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lang="ca" hreflang="ca" data-title="Bateria de liti-sofre" data-language-autonym="Català" data-language-local-name="Catalan" class="interlanguage-link-target">Català</a></li><li class="interlanguage-link interwiki-de mw-list-item"><a href="https://de.wikipedia.org/wiki/Lithium-Schwefel-Akkumulator" title="Lithium-Schwefel-Akkumulator – German" lang="de" hreflang="de" data-title="Lithium-Schwefel-Akkumulator" data-language-autonym="Deutsch" data-language-local-name="German" class="interlanguage-link-target">Deutsch</a></li><li class="interlanguage-link interwiki-el mw-list-item"><a href="https://el.wikipedia.org/wiki/%CE%9C%CF%80%CE%B1%CF%84%CE%B1%CF%81%CE%AF%CE%B1_%CE%BB%CE%B9%CE%B8%CE%AF%CE%BF%CF%85-%CE%B8%CE%B5%CE%AF%CE%BF%CF%85" title="Μπαταρία λιθίου-θείου – Greek" lang="el" hreflang="el" data-title="Μπαταρία λιθίου-θείου" data-language-autonym="Ελληνικά" data-language-local-name="Greek" class="interlanguage-link-target">Ελληνικά</a></li><li class="interlanguage-link interwiki-es mw-list-item"><a href="https://es.wikipedia.org/wiki/Bater%C3%ADa_de_litio-sulfuro" title="Batería de litio-sulfuro – Spanish" lang="es" hreflang="es" data-title="Batería de litio-sulfuro" data-language-autonym="Español" data-language-local-name="Spanish" class="interlanguage-link-target">Español</a></li><li class="interlanguage-link interwiki-fa mw-list-item"><a href="https://fa.wikipedia.org/wiki/%D8%A8%D8%A7%D8%AA%D8%B1%DB%8C_%D9%84%DB%8C%D8%AA%DB%8C%D9%85%E2%80%93%DA%AF%D9%88%DA%AF%D8%B1%D8%AF" title="باتری لیتیم–گوگرد – Persian" lang="fa" hreflang="fa" data-title="باتری لیتیم–گوگرد" data-language-autonym="فارسی" data-language-local-name="Persian" class="interlanguage-link-target">فارسی</a></li><li class="interlanguage-link interwiki-fr mw-list-item"><a href="https://fr.wikipedia.org/wiki/Accumulateur_lithium-soufre" title="Accumulateur lithium-soufre – French" lang="fr" hreflang="fr" data-title="Accumulateur lithium-soufre" data-language-autonym="Français" data-language-local-name="French" class="interlanguage-link-target">Français</a></li><li class="interlanguage-link interwiki-ko mw-list-item"><a href="https://ko.wikipedia.org/wiki/%EB%A6%AC%ED%8A%AC_%ED%99%A9_%EC%A0%84%EC%A7%80" title="리튬 황 전지 – Korean" lang="ko" hreflang="ko" data-title="리튬 황 전지" data-language-autonym="한국어" data-language-local-name="Korean" class="interlanguage-link-target">한국어</a></li><li class="interlanguage-link interwiki-hr mw-list-item"><a href="https://hr.wikipedia.org/wiki/Litij-sumporna_baterija" title="Litij-sumporna baterija – Croatian" lang="hr" hreflang="hr" data-title="Litij-sumporna baterija" data-language-autonym="Hrvatski" data-language-local-name="Croatian" class="interlanguage-link-target">Hrvatski</a></li><li class="interlanguage-link interwiki-it mw-list-item"><a href="https://it.wikipedia.org/wiki/Batteria_al_litio-zolfo" title="Batteria al litio-zolfo – Italian" lang="it" hreflang="it" data-title="Batteria al litio-zolfo" 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hreflang="pl" data-title="Akumulator litowo-siarkowy" data-language-autonym="Polski" data-language-local-name="Polish" class="interlanguage-link-target">Polski</a></li><li class="interlanguage-link interwiki-pt mw-list-item"><a href="https://pt.wikipedia.org/wiki/Bateria_de_l%C3%ADtio-enxofre" title="Bateria de lítio-enxofre – Portuguese" lang="pt" hreflang="pt" data-title="Bateria de lítio-enxofre" data-language-autonym="Português" data-language-local-name="Portuguese" class="interlanguage-link-target">Português</a></li><li class="interlanguage-link interwiki-ru mw-list-item"><a href="https://ru.wikipedia.org/wiki/%D0%9B%D0%B8%D1%82%D0%B8%D0%B9-%D1%81%D0%B5%D1%80%D0%BD%D1%8B%D0%B9_%D0%B0%D0%BA%D0%BA%D1%83%D0%BC%D1%83%D0%BB%D1%8F%D1%82%D0%BE%D1%80" title="Литий-серный аккумулятор – Russian" lang="ru" hreflang="ru" data-title="Литий-серный аккумулятор" data-language-autonym="Русский" data-language-local-name="Russian" class="interlanguage-link-target">Русский</a></li><li 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The present address (URL) is a <a href="/wiki/Help:Permanent_link" title="Help:Permanent link">permanent link</a> to this revision, which may differ significantly from the <a class="external text" href="https://en.wikipedia.org/wiki/Lithium%E2%80%93sulfur_battery">current revision</a>.<div id="revision-info-plain" style="display: none;">Revision as of 00:19, 3 January 2024 by <a href="/wiki/User:OAbot" class="mw-userlink" title="User:OAbot" data-mw-revid="1193278735"><bdi>OAbot</bdi></a> (<a href="/wiki/User_talk:OAbot" class="mw-usertoollinks-talk" title="User talk:OAbot">talk</a> | <a href="/wiki/Special:Contributions/OAbot" class="mw-usertoollinks-contribs" title="Special:Contributions/OAbot">contribs</a>) (<a href="/wiki/Wikipedia:OABOT" title="Wikipedia:OABOT">Open access bot</a>: hdl updated in citation with #oabot.)</div></div><div id="mw-revision-nav">(<a href="/w/index.php?title=Lithium%E2%80%93sulfur_battery&diff=prev&oldid=1193278735" title="Lithium–sulfur battery">diff</a>) <a href="/w/index.php?title=Lithium%E2%80%93sulfur_battery&direction=prev&oldid=1193278735" title="Lithium–sulfur battery">← Previous revision</a> | <a href="/wiki/Lithium%E2%80%93sulfur_battery" title="Lithium–sulfur battery">Latest revision</a> (<a href="/w/index.php?title=Lithium%E2%80%93sulfur_battery&diff=cur&oldid=1193278735" title="Lithium–sulfur battery">diff</a>) | <a href="/w/index.php?title=Lithium%E2%80%93sulfur_battery&direction=next&oldid=1193278735" title="Lithium–sulfur battery">Newer revision →</a> (<a href="/w/index.php?title=Lithium%E2%80%93sulfur_battery&diff=next&oldid=1193278735" title="Lithium–sulfur battery">diff</a>)</div></div></div></div></div> <div id="mw-content-text" class="mw-body-content"><div class="mw-content-ltr mw-parser-output" lang="en" dir="ltr"><div class="shortdescription nomobile noexcerpt noprint searchaux" style="display:none">Type of rechargeable battery</div> <style data-mw-deduplicate="TemplateStyles:r1257001546">.mw-parser-output .infobox-subbox{padding:0;border:none;margin:-3px;width:auto;min-width:100%;font-size:100%;clear:none;float:none;background-color:transparent}.mw-parser-output .infobox-3cols-child{margin:auto}.mw-parser-output .infobox .navbar{font-size:100%}@media screen{html.skin-theme-clientpref-night .mw-parser-output .infobox-full-data:not(.notheme)>div:not(.notheme)[style]{background:#1f1f23!important;color:#f8f9fa}}@media screen and (prefers-color-scheme:dark){html.skin-theme-clientpref-os .mw-parser-output .infobox-full-data:not(.notheme) div:not(.notheme){background:#1f1f23!important;color:#f8f9fa}}@media(min-width:640px){body.skin--responsive .mw-parser-output .infobox-table{display:table!important}body.skin--responsive .mw-parser-output .infobox-table>caption{display:table-caption!important}body.skin--responsive .mw-parser-output .infobox-table>tbody{display:table-row-group}body.skin--responsive .mw-parser-output .infobox-table tr{display:table-row!important}body.skin--responsive .mw-parser-output .infobox-table th,body.skin--responsive .mw-parser-output .infobox-table td{padding-left:inherit;padding-right:inherit}}</style><table class="infobox"><caption class="infobox-title">Lithium–sulfur battery</caption><tbody><tr><td colspan="2" class="infobox-image"><a href="/wiki/File:Li-S_battery_EN.png" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/6/69/Li-S_battery_EN.png/220px-Li-S_battery_EN.png" decoding="async" width="220" height="245" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/6/69/Li-S_battery_EN.png/330px-Li-S_battery_EN.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/6/69/Li-S_battery_EN.png/440px-Li-S_battery_EN.png 2x" data-file-width="697" data-file-height="777" /></a><div class="infobox-caption">Working principle of lithium-sulfur battery and "shuttle" effect</div></td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Specific_energy" title="Specific energy">Specific energy</a></th><td class="infobox-data">450 [Wh/kg]<a href="#cite_note-oxisapril2021-1">[1]</a></td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Energy_density" title="Energy density">Energy density</a></th><td class="infobox-data">550 [Wh/L]<a href="#cite_note-oxisapril2021-1">[1]</a></td></tr><tr><th scope="row" class="infobox-label">Charge/discharge efficiency</th><td class="infobox-data">C/5 nominal</td></tr><tr><th scope="row" class="infobox-label">Cycle durability</th><td class="infobox-data">disputed</td></tr><tr><th scope="row" class="infobox-label">Nominal cell voltage</th><td class="infobox-data">cell <a href="/wiki/Volt" title="Volt">voltage</a> varies nonlinearly in the range 2.5–1.7 V during discharge; batteries often packaged for 3 V</td></tr></tbody></table> The lithium–sulfur battery (Li–S battery) is a type of <a href="/wiki/Rechargeable_battery" title="Rechargeable battery">rechargeable battery</a>. It is notable for its high <a href="/wiki/Specific_energy" title="Specific energy">specific energy</a>.<a href="#cite_note-2">[2]</a> The low <a href="/wiki/Atomic_weight" class="mw-redirect" title="Atomic weight">atomic weight</a> of <a href="/wiki/Lithium" title="Lithium">lithium</a> and moderate atomic weight of <a href="/wiki/Sulfur" title="Sulfur">sulfur</a> means that Li–S batteries are relatively light (about the density of water). They were used on the longest and highest-altitude unmanned <a href="/wiki/Solar-powered" class="mw-redirect" title="Solar-powered">solar-powered</a> aeroplane flight (at the time) by <a href="/wiki/Airbus_Zephyr" title="Airbus Zephyr">Zephyr 6</a> in August 2008.<a href="#cite_note-3">[3]</a> Lithium–sulfur batteries may displace <a href="/wiki/Lithium-ion" class="mw-redirect" title="Lithium-ion">lithium-ion</a> cells because of their higher energy density and reduced cost. This is due to the use of <a href="/wiki/Sulfur" title="Sulfur">sulfur</a> instead of cobalt, a common element in <a href="/wiki/Lithium-ion_battery" title="Lithium-ion battery">lithium-ion batteries</a>.<a href="#cite_note-4">[4]</a> Li–S batteries offer specific energies on the order of 550 <a href="/wiki/Watt_hour" class="mw-redirect" title="Watt hour">Wh</a>/<a href="/wiki/Kilogram" title="Kilogram">kg</a>,<a href="#cite_note-oxisapril2021-1">[1]</a> while lithium-ion batteries are in the range of 150–260 Wh/kg.<a href="#cite_note-osti1561559-5">[5]</a> Li–S batteries with up to 1,500 charge and discharge cycles were demonstrated in 2017,<a href="#cite_note-6">[6]</a> but cycle life tests at commercial scale and with lean electrolyte have not been completed. As of early 2021, none were commercially available. Issues that have slowed acceptance include the polysulfide "shuttle" effect that is responsible for the progressive leakage of active material from the cathode, resulting in too few recharge cycles.<a href="#cite_note-7">[7]</a> Also, sulfur cathodes have low conductivity, requiring extra mass for a conducting agent in order to exploit the contribution of active mass to the capacity.<a href="#cite_note-8">[8]</a> Volume expansion of the sulfur cathode during S to Li2S conversion and the large amount of electrolyte needed are also issues. In the early 2000s, however, scientists began to make progress creating high-stability sulfurized-carbon cathodes<a href="#cite_note-9">[9]</a> and by 2020, scientists at Rice University had demonstrated batteries based on sulfurized carbon cathodes that retained >70% of their capacity after 1000 cycles.<a href="#cite_note-10">[10]</a> By 2023, <a href="/w/index.php?title=Zeta_Energy&action=edit&redlink=1" class="new" title="Zeta Energy (page does not exist)">Zeta Energy</a> a Texas-based startup announced that multiple national laboratories had independently verified that its lithium-sulfur batteries based on sulfurized-carbon cathodes were polysulfide shuttle free.<a href="#cite_note-11">[11]</a> <meta property="mw:PageProp/toc" /> <div class="mw-heading mw-heading2"><h2 id="History">History</h2></div> Li–S batteries were invented in the 1960s, when Herbert and Ulam patented a primary battery employing lithium or lithium alloys as anodic material, sulfur as cathodic material and an electrolyte composed of <a href="/wiki/Aliphatic_compounds" class="mw-redirect" title="Aliphatic compounds">aliphatic</a> saturated <a href="/wiki/Amines" class="mw-redirect" title="Amines">amines</a>.<a href="#cite_note-12">[12]</a><a href="#cite_note-13">[13]</a> A few years later the technology was improved by the introduction of organic solvents as <a href="/wiki/Propylene_carbonate" title="Propylene carbonate">PC</a>, <a href="/wiki/Dimethyl_sulfoxide" title="Dimethyl sulfoxide">DMSO</a> and <a href="/wiki/Dimethylformamide" title="Dimethylformamide">DMF</a> yielding a 2.35-2.5 V battery.<a href="#cite_note-14">[14]</a> By the end of the 1980s a rechargeable Li–S battery was demonstrated employing ethers, in particular <a href="/wiki/Dioxolane" title="Dioxolane">DOL</a>, as the electrolyte solvent.