CN115704097A - M 1 M 2 Preparation method and application of diatomic catalyst with support structure - Google Patents
M 1 M 2 Preparation method and application of diatomic catalyst with support structure Download PDFInfo
- Publication number
- CN115704097A CN115704097A CN202110928569.4A CN202110928569A CN115704097A CN 115704097 A CN115704097 A CN 115704097A CN 202110928569 A CN202110928569 A CN 202110928569A CN 115704097 A CN115704097 A CN 115704097A
- Authority
- CN
- China
- Prior art keywords
- catalyst
- metal
- oxide
- carbon
- carrier
- Prior art date
- Legal status (The legal status is an assumption and is not a legal conclusion. Google has not performed a legal analysis and makes no representation as to the accuracy of the status listed.)
- Pending
Links
Images
Classifications
-
- Y—GENERAL TAGGING OF NEW TECHNOLOGICAL DEVELOPMENTS; GENERAL TAGGING OF CROSS-SECTIONAL TECHNOLOGIES SPANNING OVER SEVERAL SECTIONS OF THE IPC; TECHNICAL SUBJECTS COVERED BY FORMER USPC CROSS-REFERENCE ART COLLECTIONS [XRACs] AND DIGESTS
- Y02—TECHNOLOGIES OR APPLICATIONS FOR MITIGATION OR ADAPTATION AGAINST CLIMATE CHANGE
- Y02E—REDUCTION OF GREENHOUSE GAS [GHG] EMISSIONS, RELATED TO ENERGY GENERATION, TRANSMISSION OR DISTRIBUTION
- Y02E60/00—Enabling technologies; Technologies with a potential or indirect contribution to GHG emissions mitigation
- Y02E60/30—Hydrogen technology
- Y02E60/50—Fuel cells
Abstract
The invention relates to a M 1 M 2 A preparation method and application of diatomic catalyst with a carrier structure. The active center of the diatomic catalyst comprises two distances of
Metal M of 1 And M 2 Atom, the metal M 1 、M 2 The same or different, and is independently selected from one of Mg, V, cr, mn, fe, co, ni, cu, zn, sn, ru, rh, pd, ir, pt, ag and Au, and the carrier is a carbon-based carrier or metal oxide. The preparation method of the catalyst comprises the steps of loading the binuclear complex serving as a precursor on a carrier and preparing the binuclear complex by high-temperature pyrolysis in an inert atmosphere. The diatomic catalyst has electrochemical activity and has application prospects of electrocatalytic oxygen reduction, electrocatalytic carbon dioxide reduction and electrocatalytic oxygen production.
Description
Technical Field
The invention belongs to the technical field of electrochemical reaction, and particularly relates to a diatomic catalyst, a preparation method and electrochemical reaction activity.
Background
The monatomic catalyst enables active sites to be dispersed in an atomic form, can maximize the utilization of active substances, and has important significance for reducing the dosage of the catalyst and improving the catalytic activity. However, the types of the active sites of the monatomic catalyst are relatively single, and the targeted optimization aiming at specific catalytic reactions is difficult to carry out. The diatomic catalyst comprises two metal centers which are close to each other in distance, the types of the metal centers can be the same or different, the types and the structures of active sites are greatly expanded, the precise regulation and control of the active sites are convenient for specific catalytic reaction, the structural characteristics that the active sites of the monatomic catalyst are dispersed in an atomic level are kept, and the efficient utilization of the active sites is ensured. However, the directed synthesis method of the diatomic catalyst is still lack of reports.
The development of a general synthesis method of the diatomic catalyst is of great significance for promoting the development of the diatomic catalyst.
