|Publication number||US20060102489 A1|
|Application number||US 11/260,256|
|Publication date||May 18, 2006|
|Filing date||Oct 28, 2005|
|Priority date||Oct 29, 2004|
|Also published as||WO2006050077A2, WO2006050077A3|
|Publication number||11260256, 260256, US 2006/0102489 A1, US 2006/102489 A1, US 20060102489 A1, US 20060102489A1, US 2006102489 A1, US 2006102489A1, US-A1-20060102489, US-A1-2006102489, US2006/0102489A1, US2006/102489A1, US20060102489 A1, US20060102489A1, US2006102489 A1, US2006102489A1|
|Original Assignee||Kelly Michael T|
|Export Citation||BiBTeX, EndNote, RefMan|
|Patent Citations (3), Referenced by (23), Classifications (12), Legal Events (2)|
|External Links: USPTO, USPTO Assignment, Espacenet|
This application claims the benefit of U.S. Provisional Application Ser. Nos. 60/622,789 filed on Oct. 29, 2004, and 60/662,555 filed on Mar. 17, 2005, the entire disclosures of which are incorporated herein by reference.
The invention was made with Government support under Cooperative Agreement No. DE-FC36-04GO14008 awarded by the Department of Energy. The Government has certain rights in this invention.
The present invention relates to the electrochemical reduction of active metal salt compounds with applications in active metal hydride and active metal borohydride production.
Sodium borohydride is a very versatile chemical and is used in organic synthesis, waste water treatment, and pulp and paper bleaching. The high hydrogen content of this compound also makes it a good candidate for being a hydrogen carrier, and it could play a major role as an enabler of a hydrogen economy if the cost of producing this chemical can be reduced.
Today, sodium borohydride is produced by the so-called Schlesinger process, which is a multi-step synthetic process, wherein sodium borohydride is produced from the reaction of sodium hydride and trimethyl borate in mineral oil. As none of the reagents are soluble in mineral oil, it is necessary to ensure high dispersions and the reaction must proceed at elevated temperatures, typically around 250° C. In addition, mineral oil evaporates and can contribute to VOC emissions.
U.S. Pat. No. 3,734,842, U.S. Pat. No. 4,904,357, and U.S. Pat. No. 4,931,154, the disclosures of which are incorporated by reference herein in their entirety, refer to electrochemical synthesis of sodium borohydride from aqueous sodium metaborate solution. Such processes involve conversion of sodium metaborate and water to form sodium borohydride and oxygen in an electrical cell, as shown in the following half-cell reactions:
Cathode: B(OH)4 −+4H2O+8e−→BH4 −+8OH− (1a)
Anode: 8O−−→4H2O+2O2+8e (1b)
However, none of these processes has been implemented in commercial practice.
The invention is directed to electrochemical processes and apparatus for preparing metal hydride compounds from active metal salts.
In accordance with one aspect of the present invention, molten active metal salts are electrolyzed under a hydrogen atmosphere to produce active metal hydrides.
In accordance with another aspect of the present invention, active metal salts are electrolyzed in ionic liquids under a hydrogen atmosphere to produce active metal hydrides.
In accordance with another aspect of the present invention, the electrochemical process is integrated with a chemical reaction of a boron compound to produce boron hydride compounds.
In another aspect of the present invention, the electrochemical process is integrated with an in situ chemical reaction of an oxidized boron compound to produce boron hydride compounds.
In another aspect of the present invention, oxidized boron compounds are reduced by reaction with active metal hydrides in a liquid salt to produce boron hydride compounds.
These and other features and advantages of the invention will become apparent from the following detailed description that is provided in connection with the accompanying drawings and illustrated exemplary embodiments of the invention.
