US20110200882A1 - Lithium containing transition metal sulfide compounds - Google Patents
Lithium containing transition metal sulfide compounds Download PDFInfo
- Publication number
- US20110200882A1 US20110200882A1 US13/124,051 US200913124051A US2011200882A1 US 20110200882 A1 US20110200882 A1 US 20110200882A1 US 200913124051 A US200913124051 A US 200913124051A US 2011200882 A1 US2011200882 A1 US 2011200882A1
- Authority
- US
- United States
- Prior art keywords
- lithium
- transition metal
- metal sulfide
- containing transition
- producing
- Prior art date
- Legal status (The legal status is an assumption and is not a legal conclusion. Google has not performed a legal analysis and makes no representation as to the accuracy of the status listed.)
- Abandoned
Links
- 229910052723 transition metal Inorganic materials 0.000 title claims abstract description 76
- -1 transition metal sulfide compounds Chemical class 0.000 title claims abstract description 67
- 229910052744 lithium Inorganic materials 0.000 title claims abstract description 63
- WHXSMMKQMYFTQS-UHFFFAOYSA-N Lithium Chemical compound [Li] WHXSMMKQMYFTQS-UHFFFAOYSA-N 0.000 title claims abstract description 57
- 238000000034 method Methods 0.000 claims abstract description 40
- 238000006243 chemical reaction Methods 0.000 claims abstract description 30
- INHCSSUBVCNVSK-UHFFFAOYSA-L lithium sulfate Inorganic materials [Li+].[Li+].[O-]S([O-])(=O)=O INHCSSUBVCNVSK-UHFFFAOYSA-L 0.000 claims abstract description 27
- 239000000463 material Substances 0.000 claims abstract description 27
- RBTVSNLYYIMMKS-UHFFFAOYSA-N tert-butyl 3-aminoazetidine-1-carboxylate;hydrochloride Chemical compound Cl.CC(C)(C)OC(=O)N1CC(N)C1 RBTVSNLYYIMMKS-UHFFFAOYSA-N 0.000 claims abstract description 21
- 150000003624 transition metals Chemical class 0.000 claims abstract description 14
- 239000002243 precursor Substances 0.000 claims abstract description 12
- 230000003647 oxidation Effects 0.000 claims abstract description 8
- 238000007254 oxidation reaction Methods 0.000 claims abstract description 8
- 238000010438 heat treatment Methods 0.000 claims abstract description 7
- OKTJSMMVPCPJKN-UHFFFAOYSA-N Carbon Chemical compound [C] OKTJSMMVPCPJKN-UHFFFAOYSA-N 0.000 claims description 31
- 229910052799 carbon Inorganic materials 0.000 claims description 26
- XEEYBQQBJWHFJM-UHFFFAOYSA-N Iron Chemical compound [Fe] XEEYBQQBJWHFJM-UHFFFAOYSA-N 0.000 claims description 12
- KWGKDLIKAYFUFQ-UHFFFAOYSA-M lithium chloride Chemical compound [Li+].[Cl-] KWGKDLIKAYFUFQ-UHFFFAOYSA-M 0.000 claims description 12
- 239000011230 binding agent Substances 0.000 claims description 11
- 239000003638 chemical reducing agent Substances 0.000 claims description 11
- 239000002904 solvent Substances 0.000 claims description 11
- 239000007858 starting material Substances 0.000 claims description 11
- 229910001416 lithium ion Inorganic materials 0.000 claims description 10
- HBBGRARXTFLTSG-UHFFFAOYSA-N Lithium ion Chemical compound [Li+] HBBGRARXTFLTSG-UHFFFAOYSA-N 0.000 claims description 9
- PXHVJJICTQNCMI-UHFFFAOYSA-N Nickel Chemical compound [Ni] PXHVJJICTQNCMI-UHFFFAOYSA-N 0.000 claims description 8
- UCKMPCXJQFINFW-UHFFFAOYSA-N Sulphide Chemical compound [S-2] UCKMPCXJQFINFW-UHFFFAOYSA-N 0.000 claims description 6
- 239000003792 electrolyte Substances 0.000 claims description 5
- 229910052742 iron Inorganic materials 0.000 claims description 5
- 239000011734 sodium Substances 0.000 claims description 5
- RYGMFSIKBFXOCR-UHFFFAOYSA-N Copper Chemical compound [Cu] RYGMFSIKBFXOCR-UHFFFAOYSA-N 0.000 claims description 4
- 229910017052 cobalt Inorganic materials 0.000 claims description 4
- 239000010941 cobalt Substances 0.000 claims description 4
- GUTLYIVDDKVIGB-UHFFFAOYSA-N cobalt atom Chemical compound [Co] GUTLYIVDDKVIGB-UHFFFAOYSA-N 0.000 claims description 4
- 229910052802 copper Inorganic materials 0.000 claims description 4
- 239000010949 copper Substances 0.000 claims description 4
- HSZCZNFXUDYRKD-UHFFFAOYSA-M lithium iodide Chemical compound [Li+].[I-] HSZCZNFXUDYRKD-UHFFFAOYSA-M 0.000 claims description 4
- WPBNNNQJVZRUHP-UHFFFAOYSA-L manganese(2+);methyl n-[[2-(methoxycarbonylcarbamothioylamino)phenyl]carbamothioyl]carbamate;n-[2-(sulfidocarbothioylamino)ethyl]carbamodithioate Chemical compound [Mn+2].[S-]C(=S)NCCNC([S-])=S.COC(=O)NC(=S)NC1=CC=CC=C1NC(=S)NC(=O)OC WPBNNNQJVZRUHP-UHFFFAOYSA-L 0.000 claims description 4
- 229910052759 nickel Inorganic materials 0.000 claims description 4
- DGAQECJNVWCQMB-PUAWFVPOSA-M Ilexoside XXIX Chemical compound C[C@@H]1CC[C@@]2(CC[C@@]3(C(=CC[C@H]4[C@]3(CC[C@@H]5[C@@]4(CC[C@@H](C5(C)C)OS(=O)(=O)[O-])C)C)[C@@H]2[C@]1(C)O)C)C(=O)O[C@H]6[C@@H]([C@H]([C@@H]([C@H](O6)CO)O)O)O.[Na+] DGAQECJNVWCQMB-PUAWFVPOSA-M 0.000 claims description 3
- 229910001508 alkali metal halide Inorganic materials 0.000 claims description 3
- 150000008045 alkali metal halides Chemical class 0.000 claims description 3
- 239000002002 slurry Substances 0.000 claims description 3
- 229910052708 sodium Inorganic materials 0.000 claims description 3
- OYPRJOBELJOOCE-UHFFFAOYSA-N Calcium Chemical compound [Ca] OYPRJOBELJOOCE-UHFFFAOYSA-N 0.000 claims description 2
- VMQMZMRVKUZKQL-UHFFFAOYSA-N Cu+ Chemical compound [Cu+] VMQMZMRVKUZKQL-UHFFFAOYSA-N 0.000 claims description 2
- FYYHWMGAXLPEAU-UHFFFAOYSA-N Magnesium Chemical compound [Mg] FYYHWMGAXLPEAU-UHFFFAOYSA-N 0.000 claims description 2
- ZLMJMSJWJFRBEC-UHFFFAOYSA-N Potassium Chemical compound [K] ZLMJMSJWJFRBEC-UHFFFAOYSA-N 0.000 claims description 2
- BQCADISMDOOEFD-UHFFFAOYSA-N Silver Chemical compound [Ag] BQCADISMDOOEFD-UHFFFAOYSA-N 0.000 claims description 2
- HCHKCACWOHOZIP-UHFFFAOYSA-N Zinc Chemical compound [Zn] HCHKCACWOHOZIP-UHFFFAOYSA-N 0.000 claims description 2
- 239000011575 calcium Substances 0.000 claims description 2
- 229910052791 calcium Inorganic materials 0.000 claims description 2
- 239000011777 magnesium Substances 0.000 claims description 2
- 229910052749 magnesium Inorganic materials 0.000 claims description 2
- 239000008188 pellet Substances 0.000 claims description 2
- 229910052700 potassium Inorganic materials 0.000 claims description 2
- 239000011591 potassium Substances 0.000 claims description 2
- 239000000843 powder Substances 0.000 claims description 2
- 238000002360 preparation method Methods 0.000 claims description 2
- 229910052709 silver Inorganic materials 0.000 claims description 2
- 239000004332 silver Substances 0.000 claims description 2
- 229910052725 zinc Inorganic materials 0.000 claims description 2
- 239000011701 zinc Substances 0.000 claims description 2
- AMXOYNBUYSYVKV-UHFFFAOYSA-M lithium bromide Chemical compound [Li+].[Br-] AMXOYNBUYSYVKV-UHFFFAOYSA-M 0.000 claims 2
- 239000004215 Carbon black (E152) Substances 0.000 claims 1
- 229930195733 hydrocarbon Natural products 0.000 claims 1
- 150000002430 hydrocarbons Chemical class 0.000 claims 1
- 230000008569 process Effects 0.000 abstract description 10
- 239000000203 mixture Substances 0.000 description 14
- 150000001875 compounds Chemical class 0.000 description 11
- GLNWILHOFOBOFD-UHFFFAOYSA-N lithium sulfide Chemical compound [Li+].[Li+].[S-2] GLNWILHOFOBOFD-UHFFFAOYSA-N 0.000 description 9
- XKRFYHLGVUSROY-UHFFFAOYSA-N Argon Chemical compound [Ar] XKRFYHLGVUSROY-UHFFFAOYSA-N 0.000 description 8
- 150000003839 salts Chemical class 0.000 description 8
- 238000004519 manufacturing process Methods 0.000 description 7
- 239000000047 product Substances 0.000 description 7
- FYGHSUNMUKGBRK-UHFFFAOYSA-N 1,2,3-trimethylbenzene Chemical compound CC1=CC=CC(C)=C1C FYGHSUNMUKGBRK-UHFFFAOYSA-N 0.000 description 6