Disclosure of Invention
The invention discloses a structure M 1 M 2 -a general preparation process of a supported diatomic catalyst comprising: loading a binuclear complex serving as a precursor on a carrier, and preparing the binuclear complex by high-temperature pyrolysis in an inert atmosphere; wherein the binuclear complex structure can be represented as:
M 1 M 2 L·Xn
wherein M is 1 、M 2 Represents metal atoms, can be Mg, V, cr, mn, fe, co, ni, cu, zn, sn, ru, rh, pd, ir, pt, ag and Au, the species of the two metal atoms can be same or different, and the distance between the two metal atoms in the complex is
L represents a ligand around the metal atom, which must contain five or more coordinating atoms selected from one or more of nitrogen, oxygen, sulfur, phosphorus; more preferably, the basic structural unit contained in the ligand is selected from a group unit such as carbene, pyridine, pyrrole, amino, schiff base, hydroxyl, carboxyl, carbonyl and the like.
X represents for balancing the overall chargeA counter ion, n is the number of counter ions required to make the complex electrically neutral as a whole, when n>When 1, when n>In case 1, the counter ion is plural, and the counter ions are the same as or different from each other. The counter ion is typically an anion, including but not limited to halide, nitrate, sulfate, phosphate, acetate, oxalate, OH - And the like.
More preferably, the L ligand is preferably a ligand having the structure:
wherein X is N, O, S or a P heteroatom, R 1 Substituted at any suitable position of the phenyl ring, R 1 Is selected from C 1-6 Alkyl radical, C 2-6 Alkenyl, halogen, C 6-20 Aryl, -OC 1-6 Alkyl, -OC 2-6 An alkenyl group; y is alkenylene (-CH = CH-), propylene (-CH) 2 CH 2 CH 2 -), 1,2-phenylene, one or both of which may be further substituted with R on the Y group 1 And (4) substitution.
Further, the dinuclear complex is preferably selected from:
the loading may be carried out using any means known in the art, including impregnation, adsorption, incipient wetness, precipitation, spray drying, and the like. The invention preferably uses an impregnation method, can prepare a binuclear complex solution with proper mass (or volume) according to the adsorption capacity of the carrier, ensures that the mass of the solution is 1-20 times of the adsorption capacity of the carrier, preferably the mass of the solution is 1-10 times, more preferably 1-5 times of the adsorption capacity of the carrier, mixes the carrier and the solution, fully stirs, preferably stirs for 5-400 minutes, and separates to obtain the supported catalyst precursor.
Under inert atmosphere means in the presence of a non-reactive gas selected from nitrogen, argon. The temperature of the high-temperature pyrolysis is selected from 300-1000 ℃. The pyrolysis time is from 0.2 to 20 hours, preferably from 0.5 to 8 hours.
The invention discloses a structure M 1 M 2 A supported diatomic catalyst, the active center of which comprises two diatomic sites each present in a monoatomic state and which are at a distance from each other
Metal M of 1 And M 2 Atom, the metal M 1 、M 2 The same or different, independently selected from one of Mg, V, cr, mn, fe, co, ni, cu, zn, sn, ru, rh, pd, ir, pt, ag and Au, preferably transition metal Fe, co, ni, cu, zn and Sn; the carrier is carbon-based carrier or metal oxide, and the carbon-based material is selected from Norit, ketjen Black, vulcan, black Pearl, acetylene Black, carbon nanotube, graphene, and carbon nitride (g-C) 3 N 4 ) Nitrogen-doped carbon, and the like, and the metal oxide is selected from metal oxide carriers such as cerium oxide, zinc oxide, aluminum oxide, zirconium oxide, magnesium oxide, molybdenum oxide, tungsten oxide, and the like.
The invention also discloses the use of the diatomic catalyst in electrochemical reactions, including electrocatalytic oxygen reduction, electrocatalytic carbon dioxide reduction and electrocatalytic oxygen generation, wherein M is the metal loading of 0.1-20wt%, preferably 0.1-10wt%, based on the total weight of the catalyst 1 Or M 2 Selected from Ru, rh, pd, ir, pt, ag and Au.
When the electrocatalytic oxygen reduction reaction is tested by a rotating disk electrode, the used electrolyte can be sulfuric acid, perchloric acid, sodium hydroxide and potassium hydroxide, when an acid electrolyte is used, the concentration of hydrogen ions in the electrolyte can be 0.1-1mol/L, and when an alkaline electrolyte is used, the concentration of hydroxyl ions in the electrolyte can be 0.1-1mol/L.