In accordance with an exemplary embodiment of the present invention, a metal salt or a mixture of metal salts are converted into a metal hydride via electrolysis in the presence of hydrogen. Without being limited by theory, it is thought that an electrochemical reduction of the metal salt yields metal at the cathode, and the metal formed then reacts chemically with hydrogen to give metal hydride. The overall reaction is shown in Equation (2) wherein X represents a halide anion (the reaction product of the anion will depend on the anion, X, chosen),
where M is preferably selected from the group of metals and semimetals wherein the potential of the reaction between the metal, M, and oxygen to make a metal oxide is greater than about 1.6 volts, where the potential is defined as the negative of the free energy of reaction (AG, measured in joules per mole of metal) at standard conditions, wherein temperature is 298.15 K (25° C.) and pressure is 101.325 kPa (1 atm), divided by the number of moles of electrons transferred per mole of metal (n), divided by Faraday's constant (F) (Faraday's constant=96485 coulombs/mole of electron), or Potential=−ΔG/nF; X is chosen from the group of anions comprising halides, tosylate, sulfate and sulfate derivatives, trifluoromethanesulfonate and other sulfonates, nitrate, phosphates, hexafluorophosphate, and other phosphate derivatives, phosphinates, dicyanamide, tetrafluoroborate, acetate, trifluoroacetate, borohydride, benzoate, tetrachloroaluminate, thiocyanate, thiosalicylate, tris(trifuoromethylsulfonyl)methide and other methides, and bis(trifluoromethylsufonyl)imide and other imides; and n is the valence of the metal, preferably an integer from 1 to 4. Metals and semimetals falling under this definition are herein referred to as “active metals.”
Active metals, include, but are not limited to, the alkali metals, the alkaline earth metals, transition metals from Groups 3, 4, 12, and the lanthanide family. The active metals form cations that include, but are not limited to, Li+, Na+, K+, Rb+, Cs+, Be2+, Mg2+, Ca2+ Sr2+, Ba2+, Sc3+, Ti3+, Ti4+, Zn2+, Al3+, Si4+, Y3+, Y+, Zr2+, Zr3+, Zr4+, Hf+, Hf3+, Hf3+, and lanthanides in the +3 oxidation state. M is preferably chosen from the group of alkali metals, and more preferably is lithium, sodium, potassium, and cesium; and X is preferably chloride or bromide.
An exemplary two-compartment electrolysis cell 100 employed in the process of the present invention is illustrated in
Separator 106 may preferably comprise a material such as glass, polymer, or ceramic that allows ionic transport between the cathodic and anionic compartments, but restricts reaction between the active metal produced at the cathode and the product produced at the anode. Porous separators such as porous glass, porous metal, porous plastics, and porous ceramics are suitable separators. Paper, polymer, polymer membranes, and perfluoronated ion-conducting polymer membranes, are also suitable separators. Nonlimiting examples of polymer separators include polytetrafluoroethylene (PTFE), perfluoroalkoxy polymer, perfluorosulfonated ionomers, polyamides, nylon polymers, and polyethylene. Optionally, cationic conducting ceramics may be employed as the separator. Nonlimiting examples of ceramic separators include lithium-β-aluminum oxide, lithium-β″-aluminum oxide, lithium-β/β″-aluminum oxide, lithium analogs of NaSICON ceramics, LiSICONs, and lithium ion conductors with perovskite structure, sodium-β-aluminum oxide, sodium-β″-aluminum oxide, sodium-β/β″-aluminum oxide, NaSICON ceramics, potassium-β-aluminum oxide, potassium-β″-aluminum oxide, potassium-β/β″-aluminum oxide, and potassium analogs of NaSICON ceramics.
In a preferred embodiment of the method of the present invention, one or more active metal salts of formula MXn are charged to the cathode chamber 112 to prepare a metal hydride. The cell is preferably maintained at temperatures from about 70° C. to about 500° C., so that the one or more active metal salts are in a liquid molten state. The active metal salts can be used neat, i.e., without solvent, or a solvent may be included.
