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{{Short description|Chemical compound of formula CaS}} |
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{{chembox |
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{{chembox |
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| Verifiedfields = changed |
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| Name = Calcium sulfide |
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| Watchedfields = changed |
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| ImageFile = Calcium-sulfide-3D-balls.png |
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| verifiedrevid = 460015006 |
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<!-- | ImageSize = 125px --> |
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| ImageName = Calcium sulfide |
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| Name = Calcium sulfide |
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| IUPACName = Calcium sulfide |
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| ImageFile = Calcium-sulfide-3D-balls.png |
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| OtherNames = Calcium monosulfide,<br/>Hepar calcies,<br/>Sulfurated lime<br/>Oldhamite |
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| ImageName = Calcium sulfide |
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| IUPACName = Calcium sulfide |
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| OtherNames = Calcium monosulfide,<br/>Hepar calcies,<br/>Sulfurated lime<br/>Oldhamite |
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| Section1 = {{Chembox Identifiers |
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|Section1={{Chembox Identifiers |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| ChemSpiderID = 8373113 |
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| ChemSpiderID = 8373113 |
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| UNII = <!-- blanked - oldvalue: 1MBW07J51Q --> |
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| UNII_Ref = {{fdacite|correct|FDA}} |
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| UNII = 1MBW07J51Q |
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| InChI = 1/Ca.S/rCaS/c1-2 |
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| InChI = 1/Ca.S/rCaS/c1-2 |
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| ChEBI = 81055 |
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| SMILES = =S |
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| SMILES = =S |
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| InChIKey = JGIATAMCQXIDNZ-WSLZQIQFAE |
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| InChIKey = JGIATAMCQXIDNZ-WSLZQIQFAE |
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| InChIKey1 = AGVJBLHVMNHENQ-UHFFFAOYAE |
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| InChIKey1 = AGVJBLHVMNHENQ-UHFFFAOYAE |
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| SMILES1 = . |
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| SMILES1 = . |
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| StdInChI_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChI = 1S/Ca.S/q+2;-2 |
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| StdInChI = 1S/Ca.S/q+2;-2 |
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| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChIKey = AGVJBLHVMNHENQ-UHFFFAOYSA-N |
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| StdInChIKey = AGVJBLHVMNHENQ-UHFFFAOYSA-N |
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| CASNo = 20548-54-3 |
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| CASNo = 20548-54-3 |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| PubChem = 10197613 |
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| PubChem = 10197613 |
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| RTECS = |
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| RTECS = |
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| EINECS = 243-873-5 |
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| EINECS = 243-873-5 |
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| KEGG_Ref = {{keggcite|correct|kegg}} |
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| KEGG = C17392 |
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}} |
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}} |
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| Section2 = {{Chembox Properties |
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|Section2={{Chembox Properties |
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| Formula = CaS |
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| Formula = CaS |
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| MolarMass = 72.143 g/mol |
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| MolarMass = 72.143 g/mol |
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| Appearance = white crystals <br> ] |
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| Appearance = white crystals <br> ] |
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| Density = 2.59 g/cm<sup>3</sup> |
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| Density = 2.59 g/cm<sup>3</sup> |
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| Solubility = slightly soluble |
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| Solubility = Hydrolyses |
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| SolubleOther = insoluble in ] <br> reacts with ] |
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| SolubleOther = Insoluble in ] <br> reacts with ] |
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| MeltingPt = 2525 °C |
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| MeltingPtC = 2525 |
