Classifications

• • H—ELECTRICITY
  • H01—ELECTRIC ELEMENTS
  • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
  • H01M4/00—Electrodes
  • H01M4/86—Inert electrodes with catalytic activity, e.g. for fuel cells
  • H01M4/90—Selection of catalytic material
  • H01M4/92—Metals of platinum group
  • H01M4/925—Metals of platinum group supported on carriers, e.g. powder carriers
  • H01M4/926—Metals of platinum group supported on carriers, e.g. powder carriers on carbon or graphite
• • H—ELECTRICITY
  • H01—ELECTRIC ELEMENTS
  • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
  • H01M12/00—Hybrid cells; Manufacture thereof
  • H01M12/04—Hybrid cells; Manufacture thereof composed of a half-cell of the fuel-cell type and of a half-cell of the primary-cell type
  • H01M12/06—Hybrid cells; Manufacture thereof composed of a half-cell of the fuel-cell type and of a half-cell of the primary-cell type with one metallic and one gaseous electrode
• • H—ELECTRICITY
  • H01—ELECTRIC ELEMENTS
  • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
  • H01M12/00—Hybrid cells; Manufacture thereof
  • H01M12/08—Hybrid cells; Manufacture thereof composed of a half-cell of a fuel-cell type and a half-cell of the secondary-cell type
• • H—ELECTRICITY
  • H01—ELECTRIC ELEMENTS
  • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
  • H01M4/00—Electrodes
  • H01M4/86—Inert electrodes with catalytic activity, e.g. for fuel cells
  • H01M4/8647—Inert electrodes with catalytic activity, e.g. for fuel cells consisting of more than one material, e.g. consisting of composites
  • H01M4/8652—Inert electrodes with catalytic activity, e.g. for fuel cells consisting of more than one material, e.g. consisting of composites as mixture
• • H—ELECTRICITY
  • H01—ELECTRIC ELEMENTS
  • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
  • H01M4/00—Electrodes
  • H01M4/86—Inert electrodes with catalytic activity, e.g. for fuel cells
  • H01M4/88—Processes of manufacture
  • H01M4/8878—Treatment steps after deposition of the catalytic active composition or after shaping of the electrode being free-standing body
  • H01M4/8882—Heat treatment, e.g. drying, baking
• • H—ELECTRICITY
  • H01—ELECTRIC ELEMENTS
  • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
  • H01M4/00—Electrodes
  • H01M4/86—Inert electrodes with catalytic activity, e.g. for fuel cells
  • H01M4/90—Selection of catalytic material
  • H01M4/92—Metals of platinum group
  • H01M4/921—Alloys or mixtures with metallic elements
• • H—ELECTRICITY
  • H01—ELECTRIC ELEMENTS
  • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
  • H01M8/00—Fuel cells; Manufacture thereof
  • H01M8/10—Fuel cells with solid electrolytes
• • H—ELECTRICITY
  • H01—ELECTRIC ELEMENTS
  • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
  • H01M8/00—Fuel cells; Manufacture thereof
  • H01M8/10—Fuel cells with solid electrolytes
  • H01M2008/1095—Fuel cells with polymeric electrolytes
• • 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

