Patent Grant
10718057
The disclosure relates to the field of material processing. More particularly, this disclosure relates to lithium production by an electrolysis process.
Lithium is a chemical element belonging to the alkali metal group and is soft, silvery-white, and corrosive. Lithium is an increasingly valuable metal for use in alloys for heat transfer applications, rechargeable batteries, and the like. A conventional procedure for the production of lithium metal includes crystallization of lithium chloride from an aqueous concentrated solution of lithium chloride, then electrolysis of molten lithium chloride from a eutectic mixture containing 43 to 46 wt. % lithium chloride and 54 to 57 wt. % potassium chloride. The eutectic mixture melts at 352° C. and thus requires use of materials that can withstand high temperatures in a corrosive environment. The molten-salt electrolysis process is a high-temperature process, which has high energy consumption, requires high production costs, and has a significant effect on the environment. The lithium metal resulting from the molten-salt electrolysis process typically contains impurities such as sodium and thus cannot be used in battery applications.
Lithium metal has also been produced in an electrolysis cell under an inert atmosphere at about room temperature. The process includes dissolving a lithium salt selected from LiTFSI, LiCl, LiF, LiPF6, and LiBF4 in a conductive non-aqueous solvent. The non-aqueous conductive solvent contains a bis(trifluoromethylsulfonyl)imide (TFSI) anion and may comprise at least one compound selected from 1-butyl-3-methyl-pyridinium bis(trifluoromethylsulfonyl)imide, 1-methyl-propylpiperidin-ium bis(trifluoromethylsul-fonyl)imide, and 1-ethyl-3-methyl-imidazolium bis(trifluoro-methyl sulfonyl)imide. The lithium salt is dissolved in a maximum amount of 30 wt. % with respect to the total weight of the solution. Re-oxidation of reduced lithium is avoided by the absence of an oxygen atmosphere. The foregoing process provides lithium metal that is plated onto the cathode and that contains impurities. Purification of the lithium metal is performed by heat treating the deposited lithium at 800 to 900° C. for 30 to 90 minutes in an inert gas atmosphere.
The foregoing processes are difficult to conduct in a large scale industrial process and/or high temperatures, typically well above 100° C., to produce lithium metal. Also, a subsequent purification step is often required to produce lithium with a purity of greater than 95 wt. % Accordingly, what is needed is a low temperature process that produces lithium metal with purities that are suitable for battery and other applications without the need for a subsequent purification step.
The present disclosure provides a method for producing lithium metal at a temperature below about 100° in an electrolysis cell. The method includes combining (i) phenyl trihaloalkyl sulfone and (ii) an organic cation bis(trihaloalkylsulfonyl)imide or organic cation bis(trihalosulfonyl)imidic acid in a weight ratio of (i) to (ii) of about 10:90 to about 60:40 to provide a non-aqueous electrolyte composition. A lithium compound selected from the group consisting of LiOH, Li2O and Li2CO3 is dissolved in the electrolyte composition to provide a soluble lithium ion species in the electrolyte composition. Power is applied to the anode and cathode to form lithium metal on the cathode of the electrolysis cell. The lithium metal is separated from the cathode and has a purity of greater than 95 wt. %.
Another embodiment of the disclosure provides an electrolysis cell for producing lithium metal at a temperature below about 100° C. The electrolysis cell includes a cathode compartment comprising a cathode, an anode compartment comprising an anode, a separator between the anode compartment and the cathode compartment, and a non-aqueous electrolyte composition in the anode and cathode compartments. The metal anode and metal cathode are selected from gold, platinum, tungsten, iron, copper and other precious and non-precious metals, as well as non-metal materials. The metal and non-metal materials are particularly selected from metals and non-metals that do not readily form intermetallic compositions with lithium. The non-aqueous electrolyte includes (i) phenyl trihaloalkyl sulfone and (ii) an organic cation bis(trihaloalkylsulfonyl)imide or organic cation bis(trihalosulfonyl)imidic acid in a weight ratio of (i) to (ii) about 10:90 to about 60:40. A lithium compound selected from the group consisting of LiOH, Li2O and Li2CO3 is dissolved in the electrolyte composition. Power is applied to the anode and cathode to form lithium metal on the cathode of the electrolysis cell. The lithium metal is separated from the cathode and has a purity of greater than 95 wt. %.
In some embodiments a weight ratio of soluble lithium ion species to electrolyte composition in the cathode compartment ranges from about 10:60 to about 10:25, particularly from about 10:50 to about 10:30.
In other embodiments, the electrolyte composition further includes a zwitterion or internal salt compound. In some embodiments, the zwitterion comprises a (carboxyalkyl)trialkyl ammonium compound.
In some embodiments heat is applied to the electrolyte composition at a temperature ranging from about 80° C. to less than about 100° C. In other embodiments power is applied to the anode and cathode at a current density ranging from about 0.1 mA/cm2 to about 0.83 mA/cm2.