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| MeltingPt_notes = |
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| BoilingPt = |
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| RefractIndex = 2.137 |
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| BoilingPt = |
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| RefractIndex = 2.137 |
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}} |
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}} |
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| Section3 = {{Chembox Structure |
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|Section3={{Chembox Structure |
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| CrystalStruct = ] (cubic), ] |
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| CrystalStruct = ] (cubic), ] |
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| SpaceGroup = Fm<u style="text-decoration:overline">3</u>m, No. 225 |
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| SpaceGroup = Fm<u style="text-decoration:overline">3</u>m, No. 225 |
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| Coordination = Octahedral (Ca<sup>2+</sup>); octahedral (S<sup>2–</sup>) |
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| Coordination = Octahedral (Ca<sup>2+</sup>); octahedral (S<sup>2−</sup>) |
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| LattConst_a = |
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| LattConst_a = |
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}} |
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}} |
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| Section7 = {{Chembox Hazards |
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|Section7={{Chembox Hazards |
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| ExternalMSDS = |
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| ExternalSDS = |
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| MainHazards = H<sub>2</sub>S source |
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| MainHazards = Reacts with water to release H<sub>2</sub>S |
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| NFPA-H = 2 |
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| EUClass = Irritant ('''Xi''')<br/>Dangerous for the environment ('''N''') |
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| EUIndex = 016-004-00-0 |
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| NFPA-F = 0 |
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| NFPA-R = 3 <!-- Source from 2014: https://www.sigmaaldrich.com/MSDS/MSDS/DisplayMSDSPage.do?country=US&language=en&productNumber=409553&brand=ALDRICH&PageToGoToURL=https%3A%2F%2Fwww.sigmaaldrich.com%2Fcatalog%2Fsearch%3Fterm%3Dcalcium%2Bsulfide --> |
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| NFPA-H = 2 |
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| GHSPictograms = {{GHS05}}{{GHS07}}{{GHS09}} |
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| NFPA-F = 1 |
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| GHSSignalWord = Warning |
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| NFPA-R = 1 |
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| HPhrases = {{H-phrases|315|319|335|400}} |
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| RPhrases = {{R31}}, {{R36/37/38}}, {{R50}} |
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| PPhrases = {{P-phrases|261|273|305+351+338}} |
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| SPhrases = {{S2}}, {{S28}}, {{S61}} |
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}} |
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}} |
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| Section8 = {{Chembox Related |
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|Section8={{Chembox Related |
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| OtherAnions = ] |
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| OtherAnions = ] |
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| OtherCations = ]<br/>]<br/>] |
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| OtherCations = ]<br/>]<br/>] |
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| Function = ]s |
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| OtherFunction_label = ]s |
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| OtherFunctn = ] |
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| OtherFunction = ] |
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}} |
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}} |
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}} |
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}} |
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'''Calcium sulfide''' is the ] with the formula CaS. This white material crystallizes in cubes like rock salt. CaS has been studied as a component in a process that would recycle ], a product of ]. Like many salts containing ] ions, CaS typically has an odour of ], which results from small amount of this gas formed by hydrolysis of the salt. |
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'''Calcium sulfide''' is the ] with the formula ]]. This white material crystallizes in cubes like rock salt. CaS has been studied as a component in a process that would recycle ], a product of ]. Like many salts containing ] ions, CaS typically has an odour of ], which results from small amount of this gas formed by hydrolysis of the salt. |
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In terms of its atomic structure, CaS crystallizes in the same motif as ] indicating that the bonding in this material is highly ]. The high melting point is also consistent with its description as an ionic solid. In the crystal, each ] ion is surrounded by an ] of six Ca<sup>2+</sup> ions, and complementarily, each Ca<sup>2+</sup> ion surrounded by six S<sup>2<nowiki>−</nowiki></sup> ions. |