<a href="#cite_note-15">[15]</a><a href="#cite_note-16">[16]</a> In 2020 <a href="/wiki/Arumugam_Manthiram" title="Arumugam Manthiram">Manthiram</a> identified the critical parameters needed for achieving commercial acceptance.<a href="#cite_note-sulfur-17">[17]</a><a href="#cite_note-18">[18]</a> Specifically, Li–S batteries need to achieve a sulfur loading of >5 mg cm−2, a carbon content of <5%, electrolyte-to-sulfur ratio of <5 μL mg−1, electrolyte-to-capacity ratio of <5 μL (mA h)−1, and negative-to-positive capacity ratio of <5 in pouch-type cells.<a href="#cite_note-sulfur-17">[17]</a> In 2021, researchers announced the use of a sugar-based anode additive that prevented the release of polysulfide chains from the cathodes that pollute the anode. A prototype cell demonstrated 1,000 charge cycles with a capacity of 700 mAh/g.<a href="#cite_note-19">[19]</a> In 2022, an interlayer was introduced that claimed to reduce polysulfide movement (protecting the anode) and facilitate lithium ion transfer to reduce charge/discharge times.<a href="#cite_note-20">[20]</a> Also that year, researchers employed aramid nanofibers (nanoscale <a href="/wiki/Kevlar" title="Kevlar">Kevlar</a> fibers), fashioned into cell membrane-like networks. This prevented dendrite formation. It addressed polysulfide shuttle by using ion selectivity, by integrating tiny channels into the network and adding an electrical charge.<a href="#cite_note-21">[21]</a> Also in 2022, Researchers at <a href="/wiki/Drexel_University" title="Drexel University">Drexel University</a> produced a prototype lithium-sulfur battery that did not degrade over 4000 charge cycles. Analysis has shown that the battery contained monoclinic gamma-phase sulfur, which has been thought to be unstable below 95 degrees Celsius, and only a few studies have shown this type of sulfur to be stable longer than 20 to 30 minutes.<a href="#cite_note-22">[22]</a> <div class="mw-heading mw-heading2"><h2 id="Chemistry">Chemistry</h2></div> Chemical processes in the Li–S cell include lithium dissolution from the <a href="/wiki/Anode" title="Anode">anode</a> surface (and incorporation into <a href="/wiki/Alkali_metal" title="Alkali metal">alkali metal</a> <a href="/wiki/Polysulfide" title="Polysulfide">polysulfide</a> <a href="/wiki/Salt_(chemistry)" title="Salt (chemistry)">salts</a>) during discharge, and reverse lithium <a href="/wiki/Electroplating" title="Electroplating">plating</a> to the anode while charging.<a href="#cite_note-23">[23]</a> <div class="mw-heading mw-heading3"><h3 id="Anode">Anode</h3></div> At the <a href="/wiki/Anode" title="Anode">anodic</a> surface, dissolution of the metallic lithium occurs, with the production of electrons and lithium ions during the discharge and electrodeposition during the charge. The <a href="/wiki/Half-reaction" title="Half-reaction">half-reaction</a> is expressed as:<a href="#cite_note-24">[24]</a> <math xmlns="http://www.w3.org/1998/Math/MathML" alttext="{\displaystyle {\ce {Li <=> Li+ + e-}}}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <mrow class="MJX-TeXAtom-ORD"> <mtext>Li</mtext> <mrow class="MJX-TeXAtom-REL"> <mover> <mrow class="MJX-TeXAtom-OP MJX-fixedlimits"> <mrow class="MJX-TeXAtom-ORD"> <mpadded height="0" depth="0"> <mrow class="MJX-TeXAtom-ORD"> <mo stretchy="false">↽</mo> </mrow> <mspace width="negativethinmathspace" /> <mspace width="negativethinmathspace" /> <mrow class="MJX-TeXAtom-ORD"> <mo>−</mo> </mrow> </mpadded> </mrow> </mrow> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="false" scriptlevel="0"> <mrow class="MJX-TeXAtom-ORD"> <mrow class="MJX-TeXAtom-ORD"> <mo>−</mo> </mrow> <mspace width="negativethinmathspace" /> <mspace width="negativethinmathspace" /> <mrow class="MJX-TeXAtom-ORD"> <mo stretchy="false">⇀</mo> </mrow> </mrow> </mstyle> </mrow> </mover> </mrow> <msup> <mtext>Li</mtext> <mrow class="MJX-TeXAtom-ORD"> <mo>+</mo> </mrow> </msup> <mo>+</mo> <msup> <mtext>e</mtext> <mrow class="MJX-TeXAtom-ORD"> <mo>−</mo> </mrow> </msup> </mrow> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle {\ce {Li <=> Li+ + e-}}}</annotation> </semantics> </math><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/4d04ec5bb56bb1809ceedc0a608d21e3844737b8" class="mwe-math-fallback-image-inline mw-invert skin-invert" aria-hidden="true" style="vertical-align: -0.505ex; width:15.742ex; height:2.843ex;" alt="{\displaystyle {\ce {Li <=> Li+ + e-}}}"> In analogy with lithium batteries, the dissolution / electrodeposition reaction causes over time problems of unstable growth of the solid-electrolyte interface (SEI), generating active sites for the <a href="/wiki/Nucleation" title="Nucleation">nucleation</a> and dendritic growth of lithium. Dendritic growth is responsible for the internal short circuit in lithium batteries and leads to the death of the battery itself.<a href="#cite_note-:5-25">[25]</a> <div class="mw-heading mw-heading3"><h3 id="Cathode">Cathode</h3></div> In Li–S batteries, energy is stored in the sulfur <a href="/wiki/Cathode" title="Cathode">cathode</a> (S8). During discharge, the lithium ions in the electrolyte migrate to the cathode where the sulfur is reduced to <a href="/wiki/Lithium_sulphide" class="mw-redirect" title="Lithium sulphide">lithium sulphide (Li2S)</a>. The sulfur is reoxidized to S8 during the recharge phase. The semi-reaction is therefore expressed as: <math xmlns="http://www.w3.org/1998/Math/MathML" alttext="{\displaystyle {\ce {S + 2Li+ + 2e- <=> Li2S}}}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <mrow class="MJX-TeXAtom-ORD"> <mtext>S</mtext> <mo>+</mo> <mn>2</mn> <mspace width="thinmathspace" /> <msup> <mtext>Li</mtext> <mrow class="MJX-TeXAtom-ORD"> <mo>+</mo> </mrow> </msup> <mo>+</mo> <mn>2</mn> <mspace width="thinmathspace" /> <msup> <mtext>e</mtext> <mrow class="MJX-TeXAtom-ORD"> <mo>−</mo> </mrow> </msup> <mrow class="MJX-TeXAtom-REL"> <mover> <mrow class="MJX-TeXAtom-OP MJX-fixedlimits"> <mrow class="MJX-TeXAtom-ORD"> <mpadded height="0" depth="0"> <mrow class="MJX-TeXAtom-ORD"> <mo stretchy="false">↽</mo> </mrow> <mspace width="negativethinmathspace" /> <mspace width="negativethinmathspace" /> <mrow class="MJX-TeXAtom-ORD"> <mo>−</mo> </mrow> </mpadded> </mrow> </mrow> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="false" scriptlevel="0"> <mrow class="MJX-TeXAtom-ORD"> <mrow class="MJX-TeXAtom-ORD"> <mo>−</mo> </mrow> <mspace width="negativethinmathspace" /> <mspace width="negativethinmathspace" /> <mrow