In some embodiments the electrolysis cell includes an anode compartment, a cathode compartment and a separator between the anode compartment and the cathode compartment. In other embodiments the separator is selected from a fritted glass separator, a microporous membrane, and a salt bridge.
In other embodiments, the organic cation is selected from a phosphonium ion, a sulfonium ion, an ammonium ion, an imidazolium ion, a piperidinium ion, a pyridinium ion and a pyrrolidinium ion. In some embodiments, the halo ion is a fluoride ion and the alky group is a methyl group.
A particular advantage of the method and electrolysis cell described herein is that lithium metal may be produced with a purity of greater than 95 wt. % and even 99 wt. % or greater using a unique solvent in a one-pot process without the need for a subsequent high temperature purification step.
Various advantages are apparent by reference to the detailed description in conjunction with the figure, wherein elements are not to scale so as to more clearly show the details, wherein:
In the following detailed description of the preferred and other embodiments, reference is made to the accompanying drawings, which form a part hereof, and within which are shown by way of illustration the practice of a specific embodiment of a lithium processing apparatus and method of processing lithium metal. It is to be understood that other embodiments may be utilized, and that structural changes may be made and processes may vary in other embodiments.
There are several steps involved in producing relatively pure lithium metal from a lithium compound. “Relatively pure” in this disclosure means the lithium metal has a purity, as made, above 95 wt. %, such as above 97 wt. % and suitably from about 98 to at least 99 wt. %. In the first step of the method, there is provided a non-aqueous, molten electrolyte composition that includes a composition of (i) aryl tri-haloalkyl sulfone, such as phenyl tri-fluoromethyl sulfone, phenyl tri-fluoroethyl sulfone, phenyl tri-chloromethyl sulfone, phenyl tri-chloroethyl sulfone, phenyl tri-bromomethyl sulfone or phenyl tri-bromoethyl sulfone (hereinafter referred to as “FS-13) and (ii) an organic cation bis(trihaloalkylsulfonyl)imide, wherein the cation may be selected from a phosphonium, a sulfonium, an ammonium, an imidazolium, a piperidinium, a pyridinium, a pyrrolidinium cation, and the like with varying functionality. The bis-imide may be selected from bis(trifluoromethanesulfonyl)imide, bis(trifluoroethanesulfonyl)imide, bis(trichloromethanesulfonyl)imide, bis(tricloroethane-sulfonyl)imide, bis(tribromomethanesulfonyl)imide, bis(tri-bromoethanesulfonyl)imide, and the like (hereinafter referred to as “TFSI” ionic liquid. Other compounds that may be used to form a low melting electrolyte composition with FS-13, include but are not limited to 1-butyl-3-methylimidazolium chloride, trioctylmethylammonium chloride, and the like.
The electrolyte composition of (i) and (ii) may be any combination of components (i) and (ii), but has been found to have a melting point below 100° C. around a weight ratio of (i) to (ii) of about 10:90 to about 60:40. A particularly useful weight ratio of (i) to (ii) is about 40:60.
Acidic forms of TFSI− anion may be readily dissolved in the non-aqueous electrolyte composition containing (i) and (ii). Such acidic forms include bis(trihaloalkylsulfonyl)-imidic acid (hereinafter “HTFSI”).
An optional component of the electrolyte composition may be a zwitterion or internal salt compound such as a betaine. A suitable betaine may be selected from (carboxyalkyl)tri-alkylammonium inner salt such as (carboxymethyl)trimethylammonium compound, (carboxyethyl)trimethylammonium compound, (carboxymethyl)triethylammonium compound, and the like. The zwitterion or internal salt may aid in the dissolution of the lithium compound in the electrolyte composition.
Surprisingly, and quite unexpectedly, the lithium metal plated onto the cathode in the cathode compartment has a purity that does not require additional purification subsequent to the electrolysis step of the process for many applications requiring relatively pure lithium metal, such as battery applications. It is believed that the presence of component (i), the aryl tri-haloalkyl sulfone, significantly improves the solubility of the lithium compounds in the electrolyte composition.
Suitable lithium compounds that may be electrolyzed to form lithium metal may be selected from Li2O, Li2S, Li2Se, LiCoO2, Li2Te, or lithium intercalated into a carbon support; lithium sulfates such as Li2SO4; lithium hydroxides such as LiOH; lithium carbonates such as Li2CO3 or LiHCO3 bicarbonate; lithium silicates such as Li4SiO4 or Li2SiO3; lithium nitrates such as LiNO3; lithium phosphates such as Li3PO4; lithium borates such as LiBO2 metaborate; lithium aluminates such as Li2Al2O4; the lithium oxide type minerals spodumene (LiAlSi2O6), petalite (LiAlSi4O10), lepidolite (mica with 3-4 weight percent Li2O), hectorite which is a smectite clay of composition Na0.33(Mg, Li)3Si4O10(F,OH)2; and compositions thereof. Of the foregoing, LiOH, Li2O and Li2CO3 are particularly preferred. Accordingly, embodiments of the disclosure avoid the use of lithium salts such as LiCl, LiF, LiPF6 and LiBF4 which form halogens upon electrolysis thereof. Another advantage of the electrolyte composition containing components (i) and (ii) is that the composition may enable the deposition of lithium metal on the cathode without the need for an inert gas atmosphere. However, an inert gas atmosphere such as argon may be used to reduce the likelihood of reaction of lithium metal with oxygen and moisture.