When the electrocatalytic carbon dioxide reduction reaction is tested by a gas diffusion electrode, the used electrolyte can be potassium bicarbonate or sodium bicarbonate solution, and the concentration can be 0.1-1mol/L.
When the electrocatalytic oxygen production reaction is tested by a rotating disk electrode, the used electrolyte can be sodium hydroxide solution or potassium hydroxide solution, and the concentration can be 0.1-5mol/L.
The separation state in the monoatomic site state, the monoatomic distribution, the monoatomic morphology, or the monoatomic level in the present invention means a state in which the metal atoms (ions) of the active metal elements are separated from each other independently, and the metal-metal bonds or the metal-O-metal bonds that are directly connected to each other are not formed between the active metal atoms, and are dispersed in the atomic level or in the monoatomic site state. Metals dispersed in the monoatomic site state may exist in the atomic state, may exist in the ionic state, and more may exist between the atomic and ionic states (the bond length is between two bond lengths). In the metal nanocrystalline, metal atoms in the same nanocrystalline are mutually bonded and do not belong to a monoatomic state or a monoatomic separation state defined by the patent; for oxide nanocrystals formed by metals and oxygen elements, although the metals are separated by oxygen elements, there is still a possibility that the internal metals are directly connected to each other, and the metal nanocrystals in the metallic state described above are formed after the reduction reaction, which is not in the monoatomic site state or the monoatomic separation state as defined in this patent. The metals in the monatomic site state claimed by this patent are theoretically completely independent of each other. However, random deviations from batch-to-batch manufacturing operating condition control do not preclude the presence of small amounts of agglomerated metal species, such as clusters containing one-site numbers of atoms or ions, in the resulting product; nor does it exclude that part of the metal is in the nanocrystalline state. In other words, it is possible that the active metal exists in a single-atom-site dispersed state in the catalyst of the present invention, while a cluster state containing an aggregation of metal atoms exists in part, and/or a part of the metal assumes a nanocrystalline state. And the monatomic state is transformed to the cluster and/or nano-state as the external environment changes.
Drawings
FIG. 1 is a transmission electron micrograph of an Fe2/NC catalyst.
FIG. 2 is a photograph of a Fe2/NC catalyst by spherical aberration correction transmission electron microscopy.
FIG. 3 is a linear sweep voltammogram of oxygen reduction of Fe2/NC catalyst versus commercial Pt/C catalyst in 0.5M H2SO4 electrolyte.
FIG. 4 is a linear sweep voltammogram of oxygen reduction of Co2/KB catalyst versus commercial Pt/C catalyst in a 1M KOH electrolyte.
FIG. 5 shows the Faraday efficiency (left) and stability (right) of electrochemical reduction of Ni2/BP catalyst in 0.5M KHCO3 electrolyte with carbon dioxide.
FIG. 6 is a polarization curve of the oxygen evolution reaction of a diatomic catalyst in 1M KOH electrolyte.
Detailed Description
Raw materials or products used in the examples:
NC: nitrogen-doped carbon support
KB: activated carbon KetjenBlack EC-300J
BP: activated carbon BALCK PEARLS 2000
Pt/C: commercial platinum carbon catalyst
IrO/C: from literature description information
Example 1 metallic Fe Supports of 2wt% Fe 2 The catalyst is characterized by/NC:
preparing a nitrogen-doped carbon carrier: 1.6g of Zn (NO) are weighed out 3 ) 2 ·6H 2 O and 3.7g of 2-methylimidazole were dissolved in 80mL of methanol, respectively. And mixing the two solutions, stirring for 24 hours at room temperature, performing centrifugal separation, washing with methanol, and drying to obtain ZIF-8 powder. And (3) placing 400mg of ZIF-8 into a porcelain boat, heating to 1000 ℃ at a speed of 5 ℃/min under a nitrogen atmosphere, keeping for 3 hours, and naturally cooling to obtain the nitrogen-doped carbon carrier.
