SE540226C2 - Method of producing a sodium iron (II) -hexacyanoferrate (II) material - Google Patents

Method of producing a sodium iron (II) -hexacyanoferrate (II) material

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Publication number
SE540226C2
SE540226C2 SE1651252A SE1651252A SE540226C2 SE 540226 C2 SE540226 C2 SE 540226C2 SE 1651252 A SE1651252 A SE 1651252A SE 1651252 A SE1651252 A SE 1651252A SE 540226 C2 SE540226 C2 SE 540226C2
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Prior art keywords
sodium
powder
hexacyanoferrate
xfe
electrode
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SE1651252A
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Swedish (sv)
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SE1651252A1 (en
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Brant William
Mogensen Ronnie
Younesi Reza
Dehchar Fères
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Altris Ab
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Priority to SE1651252A priority Critical patent/SE540226C2/en
Priority to JP2019536809A priority patent/JP7022135B2/en
Priority to PCT/SE2017/050917 priority patent/WO2018056890A1/en
Priority to CN201780058017.4A priority patent/CN109715558B/en
Priority to US16/332,982 priority patent/US10899632B2/en
Priority to EP17853543.1A priority patent/EP3515865B1/en
Priority to KR1020197009051A priority patent/KR102456306B1/en
Publication of SE1651252A1 publication Critical patent/SE1651252A1/en
Publication of SE540226C2 publication Critical patent/SE540226C2/en

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    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01G—COMPOUNDS CONTAINING METALS NOT COVERED BY SUBCLASSES C01D OR C01F
    • C01G49/00—Compounds of iron
    • C01G49/009—Compounds containing iron, with or without oxygen or hydrogen, and containing two or more other elements
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01C—AMMONIA; CYANOGEN; COMPOUNDS THEREOF
    • C01C3/00—Cyanogen; Compounds thereof
    • C01C3/08—Simple or complex cyanides of metals
    • C01C3/12—Simple or complex iron cyanides
    • 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
    • H01M4/02—Electrodes composed of, or comprising, active material
    • H01M4/36—Selection of substances as active materials, active masses, active liquids
    • H01M4/58—Selection of substances as active materials, active masses, active liquids of inorganic compounds other than oxides or hydroxides, e.g. sulfides, selenides, tellurides, halogenides or LiCoFy; of polyanionic structures, e.g. phosphates, silicates or borates
    • H01M4/5825—Oxygenated metallic salts or polyanionic structures, e.g. borates, phosphates, silicates, olivines
    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M10/00—Secondary cells; Manufacture thereof
    • H01M10/05—Accumulators with non-aqueous electrolyte
    • H01M10/054—Accumulators with insertion or intercalation of metals other than lithium, e.g. with magnesium or aluminium
    • 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
    • H01M4/02—Electrodes composed of, or comprising, active material
    • H01M4/36—Selection of substances as active materials, active masses, active liquids
    • H01M4/58—Selection of substances as active materials, active masses, active liquids of inorganic compounds other than oxides or hydroxides, e.g. sulfides, selenides, tellurides, halogenides or LiCoFy; of polyanionic structures, e.g. phosphates, silicates or borates
    • 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
    • H01M4/02—Electrodes composed of, or comprising, active material
    • H01M4/36—Selection of substances as active materials, active masses, active liquids
    • H01M4/58—Selection of substances as active materials, active masses, active liquids of inorganic compounds other than oxides or hydroxides, e.g. sulfides, selenides, tellurides, halogenides or LiCoFy; of polyanionic structures, e.g. phosphates, silicates or borates
    • H01M4/583—Carbonaceous material, e.g. graphite-intercalation compounds or CFx
    • H01M4/587—Carbonaceous material, e.g. graphite-intercalation compounds or CFx for inserting or intercalating light metals
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01P—INDEXING SCHEME RELATING TO STRUCTURAL AND PHYSICAL ASPECTS OF SOLID INORGANIC COMPOUNDS
    • C01P2002/00—Crystal-structural characteristics
    • C01P2002/70—Crystal-structural characteristics defined by measured X-ray, neutron or electron diffraction data
    • C01P2002/72—Crystal-structural characteristics defined by measured X-ray, neutron or electron diffraction data by d-values or two theta-values, e.g. as X-ray diagram
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01P—INDEXING SCHEME RELATING TO STRUCTURAL AND PHYSICAL ASPECTS OF SOLID INORGANIC COMPOUNDS
    • C01P2004/00—Particle morphology
    • C01P2004/01—Particle morphology depicted by an image
    • C01P2004/03—Particle morphology depicted by an image obtained by SEM
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01P—INDEXING SCHEME RELATING TO STRUCTURAL AND PHYSICAL ASPECTS OF SOLID INORGANIC COMPOUNDS
    • C01P2006/00—Physical properties of inorganic compounds
    • C01P2006/40—Electric properties
    • 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
    • H01M4/02—Electrodes composed of, or comprising, active material
    • H01M2004/026—Electrodes composed of, or comprising, active material characterised by the polarity
    • H01M2004/028—Positive electrodes
    • 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
    • Y02E60/10—Energy storage using batteries