Definitions

• the present invention relates to a hybrid catalyst for the production of electrical energy from chemical energy in various electrochemical energy conversion devices such as a polymer electrolyte membrane fuel cell (hereinafter abbreviated as "PEMFC”). , namely the acronym for “Polymer Electrolyte Membrane Fuel Cell”).
• PEMFC polymer electrolyte membrane fuel cell
• the electrochemical conversion devices with the highest energy density are those in which oxygen is used as oxidant, since oxygen is available in the air and therefore does not need to be stored in the vehicle or in the vehicle. 'apparatus. Oxygen is reduced electrochemically in water during the production of electrical energy in these systems. At low temperature (ie up to 200 ° C), this complex electrochemical reaction requires suitable catalysts to achieve acceptable power densities.
• transition metal means an element which has an incomplete d-sublayer or which can give a cation having an incomplete d-sublayer.
• This definition is that given by the International Union of Pure and Applied Chemistry (IUPAC) therefore includes all lanthanides and actinides.
• the term "catalyst of the type Metal-N-C" a catalyst comprising a nitrogen-doped carbon matrix to which is covalently bonded at least one non-precious transition metal.
• the non-precious transition metals can be selected from titanium, vanadium, chromium, manganese, nickel, copper, iron and cobalt. Preferably, it is iron and cobalt.
• a Fe-N-C type catalyst and a Co-N-C type catalyst are catalysts which comprise as transition metal respectively iron and cobalt.
• the non-precious transition metals are active sites of these metal-N-C catalysts.
• P-type / metal-NC hybrid catalyst means a catalyst of the type Metal-NC which further comprises at least one precious transition metal P.
• Said precious transition metals P can be selected from ruthenium, rhodium, palladium, silver, gold, rhenium, osmium, iridium, platinum and cerium. Preferably, it is platinum.
• Such hybrid catalysts comprise at least one of these precious transition metals or an alloy of these precious transition metals.
• the catalytic principle of hybrid P / metal-CN catalysts envisaged for various devices such as PEMFCs resides mainly in the reactivity of precious transition metal atoms such as platinum for the reduction of oxygen.
• the PEMFC cathodes comprising hybrid catalysts of the P / Metal-NC type or comprising non-hybrid catalysts based on precious transition metal particles (for example platinum) supported on a non-catalytic material require a relatively high precious transition metal mass and generally between 0.2 and 0.4 mg per square centimeter of electrode.
• it may be a mass of 0.4 g of platinum per kW electrical power produced by a PEMFC battery, or 40 g of platinum for a motor vehicle having a power of 100 kW.
• Another disadvantage of the catalysts described above and whose catalytic activity comes mainly from valuable transition metal atoms is their poisoning by a large number of chemicals that can come from either fuel or air used at the cathode .
• the anvil surface is quickly poisoned by the presence of carbon monoxide or ammonia (present in dihydrogen reformed from natural gas) or in the presence of halide anions (F ", Cl", Br “, ⁇ ) which can be in the atmosphere, the oxidant of the cathode of fuel cells and metal-air batteries.
• non-hybrid catalysts based on precious transition metals (for example platinum) and current hybrid P / metal-NC catalysts are non-selective. Indeed, they catalyze not only the reduction of dioxygen in water, but also the reduction of hydrogen peroxide in water. This allows the removal of the small amount of hydrogen peroxide formed during the main reaction of reducing oxygen to water in the electrochemical device.
• Non-hybrid catalysts based on precious transition metals (for example platinum) and current hybrid catalysts of the P / Metal-NC type have good electrochemical performances.
• precious transition metals for example platinum
• Current P-type / Metal-NC hybrids are high; which induces significant manufacturing costs of these catalysts because of the high cost of their raw materials.
• the scarcity of valuable transition metals and their low global annual production for example, about 200 tonnes of platinum are produced per year
• other consumer applications such as portable electronic devices for which the series of manufacture are important.
• Catalysts of Metal-NC type thus have the disadvantage of having a low durability, and in particular a low durability when used for the electrochemical reduction of oxygen, for example in a PEMFC, in particular in electrolyte PEMFCs. proton conductive acid.
• the catalysts of the Metal-NC type are selective: they catalyze practically only the reduction of the oxygen and are only very weakly capable of catalyzing the reduction. hydrogen peroxide in water.
• the hydrogen peroxide formed in parallel during the reduction of oxygen in water accumulates in the electrolyte or in the electrode and reacts chemically with the active sites based on the non-precious transition metal to form highly oxidative radical species (for example by Fenton-type reaction). These radical species then attack the metal-N-C type catalyst and / or the polymer electrolyte integrated in the electrode, considerably reducing the lifetime of the electrochemical device.
• the present invention overcomes these disadvantages with regard to catalysts of the Metal-NC type by proposing a novel P / Metal-NC type hybrid catalyst stable over time and which does not furthermore have the drawbacks inherent with non-hybrid metal-based catalysts.
• the performance of an electrode comprising a hybrid P-type / metal-N-C catalyst according to the invention remains stable over time during operation at the cathode of a PEMFC.
• the hybrid P / metal-N-C catalyst according to the invention has a greater durability than the catalysts of Metal-N-C type known to date.
• the subject of the present invention is therefore a P / Metal-NC type hybrid catalyst which comprises at least one nitrogen-doped carbon matrix to which at least one non-precious transition metal is covalently bonded, said catalyst being characterized in that it further comprises at least one precious transition metal P partially oxidized and whose mass percentage is less than or equal to 4.0%, preferably less than or equal to 2.0%, relative to the weight of said hybrid P-type / metal-NC catalyst.
• a precious transition metal P partially oxidized a precious transition metal P which has a mean degree of oxidation of between 0.5 and 4.0, preferably between 0 , 5 and 2.5.
• the term "average oxidation state" of a precious transition metal P the value that would be obtained by summing the degree of oxidation of each atom of precious metal P present in the catalyst and then by dividing this sum by the total number of precious metal atoms P present in the catalyst.
• the mass percentage of precious transition metal P is between 0.1% and 4.0%, preferably between 0.2% and 2%, relative to the mass of said hybrid P-type catalyst / Metal-NC according to the invention.
• the mass percentage of precious transition metal is advantageously between 0.2 and 2.0% relative to the weight of the hybrid P / metal-N-C type catalyst according to the invention. This thus corresponds to a quantity of between 8 and 80 micrograms of precious transition metal per square centimeter of electrode for a charged electrode at 4 milligrams per square centimeter of hybrid P-type / metal-N-C catalyst. An amount of between 8 and 80 micrograms of precious transition metal per square centimeter of electrode is below the threshold of 0.1 milligrams of platinum per square centimeter which is the threshold value adopted by the automotive industry for the next generation of catalysts Cathode for PEMFC.
• the amount of precious transition metal is therefore much lower than that which comprises the catalysts of the state of the art such as:
• P-type / metal-NC hybrid catalysts which comprise a precious transition metal in metallic form (this precious transition metal form in these hybrid catalysts comes from the fact that the precious transition metal salts which have been used as that raw materials of these hybrid catalysts have been completely reduced during the manufacture of said hybrid catalysts) or
• catalysts based on precious transition metals or precious transition metal alloys with various metals of transition for example a Pt 3 M type platinum alloy, where M is a transition metal such as iron, cobalt or nickel
• M is a transition metal such as iron, cobalt or nickel
• the electrochemical activity is inherent in the electrochemical activity of the valuable transition metals they include such as platinum.