- MBMLMWLHJBBADN-UHFFFAOYSA-N Ferrous sulfide Chemical compound [Fe]=S MBMLMWLHJBBADN-UHFFFAOYSA-N 0.000 description 6
- 239000007795 chemical reaction product Substances 0.000 description 6
- 239000007789 gas Substances 0.000 description 6
- 238000002156 mixing Methods 0.000 description 6
- 230000008901 benefit Effects 0.000 description 5
- 229910002804 graphite Inorganic materials 0.000 description 5
- 239000010439 graphite Substances 0.000 description 5
- 239000012535 impurity Substances 0.000 description 5
- 238000003780 insertion Methods 0.000 description 5
- 230000037431 insertion Effects 0.000 description 5
- 229910000625 lithium cobalt oxide Inorganic materials 0.000 description 5
- BFZPBUKRYWOWDV-UHFFFAOYSA-N lithium;oxido(oxo)cobalt Chemical compound [Li+].[O-][Co]=O BFZPBUKRYWOWDV-UHFFFAOYSA-N 0.000 description 5
- LWRYTNDOEJYQME-UHFFFAOYSA-N lithium;sulfanylideneiron Chemical compound [Li].[Fe]=S LWRYTNDOEJYQME-UHFFFAOYSA-N 0.000 description 5
- 150000004763 sulfides Chemical class 0.000 description 5
- IJGRMHOSHXDMSA-UHFFFAOYSA-N Atomic nitrogen Chemical compound N#N IJGRMHOSHXDMSA-UHFFFAOYSA-N 0.000 description 4
- CDBYLPFSWZWCQE-UHFFFAOYSA-L Sodium Carbonate Chemical compound [Na+].[Na+].[O-]C([O-])=O CDBYLPFSWZWCQE-UHFFFAOYSA-L 0.000 description 4
- FAPWRFPIFSIZLT-UHFFFAOYSA-M Sodium chloride Chemical compound [Na+].[Cl-] FAPWRFPIFSIZLT-UHFFFAOYSA-M 0.000 description 4
- 229910052786 argon Inorganic materials 0.000 description 4
- 230000001351 cycling effect Effects 0.000 description 4
- 229910052960 marcasite Inorganic materials 0.000 description 4
- 229910052683 pyrite Inorganic materials 0.000 description 4
- 239000012429 reaction media Substances 0.000 description 4
- 238000006722 reduction reaction Methods 0.000 description 4
- YMWUJEATGCHHMB-UHFFFAOYSA-N Dichloromethane Chemical compound ClCCl YMWUJEATGCHHMB-UHFFFAOYSA-N 0.000 description 3
- OKKJLVBELUTLKV-UHFFFAOYSA-N Methanol Chemical compound OC OKKJLVBELUTLKV-UHFFFAOYSA-N 0.000 description 3
- 229920003171 Poly (ethylene oxide) Polymers 0.000 description 3
- YXFVVABEGXRONW-UHFFFAOYSA-N Toluene Chemical compound CC1=CC=CC=C1 YXFVVABEGXRONW-UHFFFAOYSA-N 0.000 description 3
- 239000002131 composite material Substances 0.000 description 3
- 239000007772 electrode material Substances 0.000 description 3
- 238000009472 formulation Methods 0.000 description 3
- 229910021397 glassy carbon Inorganic materials 0.000 description 3
- 239000011261 inert gas Substances 0.000 description 3
- 239000000376 reactant Substances 0.000 description 3
- 239000011541 reaction mixture Substances 0.000 description 3
- 238000003860 storage Methods 0.000 description 3
- 238000012546 transfer Methods 0.000 description 3
- 229910001428 transition metal ion Inorganic materials 0.000 description 3
- QAOWNCQODCNURD-UHFFFAOYSA-L Sulfate Chemical compound [O-]S([O-])(=O)=O QAOWNCQODCNURD-UHFFFAOYSA-L 0.000 description 2
- 238000002441 X-ray diffraction Methods 0.000 description 2
- 239000000654 additive Substances 0.000 description 2
- 239000004411 aluminium Substances 0.000 description 2
- 229910052782 aluminium Inorganic materials 0.000 description 2
- XAGFODPZIPBFFR-UHFFFAOYSA-N aluminium Chemical compound [Al] XAGFODPZIPBFFR-UHFFFAOYSA-N 0.000 description 2
- 239000006229 carbon black Substances 0.000 description 2
- 239000010406 cathode material Substances 0.000 description 2
- 239000003795 chemical substances by application Substances 0.000 description 2
- 239000011248 coating agent Substances 0.000 description 2
- 238000000576 coating method Methods 0.000 description 2
- 230000001627 detrimental effect Effects 0.000 description 2
- 230000000694 effects Effects 0.000 description 2
- 230000004907 flux Effects 0.000 description 2
- 229910052739 hydrogen Inorganic materials 0.000 description 2
- 239000001257 hydrogen Substances 0.000 description 2
- 238000011065 in-situ storage Methods 0.000 description 2
- PQXKHYXIUOZZFA-UHFFFAOYSA-M lithium fluoride Chemical compound [Li+].[F-] PQXKHYXIUOZZFA-UHFFFAOYSA-M 0.000 description 2
- VNWKTOKETHGBQD-UHFFFAOYSA-N methane Chemical compound C VNWKTOKETHGBQD-UHFFFAOYSA-N 0.000 description 2
- 229910052757 nitrogen Inorganic materials 0.000 description 2
- 229920000642 polymer Polymers 0.000 description 2
- 229920001343 polytetrafluoroethylene Polymers 0.000 description 2
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- 238000000746 purification Methods 0.000 description 2
- 230000035484 reaction time Effects 0.000 description 2
- 230000009467 reduction Effects 0.000 description 2
- 229910000029 sodium carbonate Inorganic materials 0.000 description 2
- 239000011780 sodium chloride Substances 0.000 description 2
- PUZPDOWCWNUUKD-UHFFFAOYSA-M sodium fluoride Chemical compound [F-].[Na+] PUZPDOWCWNUUKD-UHFFFAOYSA-M 0.000 description 2
- 239000007787 solid Substances 0.000 description 2
- 239000000126 substance Substances 0.000 description 2
- 239000013077 target material Substances 0.000 description 2
- 238000005979 thermal decomposition reaction Methods 0.000 description 2
- 101100457021 Caenorhabditis elegans mag-1 gene Proteins 0.000 description 1
- UGFAIRIUMAVXCW-UHFFFAOYSA-N Carbon monoxide Chemical compound [O+]#[C-] UGFAIRIUMAVXCW-UHFFFAOYSA-N 0.000 description 1
- XDTMQSROBMDMFD-UHFFFAOYSA-N Cyclohexane Chemical compound C1CCCCC1 XDTMQSROBMDMFD-UHFFFAOYSA-N 0.000 description 1
- 229920001353 Dextrin Polymers 0.000 description 1
- 239000004375 Dextrin Substances 0.000 description 1
- RWSOTUBLDIXVET-UHFFFAOYSA-N Dihydrogen sulfide Chemical compound S RWSOTUBLDIXVET-UHFFFAOYSA-N 0.000 description 1
- 229920002943 EPDM rubber Polymers 0.000 description 1
- 229920000181 Ethylene propylene rubber Polymers 0.000 description 1
- 229910016955 Fe1-xMnx Inorganic materials 0.000 description 1
- UFHFLCQGNIYNRP-UHFFFAOYSA-N Hydrogen Chemical compound [H][H] UFHFLCQGNIYNRP-UHFFFAOYSA-N 0.000 description 1
- 229910011279 LiCoPO4 Inorganic materials 0.000 description 1
- 229910052493 LiFePO4 Inorganic materials 0.000 description 1
- 229910001305 LiMPO4 Inorganic materials 0.000 description 1
- 229910000668 LiMnPO4 Inorganic materials 0.000 description 1
- 229910013084 LiNiPO4 Inorganic materials 0.000 description 1
- 101100067996 Mus musculus Gbp1 gene Proteins 0.000 description 1
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- CZMRCDWAGMRECN-UGDNZRGBSA-N Sucrose Chemical compound O[C@H]1[C@H](O)[C@@H](CO)O[C@@]1(CO)O[C@@H]1[C@H](O)[C@@H](O)[C@H](O)[C@@H](CO)O1 CZMRCDWAGMRECN-UGDNZRGBSA-N 0.000 description 1
- 229930006000 Sucrose Natural products 0.000 description 1
- 239000011149 active material Substances 0.000 description 1
- 230000000996 additive effect Effects 0.000 description 1
- 150000001298 alcohols Chemical class 0.000 description 1
- 150000001335 aliphatic alkanes Chemical class 0.000 description 1
- 238000004458 analytical method Methods 0.000 description 1
- 238000013459 approach Methods 0.000 description 1
- 238000000498 ball milling Methods 0.000 description 1
- 238000010923 batch production Methods 0.000 description 1
- NFMAZVUSKIJEIH-UHFFFAOYSA-N bis(sulfanylidene)iron Chemical compound S=[Fe]=S NFMAZVUSKIJEIH-UHFFFAOYSA-N 0.000 description 1
- 229910021538 borax Inorganic materials 0.000 description 1
- 239000006227 byproduct Substances 0.000 description 1
- 229910002091 carbon monoxide Inorganic materials 0.000 description 1
- 239000003575 carbonaceous material Substances 0.000 description 1
- 230000015556 catabolic process Effects 0.000 description 1
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- 239000003610 charcoal Substances 0.000 description 1