class="MJX-TeXAtom-ORD"> <mo stretchy="false">⇀</mo> </mrow> </mrow> </mstyle> </mrow> </mover> </mrow> <msubsup> <mtext>Li</mtext> <mrow class="MJX-TeXAtom-ORD"> <mn>2</mn> </mrow> <mrow class="MJX-TeXAtom-ORD"> <mspace width="0pt" height="0pt" depth=".2em" /> </mrow> </msubsup> <mtext>S</mtext> </mrow> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle {\ce {S + 2Li+ + 2e- <=> Li2S}}}</annotation> </semantics> </math><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/374e672b6bcb74803a0c9e106c77cbe3e2ad0d6a" class="mwe-math-fallback-image-inline mw-invert skin-invert" aria-hidden="true" style="vertical-align: -1.005ex; width:25.32ex; height:3.343ex;" alt="{\displaystyle {\ce {S + 2Li+ + 2e- <=> Li2S}}}"> (E ° ≈ 2.15 V vs Li / Li+ ) Actually the sulfur reduction reaction to lithium sulphide is much more complex and involves the formation of lithium polysulphides (Li2Sx, 2 ≤ x ≤ 8) at decreasing chain length according to the order:<a href="#cite_note-26">[26]</a> <math xmlns="http://www.w3.org/1998/Math/MathML" alttext="{\displaystyle {\ce {Li2S8->Li2S6->Li2S4->Li2S2->Li2S}}}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <mrow class="MJX-TeXAtom-ORD"> <msubsup> <mtext>Li</mtext> <mrow class="MJX-TeXAtom-ORD"> <mn>2</mn> </mrow> <mrow class="MJX-TeXAtom-ORD"> <mspace width="0pt" height="0pt" depth=".2em" /> </mrow> </msubsup> <msubsup> <mtext>S</mtext> <mrow class="MJX-TeXAtom-ORD"> <mn>8</mn> </mrow> <mrow class="MJX-TeXAtom-ORD"> <mspace width="0pt" height="0pt" depth=".2em" /> </mrow> </msubsup> <mo stretchy="false">⟶</mo> <msubsup> <mtext>Li</mtext> <mrow class="MJX-TeXAtom-ORD"> <mn>2</mn> </mrow> <mrow class="MJX-TeXAtom-ORD"> <mspace width="0pt" height="0pt" depth=".2em" /> </mrow> </msubsup> <msubsup> <mtext>S</mtext> <mrow class="MJX-TeXAtom-ORD"> <mn>6</mn> </mrow> <mrow class="MJX-TeXAtom-ORD"> <mspace width="0pt" height="0pt" depth=".2em" /> </mrow> </msubsup> <mo stretchy="false">⟶</mo> <msubsup> <mtext>Li</mtext> <mrow class="MJX-TeXAtom-ORD"> <mn>2</mn> </mrow> <mrow class="MJX-TeXAtom-ORD"> <mspace width="0pt" height="0pt" depth=".2em" /> </mrow> </msubsup> <msubsup> <mtext>S</mtext> <mrow class="MJX-TeXAtom-ORD"> <mn>4</mn> </mrow> <mrow class="MJX-TeXAtom-ORD"> <mspace width="0pt" height="0pt" depth=".2em" /> </mrow> </msubsup> <mo stretchy="false">⟶</mo> <msubsup> <mtext>Li</mtext> <mrow class="MJX-TeXAtom-ORD"> <mn>2</mn> </mrow> <mrow class="MJX-TeXAtom-ORD"> <mspace width="0pt" height="0pt" depth=".2em" /> </mrow> </msubsup> <msubsup> <mtext>S</mtext> <mrow class="MJX-TeXAtom-ORD"> <mn>2</mn> </mrow> <mrow class="MJX-TeXAtom-ORD"> <mspace width="0pt" height="0pt" depth=".2em" /> </mrow> </msubsup> <mo stretchy="false">⟶</mo> <msubsup> <mtext>Li</mtext> <mrow class="MJX-TeXAtom-ORD"> <mn>2</mn> </mrow> <mrow class="MJX-TeXAtom-ORD"> <mspace width="0pt" height="0pt" depth=".2em" /> </mrow> </msubsup> <mtext>S</mtext> </mrow> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle {\ce {Li2S8->Li2S6->Li2S4->Li2S2->Li2S}}}</annotation> </semantics> </math><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/4b5973e67b6d805f4e534aa03ec0d21570fb1f2c" class="mwe-math-fallback-image-inline mw-invert skin-invert" aria-hidden="true" style="vertical-align: -1.005ex; width:46.832ex; height:2.843ex;" alt="{\displaystyle {\ce {Li2S8->Li2S6->Li2S4->Li2S2->Li2S}}}"> The final product is actually a mixture of Li2S2 and Li2S rather than pure Li2S, due to the slow reduction kinetics at Li2S.<a href="#cite_note-:2-27">[27]</a> This contrasts with conventional lithium-ion cells, where the lithium ions are <a href="/wiki/Intercalation_(chemistry)" title="Intercalation (chemistry)">intercalated</a> in the anode and cathodes. Each sulfur atom can host two lithium ions. Typically, lithium-ion batteries accommodate only 0.5–0.7 lithium ions per host atom.<a href="#cite_note-28">[28]</a> Consequently, Li–S allows for a much higher lithium storage density. Polysulfides are <a href="/wiki/Redox" title="Redox">reduced</a> on the cathode surface in sequence while the cell is discharging: <dl><dd>S 8 → Li 2S 8 → Li 2S 6 → Li 2S 4 → Li 2S 3</dd></dl> Across a porous diffusion separator, sulfur <a href="/wiki/Polymers" class="mw-redirect" title="Polymers">polymers</a> form at the <a href="/wiki/Cathode" title="Cathode">cathode</a> as the cell charges: <dl><dd>Li 2S → Li 2S 2 → Li 2S 3 → Li 2S 4 → Li 2S 6 → Li 2S 8 → S 8</dd></dl> These reactions are analogous to those in the <a href="/wiki/Sodium%E2%80%93sulfur_battery" title="Sodium–sulfur battery">sodium–sulfur battery</a>. The main challenges of Li–S batteries is the low conductivity of sulfur and its considerable volume change upon discharging and finding a suitable cathode is the first step for commercialization of Li–S batteries.<a href="#cite_note-29">[29]</a> Therefore, most researchers use a carbon/sulfur cathode and a lithium anode.<a href="#cite_note-30">[30]</a> Sulfur is very cheap, but has practically no <a href="/wiki/Electric_conductance" class="mw-redirect" title="Electric conductance">electroconductivity</a>, 5×10−30 <a href="/wiki/Siemens_(unit)" title="Siemens (unit)">S</a>⋅cm−1 at 25 °C.<a href="#cite_note-31">[31]</a> A carbon coating provides the missing electroconductivity. Carbon nanofibers provide an effective electron conduction path and structural integrity, at the disadvantage of higher cost.<a href="#cite_note-32">[32]</a> One problem with the lithium–sulfur design is that when the sulfur in the cathode absorbs lithium, volume expansion of the LixS compositions occurs, and predicted volume expansion of Li2S is nearly 80% of the volume of the original sulfur.<a href="#cite_note-33">[33]</a> This causes large mechanical stresses on the cathode, which is a major cause of rapid degradation. This process reduces the contact between the carbon and the sulfur, and prevents the flow of lithium ions to the carbon surface.<a href="#cite_note-34">[34]</a> Mechanical properties of the lithiated sulfur compounds are strongly contingent on the lithium content, and with increasing lithium content, the strength of lithiated sulfur compounds improves, although this increment is not linear with lithiation.<a href="#cite_note-35">[35]</a> One of the primary shortfalls of most Li–S cells is unwanted reactions with the electrolytes. While S and Li 2S are relatively insoluble in most electrolytes, many intermediate polysulfides are not. Dissolving Li 2S n into electrolytes causes irreversible loss of active sulfur.