• the reduced amount of valuable transition metal in the P / Metal-NC hybrid catalyst according to the invention has the advantage of reducing by about 20 to 30% the full cost of the PEMFC in which it is integrated (this percentage dependent on the cost of the precious transition metal), and this while ensuring a greater durability of said catalyst according to the invention compared to the catalysts of Metal-NC type.
• a hybrid catalyst according to the invention of the Pt / Fe-NC type (namely the non-precious transition metal is iron and the precious transition metal is platinum) whose mass percentage of platinum is 1.0 % is fully stable for at least 80 hours of operation in a PEMFC and the energy density is 0.12 g of platinum per kW, i.e. close to the target threshold of 0.1 g of platinum per kW.
• the non-precious transition metal atoms corresponding to the most active catalytic sites for the reduction of dioxygen in the hybrid P-type / metal-NC catalyst according to the invention are dispersed atomically on said nitrogen-doped carbon matrix. These catalytic sites are hereinafter referred to as "MetaIN x C y active sites.”
• the index x indicates the number of nitrogen atoms present in the first coordination sphere around the central non-precious transition metal atom and which are chemically bonded to the latter, while the index y indicates the number of carbon atoms present in the second coordination sphere around the central transition metal atom.
• These carbon atoms are either (i ) chemically bonded to at least one nitrogen atom itself belonging to the first coordination sphere around the metal, or (ii) located at a radial distance from the non-precious metal atom which is equivalent to the distance radial between the metal atom and the carbon atoms defined in (i).
• the atomic dispersion of the non-precious metal atoms (no chemical or physical bonds between two non-precious metal atoms) in the form of ions stabilized by chemical bonds with nitrogen and / or carbon atoms is responsible for the catalytic activity of the hybrid catalyst of the type P / Metal-NC according to the present invention. This dispersion at the atomic level can be demonstrated:
• Fe Mössbauer spectrometry absence of characteristic sextets and singlets with iron carbides, iron oxides and metallic iron (degree of oxidation zero) in the Môssbauer spectrum.
• the non-precious metal atoms in the catalysts of the present invention are, in addition to being dispersed atom by atom in the nitrogenous carbon matrix, located on the surface of the nitrogenous carbon matrix, and not in the mass of this matrix. .
• This surface positioning of the metal ions is verifiable by "operando" mode X-ray absorption spectroscopy, that is by measuring a series of X-ray absorption spectra of a metal catalyst electrode.
• -NC immersed in an acid electrolyte and corresponding to a series of electrochemical potentials (electrical potential difference between the catalyst surface and the electrolyte) applied to the electrode.
• Modifying ray absorption spectra X around the iron threshold with the electrochemical potential applied to the electrode, and overlapping different spectra of said isosbestic point demonstrates that sites MétalN x C y are located on the surface of the carbon matrix doped with nitrogen. Due to the atom-by-atom dispersion and the surface positioning of the MetalN x C y sites, the use of the non-precious metal atoms for the catalytic oxygen reduction reaction is therefore maximized.
• a fraction of the non-precious transition metal atoms may also be present in the form of metal particles or metal carbides. These crystalline phases of the non-precious transition metal can be produced in parallel with the active sites MetalN x C y during the high temperature synthesis of the catalyst Metal-NC which is a starting component of the hybrid catalyst of the P / Metal-NC type. according to the invention.
• the non-precious transition metal may be selected from titanium, vanadium, chromium, manganese, nickel, copper, iron and cobalt, taken alone or as a mixture thereof or in the form of a non-precious transition metal alloy. Preferably, it is iron and cobalt.
• the precious transition metal may be chosen from ruthenium, rhodium, palladium, silver, gold, rhenium, osmium, iridium, platinum and cerium, taken alone or as a mixture of those or in the form of an alloy with at least one precious or non-precious transition metal. Preferably, it is platinum.
• the precious transition metal is in the form of nanoparticles.
• the size of said nanoparticles is between 1 nm and 10 nm, preferably between 2 nm and 4 nm, and even more preferably between 1 nm and 2 nm.
• the P / Metal-NC type hybrid catalyst according to the invention comprises micropores (ie pores less than 20 Angstrom) and / or mesopores (namely pores of size between 20 and 500 Angstrom) in which are the nanoparticles of the precious transition metal.
• the surface area generated by the different types of pores can be greater than 300 m 2 g " ⁇ In one embodiment of the invention, said specific surface area is between 100 m 2 g -1 to about 1600 m 2 g
• the precious transition metal can be homogeneously dispersed and located near the active sites MétalN x C y of the catalyst P / Metal-NC according to the invention.
• the term "located in close proximity” means that, if we consider a representative catalytic center based on non-precious transition metal (in other words an active site MetalN x C y ), the metal particle of Precious transition closest to said active site MetalN x C y is at a distance of less than 50 nm, preferably at a distance of less than 20 nm.
• Particles of the partially oxidized precious transition metal chemically break down the radical species produced during the reduction of oxygen by these active sites into compounds that are harmless for the catalyst and the electrolyte, such as water and oxygen.
• This catalytic function of the partially oxidized precious transition metal particles is different from that of the precious transition metal particles used hitherto in hybrid P-type / metal-NC catalysts or in non-hybrid metal-based catalysts. precious transition.
• transition metal atoms are in their reduced form (i.e., to a zero oxidation state) within the precious transition metal particles, which provides an electro-catalytic property for both the electrochemical reduction of oxygen and for the electrochemical reduction of hydrogen peroxide.
• the Metallic platinum with zero oxidation state is known to be the most active catalyst for the electro-reduction of hydrogen peroxide.
• the P / Metal-NC type hybrid catalyst according to the invention is less sensitive, or even insensitive to the chemicals known to be poisons for precious transition metal surfaces (for example the halide ions and carbon monoxide for platinum), because of the partially oxidized state of the precious transition metal particles in the catalyst according to the invention and the known insensitivity of the active sites based on non-precious transition metal (namely the active sites MetalN x C y ) to these chemicals.
• the chemicals known to be poisons for precious transition metal surfaces for example the halide ions and carbon monoxide for platinum
• the precious transition metal is used as a stabilizer of the active sites MetalN x C y for the reduction of oxygen during operation of the electrochemical device.
• the precious transition metal which it comprises does not contribute to the catalytic activity for the reduction of the oxygen of said catalyst, but it protects in the course of time and during the operation of the electrochemical device the active sites based on non-precious transition metals (namely the active sites MetalN x C y ) of these catalysts .
• the catalytic function of reducing oxygen to water is only provided by the active sites MetalN x C y .
• the hybrid P / Metal-NC catalyst according to the invention unlike the valuable transition metal non-hybrid catalysts and the known P / Metal-NC hybrid catalysts of the state of the art where precious transition metal atoms are located inside precious transition metal particles are in a zero oxidation state, in the hybrid P / Metal-NC catalyst according to the invention, the precious transition metal atoms which it comprises are in a partially oxidized state, and this same inside the precious transition metal particles.
• This confers on the P / Metal-NC hybrid catalyst according to the invention a spectroscopic signature of the precious transition metal clearly distinct from that of the precious transition metal located in the non-hybrid catalysts based on precious transition metal or hybrid catalysts P / Metal-NC type known from the state of the art for the reduction of oxygen.
• the hybrid catalyst of P type / Metal-N-C according to the invention also has technical characteristics related to its manufacturing process.