- 239000007805 chemical reaction reactant Substances 0.000 description 1
- 239000000571 coke Substances 0.000 description 1
- 238000010924 continuous production Methods 0.000 description 1
- YOCUPQPZWBBYIX-UHFFFAOYSA-N copper nickel Chemical compound [Ni].[Cu] YOCUPQPZWBBYIX-UHFFFAOYSA-N 0.000 description 1
- 238000013480 data collection Methods 0.000 description 1
- 238000000354 decomposition reaction Methods 0.000 description 1
- 238000006731 degradation reaction Methods 0.000 description 1
- 238000011161 development Methods 0.000 description 1
- 230000018109 developmental process Effects 0.000 description 1
- 235000019425 dextrin Nutrition 0.000 description 1
- 238000007599 discharging Methods 0.000 description 1
- 238000003487 electrochemical reaction Methods 0.000 description 1
- 239000002001 electrolyte material Substances 0.000 description 1
- HQQADJVZYDDRJT-UHFFFAOYSA-N ethene;prop-1-ene Chemical group C=C.CC=C HQQADJVZYDDRJT-UHFFFAOYSA-N 0.000 description 1
- 238000000605 extraction Methods 0.000 description 1
- 235000013312 flour Nutrition 0.000 description 1
- 238000007429 general method Methods 0.000 description 1
- 239000011521 glass Substances 0.000 description 1
- 150000008282 halocarbons Chemical class 0.000 description 1
- 150000002431 hydrogen Chemical class 0.000 description 1
- 229910000037 hydrogen sulfide Inorganic materials 0.000 description 1
- 238000011835 investigation Methods 0.000 description 1
- 150000002500 ions Chemical class 0.000 description 1
- 229910000339 iron disulfide Inorganic materials 0.000 description 1
- 238000011031 large-scale manufacturing process Methods 0.000 description 1
- XIXADJRWDQXREU-UHFFFAOYSA-M lithium acetate Chemical compound [Li+].CC([O-])=O XIXADJRWDQXREU-UHFFFAOYSA-M 0.000 description 1
- 229910002102 lithium manganese oxide Inorganic materials 0.000 description 1
- 229910021450 lithium metal oxide Inorganic materials 0.000 description 1
- CJYZTOPVWURGAI-UHFFFAOYSA-N lithium;manganese;manganese(3+);oxygen(2-) Chemical compound [Li+].[O-2].[O-2].[O-2].[O-2].[Mn].[Mn+3] CJYZTOPVWURGAI-UHFFFAOYSA-N 0.000 description 1
- VROAXDSNYPAOBJ-UHFFFAOYSA-N lithium;oxido(oxo)nickel Chemical compound [Li+].[O-][Ni]=O VROAXDSNYPAOBJ-UHFFFAOYSA-N 0.000 description 1
- VLXXBCXTUVRROQ-UHFFFAOYSA-N lithium;oxido-oxo-(oxomanganiooxy)manganese Chemical compound [Li+].[O-][Mn](=O)O[Mn]=O VLXXBCXTUVRROQ-UHFFFAOYSA-N 0.000 description 1
- URIIGZKXFBNRAU-UHFFFAOYSA-N lithium;oxonickel Chemical compound [Li].[Ni]=O URIIGZKXFBNRAU-UHFFFAOYSA-N 0.000 description 1
- 229910052751 metal Inorganic materials 0.000 description 1
- 239000002184 metal Substances 0.000 description 1
- 239000007769 metal material Substances 0.000 description 1
- 239000000178 monomer Substances 0.000 description 1
- 239000004570 mortar (masonry) Substances 0.000 description 1
- 150000002816 nickel compounds Chemical class 0.000 description 1
- 239000011368 organic material Substances 0.000 description 1
- 239000002245 particle Substances 0.000 description 1
- 229920002239 polyacrylonitrile Polymers 0.000 description 1
- 229920000573 polyethylene Polymers 0.000 description 1
- 229920001223 polyethylene glycol Polymers 0.000 description 1
- 239000004926 polymethyl methacrylate Substances 0.000 description 1
- 229920002981 polyvinylidene fluoride Polymers 0.000 description 1
- 238000000634 powder X-ray diffraction Methods 0.000 description 1
- 238000001144 powder X-ray diffraction data Methods 0.000 description 1
- 230000000135 prohibitive effect Effects 0.000 description 1
- NIFIFKQPDTWWGU-UHFFFAOYSA-N pyrite Chemical compound [Fe+2].[S-][S-] NIFIFKQPDTWWGU-UHFFFAOYSA-N 0.000 description 1
- 238000002407 reforming Methods 0.000 description 1
- 238000012552 review Methods 0.000 description 1
- 239000011775 sodium fluoride Substances 0.000 description 1
- 235000013024 sodium fluoride Nutrition 0.000 description 1
- 239000004328 sodium tetraborate Substances 0.000 description 1
- 235000010339 sodium tetraborate Nutrition 0.000 description 1
- 239000011343 solid material Substances 0.000 description 1
- 238000003746 solid phase reaction Methods 0.000 description 1
- 238000010671 solid-state reaction Methods 0.000 description 1
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- 238000012360 testing method Methods 0.000 description 1
- 230000007704 transition Effects 0.000 description 1
- 150000003623 transition metal compounds Chemical class 0.000 description 1
- RIUWBIIVUYSTCN-UHFFFAOYSA-N trilithium borate Chemical compound [Li+].[Li+].[Li+].[O-]B([O-])[O-] RIUWBIIVUYSTCN-UHFFFAOYSA-N 0.000 description 1
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Images
Classifications
-
- C—CHEMISTRY; METALLURGY
- C01—INORGANIC CHEMISTRY
- C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
- C01B17/00—Sulfur; Compounds thereof
- C01B17/22—Alkali metal sulfides or polysulfides
- C01B17/24—Preparation by reduction
-
- 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
- H01M10/052—Li-accumulators
- H01M10/0525—Rocking-chair batteries, i.e. batteries with lithium insertion or intercalation in both electrodes; Lithium-ion batteries
-
- C—CHEMISTRY; METALLURGY
- C01—INORGANIC CHEMISTRY
- C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
- C01B17/00—Sulfur; Compounds thereof
- C01B17/20—Methods for preparing sulfides or polysulfides, in general
-
- C—CHEMISTRY; METALLURGY
- C01—INORGANIC CHEMISTRY
- C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
- C01B17/00—Sulfur; Compounds thereof
- C01B17/22—Alkali metal sulfides or polysulfides
- C01B17/24—Preparation by reduction
- C01B17/26—Preparation by reduction with carbon
-
- C—CHEMISTRY; METALLURGY
- C01—INORGANIC CHEMISTRY
- C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
- C01B17/00—Sulfur; Compounds thereof
- C01B17/22—Alkali metal sulfides or polysulfides
- C01B17/24—Preparation by reduction
- C01B17/28—Preparation by reduction with reducing gases
-
- C—CHEMISTRY; METALLURGY
- C01—INORGANIC CHEMISTRY
- C01D—COMPOUNDS OF ALKALI METALS, i.e. LITHIUM, SODIUM, POTASSIUM, RUBIDIUM, CAESIUM, OR FRANCIUM
- C01D15/00—Lithium compounds
-
- C—CHEMISTRY; METALLURGY
- C01—INORGANIC CHEMISTRY
- C01G—COMPOUNDS CONTAINING METALS NOT COVERED BY SUBCLASSES C01D OR C01F
- C01G3/00—Compounds of copper
- C01G3/12—Sulfides
-
- C—CHEMISTRY; METALLURGY
- C01—INORGANIC CHEMISTRY
- C01G—COMPOUNDS CONTAINING METALS NOT COVERED BY SUBCLASSES C01D OR C01F
- C01G45/00—Compounds of manganese
- C01G45/006—Compounds containing, besides manganese, two or more other elements, with the exception of oxygen or hydrogen
-
- C—CHEMISTRY; METALLURGY
- C01—INORGANIC CHEMISTRY
- C01G—COMPOUNDS CONTAINING METALS NOT COVERED BY SUBCLASSES C01D OR C01F
- C01G49/00—Compounds of iron
-
- 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, besides iron, two or more other elements, with the exception of oxygen or hydrogen
-
- C—CHEMISTRY; METALLURGY
- C01—INORGANIC CHEMISTRY
- C01G—COMPOUNDS CONTAINING METALS NOT COVERED BY SUBCLASSES C01D OR C01F
- C01G49/00—Compounds of iron
- C01G49/12—Sulfides
-
- C—CHEMISTRY; METALLURGY
- C01—INORGANIC CHEMISTRY
- C01G—COMPOUNDS CONTAINING METALS NOT COVERED BY SUBCLASSES C01D OR C01F
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Definitions
- the present invention relates to lithium-containing transition metal sulfide compounds, a method of manufacturing lithium-containing transition metal sulfide compounds, the use of lithium-containing transition metal sulfide compounds in electrode materials in the manufacture of lithium ion cells or batteries and the use of such cells or batteries in commercial products.