Fe 2 Preparation of NC catalyst: 10mg of Fe are weighed 2 Complex Fe 2 (C 24 H 26 N 4 O 2 )Cl 2 Dispersing in 1/1 volume ratio methanol-water solution, then dispersing 90mg nitrogen-doped carbon in another 1/1 volume ratio methanol-water solution, mixing the two solutions, stirring for 2 hr, filtering, and drying. Raising the temperature to 800 ℃ at the speed of 5 ℃/min under the flowing nitrogen atmosphere, preserving the heat for 2 hours, and naturally cooling to room temperature to obtain Fe 2 (ii)/NC catalyst. The morphology of the catalyst is shown in fig. 1 and fig. 2, and diatomic sites are marked by circles in fig. 2.
The chemical formula of the complex precursor is Fe 2 (C 24 H 26 N 4 O 2 )Cl 2 The structural formula is as follows:
example 2: co with metal Co loading of 4wt% 2 catalyst/KB
Preparing a catalyst: weighing 20mg of Co 2 Complex Co 2 (C 30 H 22 N 4 O 2 )(NO 3 ) 2 Dispersing in 1/1 volume ratio methanol-water solution, then taking 80mg of activated carbon (KetjenBlack EC-300J) to disperse in another 1/1 volume ratio methanol-water solution, and then mixing the two solutions, stirring for 2 hours, rotary steaming and drying. Heating to 500 ℃ at a speed of 5 ℃/min under the flowing argon atmosphere, preserving heat for 2 hours, and naturally cooling to room temperature to obtain Co 2 A catalyst of/KB. The chemical formula of the complex precursor is Co 2 (C 30 H 22 N 4 O 2 )(NO 3 ) 2 The structural formula is as follows:
example 3: metallic Ni supporting amount of 4wt% Ni 2 BP catalyst
Metallic Ni supporting amount of 4wt% Ni 2 Preparation of BP catalyst: weighing 20mg of Ni 2 Complex Ni 2 (C 24 H 26 N 4 O 2 )Cl 2 (H 2 O) 2 Dispersing in 1/1 volume ratio methanol-water solution, then dispersing 80mg of activated carbon (BALCK PEARLS 2000) in another 1/1 volume ratio methanol-water solution, mixing the two solutions, stirring for 2 hours, rotary steaming, and drying. Heating to 300 ℃ at a speed of 5 ℃/min under the flowing argon atmosphere, preserving heat for 2 hours, and naturally cooling to room temperature to obtain Ni 2 a/BP catalyst. The chemical formula of the complex precursor is Ni 2 (C 24 H 26 N 4 O 2 )Cl 2 (H 2 O) 2 The structural formula is as follows:
example 4: feNi/C catalyst with total metal loading of 5wt%
FeNi/C catalyst preparation with an overall metal loading of 5 wt%: weighing 25mg of FeNi complex FeNi (C) 24 H 26 N 4 O 2 )Cl 2 (H 2 O) 2 Dispersing in 1/1 volume ratio methanol-water solution, dispersing 80mg of activated carbon (Vulcan XC-72) in another 1/1 volume ratio methanol-water solution, mixing the two solutions, stirring for 2 hr, rotary steaming, and drying. Raising the temperature to 300 ℃ at a speed of 5 ℃/min under the flowing nitrogen atmosphere, preserving the heat for 2 hours, and naturally cooling to the room temperature to obtain the FeNi/C catalyst. Other comparative sample preparation methods: replacement of the FeNi complex by Fe as used in example 1 2 Co used in example 2 2 And Ni used in example 3 2 Otherwise unchanged, fe is obtained 2 /C，Co 2 /C，Ni 2 a/C catalyst.