• the present invention also relates to a hybrid catalyst of the P / Metal-N-C type that can be obtained by a manufacturing method that comprises at least the following steps:
• said metal-N-C type catalyst is impregnated with at least one precious transition metal salt solution P so as to obtain a homogeneous mixture
• step b) at least one heat treatment is carried out on the homogeneous mixture obtained in step b), said heat treatment consisting of heating at a temperature between 0 and 700 ° C, preferably between 100 ° C and 700 ° C, under an inert or reducing (preferably weakly reducing) atmosphere so as to obtain a P / Metal-NC type hybrid catalyst in which said precious transition metal P is partially oxidized (in other words only partially reduced with respect to its initial oxidation state as a metal salt, or alternatively partially oxidized with an average degree of oxidation greater than zero in the final hybrid catalyst),
• the concentration of the precious transition metal salt solution P being chosen in such a way that the mass percentage of said precious transition metal P is less than or equal to 4.0%, preferably less than or equal to 2.0 %, relative to the mass of the hybrid catalyst of P type / Metal-NC obtained at the end of step c).
• the concention of said precious transition metal salt solution can be chosen in a determined manner so that the mass percentage of precious transition metal is between 0.1% and 4.0%, preferably between 0.2% and 2%, relative to the weight of the hybrid catalyst of the P / Metal-NC type obtained at the end of the step c), namely the catalyst according to the invention.
• the skilled person will easily prepare the precious transition metal salt solution to a specific concentration (that is, at an appropriate concentration).
• the metal-N-C catalyst available in step a) may have been obtained pyrolytically or by organic synthesis.
• organic synthesis can be accomplished by covalently grafting non-precious transition metal macrocycles to the surface of a carbon matrix or other electronically conductive support.
• a macrocycle is either a cyclic macromolecule or the cyclic part of a macromolecule, or an organic or organometallic molecule of insufficient molecular mass to be defined as a macromolecule (macromolecule is understood to mean a molecule which contains at least about 1000 atoms) but which contains a large cyclic structure (typically, a ring of 15 atoms or more).
• organometallic macrocycles of synthesis are metal phthalocyanines and metal porphyrins.
• vitamin B 12 cycle around a central motif CoN 4
• metalloproteins which contain the substructure heme (Theme is an iron porphyrin, and contains a ring of atoms around a central FeN 4 ) motif.
• Partially carbonated or totally carbonless electronic conductive supports that are suitable for use in an electrochemical apparatus are, for example, metal carbides (titanium carbide, tungsten carbide), oxides (titanium oxide, tin oxide, tungsten oxide, molybdenum oxide). Some of these oxides are weak electronic conductors but may be doped with a second metal element, which increases their electronic conductivity One of the most commonly used metals for doping the oxides mentioned above is antimony.
• the pyrolysis can be carried out under an inert or reducing atmosphere in the presence of organic or organometallic precursors and non-precious transition metal salts.
• the catalyst of the type Metal-N-C was obtained after pyrolysis at 1050 ° C under argon for one hour of the precursors of said catalyst of the type Metal-N-C.
• Step b) can be carried out at ambient temperature and at atmospheric pressure.
• the precious transition metal salt solution is a platinum salt solution.
• it may be a solution of a platinum salt of formula [Pt (NH 3 ) 4 ] Cl 2 * H 2 O of 99% purity, marketed by the company INTERCHIM and which has been dissolved in some water.
• the heat treatment of step c) consists of heating for 2 hours at 560 ° C. in an atmosphere comprising a mixture of dihydrogen and of nitrogen (for example 5% of dihydrogen and 95% of hydrogen). % of dinitrogen expressed as molar percentages).
• the heat treatment of step c) is carried out at a temperature of between about 300 ° C and about 600 ° C, for a time of between about 15 minutes and about 2 hours, in an electrically heated oven.
• the heat treatment can be carried out in:
• classic furnace namely an oven that rises in temperature by dissipation of electrical energy in resistors
• an oven whose principle is based on electromagnetic radiation, such as microwave ovens or tube ovens.
• the sufficient duration of the heat treatment is determined according to the heater chosen to perform this step c).
• the atmosphere is inert (for example dinitrogen or argon) or reducing, preferably weakly reducing (for example dihydrogen, ammonia or a mixture of these two reducing gases with an inert gas).
• inert for example dinitrogen or argon
• reducing preferably weakly reducing (for example dihydrogen, ammonia or a mixture of these two reducing gases with an inert gas).
• the atmosphere is reducing and comprises a mixture of inert gas (for example dinitrogen, argon, helium) and reducing agent (for example dihydrogen, methane, propane, acetylene), the degree of reduction of the precious transition metal salt is controlled primarily through the molar percentage of reducing gas present in said gas mixture.
• inert gas for example dinitrogen, argon, helium
• reducing agent for example dihydrogen, methane, propane, acetylene
• the degree of salt reduction is controlled by parameters secondary to the nature of the atmosphere, such as the pyrolysis temperature and / or the pyrolysis time.
• the atmosphere is a gaseous mixture containing between 2% and 20% molar of reducing gas, so that the heat treatment time necessary to partially reduce the salt of the precious transition metal does not occur. either too long (which would be expensive) or too short (which would cause problems due to the short-term limitation of the heater, especially for electric resistance heated ovens).
• a Pt / Fe-NC type hybrid catalyst which comprises partially oxidized platinum nanoparticles with a mean degree of oxidation of the platinum atoms of between 0.5 and 2.
• the heating apparatus used for the heat treatment of step c) includes a THERMCRAFT hinged tube furnace (Express-line model, 1 heating zone), a quartz tube of 4 cm in diameter about and a nacelle of quartz.
• the Pt / Fe-NC type hybrid catalyst precursor powder (namely a [Pt (NH 3 ) 4 ] Cl 2 * H 2 0 salt premixed with a Fe-NC type catalyst such that the mass content of platinum in said Pt / Fe-NC type hybrid catalyst of 1%) is deposited in the quartz nacelle, and the quartz tube comprising the nacelle is connected to the dinitrogen.
• the tubular furnace (still under a gaseous flow of nitrogen) comprising the quartz tube and the nacelle is heated up at an average speed of 4 ° C. minute, until the temperature of 560 ° C, and then left for 2 hours at a temperature of 560 ° C under a stream of a gaseous mixture comprising 5% of dihydrogen and 95% of dinitrogen expressed as molar percentages.
• the tubular oven is opened, the quartz tube is removed from the heating zone, and it naturally cools to room temperature under a stream of dinitrogen.
• the manufacturing method further comprises a step of cooling the hybrid catalyst of P type / Metal-NC obtained at the end of step c).
• a hybrid catalyst of the P / Metal-NC type with a high specific surface area is obtained, and on the surface of which precious transition metal particles have been deposited.
• the high specific surface of the hybrid catalyst is generated by micropores and mesopores in which the particles of the precious transition metal are integrated.
• the precious transition metal particles are nanoparticles as described above.
• the present invention also relates to a hybrid P / Metal-N-C type catalyst that can be obtained by a manufacturing method slightly different from that described above and that comprises at least the following steps: i. precursors of a metal-N-C type catalyst are mixed with at least one precious transition metal salt solution P so as to obtain a homogeneous mixture,
• step ii. at least one heat treatment is carried out on the homogeneous mixture obtained in step i), said heat treatment consisting of heating at a temperature of between 500 and 1100 ° C. under an inert or reducing atmosphere so as to obtain a hybrid catalyst of type P / Metal-NC in which said precious transition metal P is partially oxidized, the concentration of the precious transition metal salt solution P being chosen in such a way that the mass percentage of said precious transition metal P is less than or equal to 4.0%, preferably less than or equal to 2.0%, relative to the weight of the hybrid catalyst of P type / Metal-NC obtained at the end of step ii).