- Lithium ion batteries are secondary batteries that comprise an anode (negative electrode), a cathode (positive electrode) and an electrolyte material. They operate by the transfer of lithium ions between the anode and the cathode, and they are not to be confused with lithium batteries, which are characterised by containing metallic lithium.
- Lithium ion batteries are currently the most commonly used type of rechargeable battery and typically the anode comprises an insertion material, for example carbon in the form of coke or graphite.
- An electroactive couple is formed using a cathode that comprises a lithium-containing insertion material.
- Typical lithium-containing insertion materials are lithium cobalt oxide (LiCoO 2 ), lithium nickel oxide (LiNiO 2 ) and lithium manganese oxide (LiMn 2 O 4 ).
- LiCoO 2 lithium cobalt oxide
- LiNiO 2 lithium nickel oxide
- LiMn 2 O 4 lithium manganese oxide
- this type of cell In its initial condition, this type of cell is uncharged, therefore to deliver electrochemical energy the cell must be charged to transfer lithium to the anode from the lithium-containing cathode. Upon discharge, the lithium ions are transferred from the anode back to the cathode. Subsequent charging and discharging operations transfers the lithium ions back and forth between the cathode and the anode over the life of the battery.
- a review of the recent developments and likely advantages of lithium rechargeable batteries is provided by Tsutomu Ohzuku and Ralph Brodd in Journal of Power Sources 2007.06.154.
- LiMPO 4 lithium-mixed metal materials
- M is at least one first row transition metal.
- Preferred compounds include LiFePO 4 , LiMnPO 4 , LiCoPO 4 , and LiNiPO 4 and mixed transition metal compounds such as Li 1-2x Fe 1-x Co x PO 4 or Li 1-2x Fe 1-x Mn x PO 4 where 0 ⁇ x ⁇ 1.
- lithium ion rechargeable batteries are limited by the prohibitive cost of providing the lithium electrode material, particularly in the case of lithium cobalt oxide. Consequently, current commercialisation is restricted to premium applications such as portable computers and mobile telephones.
- sulfides may be used in place of oxides, as cathode materials.
- the capacity of some sulfide-based cathodes can be as much as about 3 times greater. Based on this, some sulfide-based cathodes achieve an overall advantage of about 1.5 times in terms of cathode energy density for batteries measured against a lithium metal anode, as compared against their oxide counterparts, and this makes the use of these sulfides a very attractive proposition. For example, in the case of lithium iron sulfide a theoretical capacity of 400 mAhg ⁇ 1 may be obtained with an average operating voltage of 2.2V versus a lithium metal anode.
- lithium-containing transition metal sulfides will be a convenient substitute material for the lithium metal oxides described above, with lithium iron sulfide being already described in the patent literature, for example in U.S. Pat. No. 7,018,603, to be a useful cathode material in secondary cells.
- the commercialisation of lithium-containing transition metal sulfides will depend largely on their cost of production. Taking lithium iron sulfide as a specific example, the conventional process for making this material is via a solid state reaction in which lithium sulfide (Li 2 S) and ferrous sulfide (FeS), are intimately mixed together and heated under an inert atmosphere at a temperature of about 800° C.
- the starting materials ferrous sulfide (FeS) and iron disulfide (FeS 2 ) are relatively inexpensive as they are found as naturally occurring materials, and are dug out of the ground.
- FeS ferrous sulfide
- FeS 2 iron disulfide
- Li 2 S the other starting material
- the kinetics of this reaction are reported in U.S. Pat. No. 7,018,603 to be very slow and it can apparently take up to one month to complete the reaction, thus this route is believed to be highly unfavourable in terms of energy costs and not commercially viable for the production of electrode materials.
- U.S. Pat. No. 7,018,603 discloses reacting a transition metal sulfide such as FeS with lithium sulfide in a reaction medium comprising molten salt or a mixture of molten salts at high temperature (temperatures of 450° C. to 700° C. are exemplified).
- the preferred molten salts are lithium halides. Whilst this reaction proceeds at a good rate there are still several issues that make it less than ideal. Firstly, the fact it uses Li 2 S as a starting material leads to the handling and storage problems described above.
- reaction medium molten lithium halide used in 1.5 molar excess
- solvent extraction it is very difficult to separate the reaction medium (molten lithium halide used in 1.5 molar excess) from the desired reaction product other then by solvent extraction, and this type of extraction is expensive. Further, even after rigorous purification as much as 8% of the reaction medium salt is still present in the reaction product, and this level of impurity is detrimental to the charge capacity per gram of lithium iron sulfide.
- a method of producing a lithium-containing transition metal sulfide characterised in that it comprises heating at least one transition metal sulfide with lithium sulfate, or any material that is a precursor for lithium sulfate, under reducing conditions, wherein the oxidation state of the transition metal is not reduced during the reaction process.
- the reducing conditions preferably comprise a reducing agent such as carbon and/or performing the reaction process in a reducing atmosphere.
- y 0 to 1;
- z 0 to 1;
- A is selected from one or more of silver (Ag), sodium (Na), copper (Cu(I)) and potassium (K) and M is a generic representation for one or more transition metals.
- the reducing conditions used in the method of the present invention may be any well-known and used in the art of chemical reduction. Preferred examples involve one or more reducing gases, such as carbon monoxide, hydrogen, reforming gas (mixture of hydrogen and nitrogen), hydrogen sulfide, methane and other gaseous alkanes. One or more reducing agents such as carbon may also be used either alone or in combination with a reducing gas. In the present invention, it is highly preferred that the reducing conditions do not reduce the oxidation state of the transition metal ion.
- the ideal reaction temperature used in the present invention is that which is sufficient to cause the lithium sulfate to be reduced to lithium sulfide and for this intermediate to react with the transition metal sulfide. If the reaction temperature is too high, the level and number of impurities, caused for example by the over-reduction of the transition metal ion to the zero oxidation or metallic state, is found to increase. The actual temperature used, therefore, will depend on the chosen transition metal sulfide. As a general rule the reaction temperature is conveniently from 650 to 950° C., and preferably from 750 to 850° C. It is observed that the yield of target material does not significantly increase when the reaction temperature is above 860° C. (the decomposition temperature of lithium sulfate.
- reaction time varies according to reaction temperature and as one might expect, the higher the temperature, the faster the reaction.
- a suitable reaction temperature/time profile that will produce the desired lithium-containing transition metal sulfide includes heating the reaction mixture for 12 hours at 750° C. Alternatively one could heat the reaction mixture for 9 hours at 800° C.
- the at least one transition metal sulfide used in the method of the present invention may be one or more sulfide compounds comprising one or more transition metals. This includes the use of single and/or mixtures of several transition metals in the sulfide.
- the reaction method uses mono-sulfides.
- Particularly suitable transition metals comprise one or more of manganese, iron, cobalt, nickel copper and zinc.
- the transition metals are selected from magnesium, calcium, manganese, iron, cobalt and nickel. Particularly preferably the transition metals have an initial oxidation state of +2. Sulfides that comprise iron are the most preferred transition metal sulfides.
- the reaction product is itself reactive towards water. Therefore, it is advantageous to form and handle the lithium-containing transition metal sulfides under a dry and inert atmosphere such as argon or nitrogen.
- Suitable reaction vessels comprise glassy carbon or graphite crucibles that generally have a loose fitting lid, however, a sealed pressurized vessel may also be used.
- a continuous process for example, a rotary tube furnace, although a retort batch process may also be used.
- the reaction of the present invention is a solid-state in situ process and this means that all reactants are in solid form and are without the need to use a reaction medium such as a solvent.
- the present reaction process is notably distinct from the process described in U.S. Pat. No. 7,018,603, for example the present invention uses lithium sulfate directly as a starting material and moreover, it does not involve a solvent comprising a molten salt or mixture of molten salts.
- the reactants are solid materials that are first ground using a ball mill to produce a fine powder that can either be used directly or first pressed into a pellet.
- the reducing conditions in the process do not directly reduce the oxidation state of the transition metal ion.
- any amount of it may be used but it is convenient not to use too much to prevent it becoming a significant impurity in the reaction product, and thereby lowering its specific capacity. Having said this, it has been found to be of significant advantage, particularly to the conductivity of the target material, for at least a small amount of carbon to be present in the reaction product.
- the carbon is considerably intimately mixed with the lithium-containing transition metal sulfide product.
- the degree of mixing described as “intimate” refers specifically to the chemical as opposed to physical mixing that is achieved when carbon is used, at least in part, to provide the reducing conditions in the process of the present invention. This “intimate” mixing is quite different from the degree of mixing that would ever be achieved using ball milling or other physical mixing apparatus.