<a href="#cite_note-36">[36]</a> Use of highly reactive lithium as a negative electrode causes dissociation of most of the commonly used other type electrolytes. Use of a protective layer in the anode surface has been studied to improve cell safety, i.e., using <a href="/wiki/Teflon" class="mw-redirect" title="Teflon">Teflon</a> coating showed improvement in the electrolyte stability,<a href="#cite_note-37">[37]</a> LIPON, Li3N also exhibited promising performance. <div class="mw-heading mw-heading2"><h2 id="Polysulfide_"shuttle"">Polysulfide "shuttle" </h2></div> Historically, the "shuttle" effect is the main cause of degradation in a Li–S battery.<a href="#cite_note-:1-38">[38]</a> The lithium polysulfide Li2Sx (6≤x≤8) is highly soluble<a href="#cite_note-39">[39]</a> in the common electrolytes used for Li–S batteries. They are formed and leaked from the cathode and they diffuse to the anode, where they are reduced to short-chain polysulfides and diffuse back to the cathode where long-chain polysulfides are formed again. This process results in the continuous leakage of active material from the cathode, lithium corrosion, low coulombic efficiency and low battery life.<a href="#cite_note-40">[40]</a> Moreover, the "shuttle" effect is responsible for the characteristic self-discharge of Li–S batteries, because of slow dissolution of polysulfide, which occurs also in rest state.<a href="#cite_note-:1-38">[38]</a> The "shuttle" effect in a Li–S battery can be quantified by a factor fc (0<fc<1), evaluated by the extension of the charge voltage plateau. The factor fc is given by the expression:<a href="#cite_note-41">[41]</a> <math xmlns="http://www.w3.org/1998/Math/MathML" alttext="{\displaystyle fc={\frac {k_{\text{s}}q_{\text{up}}[S_{\text{tot}}]}{I_{c}}}}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <mi>f</mi> <mi>c</mi> <mo>=</mo> <mrow class="MJX-TeXAtom-ORD"> <mfrac> <mrow> <msub> <mi>k</mi> <mrow class="MJX-TeXAtom-ORD"> <mtext>s</mtext> </mrow> </msub> <msub> <mi>q</mi> <mrow class="MJX-TeXAtom-ORD"> <mtext>up</mtext> </mrow> </msub> <mo stretchy="false">[</mo> <msub> <mi>S</mi> <mrow class="MJX-TeXAtom-ORD"> <mtext>tot</mtext> </mrow> </msub> <mo stretchy="false">]</mo> </mrow> <msub> <mi>I</mi> <mrow class="MJX-TeXAtom-ORD"> <mi>c</mi> </mrow> </msub> </mfrac> </mrow> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle fc={\frac {k_{\text{s}}q_{\text{up}}[S_{\text{tot}}]}{I_{c}}}}</annotation> </semantics> </math><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/92767aff703c9811fcd59e4023389b4a8bdf304f" class="mwe-math-fallback-image-inline mw-invert skin-invert" aria-hidden="true" style="vertical-align: -2.338ex; width:16.461ex; height:6.176ex;" alt="{\displaystyle fc={\frac {k_{\text{s}}q_{\text{up}}[S_{\text{tot}}]}{I_{c}}}}"> where ks, qup, [Stot] and Ic are respectively the kinetic constant, specific capacity contributing to the anodic plateau, the total sulfur concentration and charge current. In 2022,<a href="#cite_note-auto-42">[42]</a> researchers reported the use of a cathode made from <a href="/wiki/Carbon_nanofibers" class="mw-redirect" title="Carbon nanofibers">carbon nanofibers</a>. Elemental sulfur was deposited onto the carbon substrate (cf. <a href="/wiki/Physical_vapor_deposition" title="Physical vapor deposition">physical vapor deposition</a>), which formed the rare and usually metastable monoclinic <a href="/wiki/Allotropes_of_sulfur#List_of_allotropes_and_forms" title="Allotropes of sulfur">γ-Sulfur</a> allotrope. This allotrope reversibly reacts to Li 2S without the formation of intermediate polysulfides Li 2S x. Therefore, carbonate electrolytes, which commonly react with those polysulfides, can be used instead of the rather dangerous ether based electrolytes (low flash and boiling points).<a href="#cite_note-43">[43]</a> Its initial capacity was 800 Ah/kg (classical LiCoO2/graphite batteries have a cell capacity of 100 Ah/kg). It decayed only very slowly, on average 0.04% each cycle, and retained 658 Ah/kg after 4000 cycles (82%).<a href="#cite_note-auto-42">[42]</a> <div class="mw-heading mw-heading2"><h2 id="Electrolyte">Electrolyte</h2></div> Conventionally, Li–S batteries employ a liquid organic electrolyte, contained in the pores of PP separator.<a href="#cite_note-:1-38">[38]</a> The electrolyte plays a key role in Li–S batteries, acting both on "shuttle" effect by the polysulfide dissolution and the SEI stabilization at anode surface. It has been demonstrated that the electrolytes based on organic carbonates commonly employed in Li-ion batteries (i.e. PC, <a href="/wiki/Ethylene_carbonate" title="Ethylene carbonate">EC</a>, <a href="/wiki/Diethyl_carbonate" title="Diethyl carbonate">DEC</a> and mixtures of them) are not compatible with the chemistry of Li–S batteries.<a href="#cite_note-44">[44]</a> Long-chain polysulfides undergo nucleophilic attack on electrophilic sites of carbonates, resulting in the irreversible formation of by-products as <a href="/wiki/Ethanol" title="Ethanol">ethanol</a>, <a href="/wiki/Methanol" title="Methanol">methanol</a>, <a href="/wiki/Ethylene_glycol" title="Ethylene glycol">ethylene glycol</a> and <a href="/wiki/Thiocarbonate" title="Thiocarbonate">thiocarbonates</a>. In Li–S batteries are conventionally employed cyclic ethers (as <a href="/wiki/Dioxolane" title="Dioxolane">DOL</a>) or short-chain ethers (as <a href="/wiki/Dimethyl_ether" title="Dimethyl ether">DME</a>) as well as the family of glycol ethers, including <a href="/wiki/Diglyme" title="Diglyme">DEGDME</a> and <a href="/wiki/Tetraethylene_glycol_dimethyl_ether" title="Tetraethylene glycol dimethyl ether">TEGDME</a>.<a href="#cite_note-:2a-45">[45]</a> One common electrolyte is 1M <a href="/wiki/Lithium_bis(trifluoromethanesulfonyl)imide" title="Lithium bis(trifluoromethanesulfonyl)imide">LiTFSI</a> in DOL:DME 1:1 vol. with 1%w/w di LiNO3 as additive for lithium surface passivation.<a href="#cite_note-:2a-45">[45]</a> <div class="mw-heading mw-heading2"><h2 id="Safety">Safety</h2></div> Because of the high potential energy density and the nonlinear discharge and charging response of the cell, a <a href="/wiki/Microcontroller" title="Microcontroller">microcontroller</a> and other safety circuitry is sometimes used along with <a href="/wiki/Voltage_regulator" title="Voltage regulator">voltage regulators</a> to manage cell operation and <a href="/wiki/Thermal_runaway" title="Thermal runaway">prevent rapid discharge</a>.