• the concention of said precious transition metal salt solution can be chosen in a determined manner so that the mass percentage of precious transition metal is between 0.1% and 4.0%, preferably between 0.2% and 2%, relative to the mass of the hybrid catalyst of the P / Metal-NC type according to the invention.
• the characteristics of the step ii) of this 2 nd method of manufacture can be identical to those of the first manufacturing method described above.
• the present invention also relates to an electrochemical device which comprises at least one hybrid catalyst of the P / Metal-NC type according to the invention as described above.
• said electrochemical device is chosen from metal air batteries, fuel cells operating at low temperature, for example the PEFMC.
• the electrochemical device is a device in which the electrochemical reaction at the cathode is the reduction of oxygen.
• the cathode is called depolarizing.
• Figure 1 shows dioxygen reduction polarization curves in rotating disk electrode for 6 catalysts.
• FIG. 2 represents the kinetic part of the curves presented in FIG. 1, after correction of the curves for the limitation due to the diffusion of dioxygen in an acid electrolyte, by using the Koutecky-Levich equation.
• FIG. 3 shows the reduction polarization curves (the intensity i being less than 0) and the oxidation curves (the intensity i being greater than 0) of the rotating disk electrode hydrogen peroxide for 4 catalysts tested.
• FIG. 4 shows the polarization curves of the proton reduction to dihydrogen (the intensity i being less than 0) and the oxidation of dihydrogen to protons (the intensity i being greater than 0) as a rotating disk electrode for 4 catalysts tested.
• Figure 5 shows the PEMFC polarization curves for the catalysts tested.
• Figure 6 shows the current density versus time with a PEMFC potential set at 0.5 V for the catalysts tested.
• FIG. 7 shows the polarization curves, after correction to take into account the ohmic resistance of the membrane, after 50 hours of operation of the PEMFC at 0.5 V for the catalysts tested.
• Figure 8a shows the activity for the 0.8 V oxygen reduction reaction in stack, before and after 50 hours of operation of 0.5 FC PEM for the catalysts tested.
• Figure 8b shows the current density versus time with a PEMFC potential set at 0.5 V for catalyst E tested over a period of 200 hours.
• FIG. 8c represents the catalytic activity at a PEMFC potential set at 0.8 V for the catalyst E tested, before and after 200 hours of operation of the PEMFC at a potential of 0.5 V.
• FIG. 9 represents the X-ray absorption spectra around the platinum L 3 absorption threshold of catalysts C and E and a platinum metal foil.
• FIG. 10 represents a magnification of the spectra of FIG. 9 around the absorption threshold L 3 of platinum.
• FIG. 11 is a graph of the Fourier transform of the thin structure X-ray absorption signal (hereinafter abbreviated EXAFS signal) of the platinum of the catalysts C and E according to the invention in comparison with the Fourier transform EXAFS signal of the platinum of the platinum metal sheet.
• EXAFS signal the thin structure X-ray absorption signal
• FIG. 12 shows electrochemical carbon monoxide detection test curves, a well-known probe molecule for characterizing platinum metal particles (platinum atoms having a zero degree of oxidation inside the particle); and the comparison of such curves before and after a 50 hour test in 0.5 V PEMF cell made with catalyst D.
• Fig. 13 shows the X-ray absorption spectra around the L 3 platinum L absorption threshold of catalyst D, before and after a 0.5 V battery test for 50 hours.
• catalyst A Fe-N-C type catalyst, namely a catalyst comprising a carbon matrix doped with nitrogen and on which covalently bonded iron atoms;
• Catalyst B Catalyst A which has been subjected to a heat treatment detailed below. This treatment had the effect of increasing the specific surface area of the catalyst B with respect to that of catalyst A.
• This catalyst B was the so-called "reference" platinum-free Fe-CN catalyst;
• Catalyst C the first catalyst according to the invention which was obtained after post-functionalization of the catalyst A.
• the post-functionalization consisted of the same heat treatment as that of catalyst B but in the further presence of platinum metal salt which has been reduced.
• the platinum mass content in catalyst C was 0.5% based on the total weight of catalyst C;
• Catalyst D 2 nd catalyst according to the invention which was obtained after post-functionalization of the catalyst A.
• the post-functionalization consisted of the same heat treatment as that of catalyst B but in the further presence of platinum salt which was partially reduced.
• the platinum mass content in catalyst D was 1.0% based on the total weight of catalyst D;
• catalyst E 3 i th catalyst according to the invention which was obtained after post-functionalization of catalyst A.
• the post-functionalization consisted of the same heat treatment as that of catalyst B but in the presence of further platinum salt which was partially reduced.
• the platinum mass content in catalyst E was 2.0% based on the total weight of catalyst E;
• catalyst F commercial catalyst of Pt / C type, namely a catalyst comprising a carbon matrix and on which platinum nanoparticles have been synthesized. The weight percentage of platinum was 46% relative to the total weight of catalyst F.
• This catalyst is marketed by the Japanese company Tanaka Kikinzoku.
• the precursor of the Fe-N-C type catalyst A was manufactured in a foxtail from:
• ZIF-8 Of a Fe (II) salt, namely non-hydrated iron acetate, a second nitrogen ligand for Fe (II) ions, namely 1,10-phenanthroline.
• the dry powders of ZIF-8, iron salt and phenanthroline were weighed in the desired proportions and then deposited in a zirconium oxide crucible.
• the catalyst precursor before grinding contained 1% by weight of iron and the mass ratio of phenantroline to ZIF-8 was 20/80.
• 100 zirconium oxide beads 5 mm in diameter were added to the crucible which was sealed in air and placed in a planetary mill marketed by FRITSCH under the trade name Pulverisette 7 Premium. 4 cycles of 30 minutes at a speed of 400 rpm were performed to mix the powders.
• Catalyst precursor A thus obtained was pyrolyzed at 1050 ° C. under argon for one hour to obtain catalyst A.
• hybrid catalysts C to E according to the invention were obtained as follows:
• Catalyst A 300 mg were impregnated with a solution of platinum salt, namely a platinum salt of formula [Pt (NH 3 ) 4 ] Cl 2 * H 2 0 of purity 99%, sold by the company INTERCHIM, which was dissolved in water.
• platinum salt namely a platinum salt of formula [Pt (NH 3 ) 4 ] Cl 2 * H 2 0 of purity 99%, sold by the company INTERCHIM, which was dissolved in water.
• the concentration of the platinum salt solution was suitably adjusted.
• the powder which was obtained at the end of this drying was placed in a quartz boat which was itself placed in a quartz tube.
• the assembly was introduced into a tubular furnace to undergo a heat treatment consisting of heating for 2 hours at 560 ° C. in an atmosphere comprising a mixture of dihydrogen and of nitrogen (5% of dihydrogen and 95% of dinitrogen expressed in percentages molar).
• Catalyst B was prepared from catalyst A which was not impregnated with the platinum salt solution but which underwent the same heat treatment and cooling step detailed above.
• the specific surface area of the catalysts A to E was determined by adsorption of dinitrogen and by adsorption isotherm analysis with the Brunauer-Emmett-Teller equation.
• Table 1 below details the specific surface area of catalysts A to E measured by dinitrogen adsorption, as well as the percentage increase in surface area of catalysts B to E relative to the surface area of catalyst A, ie the percentage of catalyst. increase in area after the heat treatment detailed above.
• Catalytic films comprising catalysts A to E were deposited on the rotating disk electrodes as follows:
• a catalytic ink was prepared with 10 mg of the catalyst in question, 108 ⁇ l of a solution of Nafion (5% by weight of Nafion polymer dispersed in a solution based on alcohols) marketed by the company DuPont, 300 ⁇ l of 99% pure ethanol marketed by API France and 36 ⁇ of ultra-pure water.
• the catalytic ink was homogenized in an ultrasonic bath for at least 30 minutes. Then, 7 ⁇ of this ink was deposited on a disc of diameter 5 mm made of vitreous carbon so as to obtain a rotating disk electrode with a catalytic film whose catalyst load was 800 ⁇ g / cm 2 .
• the total catalyst load was 800 ⁇ g / cm 2 .
• the platinum content at the electrode comprising:
• Catalyst C was 4 ⁇ g / cm 2