The chemical formula of the complex precursor is FeNi (C) 27 H 24 N 4 O 2 )(NO 3 ) 3 The structural formula is as follows:
application test example
Test example 1: oxygen reduction Performance test
Fe testing using a rotating disk electrode 2 The oxygen reduction performance of/NC catalysts, test methods reference nat. Cat., 2019,2,259-268. The specific test method is that the temperature is 25 ℃, and the used electrolyte is 0.5M H saturated by oxygen 2 SO 4 In the water solution, a working electrode is a glassy carbon material rotating disc electrode with the diameter of 5mm, and the rotating speed is 1600rpm; the counter electrode is a platinum wire and the reference electrodeIs a saturated Ag/AgCl electrode. The reference electrode potential was corrected by a reversible hydrogen electrode. 5mg of Fe are weighed 2 The catalyst ink was prepared by adding 990. Mu.L of isopropyl alcohol and 10. Mu.L of 5% nafion solution to the/NC catalyst (product of example 1) and ultrasonically dispersing the mixture, and 30. Mu.L of the catalyst ink was dropped onto a rotating disk electrode and air-dried. The scan rate for the oxygen reduction test was 10mV/s. The results of the rotating disk electrode testing of the catalyst are shown in figure 3 and table 1.
It can be seen that Fe 2 The half-wave potential of the/NC catalyst under the acidic condition reaches 0.814V vs RHE, and although a certain difference is still existed compared with the commercial Pt/C catalyst, the catalyst has prominent performance in the non-noble metal oxygen reduction catalyst.
TABLE 1
Test example 2: and (3) testing oxygen reduction performance:
testing of Co Using rotating disk electrodes 2 Oxygen reduction performance of/KB catalyst, test method reference j.electrochem.soc.,2018,165, j3001-J3007. The specific test method is that the temperature is 25 ℃, the electrolyte used is 0.1M KOH aqueous solution saturated by oxygen, the working electrode is a glassy carbon material rotating disk electrode with the diameter of 5mm, and the rotating speed is 1600rpm; the counter electrode was a platinum wire and the reference electrode was a Hg/HgO electrode (1M KOH). The reference electrode potential was corrected by a reversible hydrogen electrode. Weighing 5mg of Co 2 The catalyst ink was prepared by adding 900. Mu.L of water and 100. Mu.L of 5% nafion solution to the catalyst ink (example 2), dropping 20. Mu.L of the catalyst ink on a rotating disk electrode, and air-drying the catalyst ink. The scan rate for the oxygen reduction test was 5mV/s. The results of the rotating disk electrode testing of the catalyst are shown in figure 4 and table 2. It can be seen that Co is present under alkaline conditions 2 the/KB catalyst has a higher half-wave potential (0.892V vs RHE) than the commercial Pt/C, indicating that Co 2 the/KB catalyst has good oxygen reduction performance.
TABLE 2
Test example 3: and (3) testing the reduction performance of carbon dioxide:
testing of Ni Using gas diffusion electrodes 2 Carbon dioxide reduction performance of/BP catalysts, test methods reference nat. Commun.,2021,12,3264. The specific test method is that the temperature is 25 ℃, an H-shaped electrolytic cell separated by a nafion 211 membrane is used, and the electrolyte is 0.5M KHCO saturated by carbon dioxide 3 Aqueous solution, working electrode gas diffusion electrode area 1cm 2 The counter electrode is a carbon rod electrode, and the reference electrode is a saturated Ag/AgCl electrode. The gas phase product is detected on line by gas chromatography, and the liquid phase product is detected by nuclear magnetic resonance hydrogen spectrum after the reaction is finished. Weighing 5mg of Ni 2 The catalyst ink was prepared by adding 700. Mu.L of isopropyl alcohol, 200. Mu.L of water and 100. Mu.L of 5% -percent nafion solution to the/BP catalyst, ultrasonically dispersing the mixture, and then 100. Mu.L of the catalyst ink was dropped onto the gas diffusion electrode and air-dried. The scan rate for the carbon dioxide reduction test was 5mV/s. The results of the carbon dioxide reduction performance test of the catalyst are shown in fig. 5. It can be seen that Ni 2 the/BP catalyst reduces CO in the voltage range of-0.65 to-1V vs RHE 2 The faradaic efficiency to CO was over 90% and the performance was maintained after 2h of continuous reaction.