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  • Chemical & Material Sciences (AREA)
  • Organic Chemistry (AREA)
  • Inorganic Chemistry (AREA)
  • General Chemical & Material Sciences (AREA)
  • Chemical Kinetics & Catalysis (AREA)
  • Electrochemistry (AREA)
  • Toxicology (AREA)
  • General Health & Medical Sciences (AREA)
  • Health & Medical Sciences (AREA)
  • Engineering & Computer Science (AREA)
  • Materials Engineering (AREA)
  • Manufacturing & Machinery (AREA)
  • Crystallography & Structural Chemistry (AREA)
  • Battery Electrode And Active Subsutance (AREA)
  • Compounds Of Iron (AREA)

Abstract

The present invention relates to a method of producing a sodium iron(ll)-hexacyanoferrate(ll) (NaFe[Fe(CN)] .mHO), where x is < 0.4) material commonly referred to as Prussian White. The method comprises the steps of acid decomposition of NaFe(CN).10HO to a powder of NaFe[Fe(CN)] .mHO, drying andenriching the sodium content in the NaFe[Fe(CN)] .mHO powder by mixing the powder with a supersaturated solution of a reducing agent containing sodium in dry solvent under an inert gas.The steps of acid decomposition and enriching the sodium content are performed under non-hydrothermal conditions.