• Catalyst E was 16 ⁇ g / cm 2 .
• the platinum loading at this electrode was 20 ⁇ g / cm 2 .
• 1.4 mg of catalyst F were dispersed in 3 ml of water by ultrasonic treatment, and 20 ⁇ were deposited on a glassy carbon endcake and air dried.
• the electrochemical device comprising the rotating disk electrode furthermore comprises:
• ERP hydrogen reference electrode
• a hydrogen reference electrode consisting of a platinum wire immersed in a separate compartment and containing the same electrolyte but saturated with dihydrogen, this compartment being electrolytically connected to the main compartment by a sintered glass, a potentiostat marketed by Princeton Applied Research under the trade name Versastat ®.
• rotation speed of the electrode 1600 rev / min, 20 voltammetric cycles between 0.05 and 1.1 V with respect to the ERH were conducted to clean the rotating disc electrode.
• the voltammetric cycles were conducted between 0.2 and 1.0 V E H at a scanning rate of 10 mV / s in the electrolyte saturated with dinitrogen, then with oxygen, and the curves measured under nitrogen were subtracted. to those measured under oxygen, in order to eliminate non-faradic currents (that is, currents unrelated to the reduction of oxygen, such as the capacitive current). Moreover, the curves were corrected for the ohmic drop in the electrolyte (about 20 ohms of resistance for this device).
• FIG. 1 shows the dioxygen reduction polarization curves obtained from a rotating disk electrode, with the catalysts A to F tested.
• Catalyst A has a kinetic portion of its polarization curve for the oxygen reduction reaction which is shifted to the more negative potentials of about -150 mV. This means slower kinetics.
• the low potential diffusion current is nevertheless close to that of the catalyst F indicating that the product of the reduction reaction of the oxygen on the catalyst A is mainly water.
• Catalyst B corresponds to catalyst A which has been subjected to a heat treatment; which has resulted in increasing its surface.
• the activity of the catalyst B is about 50 mV higher than that of the catalyst A and about 100 mV lower than that of the catalyst F.
• the kinetic rate of the curves is between 0 and -2 mA / cm 2 .
• Its diffusion limit current is equal to that of the catalyst F mainly indicating a reduction of oxygen in water.
• the three hybrid catalysts C to E according to the invention have an activity for the reaction. reduction of oxygen almost identical to that of the catalyst B reference.
• FIG. 2 represents the kinetic part of the curves represented in FIG. 1, after correction of the curves to correct the limitation due to the diffusion of the oxygen, and this by using the Koutecky-Levich equation.
• the kinetics of the dioxygen reaction is defined by an exponential law between the current and the electrochemical potential, that is to say a straight line on a semi-logarithmic scale E E RH VS log (i).
• the activity of the dioxygen reduction reaction is quantifiable by raising the current density to a given electrochemical potential, for example at 0.9 V vs. ERH: about 6 mA / cm 2 for catalyst F, 0.2 mA / cm 2 for catalyst B and between 0.2 and 0.3 mA / cm 2 for catalysts C to E.
• the electrode comprising the catalyst F indeed contains 20 ⁇ g of platinum per cm 2 and the electrode comprising the catalyst E contains an almost equivalent content of platinum, namely 16 ⁇ g / cm 2 , and considering also that the size of the Platinum nanoparticles in these two catalysts is similar, a similar dioxygen-reducing reaction activity should have been found between these two catalysts E and F. Except this was not the case.
• Fig. 3 shows the polarization curves for reducing hydrogen peroxide to rotating disk electrode.
• the catalysts A, B and D are not very active for the reduction and oxidation reactions of hydrogen peroxide. This is characteristic of catalysts whose active sites are iron-based.
• the curves of FIG. 3 also clearly show that the platinum structures that comprise the catalysts according to the invention are not platinum metal such as that of the catalyst F.
• the platinum present in the catalysts according to the invention does not contribute to the electrochemical reduction of small amounts of hydrogen peroxide produced during the dioxygen reduction reaction.
• radical species such as OH and OOH. These radical species can attack the membrane or the catalyst.
• Figure 4 shows polarization curves of proton reduction and oxidation of dihydrogen to rotating disk electrode.
• catalyst F when a catalyst F is used at the cathode, the small amount of hydrogen that flows from the anode to the cathode by diffusion through the membrane is immediately electro-oxidized to protons; catalyst A is totally inactive for this reaction (see curve A in FIG. This catalyst rather promotes a chemical reaction between the dihydrogen and the oxygen to form free radicals.
• FIG. 4 shows that the curve of catalyst E according to the invention is almost superimposed on the theoretical curve (see calculated curve) corresponding to infinite kinetics of oxidation of dihydrogen, namely that the only experimentally observable loss is due to the diffusion of the dihydrogen dissolved in the electrolyte towards the electrode, the kinetics being so much faster than the diffusion that the kinetics are not quantifiable by this experimental method.
• the curves of FIG. 4 show that the platinum structures in the hybrid catalysts according to the invention are active for the oxidation reaction of dihydrogen, with respect to the positive currents of FIG. 4, but also for the reduction of protons. dihydrogen, and this with regard to the negative currents of Figure 4.
• Catalyst A is totally inactive for dihydrogen oxidation and proton reduction reactions. This inactivity with respect to dihydrogen and protons is a known property for the family of Fe-N-C and Co-N-C catalysts.
• the hybrid catalysts C to E according to the invention show a proportional increase in their catalytic activity for dihydrogen and H + protons with the increase of the platinum content. This may be related to the better stabilization observed in PEFMC of catalysts D and E according to the invention, the platinum mass content of which is 1% and 2%, respectively. Catalysts A to E have in fact also been tested in PEMFCs. This better stabilization is detailed below.
• the curves show the electric potential difference "cathode less anode” of the PEMFC as a function of the current density, and this after correction to take into account the ohmic resistance of the membrane.
• Catalytic cathode inks were prepared by mixing 20 mg of the catalyst in question, 652 ⁇ l of a 5% by weight solution of Nafion® containing 15-20% by weight of water, 326 ⁇ l of ethanol and 272 ⁇ l of water. deionized water. The inks were homogenized by alternately subjecting them to ultrasound and to mechanical stirring in a vortex mixer every 15 minutes for a total of one hour.
• the cathode was placed in a vacuum oven at 90 ° C for one hour to be dried.
• the anode contained a commercial Pt / C type catalyst with a platinum loading of 0.5 mg / cm 2 pre-deposited on a microporous layer of the same carbon fabric, Sigracet S10-BC.
• the anode-membrane-cathode assembly was prepared by hot pressing at 135 ° C. for 2 minutes 4.48 cm 2 of the anode and the cathode on either side of a membrane marketed by DuPont. under the trade name Nafion® NRE-211.
• the PEMFC experiments were conducted in a single-cell commercial fuel cell comprising serpentine-shaped gas distribution channels (Fuel Cell Technologies), using a laboratory-internal PEMFC test bench, and controlling the electric potential of the battery and the current produced with a commercial potentiostat of the company Biology, coupled with a 50 A amplifier of the same company.
• dihydrogen and dioxygen wetted 100% at a temperature of 85 ° C, relative pressure of the gases of 1 bar at the inlet of the anode and the cathode, gas flow of 50-70 cm 3 / minute for humidified dioxygen and dihydrogen,
• Catalysts B to E are more efficient initially than the catalyst
• the initial current densities at 0.5 V of the catalysts B to E being higher than that of catalyst A of about 150 mA / cm 2 . This is because catalysts B to E have been heat treated. This thus testifies to the effect of heat treatment on metal-NC type catalysts.
• the potential difference of the PEMFC was set at 0.5 V and the current density a measured over 50 hours. This time is sufficient to observe a decrease in the performance of the standard Fe-N-C catalyst, that is to say catalyst B.
• Figure 6 shows the current density versus time for PEMFC potential set at 0.5 V for 50 hours.
• the catalysts Fe-NC (catalysts A and B), reproducibly, become activated during the first hours of operation of the PEFMC, then show a continuous degradation of performance over time ( approximately 20-25% loss of current compared to the maximum observed after 3-6 hours).