Test example 4: and (3) testing the electrochemical oxygen generation performance:
the electrochemical oxygen generation performance of the FeNi/C catalyst was tested using a rotating disk electrode, test methods reference j.electrochem.soc.,2019,166, F458-F464. The temperature is 25 ℃, the electrolyte used is 1MKOH aqueous solution saturated by nitrogen, and the diameter of the glassy carbon material rotating disk electrode is 5mm. Weighing 5mg FeNi/C catalyst, adding 990 μ L isopropanol and 10 μ L5% nafion solution, ultrasonically dispersing to obtain catalyst ink, dripping 25 μ L catalyst ink on a rotary disk electrode, and naturally drying. The rotation speed of the electrochemical oxygen production test is 1600rpm, and the scanning speed is 10mV/s. Other comparative catalysts were tested for electrochemical oxygen generation performance under the same conditions. The results of the electrochemical oxygen production performance test of the catalyst are shown in fig. 6 and table 3. According to the document ACS Nano,2017,11,11031-11040 reports, commercial IrO 2 10mA cm of/C in 1M KOH electrolyte -2 The overpotential is 360mV, and it can be seen that the FeNi/C catalyst shows far better than commercial IrO 2 Oxygen evolution behaviour of/C (overpotential 287 mV), while Fe 2 /C、Co 2 C and Ni 2 the/C also shows near commercial IrO 2 Oxygen evolution performance of/C.
TABLE 3
And (4) conclusion: the diatomic catalyst of the present invention has a variety of electrochemical activities including oxygen reduction activity, carbon dioxide reduction activity and water decomposition oxygen evolution reaction activity. Particularly, the invention uses non-noble metal as an active center, the corresponding electrochemical activity of the non-noble metal is more than or slightly lower than that of a corresponding noble metal catalyst, the noble metal can be replaced in the fields of new energy sources such as fuel cells, electrolyzed water and the like, and the good industrial economy is shown.
The above examples are given for the purpose of illustrating the invention clearly and not for the purpose of limiting the same, and it will be apparent to those skilled in the art that, in light of the foregoing description, numerous modifications and variations can be made in the form and details of the embodiments of the invention described herein, and it is not intended to be exhaustive or to limit the invention to the precise forms disclosed.
Claims (9)
1. M 1 M 2 -a process for the preparation of a diatomic catalyst of support structure comprising: loading the binuclear complex serving as a precursor on a carrier, and pyrolyzing the binuclear complex at high temperature in an inert atmosphere to obtain the binuclear complex; wherein, catalyst M 1 、M 2 Loaded on a carrier in a respective atomic state with a distance between two metal atoms of
The carrier is a carbon-based carrier or a metal oxide;
the binuclear complex structure can representComprises the following steps: m 1 M 2 L·Xn
M 1 、M 2 Represent metal atoms, equal to or different from each other, independently selected from Mg, V, cr, mn, fe, co, ni, cu, zn, sn, ru, rh, pd, ir, pt, ag or Au; the distance between two metal atoms in the complex is
L represents a ligand coordinated with a metal atom, and the ligand compound comprises at least five coordination atoms, wherein the coordination atoms are selected from one or more of nitrogen, oxygen, sulfur and phosphorus; further preferably, the basic structural unit containing coordination atoms in the ligand is selected from carbene, pyridine, pyrrole, amino, schiff base, hydroxyl, carboxyl and carbonyl group units; x represents a counter ion for balancing the overall charge, n is the number of counter ions required to render the complex electrically neutral overall, when n is>In case 1, the counter ion is plural, and the counter ions are the same as or different from each other.
2. The process according to claim 1, wherein the ligand L is preferably a ligand having the structure:
wherein X is N, O, S or a P heteroatom, R 1 Substituted at any suitable position of the phenyl ring, R 1 Is selected from C 1-6 Alkyl radical, C 2-6 Alkenyl, halogen, C 6-20 Aryl, -OC 1-6 Alkyl, -OC 2-6 An alkenyl group; y is alkenylene (-CH = CH-), propylene (-CH) 2 CH 2 CH 2 -), 1,2-phenylene, one or both of which may be further substituted with R on the Y group 1 Substitution; the carbon-based material is selected from Norit, ketjen Black, vulcan, black Pearl, acetylene Black, carbon nanotube, graphene, and carbon nitride (g-C) 3 N 4 ) Nitrogen-doped carbon, and the like, and the metal oxide is selected from metal oxide carriers such as cerium oxide, zinc oxide, aluminum oxide, zirconium oxide, magnesium oxide, molybdenum oxide, tungsten oxide, and the like.