Description

Method of producing a sodium iron(ll)-hexacyanoferrate(ll) material Field of the Invention The present invention relates to a method of producing sodium iron(ll)-hexacyanoferrate(ll) material and devices incorporating sodium iron(ll)-hexacyanoferrate(ll) material (Na2-xFe[Fe(CN)6] .mH20) where x is < 0.4. In particular the invention relates to a method of producing a high voltage and high capacity positive electrode for sodium ion batteries comprising sodium iron(ll)-hexacyanoferrate(ll) material.
Background Li-ion based batteries dominate the market for rechargeable batteries. However, the technology has drawbacks, not at least the relatively scarce resources of Li. Although better than previous generations of secondary battery technologies, the Li-ion based batteries are not environmentally friendly and costly from a recycling perspective. Sodium ion batteries represent an attractive alternative to Li-ion batteries and are arguably the most viable means of supporting renewable energy sources for the purpose of load leveling and storing excess energy. However, in order to be commercially viable materials that are both high performing and cheap to produce must be implemented.
Contrary to Li, Na has abundant natural resources in Earth's crust and sea water. The abundance of Na in the Earth's crust is about 23,000 ppm compared to 20 ppm for Li. Due to such abundance, the price of Na compounds is several times lower compared to their Li counterpart products. For example, the price of Na2C03is about 40 times lower than that of Li2C03. Also, the common current collector of negative electrodes in Li-ion batteries is Cu, which could be replaced by Al in Na-ion batteries since Na does not react with Al. This is another advantage, to decrease production cost, for Na-ion batteries compared to Li-ion batteries as Al is cheaper and more abundant than Cu.
The success of a sodium ion battery technology however is heavily dependent on the sodium content of the positive electrode material, something which will prevent a given material from obtaining commercial success. Recently considerable attention has been given to a class of materials with a perovskite-like structure commonly referred to as Prussian blue analogues, due to their, at least in theory, unrivaled capacity in storing sodium ions. Focus has been to develop Na2-xFe[Fe(CN)6] .mH2O (sodium iron(ll)-hexacyanoferrate(ll)) with a high Na content and low H2O via the acid decomposition of Na4Fe(CN)6. The final product should preferably contain Na-content at, or close, to 2.0 and with negligible water content, i.e. Prussian White. Prussian White is the Prussian Blue analogue a with the chemical formula of Na2Fe2(CN)6with a negligible water content (<0.08 H/2fO.u.). Disclosed procedures typically involve the use of a reducing agent to preserve the Fe oxidation state and the use of NaCl to increase the sodium content.
Syntheses typically take place under a protective atmosphere but low pressures or in hydrothermal conditions. A number of published works exist following this method and have achieved modest sodium content, however the electrochemistry is either not ideal nor does the resulting material reflect typical behavior of water free Prussian white. Examples of recent methods and materials are described in Y. Liu, Y. Qiao, W. Zhang, Z. Li, X. Ji, L. Miao, L. Yuan, X. Hu, Y. Huang, Nano Energy, 12 (2015) 386, and D. Yang, J. Xu, X.-Z. Liao, H. Wang, Y.-S. He, Z.-F. Ma, Chem. Comm., 51 (2015) 8181. Goodenough et al however, have successfully produced Prussian white with high sodium content and ideal electrochemical properties, as published in L. Wang, J. Song, R. Qiao, L.A. Wray, M.A. Hossain, Y.-D. Chuang, W. Yang, Y. Lu, D. Evans, J.-J. Lee, S. Vail, X. Zhao, M. Nishijima, S. Kakimoto, J.B. Goodenough, J. Am. Chem. Soc., 137 (2015) 2548.. However, they achieved this via a hydrothermal reaction route which is more expensive and does not always produce pure compounds after scaling up.
In addition to being used as a positive electrode in sodium ion batteries, Prussian White may also be applicable for electrochromic devices and sensors. This is because Prussian Blue has been applied in these areas and the higher sodium content of Prussian White might prove to be advantageous. These applications have been described in Chem.
Common., 50 (2014) 802, and 7. Appl. Phys. 53, (1982) 804.
Summary Recent developments in sodium ion battery technology have addressed the issue of sufficient loading capacity of Na-ions in the positive electrode. Although improved, an industrially viable method of producing Prussian white is lacking.
The object of the invention is to provide a production method and an electrode material that overcomes the drawbacks of prior art techniques. This is achieved by the method as defined in claim 1 the material as defined in claim 6 and the electrode as defined in claim 9.
Described herein is a synthesis method to produce high sodium content Prussian white, (Na2xFe[Fe(CN)6] .mH2O), where x is < 0.4, which is possible to scale up and produces high quality material. The first part of the inventive method generally follows what has been described in the prior art on synthesizing the material via an acid decomposition of Na4Fe(CN)6.10H2O without using hydrothermal conditions. The second part of the method comprises steps to increase the sodium content such that Prussian white with electrochemical properties comparable to those reported by Goodenough et al. are achieved. These steps are performed under a protective atmosphere in dry solvent using a reducing agent in the presence of sodium ions. The resulting material is dried and can be used directly in the production of an electrode for example for the use in sodium ion batteries.