- the carbon is dispersed at the microscopic level on individual particles of the lithium-containing transition metal sulfide.
- the ratio of reaction starting materials is typically 1 mole of transition metal sulfide: the equivalent of from 0.5 to 4 moles of lithium sulfate ion: from 0.25 to 5 moles of the one or more reducing agent.
- the preferred ratio of starting materials, that is transition metal sulfide: number of mole equivalents of lithium supplied by sulfate: number of moles of one or more reducing agent is 1:0.5-1.5:0.5-4, further preferably 1:0.5-1:0.5-3.
- the most preferred ratio of reactants that is, transition metal sulfide: number of mole equivalents of lithium supplied by the lithium sulfate: carbon, is 1:1:2.
- the carbon used may be in any suitable form, for example, graphite, charcoal and carbon black, although it is preferred to use high surface area carbons that are typically used in electrode formulations, for example Super P, Denka Black, Ensaco etc.
- An alternative source of carbon may be derived in situ from any suitable carbonaceous material, for example by the thermal decomposition of an organic material such as lithium acetate, dextrin, starch, flour cellulosic substance or sucrose or a polymeric material such as polyethylene, polyethylene glycol, polyethylene oxide, and ethylene propylene rubber.
- an organic material such as lithium acetate, dextrin, starch, flour cellulosic substance or sucrose
- a polymeric material such as polyethylene, polyethylene glycol, polyethylene oxide, and ethylene propylene rubber.
- most carbon containing materials may be used, provided their thermal decomposition does not involve the production of detrimental by-products.
- the target lithium-containing transition metal sulfide compound produced by the first aspect of the present invention has a formula in the range Li 1.5-2.0 FeS 2 , however, the reaction temperature and duration of the heating step, for example, will determine the precise reaction product formulation.
- a flux agent also known as a mineraliser
- a flux agent also known as a mineraliser
- Flux agents or mineralisers are commonly used in the ceramics industry to lower the reaction temperature and shorten reaction times.
- Mineralisers such as sodium chloride, borax, lithium chloride, lithium fluoride, sodium fluoride, lithium borate and sodium carbonate are known.
- the present applicant has found that using a very small amount of a mineraliser, in particular an alkali metal halide will result in a lithium-containing transition metal sulfide product that exhibits enhanced crystalinity with lower levels of impurities.
- amount of mineraliser used in the present invention is up to 5% by weight of the starting materials, preferably from 0.5 to 2% by weight and further preferably 1% by weight of the starting materials.
- a typical electrode comprises 94% of a lithium-containing material, 3% of a binder and 3% of a carbon-containing material.
- the lithium-containing material is preferably a lithium-containing transition metal sulfide and further preferably one that is made by the method of the present invention described above.
- the binder can be any material known in the art to be suitable for use as a binder, usually a highly inert polymer such as polytetrafluoroethylene (PTFE), polymers of ethylene propylene diamine monomer (EPDM), polyethylene oxide (PEO), polyacrylonitrile and polyvinylidene fluoride.
- PTFE polytetrafluoroethylene
- EPDM ethylene propylene diamine monomer
- PEO polyethylene oxide
- polyacrylonitrile polyvinylidene fluoride
- the Applicant's preferred binder is ethylene propylene diene monomer (EPDM).
- the key feature of the binder is that it needs to be able to form a slurry or paste with the lithium-containing transition metal sulfide, which in turn may be coated onto a current collector.
- mixing the binder with a solvent facilitates coating. Any solvent may be used, provided it is non polar and does not react with either the binder or the lithium-containing transition metal sulfide, and also provided it is dry. Desirably the solvent is reasonably volatile to facilitate its removal at room temperature.
- Suitable solvents might include low molecular weight halogenated compounds, particularly halogenated hydrocarbons such as methylene chloride or low molecular weight materials such as cyclohexane, trimethylbenzene (TMB), toluene, and xylene, or low molecular weight alcohols such as methanol, and mixtures of any of these compounds. Trimethylbenzene is a preferred solvent.
- the binder/solvent/lithium-containing transition metal sulfide slurry/paste may also include additives adapted to modify the properties of the binder.
- the chosen additive must be naturally compatible with the binder, the lithium-containing transition metal sulfide and the electrolyte, and must not affect the performance of the finished cell.
- the lithium-containing transition metal sulfide materials produced by the method of the present invention are useful in a wide variety of applications where a low voltage rechargeable battery power source may be used, for example, in mobile phones, vehicles, lap top computers, computer games, cameras, personal CD and DVD players, drills, screw drivers and flash lights and other hand-held tools and appliances.
- an electrochemical cell comprising a plurality of anode plates and a plurality of cathode plates, each comprising respective insertion materials for example graphite in the anode plates and the lithium-containing transition metal sulfides of the present invention in the cathode plates.
- the method involves forming a stack of discrete, separate cathode plates and discrete, separate anode plates stacked alternately, each comprising a layer of a respective ion insertion material bonded to a metal current collector, and interleaving a continuous separator/electrolyte layer between successive plates so it forms a zig zag.
- FIG. 1 shows the overall reaction scheme for the process of the present invention when carbon is used to provide the reducing conditions.
- the reaction proceeds by the reduction of lithium sulfate to lithium sulfide followed by the reaction of the latter with the transition metal sulfide to produce the target lithium-containing transition metal sulfide.
- FIG. 2 shows powder x-ray diffraction patterns for compounds with the formula Li 2-x-y A y Fe 1-z M z S 2 made according to Examples 1 to 3 of the present invention.
- FIG. 3 shows 1 st cycle data for Li 2-x-y A y Fe 1-z M z S 2 compounds made according to Examples 1 to 3 of the present invention.
- FIG. 4 shows further cycle data for Li 2-x-y A y Fe 1-z M z S 2 compounds made according to Examples 1 to 3 of the present invention.
- the lithium sulfate, transition metal sulfide and reducing agent are weighed out into a ball mill pot, this mixture is milled for 1-12 hrs depending on the size of the precursor mix at a rate of 200-350 rpm.
- the precursor mix is then pelletised, and placed into a glassy carbon crucible with or without a lid.
- the carbon crucible is placed into the furnace under a gentle flow of an inert gas, and heated between 500 and 1500° C. at a rate of 1 to 10° C. per minute over a period of 1 to 24 hours.
- the crucible is allowed to cool under the inert gas flow and transferred directly into a glove box.
- a suitable furnace for carrying out the above process may be a graphite lined rotary furnace, a retort furnace or a static tube furnace.
- the lithium sulfate and transition metal sulfide are weighed out into a ball mill pot, this mixture is milled for 1-12 hrs depending on the size of the precursor mix at a rate of 200-350 rpm.
- the precursor mix is then pelletised, and placed into a glassy carbon crucible.
- the carbon crucible is placed into the furnace under a gentle flow of a reducing gas, and heated between 500 and 800° C. for 1 -20 hours dwell.
- the crucible is allowed to cool under the inert gas flow and transferred directly into a glove box and processed and analysed as described above.
- Example sulfate sulfide conditions Mineraliser Temp/Time 1 Li 2 SO 4 FeS Carbon None 800° C./9 hr (110 g; 1.0 mole) (87.91; Denka Black under argon 1.0 mole) (24 g; in small tube 2.0 moles) furnace 2 Li 2 SO 4 FeS Carbon LiCl 800° C./9 hr (110 g; 1.0 mole) (87.91 g; Denka Black (1.3 g; 1 wt %) under argon 1.0 mole) (24 g; in small tube 2.0 moles) furnace 3 Li 2 SO 4 FeS Carbon LiCl 800° C./9 hr (110 g; 1.0 mole) (87.91 g; Denka Black (2.6 g; 2 wt %) under argon 1.0 mole) (24 g; in small tube 2.0 moles) furnace
- Composite cathode electrodes were made by coating a composite comprising 6% carbon black, 1% EPDM and 93% active material onto an aluminium current collector from which discs were cut.
- a cell stack was constructed by placing a glass filter paper separator between a lithium anode disk and a composite cathode disk then made into a small pouch type cell. Tags of aluminium one side and nickel on the opposing side were sealed into the sides of a pouch. Electrolyte was pipetted onto the separator and the end of the pouch was then vacuum sealed. Constant current tests were performed on a MACCOR between the voltage limits 2.65V and 1.45V using an initial rate of 10 mAg ⁇ 1 , (e.g. as shown in FIG. 3 ) followed by a rate of 15 mAg ⁇ 1 for subsequent cycles (e.g. as shown in FIG. 4 ).
- Powder X-ray diffraction data was obtained using a SIEMANS D5000 using a copper K ⁇ 1 and K ⁇ 2 source, fitted with a monochromator. The sample was placed into an air sensitive holder, which consisted of a Perspex dome which was sealed over the sample, thus preventing degradation of the material during data collection. Phase analysis data were collected over a period of 4 hours 10-80° 2 theta, whilst high quality data were collected 10-90° 2 theta over a period of 16 hours.
- Cells were made using the general method described above and were cycled vs lithium between the voltage ranges 2.65V and 1.45V.
- the first cycle was performed at a rate of 10 mAg ⁇ 1 (see FIG. 3 )
- subsequent cycles were performed at a charge rate of 15 mAg ⁇ 1 (see FIG. 4 ) and a discharge rate of 75 mAg ⁇ 1 .