Alternatively, the one or more active metal salts can be dissolved in an ionic liquid. Ionic liquids are defined herein as salts with a melting point between about −100° C. and about 200° C., and preferably containing at least 1 carbon atom in the cation. Typical ionic liquid cations include, but are not limited to, mono-, di-, tri-, and tetra substituted ammonium; mono-, di-, tri-, and tetra substituted phosphonium, N-alkylpyridinium, 1,3-disubstituted pyridiniums, 1,4-disubstituted pyridiniums, 1,3-disubstituted imidazolium, 1,2,3-trisubstituted imidazolium, 1,1 disubstituted pyrrolidiums, trialkylsulfonium, and trialkyloxonium cations. The anion in an ionic liquid can be any anion. Some typical anions are halides, but other representative and non-limiting examples include the group of common complex ions such as tosylate, sulfate and sulfate derivatives, trifluoromethanesulfonate and other sulfonates, nitrate, phosphates, hexafluorophosphate, and other phosphate derivatives, phosphinates, dicyanamide, tetrafluoroborate, acetate, trifluoroacetate, borohydride, benzoate, tetrachloroaluminate, thiocyanate, thiosalicylate, tris(trifuoromethylsulfonyl)methide and other methides, and bis(trifluoromethylsufonyl)imide and other imides. Preferably, neither the cation nor the anion of the ionic liquid is easily reducible by strong hydrides. It is not necessary that the liquid salt be a liquid at room temperature, but only that at least a portion of the salt be liquid at the reaction temperature.
Hydrogen is preferably supplied to the cathode chamber as a gas stream via a gas inlet means. Suitable gas inlet means for supplying a hydrogen or hydrogen-containing gas stream include a pipe, a sparger, a hose, or a hydrogen gas diffusion material. Alternatively, hydrogen can be absorbed in a metal or metal alloy which can be released as the temperature increases. Such metals or alloys can be impregnated with hydrogen and used as the cathode. Preferably, a gas stream comprising hydrogen bubbles through or otherwise agitates the catholyte.
Upon the application of an electric potential, preferably from about 1.0 to about 10.0 V, preferably from about 1.0 V to about 5.0 V, the active metal ions are reduced at the cathode to the metal or semimetal as shown in Equation (3), and the anion is oxidized at the anode as shown in Equation (4a) for a monovalent anion such as a halide:
Cathode: 2My++ye−→M (3)
Anode: yX−→y/2X2+ye− (4a)
The active metal reacts with the hydrogen gas to form an active metal hydride compound as shown in Equation (5):
In Equations (3), (4), and (5), y is an integer from 1 to 4 and typically depends on the preferred (i.e. the most stable) oxidation state of the active metal when it combines with oxygen to make the active metal oxide. Some exceptions are known, such as titanium, which preferentially forms a TiH2 hydride, rather than TiH3 or TiH4.
Hydrogen may be supplied to the anode as well as to the cathode to convert the anion oxidation product to a desirable or valuable reaction product as shown in Equations (4b) and (4c) wherein X is a halide, and halogen is converted to HX. Electrochemically oxidizing H2 at the anode in preference to X− will generally result in a lower cell potential than the comparable electrochemical system that generates X2 depicted in Equation (4a).
Anode: ½H2→H++e− (4b)
In another aspect of the present invention, the electrochemical-chemical process for obtaining metal hydrides according to the present invention can be incorporated into a process for producing boron hydride compounds. In this embodiment, oxidized boron compounds are reduced by a hydride carrier in a liquid salt to produce a boron hydride compound. The hydride carrier may be, for example, derived from the electrochemical reduction of active metal salts as described, wherein a molten active metal salt or mixture of molten active metal salts, either neat or in an ionic liquid, is converted into an active metal hydride via electrolysis under an atmosphere of hydrogen. The process of the present invention provides a ready “one-pot” means to reduce boron compounds such as boron-oxygen compounds and boron halide compounds, to boron hydride compounds including borohydride anions (BH4 −).
To produce a boron hydride compound, at least one active metal salt is charged to the cathode compartment of an electrolytic cell and an electric potential from about 1.0 V to about 10.0 V and preferably from about 1.0 V to about 5.0 V is applied to form the active metal as described above.