"Electrode" should in this application be given a broad interpretation as an ion source member in various electrochemical devices such as, but not limited to batteries, fuel cells, electrochromic devices and sensors. The sodium ion battery represents an illustrating example and an important product category.
The method of producing a sodium iron(ll)-hexacyanoferrate(ll) material according to the invention comprises the steps of: - acid decomposition of Na4Fe(CN)6.10H2O to a powder of Na2-xFe[Fe(CN)6] .mH2O, where x is < 0.4 and m is between 0 and 10; -filtering and drying the Na2-xFe[Fe(CN)6] .mH2O powder; and - enriching the sodium content in the Na2-xFe[Fe(CN)6] .mH20 powder by mixing the dried Na2-xFe[Fe(CN)6] .mH20 powder with a supersaturated solution of a reducing agent containing sodium in dry solvent under an inert gas, resulting in a Na2-yFe[Fe(CN)6] .mH20 powder, where y According to one aspect of the invention the supersaturated solution used in the enriching step comprises a sodium salt, preferably sodium iodide or sodium bromide.
According to another aspect of the invention the dry solvent in the supersaturated solution used in the enriching step is anhydrous acetonitrile.
According to another aspect of the invention the enriching step comprises enriching the sodium content, 2-y, to above 1.8, preferably above 1.9 or even more preferably to 1.92.
According a further aspect of the invention the method comprises forming an electrode comprising the sodium iron(ll)- hexacyanoferrate(ll) material, the method comprising the further steps of: -mixing the enriched, separated and dried Na2-yFe[Fe(CN)e] .mH20 powder with solvent, conductive additive and binder by milling, forming a slurry; -forming the slurry to a desired shape and removing the solvent by drying.
Provided by the present invention is a sodium iron(ll)-hexacyanoferrate(ll) material produced by the steps of: - acid decomposition of Na4Fe(CN)6.10H2O to a powder of Na2-xFe[Fe(CN)e] .mH20, where x is < 0.4 and m is between 0 and 10; -filtering and drying the Na2-xFe[Fe(CN)e] .mH20 powder; and - enriching the sodium content in the Na2-xFe[Fe(CN)e] .mH20 powder by mixing the dried Na2-xFe[Fe(CN)6] .mH20 powder with a supersaturated solution of a reducing agent containing sodium in dry solvent under an inert gas, resulting in a Na2-yFe[Fe(CN)6] .mH20 powder, where y According to one aspect of the invention the sodium iron(ll)-hexacyanoferrate(ll) material has a sodium content of above 1.8, preferably above 1.9 or even more preferably at 1.92. The water content should preferably be negligible, i.e. <0.08 H20/f.u..
According to the invention an electrode comprising the above described sodium iron(ll)-hexacyanoferrate(ll) material is provided. Preferably the electrode exhibits a capacity of 130-140 mAh g<1>as determined by galvanostatic cycling.
Thanks to the method according to the present it is possible to produce, at an industrial scale, sodium iron(ll)-hexacyanoferrate(ll) material (Na2-xFe[Fe(CN)6] .mH20) with a Nacontent at, or close, to 1.6 and with a negligible water content.
One advantage afforded by the present invention is that the method utilizes the economically attractive option of a non-hydrothermal synthesis method while still obtaining ideal electrochemical properties.
A further advantage is that the reaction is performed at essentially ambient or nearambient conditions and as such the energy cost is minimized.
A yet further advantage is, with a view to develop the technique to synthesise materials for electrochromic or sensor applications, the sodium content in the sample can be controlled.
Description of drawings A more complete understanding of the above mentioned and other features and advantages of the present invention will be apparent from the following detailed description of preferred embodiments in conjunction with the appended drawings, wherein: Figure 1 is a flowchart illustrating the method according to the invention for synthesizing Na2-xFe[Fe(CN)6] .mH2O where x is < 0.4; Figure 2a-b are graphs representing the electrochemical behavior of Na2-xFe[Fe(CN)6] .mH2O synthesised via the modified acid decomposition synthesis procedure; Figure 3a-b are X-ray diffraction patterns of: (a) the pure rhombohedral Prussian white phase and a comparison with Prussian blue (b).
Detailed description The method according to the present invention of producing a sodium iron(ll)-hexacyanoferrate(ll) material, Na2-xFe[Fe(CN)6] .mH2O), where x is < 0.4, comprises two stages: (A) acid decomposition of Na4Fe(CN)6and drying to a powder material and (B) enriching the sodium content of the powder material, Na2-xFe[Fe(CN)6] .mH2O where x is < 0.4. The method according to the present invention of producing a positive electrode for a sodium battery comprises a further stage (C) of forming an electrode comprising the powder material, Na2-xFe[Fe(CN)6] .mH2O where x is < 0.4.
The first stage (A) of the method according to the invention comprises acid decomposition of Na4Fe(CN)6.10H2O, which is known in the art. However, a significant aspect is that the chemical reaction occurring during the method according to the invention is performed below 100°C and at, or near, ambient pressure. The reaction begins with the acid decomposition, for example using HCI, of Na4Fe(CN)6.H20 in deoxygenated H20 at between 40-100°C and in the presence of a saturated solution of sodium ions. As appreciated by the skilled person, other acids may be utilized. The reaction is kept under an inert gas, eg N2, and left for some time (generally 12-36 hrs). Inert gas should be interpreted as a gas, or gas mixture, that does not react with the used substances. The reaction mixture was then cooled to room temperature (RT) and filtered in air. The residue was rinsed with deionised water and ethanol. The resulting powder, Na2-xFe[Fe(CN)6] .mH20, is then dried at 100-120 °C under vacuum overnight.