• the hybrid catalyst C according to the invention is not completely stable because of the low platinum content (ie 0.5%). This is possibly related to a too great average distance between any catalytic iron-based site and the nearest platinum particle in this hybrid catalyst.
• FIG. 7 represents the corrected polarization curves taking into account the ohmic resistance of the membrane, measured after 50 hours of operation at 0.5 V of the PEMFC.
• the final activity of the dioxygen reduction reaction is getting closer and closer to the initial activity with the increase of the platinum content of the hybrid catalysts C to E. testifies that the low platinum content that comprise the hybrid catalysts according to the invention has the effect of stabilizing their active sites based on the non-precious transition metal.
• FIG. 8b represents the current density (i) as a function of time (expressed in hours) with a PEMFC potential set at 0.5 V for the catalyst E tested over a period of 200 hours.
• Figure 8b shows that the stabilization observed over 50 hours ( Figure 6) is also effective over longer periods such as 200 hours.
• the final performance at 0.5 V is also similar to that observed after 50 hours of testing.
• FIG. 8c represents the catalytic activity with a PEMFC potential set at 0.8 V (current density divided by the total loading of P-type metal / NC catalyst) for the catalyst E tested, before and after 200 hours. of the PEMFC.
• the initial activity and the final activity are very similar.
• the partially oxidized platinum in the catalyst according to the invention can stabilize the Fe-NC catalyst in the long term, and also demonstrates that the platinum was not reduced (activated) during the 0.5 V test. if not, a significant increase in activity would have been observed after 200 hours, which is not the case.
• FIG. 9 represents X-ray absorption spectra around the L 3 absorption threshold of platinum at 11562 eV (known by the acronym "XANES” for "X-ray Absorption Near Edge Structure”) of platinum atoms.
• hybrid catalysts C and E according to the invention in comparison with the XANES spectrum around the platinum L 3 absorption threshold of a platinum metal sheet in which the platinum atoms are in metallic form.
• Figure 9 shows the XANES spectra of some eV below platinum L 3 threshold up to 50 eV above this threshold.
• the platinum atoms have a zero oxidation state and have a face-centered cubic crystal structure (i.e., each platinum atom has 12 adjacent platinum atoms).
• FIG. 10 represents an enlargement of the spectra of FIG. 9 at platinum L 3 absorption threshold, namely at 11562 eV.
• the XANES part of the absorption spectrum is characteristic of the local order around the X-ray absorber atom, here platinum.
• the type of atom and the number of atoms around the platinum atoms is therefore according to FIGS. 9 and 10 fundamentally different between the hybrid catalyst according to the invention and the catalysts of the state of the art.
• the platinum which comprises the catalysts according to the invention does not have a platinum structure in metallic form (namely a cubic face-centered structure).
• the spectra of the catalysts according to the invention are positively shifted by 0.5-1.0 eV relative to the spectrum of the platinum metal foil. This positive offset of 0.5-1.0 eV relative to the platinum metal sheet corresponds to an average degree of oxidation between 1.1 and 2.3 of the platinum atoms in the Pt / Fe type hybrid catalysts. -NC according to the invention.
• the average oxidation state of the platinum atoms of the hybrid catalysts according to the invention is not zero, as is the case for the platinum of the platinum metal sheet.
• the platinum salt precursor was therefore not completely reduced during the manufacture of the catalyst according to the invention, that is to say during the heat treatment with gaseous mixture of dihydrogen and dinitrogen.
• FIG. 11 is a graph of the Fourier transform of fine-structure X-ray absorption spectroscopy experiments (namely the following abbreviated experiments "EXAFS", English acronym for "Extended X-ray Absorption Fine Structure”) of the platinum hybrid catalysts C and E according to the invention in comparison with the Fourier transform of the EXAFS signal for the platinum of the platinum metal sheet.
• EXAFS extended X-ray Absorption Fine Structure
• This analysis makes it possible to plot the amplitude of the signal EXAFS (k 2 x (R)), which depends on the average number of neighboring atoms around each platinum atom, as a function of the distance between the absorber platinum atom and the neighboring atoms.
• Figure 11 shows that the long-range structure around the platinum atoms of the hybrid catalysts of the invention is also very different from that of the platinum atoms in a face-centered cubic metal structure.
• the platinum coordination number of the catalysts according to the invention is lower than that of the platinum platinum metal sheet.
• the EXAFS signal observed at 1.5 ⁇ for the Pt / Fe-NC type hybrid catalysts according to the invention can be attributed to platinum-carbon and platinum-nitrogen bonds, ie bonds that are absent in the cubic structure. center platinum face of the platinum metal sheet.
• FIG 12 shows electrochemical carbon monoxide detection test curves.
• Carbon monoxide is a molecule known to characterize platinum metal particles (platinum atoms having a zero oxidation state inside the particle). Carbon monoxide is conventionally used in the field of electrochemistry to quantify the area of reduced platinum-based catalysts.
• Carbon monoxide is first injected into the battery system as a gas at the cathode.
• the carbon monoxide molecule adsorbs strongly on the reduced platinum surface, covering its entire surface with a monolayer.
• the unadsorbed and excess carbon monoxide gas is then purged from the cathode with an inert gas which is the dinitrogen. Only this monolayer of carbon monoxide adsorbed on the reduced platinum remains present in the cathode (the potential of the cathode is controlled around 0 V during this time, to avoid premature oxidation of carbon monoxide).
• the amount of carbon monoxide adsorbed is then quantified by electrochemically desorbing the carbon monoxide (electrochemical oxidation of carbon monoxide which is then desorbed in oxidized form), progressively increasing the electrochemical potential of the cathode from 0 to 1 V.
• the electrical charge corresponding to the area under the oxidation peak of carbon monoxide in the voltammogram is directly proportional to the amount of carbon monoxide adsorbed, and thus to the reduced platinum area in the catalyst.
• the position of this oxidation peak of carbon monoxide is approximately 0.8 V vs.. a reference electrode with hydrogen.
• Figure 12 shows the comparison of curves before and after a 50 hour PEMFC test at 0.5 V with catalyst D.
• FIG. 12 More precisely, in FIG. 12:
• the curve labeled "initial” represents the voltammogram determined after injection of carbon monoxide, then dinitrogen at the cathode;
• the "after 50 hours" curve represents the voltammogram determined after injecting carbon monoxide, from the dinitrogen to the cathode, and then performing a 50-hour PEMFC performance test at 0.5
• Figure 12 shows no signal corresponding to the electrochemical oxidation of carbon monoxide for catalyst D, either before or after the 50 hour battery test.
• the curve called “initial” is indeed superimposed on the curve called “white”.
• FIG. 12 shows the absence of adsorption of carbon monoxide on the platinum present in the catalyst D.
• the absence of oxidation peak (that is to say the oxidation of the carbon monoxide potentially adsorbed on the platinum , which would result in a positive current peak when increasing the electrochemical potential from 0 to 1 V) demonstrates that platinum is initially unable to adsorb carbon monoxide. This is explained by the partially oxidized state of platinum in the catalyst according to the invention. After 50 hours of operation at 0.5 V, platinum is still unable to adsorb carbon monoxide, demonstrating that platinum has not been reduced in the battery test.
• FIG. 13 shows X-ray absorption spectra around the L 3 absorption threshold of platinum at 11562 eV of the platinum atoms of catalyst D (i.e., "XANES" spectra), before and after a battery test at 0.5 V for 50 hours.
• the superposition of the spectra shows that the coordination and the average degree of oxidation of the platinum in the catalyst D did not change during the stack test. Platinum is therefore inactive for the oxygen reduction reaction throughout the test, but it stabilizes the FeNxCy iron catalytic sites.