3. The process according to claim 1 or 2, wherein the dinuclear complex is preferably selected from:
4. the method according to any one of claims 1 to 3, wherein the carrier is selected from Norit, ketjen Black, vulcan, black Pearl, acetylene Black, carbon nanotube, graphene, carbon nitride (g-C) 3 N 4 ) And nitrogen-doped carbon.
5. The process according to any one of claims 1 to 4, wherein the loading is carried out by any means known in the art, including impregnation, adsorption, incipient wetness, precipitation, spray drying.
6. The method according to any one of claims 1 to 5, wherein the inert atmosphere is a non-reactive gas selected from the group consisting of nitrogen, argon; the temperature of the high-temperature pyrolysis is selected from 300-1000 ℃; the pyrolysis time is from 0.2 to 20 hours, preferably from 0.5 to 8 hours.
7. A structure of M 1 M 2 A supported diatomic catalyst, the active center of which comprises two diatomic sites each present in a monoatomic state and which are at a distance from each other
Metal M of 1 And M 2 Atom, the metal M 1 、M 2 The same or different, are independently selected from Mg, V, cr, mn, fe, co, ni, cu, zn, sn, ru, rh,Pd, ir, pt, ag and Au, wherein the carrier is a carbon-based carrier or a metal oxide.
8. The catalyst according to claim 7, wherein the metal is selected from the group consisting of transition metals Fe, co, ni, cu, zn, and the metal loading is 0.1-20wt%, preferably 0.1-10wt%, based on the total weight of the catalyst; the carbon-based material is selected from Norit, ketjen Black, vulcan, black Pearl, acetylene Black, carbon nanotube, graphene, and carbon nitride (g-C) 3 N 4 ) Nitrogen-doped carbon; the metal oxide is selected from cerium oxide, zinc oxide, aluminum oxide, zirconium oxide, magnesium oxide, molybdenum oxide, and tungsten oxide.
9. Use of the catalyst of claim 7 or 8 for electrochemical reactions including electrocatalytic oxygen reduction, electrocatalytic carbon dioxide reduction, electrocatalytic oxygen production.
Priority Applications (1)
| Application Number | Priority Date | Filing Date | Title |
|---|---|---|---|
| CN202110928569.4A CN115704097A (en) | 2021-08-13 | 2021-08-13 | M 1 M 2 Preparation method and application of diatomic catalyst with support structure |
Applications Claiming Priority (1)
| Application Number | Priority Date | Filing Date | Title |
|---|---|---|---|
| CN202110928569.4A CN115704097A (en) | 2021-08-13 | 2021-08-13 | M 1 M 2 Preparation method and application of diatomic catalyst with support structure |
Publications (1)
| Publication Number | Publication Date |
|---|---|
| CN115704097A true CN115704097A (en) | 2023-02-17 |
Family
ID=85181058
Family Applications (1)
| Application Number | Title | Priority Date | Filing Date |
|---|---|---|---|
| CN202110928569.4A Pending CN115704097A (en) | 2021-08-13 | 2021-08-13 | M 1 M 2 Preparation method and application of diatomic catalyst with support structure |
Country Status (1)
| Country | Link |
|---|---|
| CN (1) | CN115704097A (en) |
Cited By (2)
| Publication number | Priority date | Publication date | Assignee | Title |
|---|---|---|---|---|
| CN115064705A (en) * | 2022-07-05 | 2022-09-16 | 清华大学 | Catalyst of dissimilar metal atom pair, preparation method and application thereof |
| CN116759593A (en) * | 2023-06-14 | 2023-09-15 | 哈尔滨工业大学 | Ru-M bimetallic monoatomic catalyst and preparation method and application thereof |
-
2021
- 2021-08-13 CN CN202110928569.4A patent/CN115704097A/en active Pending
Cited By (3)
| Publication number | Priority date | Publication date | Assignee | Title |
|---|---|---|---|---|
| CN115064705A (en) * | 2022-07-05 | 2022-09-16 | 清华大学 | Catalyst of dissimilar metal atom pair, preparation method and application thereof |