<a href="#cite_note-46">[46]</a> <div class="mw-heading mw-heading2"><h2 id="Research">Research</h2></div> <table class="wikitable"> <caption>Research </caption> <tbody><tr> <th>Anode</th> <th>Cathode</th> <th>Date</th> <th>Source</th> <th>Specific Capacity after cycling</th> <th>Notes </th></tr> <tr> <td>Lithium metal</td> <td><a href="/wiki/Polyethylene_glycol" title="Polyethylene glycol">Polyethylene glycol</a> coated, pitted mesoporous carbon</td> <td>17 May 2009</td> <td><a href="/wiki/University_of_Waterloo" title="University of Waterloo">University of Waterloo</a><a href="#cite_note-:0-47">[47]</a></td> <td>1,110 mA⋅h/g after 20 cycles at a current of 168 mA⋅g−1<a href="#cite_note-:0-47">[47]</a> </td> <td>Minimal degradation during charge cycling. To retain polysulfides in the cathode, the surface was functionalized to repel (hydrophobic) polysulfides. In a test using a <a href="/wiki/Glycol_ethers" title="Glycol ethers">glyme</a> solvent, a traditional sulfur cathode lost 96% of its sulfur over 30 <a href="/wiki/Charge_cycle" title="Charge cycle">cycles</a>, while the experimental cathode lost only 25%. </td></tr> <tr> <td>Lithium metal</td> <td>Sulfur-coated, disordered carbon hollow carbon nanofibers</td> <td>2011</td> <td><a href="/wiki/Stanford_University" title="Stanford University">Stanford University</a><a href="#cite_note-48">[48]</a><a href="#cite_note-Keller-49">[49]</a></td> <td>730 mA⋅h/g after 150 cycles (at 0.5 C)</td> <td>An electrolyte additive boosted the <a href="/wiki/Faraday_efficiency" title="Faraday efficiency">faraday efficiency</a> from 85% to over 99%. </td></tr> <tr> <td>Silicon nanowire/carbon</td> <td>Sulfur-coated, disordered carbon nanotubes made from carbohydrates</td> <td>2013</td> <td>CGS<a href="#cite_note-50">[50]</a><a href="#cite_note-51">[51]</a></td> <td>1,300 mA⋅h/g after 400 cycles (at 1 C)</td> <td>Microwave processing of materials and laser-printing of electrodes. </td></tr> <tr> <td>Silicon carbon</td> <td>Sulfur</td> <td>2013</td> <td><a href="/wiki/Fraunhofer_Institute" class="mw-redirect" title="Fraunhofer Institute">Fraunhofer Institute</a> for Material and Beam Technology IWS<a href="#cite_note-52">[52]</a></td> <td>? after 1,400 cycles </td></tr> <tr> <td></td> <td><a href="/wiki/Copolymer" title="Copolymer">Copolymerized</a> sulfur</td> <td>2013</td> <td><a href="/wiki/University_of_Arizona" title="University of Arizona">University of Arizona</a><a href="#cite_note-53">[53]</a><a href="#cite_note-54">[54]</a> </td> <td>823 mA⋅h/g at 100 cycles</td> <td>Uses "inverse <a href="/wiki/Vulcanization" title="Vulcanization">vulcanization</a>" on mostly sulfur with a small amount of 1,3-diisopropenylbenzene (DIB) additive </td></tr> <tr> <td></td> <td>Porous TiO 2-encapsulated sulfur nanoparticles</td> <td>2013</td> <td>Stanford University<a href="#cite_note-55">[55]</a><a href="#cite_note-56">[56]</a></td> <td>721 mA⋅h/g at 1,000 cycles (0.5 C)</td> <td>shell protects the sulfur-lithium intermediate from electrolyte solvent. Each cathode particle is 800 nanometers in diameter. <a href="/wiki/Faraday_efficiency" title="Faraday efficiency">Faraday efficiency</a> of 98.4%. </td></tr> <tr> <td></td> <td>Sulfur</td> <td>June 2013</td> <td><a href="/wiki/Oak_Ridge_National_Laboratory" title="Oak Ridge National Laboratory">Oak Ridge National Laboratory</a></td> <td>1200 mA·h/g at 300 cycles at 60 °C (0.1 C) 800 mA·h/g at 300 cycles at 60 °C (1 C)<a href="#cite_note-57">[57]</a> </td> <td>Solid lithium polysulfidophosphate electrolyte. Half the voltage of typical LIBs. Remaining issues include low electrolyte ionic conductivity and brittleness in the ceramic structure.<a href="#cite_note-58">[58]</a><a href="#cite_note-59">[59]</a> </td></tr> <tr> <td>Lithium</td> <td>Sulfur-<a href="/wiki/Graphene_oxide" class="mw-redirect" title="Graphene oxide">graphene oxide</a> nanocomposite with <a href="/wiki/Styrene-butadiene" title="Styrene-butadiene">styrene-butadiene</a>-<a href="/wiki/Carboxymethyl_cellulose" title="Carboxymethyl cellulose">carboxymethyl cellulose</a> copolymer binder</td> <td>2013</td> <td><a href="/wiki/Lawrence_Berkeley_National_Laboratory" title="Lawrence Berkeley National Laboratory">Lawrence Berkeley National Laboratory</a><a href="#cite_note-60">[60]</a></td> <td>700 mA·h/g at 1,500 cycles (0.05 C discharge) 400 mA·h/g at 1,500 cycles (0.5 C charge / 1 C discharge) </td> <td>Voltage between about 1.7 and 2.5 volts, depending on charge state. Lithium bis(trifluoromethanesulfonyl)imide) dissolved in a mixture of nmethyl-(n-butyl) pyrrolidinium bis(trifluoromethanesulfonyl)-imide (PYR14TFSI), 1,3-dioxolane (DOL), dimethoxyethane (DME) with 1 M <a href="/wiki/Lithium_bis(trifluoromethanesulfonyl)imide" title="Lithium bis(trifluoromethanesulfonyl)imide">lithium bis-(trifluoromethylsulfonyl)imide</a> (LiTFSI), and lithium nitrate (LiNO 3). High porosity polypropylene separator. Specific energy is 500 W⋅h/kg (initial) and 250 W⋅h/kg at 1,500 cycles (C=1.0) </td></tr> <tr> <td>Lithiated graphite</td> <td>Sulfur</td> <td>February 2014</td> <td><a href="/wiki/Pacific_Northwest_National_Laboratory" title="Pacific Northwest National Laboratory">Pacific Northwest National Laboratory</a></td> <td>400 cycles</td> <td>Coating prevents polysulfides from destroying the anode.<a href="#cite_note-61">[61]</a> </td></tr> <tr> <td>Lithiated graphene </td> <td>Sulfur/Lithium-sulfide passivation layer </td> <td>2014 </td> <td>OXIS Energy<a href="#cite_note-62">[62]</a><a href="#cite_note-63">[63]</a> </td> <td>240 mA·h/g (1000 cycles) 25 A·h/cell </td> <td>Passivation layer prevents sulfur loss </td></tr> <tr> <td>Lithiated hard-carbon</td> <td>Sulfur-copolymer (poly(S-co-DVB))</td> <td>2019</td> <td><a href="/wiki/Chungnam_National_University" title="Chungnam National University">Chungnam National University</a></td> <td>400 mAh/g for 500 cycles at 3C</td> <td>The SEI of hard-carbon prevents polysulphides deposition at anode and enables high-rate performance.