The stage of increasing the sodium content (B) makes it possible to omit the hydrothermal synthesis utilized in prior methods. The dried sodium iron(ll)-hexacyanoferrate(ll) powder is mixed with a solution of a reducing agent containing sodium in dry solvent under an inert gas for several days. If complete sodiation is desired then a saturated solution of the reducing agent should be employed. A preferred sodiation agent is sodium iodide, Nal. Alternatively other sodium containing reducing agents are suitable, for example NaBr. A preferred dry solvent is anhydrous acetonitrile, however anhydrous methanol or anhydrous acetone could also be used. The resulting Prussian White powder was separated by centrifugation and decanting the solvent under inert atmosphere and washed with dry solvent (for example anhydrous acetonitrile) and can be readily used directly in the production of electrodes for sodium ion batteries.
The third stage (C) comprises forming of an electrode comprising the Prussian white powder. Electrodes are be prepared by conventional slurry casting where the Prussian white material is mixed with conductive additive, binder and solvent in a ball mill. The slurry is then deposited onto a current collector; the film thickness is controlled by the doctor blade technique. One or more electrodes comprising Prussian white are arranged in a battery cell and will form high voltage and high capacity positive electrode(s).
Devices similar to the above described electrode, for example fuel cell electrodes could advantageously comprise Prussian white produced by the method according to the invention.
Prussian white powder could advantageously be utilized also in electrochromic devices and sensors.
The method according to invention will be described in detail with references to the flow chart of Figure 1. As realized by the skilled person, the processing times and temperatures in the individual steps should be seen as non-limiting guidance. The skilled person, given the information of the essential steps of the method, will be able to adapt the process, to the present conditions and requirements, for example reaction vessel sizes, heating capabilities etc. 1) A specific volume of water is deoxygenated by bubbling N2gas through it for an hour. This solution was then supersaturated with NaCI. The entire reaction vessel is kept under flowing N2. 2) To the super saturated solution a given quantity (dependent on the desired yield) of Na4Fe(CN)6.10H2O was added and allowed to dissolve. HCl is then added to the solution to control the pH to be less than 6.5. The reaction vessel is heated to a temperature of 40-100 °C and allowed to react for a period of time between 12 and 24 hrs. 3) a. The resulting powder is separated and washed. Preferably the powder is separated by filtering in air and washed with deionised, deoxygenated water and then ethanol. Alternatively, the resulting powder can be separated by centrifugation, decanting the solution and then washing with water and ethanol followed by further centrifugation and decanting. Also other commonly used separation and washing methods can be utilized b. A concentrated solution of reducing NaX is produced in anhydrous acetonitrile under an inert atmosphere (Ar, N2). 4) The powder is added to the acetonitrile solution and allowed to stir under a dry inert atmosphere (Ar, N2) until a white powder is obtained, Prussian white (Na2-xFe[Fe(CN)6] .mH20) with a Na-content at, or close, to 1.6 and with a negligible water content.
) The resulting Na2-xFe[Fe(CN)6] .mH20 powder is separated from the acetonitrile and washed with dry acetonitrile typically 3-4 times under an inert atmosphere. The resulting powder is dried again at a moderate temperature, for example 120 °C for 12 hrs.
The so produced Prussian white material may be formed into an electrode by the additional steps of: 6) The dried Prussian white powder is mixed with solvent, conductive additive and binder by milling, for example ball milling, under inert atmosphere for about 1 hrs. 7) Forming the resulting slurry to the desired shape. For example by applying the resulting slurry is to a metal foil and evenly distributed by a doctor blade. The solvent is removed from the electrodes by drying at 120 °C for 12 hrs.
Alternatively various casting or pressing procedures may be used.
Examples/results Using the above described synthesis method Prussian white can be synthesized via a method that uses similar reagents without the need for the expensive hydrothermal synthesis procedures. Evidence that Prussian white is synthesized is shown in both the X-ray diffraction pattern (Figure 3a-b) and the characteristic voltage profiles (Figure 2a-b), both of which are similar to the material produced via the hydrothermal synthesis method in the prior art. The voltage profiles was measured with the standard method galvanostatic cycling using a Digatron BTS from Digatron Power Electronics. The galvanostatic cycling of multiple cells was performed between 2 & 4.2 Volts at a current of 11.5 mA*g<-1>. X-ray diffraction patterns were obtained by measurement of samples sealed in borosilicate glass capillaries, the instrument was a STOE-STADI P diffractometer with a Mythen Dectris IK strip detector with a 0.15° angular resolution. Samples were measured between 10-60° two-theta and the X-ray source used was a single wavelength Cu K?1 The X-ray diffraction pattern is distinctly Prussian White and not Prussian Blue because these two materials have different crystal structures. Specifically, Prussian Blue's crystal structure has cubic symmetry (space group Fm-3m) while Prussian White exhibits rhombohedral symmetry (space group R-3m). This symmetry difference produces a different characteristic diffraction pattern (Figure 3b). Additionally, the two voltage plateaus have only ever been observed for Prussian White. As seen in figure 2a a stable capacity of 130-140 mAh g<-1>is achieved for the material according to the invention.