| CN116759593A (en) * | 2023-06-14 | 2023-09-15 | 哈尔滨工业大学 | Ru-M bimetallic monoatomic catalyst and preparation method and application thereof |
| CN116759593B (en) * | 2023-06-14 | 2024-01-12 | 哈尔滨工业大学 | Ru-M bimetallic monoatomic catalyst and preparation method and application thereof |
Similar Documents
| Publication | Publication Date | Title |
|---|---|---|
| Cai et al. | Bi-modified Pd/C catalyst via irreversible adsorption and its catalytic activity for ethanol oxidation in alkaline medium | |
| Qin et al. | Ultrathin IrRu nanowire networks with high performance and durability for the hydrogen oxidation reaction in alkaline anion exchange membrane fuel cells | |
| KR101797782B1 (en) | Catalyst with metal oxide doping for fuel cells | |
| Shao et al. | Boosting oxygen evolution by surface nitrogen doping and oxygen vacancies in hierarchical NiCo/NiCoP hybrid nanocomposite | |
| KR100868756B1 (en) | Pt/Ru alloy supported catalyst, manufacturing method thereof, and fuel cell using the same | |
| da Silva et al. | PdPt-TiO2 nanowires: correlating composition, electronic effects and O-vacancies with activities towards water splitting and oxygen reduction | |
| US20120094199A1 (en) | Catalyst for electrochemical applications | |
| CN114293223B (en) | Method for preparing superfine cerium dioxide supported metal monoatomic catalyst from cluster-based framework material | |
| CN111569928B (en) | MOFs-derived carbon-based material anchored high-dispersion metal Pt nanocluster and preparation method and application thereof | |
| CN114108004B (en) | Ruthenium-based alloy catalyst and preparation method and application thereof | |
| Zignani et al. | Investigation of PtNi/C as methanol tolerant electrocatalyst for the oxygen reduction reaction | |
| KR20200001064A (en) | The platinum-transition metal composite supported on carbon and method for preparing the same | |
| CN111668501B (en) | Fuel cell anode catalyst and preparation method and application thereof | |
| CN115704097A (en) | M 1 M 2 Preparation method and application of diatomic catalyst with support structure | |
| Chalgin et al. | Ternary Pt–Pd–Ag alloy nanoflowers for oxygen reduction reaction electrocatalysis | |
| CN112002915B (en) | Oxygen electrode bifunctional catalyst, preparation method and application | |
| Rahmani et al. | Excellent electro-oxidation of methanol and ethanol in alkaline media: Electrodeposition of the NiMoP metallic nano-particles on/in the ERGO layers/CE | |
| US7625660B2 (en) | Fuel cell and membrane electrode assembly | |
| CN110380069A (en) | A kind of noble metal catalyst of active carbon confinement and preparation method thereof and application | |
| Du et al. | Novel Pd 13 Cu 3 S 7 nanotubes with high electrocatalytic activity towards both oxygen reduction and ethanol oxidation reactions | |
| Sheelam et al. | Iron (III) chloride-benzotriazole adduct for oxygen reduction reaction in alkaline medium | |
| Belenov et al. | PtCu/C materials doped with different amounts of gold as the catalysts of oxygen electroreduction and methanol electrooxidation | |
| US20220416260A1 (en) | Hybrid catalyst suitable for use in proton exchange membrane fuel cell | |
| Feng et al. | Facile pyrolysis synthesis of abundant FeCo dual-single atoms anchored on N-doped carbon nanocages for synergistically boosting oxygen reduction reaction | |
| KR102425951B1 (en) | Method of preparing transition metal nanoparticle-decorated manganese oxide nanorod electrocatalysts and nanorod electrocatalysts prepared thereby |
Legal Events
| Date | Code | Title | Description |
|---|---|---|---|
| PB01 | Publication | ||
| PB01 | Publication |