<a href="#cite_note-64">[64]</a> </td></tr> <tr> <td>Lithium sulfur batteries </td> <td>Carbon nanotube/Sulfur </td> <td>2014 </td> <td>Tsinghua University<a href="#cite_note-65">[65]</a> </td> <td>15.1 mA·h⋅cm−2 at a sulfur loading of 17.3 mgS⋅cm−2 </td> <td>A free-standing CNT–S paper electrode with a high areal sulfur-loading was fabricated, in which short MWCNTs served as the short-range electrical conductive network and super-long CNTs acted as both the long-range conductive network and intercrossed binders. </td></tr> <tr> <td> </td> <td>Glass-coated sulfur with mildly reduced <a href="/wiki/Graphene_oxide" class="mw-redirect" title="Graphene oxide">graphene oxide</a> for structural support </td> <td>2015 </td> <td>University of California, Riverside<a href="#cite_note-66">[66]</a> </td> <td>700 mA⋅h⋅g−1 (50 cycles)<a href="#cite_note-67">[67]</a> </td> <td>Glass coating prevents lithium polysulfides from permanently migrating to an electrode </td></tr> <tr> <td>Lithium </td> <td>Sulfur </td> <td>2016 </td> <td><a rel="nofollow" class="external text" href="https://projects.leitat.org/alise">LEITAT</a> </td> <td>500 W⋅h/kg </td> <td>ALISE H2020 project developing a Li–S battery for cars with new components and optimized regarding anode, cathode, electrolyte and separator </td></tr> <tr> <td>Lithium metal </td> <td>Sulfurized graphene </td> <td>2021 </td> <td>CATRIN, Palacký University <a rel="nofollow" class="external autonumber" href="https://www.catrin.com/">[1]</a> </td> <td>644 mA⋅h⋅g−1 (250 cycles) </td> <td>An efficient and straightforward approach to prepare a covalently sulfurized graphene cathode for Li–S batteries with high sulfur content and high cycling stability.<a href="#cite_note-68">[68]</a> </td></tr> <tr> <td> </td> <td>Sulfur-loaded carbon nanotubes </td> <td>2022 </td> <td><a href="/wiki/Korea_Electrotechnology_Research_Institute" title="Korea Electrotechnology Research Institute">Korea Electrotechnology Research Institute</a><a href="#cite_note-69">[69]</a> </td> <td>850 mA⋅h⋅g−1 (100 cycles) </td> <td>Uses a phosphorus-doped <a href="/wiki/Activated_carbon" title="Activated carbon">activated carbon</a> separator layer to minimize the polysulfide shuttle effect, while creating a foldable battery. </td></tr> <tr> <td>Lithium metal </td> <td>Lithium thiophosphate catholyte </td> <td>2023 </td> <td><a href="/wiki/Dartmouth_College" title="Dartmouth College">Dartmouth College</a>, <a href="/wiki/Stanford_University" title="Stanford University">Stanford University</a><a href="#cite_note-70">[70]</a> </td> <td>1271 mA⋅h⋅g−1 (200 cycles) </td> <td>Adding <a href="/wiki/Phosphorus_pentasulfide" title="Phosphorus pentasulfide">phosphorus pentasulfide</a> to a Li–S catholyte leads to the formation of complexes that accommodate the discharge product (Li2S) and allow high cyclability and low temperature performance. </td></tr></tbody></table> <div class="mw-heading mw-heading2"><h2 id="Commercialization">Commercialization</h2></div> As of 2021 few companies had been able to commercialize the technology on an industrial scale. Companies such as Sion Power have partnered with <a href="/wiki/Airbus_Defence_and_Space" title="Airbus Defence and Space">Airbus Defence and Space</a> to test their lithium sulfur battery technology. Airbus Defense and Space successfully launched their prototype <a href="/wiki/High_Altitude_Pseudo-Satellite" class="mw-redirect" title="High Altitude Pseudo-Satellite">High Altitude Pseudo-Satellite</a> (HAPS) aircraft powered by solar energy during the day and by lithium sulfur batteries at night in real life conditions during an 11-day flight. The batteries used in the test flight utilized Sion Power's Li–S cells that provide 350 W⋅h/kg.<a href="#cite_note-71">[71]</a> Sion originally claimed to be in the process of volume manufacturing with availability by end of 2017; however more recently it can be seen that they have dropped work on their lithium sulfur battery in favor of a lithium-metal battery.<a href="#cite_note-72">[72]</a><a href="#cite_note-73">[73]</a> British firm OXIS Energy developed prototype lithium sulfur batteries.<a href="#cite_note-74">[74]</a><a href="#cite_note-75">[75]</a> Together with <a href="/wiki/Imperial_College_London" title="Imperial College London">Imperial College London</a> and <a href="/wiki/Cranfield_University" title="Cranfield University">Cranfield University</a>, they published <a href="/wiki/Equivalent-circuit-network" class="mw-redirect" title="Equivalent-circuit-network">equivalent-circuit-network</a> models for its cells.<a href="#cite_note-76">[76]</a> With Lithium Balance of Denmark they built a prototype scooter battery system primarily for the Chinese market, which had a capacity of 1.2 kWh using 10 Ah Long Life cells, and weighed 60% less than lead acid batteries with a significant increase in range.<a href="#cite_note-77">[77]</a> They also built a 3U, 3,000 W⋅h Rack-Mounted Battery that weighed only 25 kg and was said to be fully scalable.<a href="#cite_note-78">[78]</a> They claimed their Lithium-Sulfur batteries would cost about $200/kWh in mass production.<a href="#cite_note-79">[79]</a> However, the firm entered bankruptcy (insolvency) status in May 2021.<a href="#cite_note-80">[80]</a> <a href="/wiki/Sony" title="Sony">Sony</a>, which also commercialized the first lithium-ion battery, planned to introduce lithium–sulfur batteries to the market in 2020, but has provided no updates since the initial announcement in 2015.<a href="#cite_note-81">[81]</a> Monash University's Department of Mechanical and Aerospace Engineering in Melbourne, Australia developed an ultra-high capacity Li–S battery that has been manufactured by partners at the Fraunhofer Institute for Material and Beam Technology in Germany. It is claimed the battery can provide power to a smartphone for five days.<a href="#cite_note-82">[82]</a> In 2022, the German company Theion claimed to introduce lithium–sulfur batteries for mobile devices in 2023 and for vehicles by 2024.<a href="#cite_note-83">[83]</a> In January 2023, <a href="/wiki/Houston,_Texas" class="mw-redirect" title="Houston, Texas">Houston, Texas</a> company <a href="/w/index.php?title=Zeta_Energy&action=edit&redlink=1" class="new" title="Zeta Energy (page does not exist)">Zeta Energy</a> was awarded $4 million by the <a href="/wiki/United_States_Department_of_Energy" title="United States Department of Energy">United States Department of Energy</a> <a href="/wiki/ARPA-E" title="ARPA-E">ARPA-E</a> program to advance its lithium-sulfur batteries based on a sulfurized-carbon cathode and a vertically-aligned carbon nanontube anode.<a href="#cite_note-84">[84]</a> In June 2023, <a href="/wiki/San_Jose,_California" title="San Jose, California">San Jose, California</a> company Lyten started up a pilot production line making about 100 batteries a day.