After the active metal has reacted with hydrogen gas to produce the active hydride, the applied potential may be removed and the cell maintained at a temperature such that the metal hydride is at least partially dissolved in a liquid salt. Thus, for neat metal salt systems, the cell is maintained at temperatures above the melting point of the active metal salt or mixture of active metal salts. For systems wherein the metal salt was dissolved in an ionic liquid, the cell is maintained at a temperature that allows the solvent to be liquid.
As shown schematically in
The oxidized boron compound reacts with the active hydride. Equation (6a) illustrates the formation of borohydride from a trialkyl borate and an active metal hydride such as MH:
The stoichiometry of the reduction reaction can be adjusted as shown in Equations (6b) to (6d) to ensure the generation of a borohydride compound from various active metal hydrides and other oxidized boron compounds:
Higher boron hydride compounds, such as diborane and triborohydride compounds, can be prepared by varying the stoichiometric ratio between the hydride and the oxidized boron compound, as illustrated in Equation (6e) for the formation of the diborane ion from a trialkyl borate:
The use of triborohydride compounds for hydrogen storage and related methods for their preparation are described in co-pending U.S. patent application Ser. No. 10/741,192, entitled “Triborohydride Salts as Hydrogen Storage Materials and Preparation Thereof,” filed Dec. 19, 2003, the disclosure of which is incorporated by reference herein in its entirety.
The oxidized boron compound/alkali metal salt mixture is subjected to a potential from about 1.0 V to about 5.0 V to form the active metal as described above. The oxidized boron compound reacts with the active hydride as it is produced, to form a boron hydride. In this case, the reactions illustrated in Equations (6a)-(6d) occur continuously as the metal hydride is formed.
Alkali metal borates, B2O3, and trialkyl borates such as B(OR)3, may be reacted with alkali metal hydrides to obtain borohydride compounds in suspension. For example, at 275° C., NaH and B(OCH)3 react in mineral oil to form NaBH4, and NaOCH3. The present invention can achieve this reaction in a liquid salt, a solvent system that supports ionic conduction, and therefore electrochemical synthesis, wherein the reactants and products are in a dissolved state. The liquid salts include molten active metal salts and ionic liquids.
As an example of the process of this exemplary embodiment of the present invention, borohydride anions are obtained from a molten mixture of lithium bromide, potassium bromide, and cesium bromide under a hydrogen atmosphere by the electrolytic process of the present invention, where boric oxide is added to the melt before the application of a potential. Without being limited to any one particular theory, it is believed that electrolysis reduces the metal ions in the melt to the corresponding metals, which then react with hydrogen to make the metal hydrides. One or more of the metal hydrides then react with the boric oxide to make borohydride anions. A borohydride compound may then be isolated by suitable separation and extraction steps.
For the particular case where the oxidized boron compound is sodium metaborate, NaBO2, it is preferable that the active metal hydride be lithium hydride. Lithium hydride can be formed in situ according to the teachings herein by the electrolytic reduction of lithium bromide, either as a liquid molten salt or dissolved in an ionic liquid, under a hydrogen atmosphere to form lithium hydride.
Hydrogen may be supplied to the anode as well as the cathode to convert the anion oxidation product and to lower cell potential according to the teachings herein.
In another embodiment of the invention, oxidized boron compounds are converted to boron hydride compounds via reaction with metal hydrides dissolved in liquid salts, wherein the metal hydrides may be, for example, commercially available products and/or not otherwise derived from the electrochemical reduction of active metal salts as taught herein. The metal hydrides should preferably be at least sparingly soluble in the liquid salt solvent. The liquid salt may be a molten metal salt, or a mixture of molten metal salts, or an ionic liquid.
The metal hydrides may be selected from, for example, the group of alkali metal hydrides, alkaline earth metal hydrides, aluminum hydrides including alane (AlH3), and zinc hydride. A suitable metal hydride is chosen based on the standard reduction potential of the metal. Any metal wherein the standard reduction potential for the reaction of that metal with oxygen to yield the most thermodynamically stable metal oxide is more than about 1.6 V could be employed in this reaction.
The following examples further describe and demonstrate features of the present invention. The examples are given solely for illustration and are not to be construed as a limitation of the present invention.