- Initial charge capacity of 320 mAhg ⁇ 1 were observed and a discharge capacity approximately 350 mAhg ⁇ 1
- All 1 st cycles were similar, however the samples made with no mineraliser exhibited slightly higher discharge capacities than that made with mineraliser addition.
- the Li 2-x FeS 2 compound made according to Example 2 includes 1%/wt LiCl mineraliser in its formulation.
- the effect of this mineraliser on the capacity of Li 2-x FeS 2 is indicated by the 1 st cycle data shown in FIG. 2 , and the cycling data shown in FIG. 3 .
- the cycling data shows that the discharge capacities obtained at 10 mAg-1 are slightly high for the sample with no mineraliser, however upon cycling the capacity of this material fades rapidly compared to that with 1% mineraliser. After 40 cycles the material with no mineraliser shows a 17% drop in capacity, whereas the sample made with mineraliser shows only an 8% drop in capacity.
Abstract
The present invention provides a convenient process for making lithium-containing transition metal sulfides involving heating at least one transition metal sulfide with lithium sulfate or any material that is a precursor for lithium sulfate, under reducing reaction conditions, wherein the oxidation state of the transition metal is not reduced during the reaction process.
Description
- This application is a United States national phase application under 35 U.S.C. §371 of International Patent Application No. PCT/GB2009/051314 filed on Oct. 6, 2009, and claims the benefit of Great Britain Patent Application No. 0818758.5 filed on Oct. 14, 2008 and Great Britain Patent Application No. 0906601.0 filed on Apr. 17, 2009, all of which are herein incorporated in their entirety by reference. The International Application was published as International Publication No. WO 2010/043886 on Apr. 22, 2010.
- The present invention relates to lithium-containing transition metal sulfide compounds, a method of manufacturing lithium-containing transition metal sulfide compounds, the use of lithium-containing transition metal sulfide compounds in electrode materials in the manufacture of lithium ion cells or batteries and the use of such cells or batteries in commercial products.
- Lithium ion batteries are secondary batteries that comprise an anode (negative electrode), a cathode (positive electrode) and an electrolyte material. They operate by the transfer of lithium ions between the anode and the cathode, and they are not to be confused with lithium batteries, which are characterised by containing metallic lithium. Lithium ion batteries are currently the most commonly used type of rechargeable battery and typically the anode comprises an insertion material, for example carbon in the form of coke or graphite. An electroactive couple is formed using a cathode that comprises a lithium-containing insertion material. Typical lithium-containing insertion materials are lithium cobalt oxide (LiCoO2), lithium nickel oxide (LiNiO2) and lithium manganese oxide (LiMn2O4). In its initial condition, this type of cell is uncharged, therefore to deliver electrochemical energy the cell must be charged to transfer lithium to the anode from the lithium-containing cathode. Upon discharge, the lithium ions are transferred from the anode back to the cathode. Subsequent charging and discharging operations transfers the lithium ions back and forth between the cathode and the anode over the life of the battery. A review of the recent developments and likely advantages of lithium rechargeable batteries is provided by Tsutomu Ohzuku and Ralph Brodd in Journal of Power Sources 2007.06.154.
- Unfortunately, lithium cobalt oxide is a relatively expensive material and the nickel compounds are difficult to synthesize. Not only that, cathodes made from lithium cobalt oxide and lithium nickel oxide suffer from the disadvantage that the actual charge capacity of a cell is significantly less than its theoretical capacity. The reason for this is that less than 1 atomic unit of lithium engages in the electrochemical reaction. Moreover, the initial capacity is reduced during the initial charging operation and still further reduced during each charging cycle. Prior art U.S. Pat. No. 4,828,834 attempts to control capacity loss through the use of a cathode mainly composed of LiMn2O4. U.S. Pat. No. 5,910,382 on the other hand, describes another approach using lithium-mixed metal materials such as LiMPO4 where M is at least one first row transition metal. Preferred compounds include LiFePO4, LiMnPO4, LiCoPO4, and LiNiPO4 and mixed transition metal compounds such as Li1-2xFe1-xCoxPO4 or Li1-2xFe1-xMnxPO4 where 0<x<1.
- The use of lithium ion rechargeable batteries is limited by the prohibitive cost of providing the lithium electrode material, particularly in the case of lithium cobalt oxide. Consequently, current commercialisation is restricted to premium applications such as portable computers and mobile telephones. However, it would be highly desirable to gain access to wider markets, for example the powering of electric vehicles and work has been ongoing in recent years to produce materials that maintain the high performance of lithium ion batteries, but which at the same time, are much cheaper to produce. To achieve this goal, it has been suggested, for example in JP Kokai No 10208782 and Solid State Ionics 117 (1999) 273-276), that sulfides may be used in place of oxides, as cathode materials. Although the use of many sulfides achieves less voltage, measured against lithium of the corresponding oxides, the capacity of some sulfide-based cathodes, measured in milliampere hours per gram, can be as much as about 3 times greater. Based on this, some sulfide-based cathodes achieve an overall advantage of about 1.5 times in terms of cathode energy density for batteries measured against a lithium metal anode, as compared against their oxide counterparts, and this makes the use of these sulfides a very attractive proposition. For example, in the case of lithium iron sulfide a theoretical capacity of 400 mAhg−1 may be obtained with an average operating voltage of 2.2V versus a lithium metal anode.
- Thus, lithium-containing transition metal sulfides will be a convenient substitute material for the lithium metal oxides described above, with lithium iron sulfide being already described in the patent literature, for example in U.S. Pat. No. 7,018,603, to be a useful cathode material in secondary cells. The commercialisation of lithium-containing transition metal sulfides will depend largely on their cost of production. Taking lithium iron sulfide as a specific example, the conventional process for making this material is via a solid state reaction in which lithium sulfide (Li2S) and ferrous sulfide (FeS), are intimately mixed together and heated under an inert atmosphere at a temperature of about 800° C. The starting materials ferrous sulfide (FeS) and iron disulfide (FeS2) are relatively inexpensive as they are found as naturally occurring materials, and are dug out of the ground. However, a notable disadvantage of the reaction process is that the other starting material, Li2S, is not only expensive but also highly moisture sensitive. The latter problem in particular has obvious implications for the complexity, and therefore the cost, of storing and handling the starting material, especially for large-scale commercial production. In addition, the kinetics of this reaction are reported in U.S. Pat. No. 7,018,603 to be very slow and it can apparently take up to one month to complete the reaction, thus this route is believed to be highly unfavourable in terms of energy costs and not commercially viable for the production of electrode materials.
- As an alternative route for making lithium-containing transition metal sulfides, U.S. Pat. No. 7,018,603 discloses reacting a transition metal sulfide such as FeS with lithium sulfide in a reaction medium comprising molten salt or a mixture of molten salts at high temperature (temperatures of 450° C. to 700° C. are exemplified). The preferred molten salts are lithium halides. Whilst this reaction proceeds at a good rate there are still several issues that make it less than ideal. Firstly, the fact it uses Li2S as a starting material leads to the handling and storage problems described above. Secondly, it is very difficult to separate the reaction medium (molten lithium halide used in 1.5 molar excess) from the desired reaction product other then by solvent extraction, and this type of extraction is expensive. Further, even after rigorous purification as much as 8% of the reaction medium salt is still present in the reaction product, and this level of impurity is detrimental to the charge capacity per gram of lithium iron sulfide.
- The authors of U.S. Pat. No. 7,018,603 also describe that the lithium sulfide used their molten salt process may be prepared via the reduction of lithium sulfate, for example by heating it to above 860° C. in the presence of carbon, and they suggest that this is more convenient for the large scale production of lithium iron sulfide, than buying lithium sulfide commercially. However, the handling, storage, and purification difficulties encountered with their molten salt method, as highlighted above, remain a problem.
- Given the difficulties associated with the above synthetic routes to make lithium transition metal sulfides, it is highly desirable to find further alternative routes which rely on inexpensive and non-moisture sensitive starting materials, and which involve a simple, energy efficient reaction method to produce a clean product.
- Thus, in the first aspect of the above invention there is provided a method of producing a lithium-containing transition metal sulfide characterised in that it comprises heating at least one transition metal sulfide with lithium sulfate, or any material that is a precursor for lithium sulfate, under reducing conditions, wherein the oxidation state of the transition metal is not reduced during the reaction process. The reducing conditions preferably comprise a reducing agent such as carbon and/or performing the reaction process in a reducing atmosphere. Further preferably the transition metal sulfide made by the above method is of the formula Li2-x-y Ay Fe1-z MzS2 where x=0 to 1.5, preferably x=0 to 1, further preferably x=0 to 0.5 and particularly preferably x=0 to 0.3. Preferably, y=0 to 1; z=0 to 1, A is selected from one or more of silver (Ag), sodium (Na), copper (Cu(I)) and potassium (K) and M is a generic representation for one or more transition metals.
- The reducing conditions used in the method of the present invention may be any well-known and used in the art of chemical reduction. Preferred examples involve one or more reducing gases, such as carbon monoxide, hydrogen, reforming gas (mixture of hydrogen and nitrogen), hydrogen sulfide, methane and other gaseous alkanes. One or more reducing agents such as carbon may also be used either alone or in combination with a reducing gas. In the present invention, it is highly preferred that the reducing conditions do not reduce the oxidation state of the transition metal ion.