<a href="#cite_note-SJMN_2023-06-14-85">[85]</a> <div class="mw-heading mw-heading2"><h2 id="See_also">See also</h2></div> <style data-mw-deduplicate="TemplateStyles:r1259569809">.mw-parser-output .portalbox{padding:0;margin:0.5em 0;display:table;box-sizing:border-box;max-width:175px;list-style:none}.mw-parser-output .portalborder{border:1px solid var(--border-color-base,#a2a9b1);padding:0.1em;background:var(--background-color-neutral-subtle,#f8f9fa)}.mw-parser-output .portalbox-entry{display:table-row;font-size:85%;line-height:110%;height:1.9em;font-style:italic;font-weight:bold}.mw-parser-output .portalbox-image{display:table-cell;padding:0.2em;vertical-align:middle;text-align:center}.mw-parser-output .portalbox-link{display:table-cell;padding:0.2em 0.2em 0.2em 0.3em;vertical-align:middle}@media(min-width:720px){.mw-parser-output .portalleft{clear:left;float:left;margin:0.5em 1em 0.5em 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id="References">References</h2></div> <style data-mw-deduplicate="TemplateStyles:r1239543626">.mw-parser-output .reflist{margin-bottom:0.5em;list-style-type:decimal}@media screen{.mw-parser-output .reflist{font-size:90%}}.mw-parser-output .reflist .references{font-size:100%;margin-bottom:0;list-style-type:inherit}.mw-parser-output .reflist-columns-2{column-width:30em}.mw-parser-output .reflist-columns-3{column-width:25em}.mw-parser-output .reflist-columns{margin-top:0.3em}.mw-parser-output .reflist-columns ol{margin-top:0}.mw-parser-output .reflist-columns li{page-break-inside:avoid;break-inside:avoid-column}.mw-parser-output .reflist-upper-alpha{list-style-type:upper-alpha}.mw-parser-output .reflist-upper-roman{list-style-type:upper-roman}.mw-parser-output .reflist-lower-alpha{list-style-type:lower-alpha}.mw-parser-output .reflist-lower-greek{list-style-type:lower-greek}.mw-parser-output .reflist-lower-roman{list-style-type:lower-roman}</style><div class="reflist reflist-columns references-column-width" style="column-width: 30em;"> <ol class="references"> <li id="cite_note-oxisapril2021-1">^ <a href="#cite_ref-oxisapril2021_1-0">a</a> <a href="#cite_ref-oxisapril2021_1-1">b</a> <a href="#cite_ref-oxisapril2021_1-2">c</a> <style data-mw-deduplicate="TemplateStyles:r1238218222">.mw-parser-output cite.citation{font-style:inherit;word-wrap:break-word}.mw-parser-output .citation q{quotes:"\"""\"""'""'"}.mw-parser-output .citation:target{background-color:rgba(0,127,255,0.133)}.mw-parser-output .id-lock-free.id-lock-free a{background:url("//upload.wikimedia.org/wikipedia/commons/6/65/Lock-green.svg")right 0.1em center/9px no-repeat}.mw-parser-output .id-lock-limited.id-lock-limited a,.mw-parser-output .id-lock-registration.id-lock-registration a{background:url("//upload.wikimedia.org/wikipedia/commons/d/d6/Lock-gray-alt-2.svg")right 0.1em center/9px no-repeat}.mw-parser-output .id-lock-subscription.id-lock-subscription 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Archived from <a rel="nofollow" class="external text" href="http://pdf-s3.xuebalib.com:1262/3p53gUMPTEVW.pdf">the original</a> (PDF) on 2020-01-03.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Acc.+Chem.+Res.&rft.atitle=Challenges+and+Prospects+of+Lithium%E2%80%93Sulfur+Batteries&rft.volume=46&rft.issue=5&rft.pages=1125-1134&rft.date=2013&rft_id=info%3Adoi%2F10.1021%2Far300179v&rft_id=info%3Apmid%2F23095063&rft.aulast=Manthiram&rft.aufirst=Arumugam&rft.au=Fu%2C+Yongzhu&rft.au=Su%2C+Yu-Sheng&rft_id=http%3A%2F%2Fpdf-s3.xuebalib.com%3A1262%2F3p53gUMPTEVW.pdf&rfr_id=info%3Asid%2Fen.wikipedia.org%3ALithium%E2%80%93sulfur+battery" class="Z3988"> </li> <li id="cite_note-osti1561559-5"><a href="#cite_ref-osti1561559_5-0">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite class="citation report cs1"><a rel="nofollow" class="external text" href="https://www.osti.gov/servlets/purl/1561559">Automotive Li-Ion Batteries: Current Status and Future Perspectives</a> (Report). 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Retrieved January 9, 2020.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=unknown&rft.jtitle=The+Engineer&rft.atitle=%27World%27s+most+efficient+lithium-sulphur+battery%27+set+for+launch&rft.date=2020-01-06&rft_id=https%3A%2F%2Fwww.theengineer.co.uk%2Flithium-sulphur-battery%2F&rfr_id=info%3Asid%2Fen.wikipedia.org%3ALithium%E2%80%93sulfur+battery" class="Z3988"> </li> <li id="cite_note-83"><a href="#cite_ref-83">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFMorris" class="citation web cs1">Morris, James. <a rel="nofollow" class="external text" href="https://www.forbes.com/sites/jamesmorris/2022/04/02/sulfur-battery-technology-could-make-electric-cars-go-three-times-further-by-2024/">"Sulfur Battery Technology Could Make Electric Cars Go Three Times Further By 2024"</a>. Forbes. 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Polyplus.com. Archived from <a rel="nofollow" class="external text" href="http://polyplus.com/lisulfur.html">the original</a> on 2013-04-20. Retrieved 2013-04-06.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=unknown&rft.btitle=PolyPlus+Lithium+Sulfur&rft.pub=Polyplus.com&rft_id=http%3A%2F%2Fpolyplus.com%2Flisulfur.html&rfr_id=info%3Asid%2Fen.wikipedia.org%3ALithium%E2%80%93sulfur+battery" class="Z3988"></li> <li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite class="citation web cs1"><a rel="nofollow" class="external text" href="http://sionpower.com/">"Sion Power"</a>. Sion Power. Retrieved 2013-04-06.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=unknown&rft.btitle=Sion+Power&rft.pub=Sion+Power&rft_id=http%3A%2F%2Fsionpower.com%2F&rfr_id=info%3Asid%2Fen.wikipedia.org%3ALithium%E2%80%93sulfur+battery" class="Z3988"></li> <li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite class="citation web cs1"><a rel="nofollow" class="external text" href="https://web.archive.org/web/20140325161004/http://en.winston-battery.com/index.php/products/power-battery/category/lsp-battery">"Winston Battery Limited"</a>. En.winston-battery.com. Archived from <a rel="nofollow" class="external text" href="http://en.winston-battery.com/index.php/products/power-battery/category/lsp-battery">the original</a> on 2014-03-25. Retrieved 2013-04-06.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=unknown&rft.btitle=Winston+Battery+Limited&rft.pub=En.winston-battery.com&rft_id=http%3A%2F%2Fen.winston-battery.com%2Findex.php%2Fproducts%2Fpower-battery%2Fcategory%2Flsp-battery&rfr_id=info%3Asid%2Fen.wikipedia.org%3ALithium%E2%80%93sulfur+battery" class="Z3988"></li> <li><a rel="nofollow" class="external text" href="https://www.eemb.com/">"EEMB Battery"</a>. EEMB Battery. 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