A schematic illustration of the reactions taking place in the process is provided in
A mixture consisting of about 39.2 g LiBr, 18.1 g KBr, and 42.8 g of CsBr was charged to cathode compartment and was electrolyzed at about 5 V for about 5 hours under a hydrogen atmosphere to produce lithium metal at the cathode and bromine at the anode. The tube impeded mixing of the bromine that formed at the anode with the melt external to the tube, and thus slowed the back-reaction of lithium and bromine to lithium bromide. The tube also facilitated removal of gaseous bromine from the reactor under a stream of flowing nitrogen. The reaction flask containing the melt was maintained in a constant temperature bath at about 300° C.
After about 5 hours, 587 mAh of current passed through the cell. The nickel cathode and the sparging tube containing the anode were both removed from the melt, and a cold-water condenser was attached to the reaction flask. About 1.25 mL of tri-n-butyl borate was injected directly into the melt using a syringe. The reaction was allowed to proceed for about 15 minutes, and the reaction flask was removed from the constant temperature bath and allowed to cool. The melt solidified as it cooled. The cool, solid melt was dissolved in 0.5 M NaOH aqueous solution. A 50 mL sample of the solution was titrated using the iodate assay for borohydride as put forth in the Sodium Borohydride Digest by Rohm and Haas Company. The titration indicated that 3.15×10−4 mol BH4 − was formed, a yield of 5.7% based on the 587 mAh of charge that passed through the cell. Boron NMR of the aqueous solution confirmed the presence of borohydride anion (chemical Shift=−40.85 ppm, Splitting=80.6 Hz).
Using the procedure described in Example 1, a melt consisting of about 39.2 g LiBr, 18.1 g KBr, and 42.8 g of CsBr was electrolyzed under an argon atmosphere at about 3 V for 34 minutes. The potential, at 3 V, was too low to reduce the cations in the melt to metal, and instead reduced the Ni surface of the cathode and generated bromine at the anode. The reactor 400 was assembled as shown in
The electrolysis was reset to run for about 20 hours at about 5 V. After 20 hours, 1975 mAh of current passed through the cell. The nickel frit cathode and the sparging tube containing the anode were both removed from the melt. The reaction flask was removed from the constant temperature bath and allowed to cool. The melt solidified as it cooled, and the melt was dissolved in 0.5 M NaOH aqueous solution. A 50 mL sample of the solution was titrated using the iodate method for borohydride. The titration indicated that 2.34×10−4 mol BH4 − anion was formed, a yield of 1.3% based on the 1975 mAh of charge that passed through the cell. Boron NMR of the aqueous solution confirmed the presence of borohydride anion.
A melt consisting of about 9.8 g LiBr, 4.5 g KBr, and 10.7 g of CsBr under a nitrogen atmosphere was heated to about 250° C. To this melt, 1.6 grams of B2O3 was added. With stirring, 0.27 g of LiH was added to the melt. After adding LiH, the temperature bath was turned off, but stirring was continued until melt solidified. After dissolving the cooled melt in 100 mL of 0.5 M NaOH, a 50 mL sample of the solution was titrated using the iodate method for borohydride. The titration indicated that 5.3×10−3 mol BH4 − was formed, a yield of 62% based on the 0.27 grams of LiH added to the reactor. Boron NMR of the aqueous solution confirmed the presence of the borohydride anion.
A mixture of about 39.2 g of LiBr, 18.1 g of KBr, and 42.8 g of CsBr, and 0.5 g of B2O3 were added to a 3-neck flask. The solids were heated to about 300° C., a temperature at which this mixture is molten. A nickel metal sparging tube was inserted into the solution of molten alkali bromides, and H2 gas passed through the sparger and bubbled through the solution. This tube comprised the cathode. H2 gas was allowed to escape from the cell through one of the necks of the flask. A glass tube terminating in a porous glass sparger was also inserted into the solution. Platinum wire and platinum gauze were inside the tube, and the platinum comprised the anode. The porous glass of the sparging tube acted as a separator between the anode compartment (inside the glass tube) and the cathode compartment (outside the tube). The application of about 5 V of potential led to the passage of 1448 mAh of charge over 20 hours.
