Cu-Ce-NC catalyst; Figure 7 Linear sweep voltammetry (LSV) plot of electrocatalytic carbon dioxide reduction using Cu-NC catalyst; Figure 8Linear sweep voltammetry (LSV) plot of electrocatalytic carbon dioxide reduction using Ce-NC catalyst; Figure 9 Linear sweep voltammetry (LSV) plot of electrocatalytic carbon dioxide reduction using Co2-NC catalyst; Figure 10 The image shows the linear sweep voltammetry (LSV) curve of the electrocatalytic reduction of carbon dioxide by the Cu2-NC catalyst.

[0090] from Figures 5-10 As can be seen, the Co2-NC and Cu2-NC catalysts did not catalyze the reduction of carbon dioxide (almost all of them produced hydrogen), while the polarization currents of the remaining catalysts in carbon dioxide were significantly greater than those in argon, indicating that the materials possess electrocatalytic carbon dioxide reduction performance. Among them, the CuCe-NC catalyst exhibits better electrocatalytic CO2 reduction performance and also has a higher current density, reaching 100 Mv / cm² at -1.3 (V vs. RHE). 2 Cu-Ce-NC and Cu-NC catalysts exhibit poor electrocatalytic CO2 reduction performance.

[0091] 2. The qualitative measurement method for electrocatalytic carbon dioxide reduction products is as follows:

[0092] Following the aforementioned preparation method, an H-type electrolytic cell was used for electrolysis, with BE electrolysis selected. The specific testing process was as follows: Carbon dioxide was bubbled into the electrolyte for 30 minutes to ensure that the CO2 gas in the electrolyte reached saturation. Then, electrolysis was performed in the electrolytic cell at different potentials (e.g., -1.1V, -1.0V, -0.9V, -0.8V).

[0093] Gas phase products were detected using a gas chromatograph (Shimadzu GC-2012): 0.2 mL of gas was extracted from the empty cavity of the electrolytic cell and injected into the gas chromatograph to obtain chromatographic information. The product and yield were determined by the peak position and peak area. The Faraday efficiency was determined by the ideal gas law and Faraday formula and plotted as a bar chart.

[0094] The results are as follows Figures 11-14 As shown in the figure, the dark-colored columns at the bottom represent H2, and the light-colored columns at the top represent CO. Figure 11 The Faraday efficiency diagram for the electrocatalytic carbon dioxide reduction of the CuCe-NC catalyst; Figure 12 The Faraday efficiency diagram for the electrocatalytic reduction of carbon dioxide by the Cu-Ce-NC catalyst; Figure 13 The diagram shows the Faraday efficiency of the Cu-NC catalyst for the electrocatalytic reduction of carbon dioxide. Figure 14 The Faraday efficiency diagram for the electrocatalytic reduction of carbon dioxide using Ce-NC catalyst.

[0095] from Figure 11As can be seen, the prepared CuCe-NC catalyst has a proportional relationship between the electrocatalytic reduction of CO2 to CO and the generated H2. The Faradaic efficiency of CO can reach about 50% within the potential electrolysis window of -0.8V to -1.1V.

[0096] from Figure 12 As can be seen, the CO and H2 produced by the electrocatalytic reduction of CO2 by the prepared Cu-Ce-NC catalyst are in a proportional relationship, but there is slightly more hydrogen and poor CO selectivity.

[0097] from Figure 13 It can be seen that the CO and H2 produced by the electrocatalytic reduction of CO2 by the prepared Cu-NC catalyst are in a proportional relationship, with hydrogen being produced more.

[0098] from Figure 14 The prepared Ce-NC catalyst showed that the electrocatalytic reduction of CO2 yielded slightly less CO than H2.

[0099] Comparing the catalytic performance of the four catalysts, the atomic confinement and coordination strategies of this invention are successful. All four catalysts show a proportional relationship between the Faraday efficiencies of CO and H2, and the ratio decreases. However, the CO selectivity of this invention, which uses a binuclear complex as the metal source, is higher. The confinement effect of the Formula I complex on the bimetal and the synergistic effect of the Cu and Ce bimetals make the CuCe-NC catalyst more selective for CO in the electrocatalytic reduction of CO2. Furthermore, the composition of CO and H2 is adjustable, with the ratio ranging from 0.67 to 1.5.

[0100] The above embodiments are preferred embodiments of the present invention, but the embodiments of the present invention are not limited to the above embodiments. Any changes, modifications, substitutions, combinations, or simplifications made without departing from the spirit and principle of the present invention shall be considered equivalent substitutions and shall be included within the protection scope of the present invention.

Claims

1. An electrocatalyst, characterized in that: The product includes a support and an active ingredient. The support comprises a carbon-nitrogen material, and the active ingredient comprises Cu and Ce. Cu and Ce are confined by coordination bonds of formula I ligands. ； The raw materials for preparing the electrocatalyst include MOF materials, nitrogen source, Cu salt, Ce salt and formula I ligand; The preparation method of the electrocatalyst includes the following steps: S1: Bimetallic complexes are prepared by coordinating Cu salt, Ce salt and formula I ligand. S2: After reacting the bimetallic complex, MOF material with a nitrogen source, the mixture is freeze-dried, calcined under an inert atmosphere, and then acid-etched to obtain an electrocatalyst; the calcination temperature is 800℃~1000℃ and the time is 1h~4h.

2. The electrocatalyst according to claim 1, characterized in that: In the electrocatalyst, the molar ratio of Cu to Ce is (0.9~1.1):(0.9~1.1).

3. The electrocatalyst according to claim 1, characterized in that: In the electrocatalyst, the mass ratio of the support to the active ingredient is (497~499):(1~3).

4. The electrocatalyst according to claim 1, characterized in that: The MOFs materials include any one of HKUST-1, M2(dobpdc), MIL-100, MIL-101, MIL-53, MOF-74, NU-1000, PCN-222, PCN-224, UiO-66, UiO-67, ZIF-8, and ZIFs.

5. A method for preparing an electrocatalyst as described in any one of claims 1 to 4, characterized in that: Includes the following steps: S1: Bimetallic complexes are prepared by coordinating Cu salt, Ce salt and formula I ligand. S2: After reacting the bimetallic complex, MOF material with a nitrogen source, the mixture is freeze-dried, calcined under an inert atmosphere, and then acid-etched to obtain an electrocatalyst; the calcination temperature is 800℃~1000℃ and the time is 1h~4h.

6. The method for preparing the electrocatalyst according to claim 5, characterized in that: Specifically, S1 involves dissolving the formula I ligand in an organic solvent, adding ethylenediamine and Ce salt to react, then adding Cu salt to react, and finally evaporating to obtain a bimetallic complex.

7. The method for preparing the electrocatalyst according to claim 5, characterized in that: In S2, the mass ratio of the bimetallic complex to the MOFs material is (3~4):(24~26).

8. A battery electrode, characterized in that: It includes a current collector and an electrode material coated on the current collector, the electrode material including the electrocatalyst as described in any one of claims 1 to 4.

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