Referring to
The separator 20 between the anode compartment 12 and the cathode compartment 16 enables the flow of lithium ionic compounds from the anode compartment 12 to the cathode compartment 16 (arrow 24) and the flow of lithium depleted TFSI compounds from the cathode compartment 16 to the anode compartment 12 (arrow 26). A particularly suitable separator 20 may be a fritted glass salt bridge having a porosity ranging from 4 to 90 microns, such as from about 4 to 15 microns. Other separators 20 may be selected from permionic membranes, microporous membranes, and the like.
Each compartment 12 and 16 is filled with a low melting electrolyte composition 28 that is produced by combining aryl tri-haloalkyl sulfone (FS-13) with an organic cation bis(trihaloalkylsulfonyl)imide (cation+TFSI−). In one embodiment, the composition is about 33.3 weight percent FS-13 and about 66.6 weight percent cation+TFSI−, which has been found to have relatively low viscosity, good fluidity, and high solubility for LiTFSI.
During the electrolysis process, the following electrochemical and chemical reactions occur when power is applied across the electrolysis cell 10 by the power supply 22:
With agitation or a mild application of heat, the electrolyte composition 28 remains liquid and the lithium compound 30 is readily dissolved in the electrolyte composition 28. The electrolysis cell 10 may be operated at temperatures ranging from above about 15° C. to less than about 100° C., such as from about 22° C. to about 80° C., or from about 30° C. to about 60° C. Since lithium metal melts at about 186° C., the operating temperature of the electrolysis cell should not be above about 150° C.
Electrons flow in the direction of arrows 32 from the anode 14 to the cathode 18 wherein lithium metal 34 is reduced from the electrolyte composition 28 and plated onto the cathode 18. The metal lithium 34 has a purity of greater than 95 wt. %, such as from about 97 to at least 99 wt. %. The lithium metal 34 may be scraped from the cathode 18, intermittingly or continuously, rinsed with hexane to remove traces of the electrolyte mixture, and collected for use. The process described above may be easily scaled to provide an industrial scale production of relatively pure lithium metal that does not require a subsequent high temperature purification step.
With reference to the following non-limiting example, other aspects of the invention may be illustrated.
A bulk deposition experiment was done in an H-cell with a fine frit salt bridge connector. The cathode compartment was filled with 30 grams of 60:40 wt. % FS-13:tetra-butylphosphoniumTFSI composition containing 25 wt. % LiTFSI, a tungsten cathode rod, and a platinum wire reference electrode. The anode compartment was filled with 30 grams of 60:40 wt. % FS-13:tetra-butlyphosphoniumTFSI composition containing 2 wt. % HTFSI, 10 grams of Li2O powder, and a carbon anode rod. Lithium was electrodeposited on the tungsten cathode rod at a current density of 0.83 mA/cm2 and a voltage of about 7 volts across the electrolysis cell. A total of 518.4 coulombs of charge were passed through the electrolyte composition to produce 35 mg of Li at a coulombic efficiency of 94.2%.
The foregoing descriptions of embodiments have been presented for purposes of illustration and exposition. They are not intended to be exhaustive or to limit the embodiments to the precise forms disclosed. Obvious modifications or variations are possible in light of the above teachings. The embodiments are chosen and described in an effort to provide the best illustrations of principles and practical applications, and to thereby enable one of ordinary skill in the art to utilize the various embodiments as described and with various modifications as are suited to the particular use contemplated. All such modifications and variations are within the scope of the appended claims when interpreted in accordance with the breadth to which they are fairly, legally, and equitably entitled.
The U.S. Government has rights to this invention pursuant to contract number DE-NA0001942 between the U.S. Department of Energy and Consolidated Nuclear Security, LLC.
| Number | Name | Date | Kind |
|---|---|---|---|
| 4455202 | Sintim-Damoa et al. | Jun 1984 | A |
| 7550028 | Riquet et al. | Jun 2009 | B2 |
| 7713396 | Kakuta et al. | May 2010 | B2 |
| 7820317 | Tedjar et al. | Oct 2010 | B2 |
| 20050100793 | Jonghe | May 2005 | A1 |
| 20090017386 | Xu | Jan 2009 | A1 |
| 20090325065 | Fujii | Dec 2009 | A1 |
| 20140147330 | Lee | May 2014 | A1 |
| 20150014184 | Swonger | Jan 2015 | A1 |
| 20160351889 | Swonger | Dec 2016 | A1 |
| Entry |
|---|
| Kipouros, G. J.; Sadoway, D. R., Toward New Technologies for the Production of Lithium, JOM, May 1998, pp. 24-25. |