The net reaction at the cathode was the generation of alkali metal and boron-hydride compounds. At the anode Br2 gas was evolved. A stream of Ar gas helped carry the Br2 gas out of the anode compartment.
After about 20 hours, the potential was removed, and the cathode sparger and the anode tube were withdrawn from the molten solution and the solution was allowed to cool to room temperature and solidify. The resulting solid was dissolved in about 100 mL of 0.5 M aqueous NaOH solution. A small aliquot of solution was submitted to 11B-NMR analysis, which showed the presence of borohydride (BH4 −) anions in solution. Another sample of the same aqueous solution was titrated, determining the yield of boron-hydride anions to be 4%, with respect to the number of mAh of current passed through the cell.
Using the process described in Example 4, about 39.2 g of LiBr, 18.1 g of KBr, and 42.8 g of CsBr, and 1 g of B2O3 were added to a 3-neck flask. The solids were heated to about 300° C., a temperature at which this mixture is molten. A nickel metal sparging tube was inserted into the solution of molten alkali bromides, and H2 gas passed through the sparger and bubbled through the solution. This tube is the cell cathode. H2 gas was allowed to escape from the cell through one of the necks of the flask. A glass tube terminating in a porous glass sparger was also inserted into the solution. Platinum wire and platinum gauze were inside the tube, and the platinum comprised the anode. The porous glass of the sparging tube acted as a separator between the anode compartment (inside the glass tube) and the cathode compartment (outside the tube). The application of about 5 V of potential led to the passage of 1000 mAh of charge over about 6 hours.
After the 6 hour period, the potential applied across the anode and cathode was removed. The cathode sparger and the anode tube were withdrawn from the molten solution and the solution was allowed to cool to room temperature and solidify. The resulting solid was dissolved in about 100 mL of 0.5 M aqueous NaOH solution. A small aliquot of solution was submitted to 11B-NMR analysis, which showed the presence of both BH4 − (borohydride) and B3H8— (triborohydride) anions in solution. Another sample of the same aqueous solution was titrated, determining the yield of boron hydride anions to be 8.3%, with respect to the number of mAh of current passed through the cell.
Tetra-n-butylammonium bromide was heated to about about 120° C., and about 1.5 mL of tri-n-butyl borate (B(O-Bu)3) followed by about 0.5 grams of sodium hydride was added to the hot ionic liquid. The starting materials are only sparingly soluble in the melt and fast stirring was necessary to ensure adequate dispersion. After addition of the sodium hydride was complete, the melt was cooled to room temperature and dissolved in the minimum amount of aqueous 0.5 M NaOH. The presence of borohydride in the aqueous solution was verified by NMR spectroscopy.
The above description and drawings illustrate preferred embodiments that achieve the objects, features and advantages of the present invention. It is not intended that the present invention be limited to the illustrated embodiments. Any modification of the present invention that comes within the spirit and scope of the following claims should be considered part of the present invention.
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|U.S. Classification||205/357, 205/358, 204/246, 204/245|
|International Classification||C25C3/00, C25B1/00|
|Cooperative Classification||C25B1/14, C25B9/08, C25B1/00|
|European Classification||C25B9/08, C25B1/00, C25B1/14|
|Jan 20, 2006||AS||Assignment|
Owner name: MILLENNIUM CELL, INC., NEW JERSEY
Free format text: ASSIGNMENT OF ASSIGNORS INTEREST;ASSIGNOR:KELLY, MICHAEL T.;REEL/FRAME:017482/0345
Effective date: 20060104
|May 15, 2006||AS||Assignment|
Owner name: ENERGY, UNITED STATES DEPARTMENT OF, DISTRICT OF C
Free format text: CONFIRMATORY LICENSE;ASSIGNOR:MILLENNIUM CELL, INC.;REEL/FRAME:017895/0826
Effective date: 20060329