- The ideal reaction temperature used in the present invention is that which is sufficient to cause the lithium sulfate to be reduced to lithium sulfide and for this intermediate to react with the transition metal sulfide. If the reaction temperature is too high, the level and number of impurities, caused for example by the over-reduction of the transition metal ion to the zero oxidation or metallic state, is found to increase. The actual temperature used, therefore, will depend on the chosen transition metal sulfide. As a general rule the reaction temperature is conveniently from 650 to 950° C., and preferably from 750 to 850° C. It is observed that the yield of target material does not significantly increase when the reaction temperature is above 860° C. (the decomposition temperature of lithium sulfate. The reaction time varies according to reaction temperature and as one might expect, the higher the temperature, the faster the reaction. By way of example, a suitable reaction temperature/time profile that will produce the desired lithium-containing transition metal sulfide includes heating the reaction mixture for 12 hours at 750° C. Alternatively one could heat the reaction mixture for 9 hours at 800° C. The at least one transition metal sulfide used in the method of the present invention may be one or more sulfide compounds comprising one or more transition metals. This includes the use of single and/or mixtures of several transition metals in the sulfide. Preferably the reaction method uses mono-sulfides. Particularly suitable transition metals comprise one or more of manganese, iron, cobalt, nickel copper and zinc. Preferably, the transition metals are selected from magnesium, calcium, manganese, iron, cobalt and nickel. Particularly preferably the transition metals have an initial oxidation state of +2. Sulfides that comprise iron are the most preferred transition metal sulfides.
- Although the starting materials are not air or moisture sensitive, and these positive attributes aid the storage and handling of these materials, the reaction product is itself reactive towards water. Therefore, it is advantageous to form and handle the lithium-containing transition metal sulfides under a dry and inert atmosphere such as argon or nitrogen.
- Suitable reaction vessels comprise glassy carbon or graphite crucibles that generally have a loose fitting lid, however, a sealed pressurized vessel may also be used. For commercial scale production, it is advantageous to use a continuous process, for example, a rotary tube furnace, although a retort batch process may also be used.
- The reaction of the present invention is a solid-state in situ process and this means that all reactants are in solid form and are without the need to use a reaction medium such as a solvent. Thus, the present reaction process is notably distinct from the process described in U.S. Pat. No. 7,018,603, for example the present invention uses lithium sulfate directly as a starting material and moreover, it does not involve a solvent comprising a molten salt or mixture of molten salts. The reactants are solid materials that are first ground using a ball mill to produce a fine powder that can either be used directly or first pressed into a pellet.
- In the present invention, it is highly desirable that the reducing conditions in the process do not directly reduce the oxidation state of the transition metal ion. When carbon is used as a reducing agent, any amount of it may be used but it is convenient not to use too much to prevent it becoming a significant impurity in the reaction product, and thereby lowering its specific capacity. Having said this, it has been found to be of significant advantage, particularly to the conductivity of the target material, for at least a small amount of carbon to be present in the reaction product. Moreover, there are further specific advantages to be gained in the carbon being residual from the use of carbon in the present invention, as opposed to it merely being added later to a sample of the target lithium-containing transition metal sulfide material; during the process, the carbon is considerably intimately mixed with the lithium-containing transition metal sulfide product. The degree of mixing described as “intimate” refers specifically to the chemical as opposed to physical mixing that is achieved when carbon is used, at least in part, to provide the reducing conditions in the process of the present invention. This “intimate” mixing is quite different from the degree of mixing that would ever be achieved using ball milling or other physical mixing apparatus. In particular, the carbon is dispersed at the microscopic level on individual particles of the lithium-containing transition metal sulfide.
- The ratio of reaction starting materials is typically 1 mole of transition metal sulfide: the equivalent of from 0.5 to 4 moles of lithium sulfate ion: from 0.25 to 5 moles of the one or more reducing agent. The preferred ratio of starting materials, that is transition metal sulfide: number of mole equivalents of lithium supplied by sulfate: number of moles of one or more reducing agent, is 1:0.5-1.5:0.5-4, further preferably 1:0.5-1:0.5-3. In the case where carbon is used as the reducing agent, the most preferred ratio of reactants, that is, transition metal sulfide: number of mole equivalents of lithium supplied by the lithium sulfate: carbon, is 1:1:2.
- As a general rule, lower amounts of carbon are required when a reducing gas and/or another reducing agent is also used.
- When present, the carbon used may be in any suitable form, for example, graphite, charcoal and carbon black, although it is preferred to use high surface area carbons that are typically used in electrode formulations, for example Super P, Denka Black, Ensaco etc.
- An alternative source of carbon may be derived in situ from any suitable carbonaceous material, for example by the thermal decomposition of an organic material such as lithium acetate, dextrin, starch, flour cellulosic substance or sucrose or a polymeric material such as polyethylene, polyethylene glycol, polyethylene oxide, and ethylene propylene rubber. In fact, most carbon containing materials may be used, provided their thermal decomposition does not involve the production of detrimental by-products.
- The target lithium-containing transition metal sulfide compound produced by the first aspect of the present invention has a formula in the range Li1.5-2.0FeS2, however, the reaction temperature and duration of the heating step, for example, will determine the precise reaction product formulation.
- Although not critical to the performance of the present invention, the applicants have found it is possible reduce the quantity of impurities formed and to optimise the reaction conditions, by the addition of a flux agent, also known as a mineraliser, to the reaction mixture. Flux agents or mineralisers are commonly used in the ceramics industry to lower the reaction temperature and shorten reaction times. Mineralisers such as sodium chloride, borax, lithium chloride, lithium fluoride, sodium fluoride, lithium borate and sodium carbonate are known. The present applicant has found that using a very small amount of a mineraliser, in particular an alkali metal halide will result in a lithium-containing transition metal sulfide product that exhibits enhanced crystalinity with lower levels of impurities. Any alkali metal halide may be used but lithium chloride and lithium iodide are most preferred. Alternatively, sodium carbonate or sodium chloride may be used however in this case it is likely that at least some substitution of the lithium for sodium will occur in the target product. Thus, amount of mineraliser used in the present invention is up to 5% by weight of the starting materials, preferably from 0.5 to 2% by weight and further preferably 1% by weight of the starting materials.
- A typical electrode comprises 94% of a lithium-containing material, 3% of a binder and 3% of a carbon-containing material. In this aspect of the present invention the lithium-containing material is preferably a lithium-containing transition metal sulfide and further preferably one that is made by the method of the present invention described above. The binder can be any material known in the art to be suitable for use as a binder, usually a highly inert polymer such as polytetrafluoroethylene (PTFE), polymers of ethylene propylene diamine monomer (EPDM), polyethylene oxide (PEO), polyacrylonitrile and polyvinylidene fluoride. The Applicant's preferred binder is ethylene propylene diene monomer (EPDM). The key feature of the binder is that it needs to be able to form a slurry or paste with the lithium-containing transition metal sulfide, which in turn may be coated onto a current collector. Conveniently, mixing the binder with a solvent facilitates coating. Any solvent may be used, provided it is non polar and does not react with either the binder or the lithium-containing transition metal sulfide, and also provided it is dry. Desirably the solvent is reasonably volatile to facilitate its removal at room temperature. Suitable solvents might include low molecular weight halogenated compounds, particularly halogenated hydrocarbons such as methylene chloride or low molecular weight materials such as cyclohexane, trimethylbenzene (TMB), toluene, and xylene, or low molecular weight alcohols such as methanol, and mixtures of any of these compounds. Trimethylbenzene is a preferred solvent.
- The binder/solvent/lithium-containing transition metal sulfide slurry/paste may also include additives adapted to modify the properties of the binder. The chosen additive must be naturally compatible with the binder, the lithium-containing transition metal sulfide and the electrolyte, and must not affect the performance of the finished cell.
- The lithium-containing transition metal sulfide materials produced by the method of the present invention are useful in a wide variety of applications where a low voltage rechargeable battery power source may be used, for example, in mobile phones, vehicles, lap top computers, computer games, cameras, personal CD and DVD players, drills, screw drivers and flash lights and other hand-held tools and appliances.