Landscapes

• Chemical & Material Sciences (AREA)
• Chemical Kinetics & Catalysis (AREA)
• Electrochemistry (AREA)
• General Chemical & Material Sciences (AREA)
• Engineering & Computer Science (AREA)
• Materials Engineering (AREA)
• Manufacturing & Machinery (AREA)
• Composite Materials (AREA)
• Physics & Mathematics (AREA)
• Thermal Sciences (AREA)
• Life Sciences & Earth Sciences (AREA)
• Sustainable Development (AREA)
• Sustainable Energy (AREA)
• Catalysts (AREA)
• Inert Electrodes (AREA)
• Fuel Cell (AREA)

Applications Claiming Priority (2)

Publications (1)

Family

ID=54329820

Family Applications (1)

Country Status (9)

Cited By (1)

Families Citing this family (15)

Family Cites Families (8)

• 2015
  • 2015-09-11 FR FR1558452A patent/FR3041163A1/fr not_active Withdrawn
• 2016
  • 2016-09-12 EP EP16775302.9A patent/EP3347937A1/fr not_active Withdrawn
  • 2016-09-12 WO PCT/FR2016/052289 patent/WO2017042520A1/fr active Application Filing
  • 2016-09-12 US US15/759,505 patent/US20180241047A1/en not_active Abandoned
  • 2016-09-12 CN CN201680065789.6A patent/CN108352533A/zh active Pending
  • 2016-09-12 CA CA2997616A patent/CA2997616A1/fr not_active Abandoned
  • 2016-09-12 JP JP2018512943A patent/JP2018528855A/ja active Pending
  • 2016-09-12 KR KR1020187009750A patent/KR20180051574A/ko unknown
• 2019
  • 2019-01-16 HK HK19100767.0A patent/HK1258462A1/zh unknown

Also Published As

Similar Documents

Legal Events