Claims (11)

Claims:
1. A method of producing a sodium iron(ll)-hexacyanoferrate(ll) material, Na2-xFe[Fe(CN)6] .mH20), where x is < 0.4, the method comprising the steps of: - acid decomposition of Na4Fe(CN)6.10H2O to a powder of Na2-xFe[Fe(CN)e] .mH20, where x is < 0.4 and m is between 0 and 10; -filtering and drying the Na2-xFe[Fe(CN)e] .mH20 powder; and - enriching the sodium content in the Na2-xFe[Fe(CN)e] .mH20 powder, resulting in a Na2-yFe[Fe(CN)6] .mH20 powder, where y
2. The method according to claim 1, wherein the supersaturated solution comprises a sodium salt, preferably sodium iodide or sodium bromide.
3. The method according to claim 1 or 2, wherein the dry solvent in the supersaturated solution is anhydrous acetonitrile.
4. The method according to any of claims 1 to 3, wherein the enriching step comprises enriching the sodium content, 2-y, to above 1.8, preferably above 1.9 or even more preferably to 1.92.
5. The method according to any of claims 1 to 4, wherein an electrode comprising the sodium iron(ll)- hexacyanoferrate(ll) material is formed, the method comprising the further steps of: -mixing the enriched, separated and dried Na2-yFe[Fe(CN)e] .mH20 powder with solvent, conductive additive and binder by milling, forming a slurry; -forming the slurry to a desired shape and removing the solvent by drying.
6. A sodium iron(ll)-hexacyanoferrate(ll) material produced by the steps of: - acid decomposition of Na4Fe(CN)6.10H2O to a powder of Na2-xFe[Fe(CN)6] .mH2O, where x is < 0.4 and m is between 0 and 10; -filtering and drying the Na2-xFe[Fe(CN)6] .mH2O powder; and - enriching the sodium content in the Na2-xFe[Fe(CN)6] .mH2O powder, resulting in a Na2-yFe[Fe(CN)6] .mH2O powder, where y
7. The sodium iron(ll)-hexacyanoferrate(ll) material according to claim 6, wherein the sodium iron(ll)-hexacyanoferrate(ll) material has a sodium sodium content of above 1.8, preferably above 1.9 or even more preferably at 1.92.
8. The sodium iron(ll)-hexacyanoferrate(ll) material according to claim 7, wherein the sodium iron(ll)-hexacyanoferrate(ll) has a water content below 0.08 H2O/f u.
9. An electrode comprising the sodium iron(ll)-hexacyanoferrate(ll) material according to any of claims 6 to 8.
10. The electrode according to claim 9, characterized by a capacity of 130-140 mAh g<1>as determined by galvanostatic cycling of multiple cells.
11. A battery cell comprising at least one electrode according to claim 9 or 10, the electrode forming a positive electrode and sodium source in the battery cell.
SE1651252A 2016-09-22 2016-09-22 Method of producing a sodium iron (II) -hexacyanoferrate (II) material SE540226C2 (en)

Priority Applications (7)

Application Number Priority Date Filing Date Title
SE1651252A SE540226C2 (en) 2016-09-22 2016-09-22 Method of producing a sodium iron (II) -hexacyanoferrate (II) material
JP2019536809A JP7022135B2 (en) 2016-09-22 2017-09-21 Method for Producing Sodium Iron (II) -Hexacyanoferric (II) Salt Material
PCT/SE2017/050917 WO2018056890A1 (en) 2016-09-22 2017-09-21 Method of producing a sodium iron(ii)-hexacyanoferrate(ii) material
CN201780058017.4A CN109715558B (en) 2016-09-22 2017-09-21 Method for producing iron (II) sodium hexacyanoferrate (II) material
US16/332,982 US10899632B2 (en) 2016-09-22 2017-09-21 Method of producing a sodium iron(II)-hexacyanoferrate(II) material
EP17853543.1A EP3515865B1 (en) 2016-09-22 2017-09-21 Method of producing a sodium iron(ii)-hexacyanoferrate(ii) material
KR1020197009051A KR102456306B1 (en) 2016-09-22 2017-09-21 Process for the preparation of sodium iron(II)-hexacyanoferrate(II) material

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SE540226C2 true SE540226C2 (en) 2018-05-02

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