- In order for the lithium-containing transition metal sulfides of the present invention to be used in such applications it is necessary to construct them into an electrochemical cell. Different methods of making such cells are described in the literature, but one particularly convenient example is described in
EP 1 295 355 B1. In this case, an electrochemical cell is assembled comprising a plurality of anode plates and a plurality of cathode plates, each comprising respective insertion materials for example graphite in the anode plates and the lithium-containing transition metal sulfides of the present invention in the cathode plates. In particular, the method involves forming a stack of discrete, separate cathode plates and discrete, separate anode plates stacked alternately, each comprising a layer of a respective ion insertion material bonded to a metal current collector, and interleaving a continuous separator/electrolyte layer between successive plates so it forms a zig zag. - The invention will now be particularly described by way of example with reference to the following drawings in which:
-
FIG. 1 shows the overall reaction scheme for the process of the present invention when carbon is used to provide the reducing conditions. In this case, the reaction proceeds by the reduction of lithium sulfate to lithium sulfide followed by the reaction of the latter with the transition metal sulfide to produce the target lithium-containing transition metal sulfide. -
FIG. 2 shows powder x-ray diffraction patterns for compounds with the formula Li2-x-yAyFe1-zMzS2 made according to Examples 1 to 3 of the present invention. -
FIG. 3 shows 1st cycle data for Li2-x-yAyFe1-zMzS2 compounds made according to Examples 1 to 3 of the present invention. -
FIG. 4 shows further cycle data for Li2-x-yAyFe1-zMzS2 compounds made according to Examples 1 to 3 of the present invention. - The lithium sulfate, transition metal sulfide and reducing agent are weighed out into a ball mill pot, this mixture is milled for 1-12 hrs depending on the size of the precursor mix at a rate of 200-350 rpm. The precursor mix is then pelletised, and placed into a glassy carbon crucible with or without a lid. The carbon crucible is placed into the furnace under a gentle flow of an inert gas, and heated between 500 and 1500° C. at a rate of 1 to 10° C. per minute over a period of 1 to 24 hours. The crucible is allowed to cool under the inert gas flow and transferred directly into a glove box. The resulting product is ground initially using a pestle and mortar and then milled more finely using a ball mill. The lithium-containing transition metal sulfide product may then be analysed using X-ray diffraction and/or electrochemical techniques. A suitable furnace for carrying out the above process may be a graphite lined rotary furnace, a retort furnace or a static tube furnace.
- The lithium sulfate and transition metal sulfide are weighed out into a ball mill pot, this mixture is milled for 1-12 hrs depending on the size of the precursor mix at a rate of 200-350 rpm. The precursor mix is then pelletised, and placed into a glassy carbon crucible. The carbon crucible is placed into the furnace under a gentle flow of a reducing gas, and heated between 500 and 800° C. for 1 -20 hours dwell. The crucible is allowed to cool under the inert gas flow and transferred directly into a glove box and processed and analysed as described above.
- Compounds with the Formula Li2-x-yAyFe1-zMzS2 (x, y and z are as defined above) were prepared according to Examples 1 to 3 summarised in Table 1 below:
-
TABLE 1 Transition Reaction Lithium metal Reducing conditions Example sulfate sulfide conditions Mineraliser Temp/ Time 1 Li2SO4 FeS Carbon None 800° C./9 hr (110 g; 1.0 mole) (87.91; Denka Black under argon 1.0 mole) (24 g; in small tube 2.0 moles) furnace 2 Li2SO4 FeS Carbon LiCl 800° C./9 hr (110 g; 1.0 mole) (87.91 g; Denka Black (1.3 g; 1 wt %) under argon 1.0 mole) (24 g; in small tube 2.0 moles) furnace 3 Li2SO4 FeS Carbon LiCl 800° C./9 hr (110 g; 1.0 mole) (87.91 g; Denka Black (2.6 g; 2 wt %) under argon 1.0 mole) (24 g; in small tube 2.0 moles) furnace - General Procedure To Obtain Cycle Data For the Li2-x-yA-yFe1-zMzS2 Compounds Made According To the Present Invention
- Composite cathode electrodes were made by coating a composite comprising 6% carbon black, 1% EPDM and 93% active material onto an aluminium current collector from which discs were cut. A cell stack was constructed by placing a glass filter paper separator between a lithium anode disk and a composite cathode disk then made into a small pouch type cell. Tags of aluminium one side and nickel on the opposing side were sealed into the sides of a pouch. Electrolyte was pipetted onto the separator and the end of the pouch was then vacuum sealed. Constant current tests were performed on a MACCOR between the voltage limits 2.65V and 1.45V using an initial rate of 10 mAg−1, (e.g. as shown in
FIG. 3 ) followed by a rate of 15 mAg−1for subsequent cycles (e.g. as shown inFIG. 4 ). - Powder X-ray diffraction data was obtained using a SIEMANS D5000 using a copper Kα1 and Kα2 source, fitted with a monochromator. The sample was placed into an air sensitive holder, which consisted of a Perspex dome which was sealed over the sample, thus preventing degradation of the material during data collection. Phase analysis data were collected over a period of 4 hours 10-80° 2 theta, whilst high quality data were collected 10-90° 2 theta over a period of 16 hours.
- Cells were made using the general method described above and were cycled vs lithium between the voltage ranges 2.65V and 1.45V. The first cycle was performed at a rate of 10 mAg−1 (see
FIG. 3 ), subsequent cycles were performed at a charge rate of 15 mAg−1 (seeFIG. 4 ) and a discharge rate of 75 mAg−1. Initial charge capacity of 320 mAhg−1 were observed and a discharge capacity approximately 350 mAhg−1, All 1st cycles were similar, however the samples made with no mineraliser exhibited slightly higher discharge capacities than that made with mineraliser addition. - Investigation of the Effect of Adding 1%/wt Mineraliser During the Preparation of Li2-xFeS2
- The Li2-xFeS2 compound made according to Example 2 includes 1%/wt LiCl mineraliser in its formulation. The effect of this mineraliser on the capacity of Li2-xFeS2 is indicated by the 1st cycle data shown in
FIG. 2 , and the cycling data shown inFIG. 3 . The cycling data shows that the discharge capacities obtained at 10 mAg-1 are slightly high for the sample with no mineraliser, however upon cycling the capacity of this material fades rapidly compared to that with 1% mineraliser. After 40 cycles the material with no mineraliser shows a 17% drop in capacity, whereas the sample made with mineraliser shows only an 8% drop in capacity.
Claims (20)
1. A method of producing a lithium-containing transition metal sulfide, characterised in that it comprises heating at least one transition metal sulfide with lithium sulfate, or any material that is a precursor for lithium sulfate, under reducing reaction conditions, wherein the oxidation state of the transition metal is not reduced during the reaction process.
2. A method of producing a lithium-containing transition metal sulfide, characterised in that it comprises heating at least one transition metal sulfide with lithium sulfate, or any material that is a precursor for lithium sulfate, in the presence of carbon, wherein the oxidation state of the transition metal is not reduced during the reaction process.
3. A method of producing a lithium-containing transition metal sulfide according to claim 1 or 2 wherein the lithium-containing transition metal sulfide is of the formula Li2-x-yAy Fe1-zMzS2 where x=0 to 1.5, y=0 to 1, z=0 to 1, A is selected from one or more of silver (Ag), sodium (Na), copper (Cu(I)) and potassium (K) and M is a generic representation for one or more transition metals.
4. A method of producing a lithium-containing transition metal sulfide according to claim 1 , 2 or 3 wherein the at least one transition metal sulfide and lithium sulfate, or precursor therefor, are heated at a temperature of from 650° C. to 950° C.
5. A method of producing a lithium-containing transition metal sulfide according to claims 1 to 4 wherein the at least one transition metal sulfide comprises one or more of magnesium, calcium, manganese, iron, cobalt, nickel, copper and zinc.
6. A method of producing a lithium-containing transition metal sulfide according to claim 5 wherein the at least one transition metal sulfide comprises one or more of manganese, iron, cobalt and nickel.
7. A method of producing a lithium-containing transition metal sulfide according to any preceding claim wherein the at least one transition metal sulfide comprises one or more monosulfide.
8. A method of producing a lithium-containing transition metal sulfide according to any preceding claim, wherein the molar ratio of transition metal sulfide:lithium sulfate, or precursor thereof, one or more reducing agent is 1:0.5 to 4:0.25 to 5.
9. A method of producing a lithium transition metal sulfide according to any preceding claim, wherein the molar ratio of transition metal sulfide:lithium sulfate, or precursor thereof, carbon is 1:1:2.
10. A method of producing a lithium-containing transition metal sulfide according to any preceding claim, wherein the at least one transition metal sulfide and the lithium sulfate, or precursor thereof, are in powder form and/or pellet form.
11. A method according to any of claims 1 to 10 , further comprising the addition of one or more mineralisers in a total amount of up to 5% by weight of the starting materials.
12. A method of claim 11 wherein the one or more mineralisers comprise an alkali metal halide.
13. A method according to claim 12 wherein the one or more mineralisers comprise one or more of lithium iodide, lithium bromide and lithium chloride.
14. Use of the lithium-containing transition metal sulfide produced according to the method in any of claims 1 to 13 in the preparation of an electrode.
15. Use according to claim 14 wherein the electrode is a cathode.
16. An electrode made according to either of claim 14 or 15 further comprising a binder that is used in conjunction with a solvent to form a slurry or paste with the lithium-containing transition metal sulfide.
17. An electrode according to claim 16 wherein the solvent comprises a non-polar hydrocarbon solvent.
18. An electrode according to any of claims 14 to 17 used, in conjunction with a counter electrode and an electrolyte, in a lithium ion battery.
19. An electrode according to claim 18 used, in conjunction with a counter electrode and an electrolyte, in a rechargeable battery power source.
20. A lithium ion battery comprising a cathode comprising one or more lithium-containing transition metal sulfides produced according to the method of any of claims 1 to 13 .
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JP2015074567A (en) * | 2013-10-07 | 2015-04-20 | 古河機械金属株式会社 | Method for producing lithium sulfide |
WO2024064060A1 (en) * | 2022-09-19 | 2024-03-28 | California Institute Of Technology | LITHIUM-RICH ALUMINUM IRON SULFIDE Li-ION BATTERY CATHODES |
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