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In terms of its atomic structure, CaS crystallizes in the same motif as ] indicating that the bonding in this material is highly ]. The high melting point is also consistent with its description as an ionic solid. In the crystal, each ] ion is surrounded by an ] of six Ca<sup>2+</sup> ions, and complementarily, each Ca<sup>2+</sup> ion surrounded by six S<sup>2−</sup> ions. |
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==Production== |
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==Production== |
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CaS is produced by "carbothermic reduction" of ], which entails the conversion of carbon, usually as charcoal, to ]: |
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CaS is produced by ] of ], which entails the conversion of carbon, usually as charcoal, to ]: |
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:CaSO<sub>4</sub> + 2 C → CaS + 2 CO<sub>2</sub> |
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:CaSO<sub>4</sub> + 2 C → CaS + 2 CO<sub>2</sub> |
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and can react further: |
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and can react further: |
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:3 CaSO<sub>4</sub> + CaS → 4 CaO + 4 ] |
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:3 CaSO<sub>4</sub> + CaS → 4 ] + 4 ] |
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In the second reaction the ] (+6 ]) oxidizes the ] (-2 oxidation state) to ] (+4 oxidation state), while it is being reduced to sulfur dioxide itself (+4 oxidation state). |
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In the second reaction the ] (+6 ]) oxidizes the ] (-2 oxidation state) to ] (+4 oxidation state), while it is being reduced to sulfur dioxide itself (+4 oxidation state). |
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CaS is also a byproduct in the ], a once major industrial process for producing sodium carbonate. In that process sodium sulfide reacts with calcium carbonate:<ref>{{cite encyclopedia|author=Christian Thieme|title=Sodium Carbonates |encyclopedia=Ullmann's Encyclopedia of Industrial Chemistry|publisher=Wiley-VCH|location=Weinheim|year=2000|doi=10.1002/14356007.a24_299|isbn=978-3527306732}}</ref> |
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CaS is also a byproduct in the ]. |
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:Na<sub>2</sub>S + CaCO<sub>3</sub> → CaS + Na<sub>2</sub>CO<sub>3</sub> |
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Millions of tons of this calcium sulfide byproduct was discarded, causing extensive pollution and controversy.<ref name="Kiefer">{{cite journal |last1=Kiefer |first1=David M. |date=January 2002 |url=http://pubs.acs.org/subscribe/journals/tcaw/11/i01/html/01chemchron.html |title=It was all about alkali |journal=Today's Chemist at Work |volume=11 |issue=1 |pages=45–6}}</ref> |
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], Ca(OH)<sub>2</sub>, reacts with elemental sulfur to give a "]", which has been used as an ]. The active ingredient is probably a calcium ], not CaS.<ref>Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. {{ISBN|0-12-352651-5}}.</ref> |
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==Reactivity and uses== |
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==Reactivity and uses== |
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:CaS + H<sub>2</sub>O → Ca(SH)(OH) |
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:CaS + H<sub>2</sub>O → Ca(SH)(OH) |
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:Ca(SH)(OH) + H<sub>2</sub>O → Ca(OH)<sub>2</sub> + H<sub>2</sub>S |
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:Ca(SH)(OH) + H<sub>2</sub>O → Ca(OH)<sub>2</sub> + H<sub>2</sub>S |
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], Ca(OH)<sub>2</sub>, reacts with elemental sulfur to give a "]", which has been used as an ]. The active ingredient is probably a calcium ], not CaS.<ref>Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.</ref> |
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It reacts with ]s such as ] to release toxic ] gas. |
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It reacts with ]s such as ] to release toxic ] gas. |
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: CaS + 2 HCl → CaCl<sub>2</sub> + H<sub>2</sub>S |
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: CaS + 2 HCl → ] + H<sub>2</sub>S |
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Calcium sulfide is ], and will glow a blood red for up to an hour after a light source is removed.<ref>{{Cite web | url=https://www.technoglowproducts.com/red-glow-in-the-dark-powder-calcium-sulfide/ |title = Red Glow in the Dark Powder - Calcium Sulfide}}</ref> |
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As a noxious byproduct of the ], it can be converted to ] and ], the latter of which can be used as a sulfur source for the ] to produce the ] necessary for the Leblanc process: |
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:{{chem2| CaS(s) + CO2(g) + H2O(l) -> CaCO3(s) + H2S(g)}} |
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== Natural occurrence == |
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== Natural occurrence == |
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Oldhamite is the name for mineralogical form of CaS. It is a rare component of some meteorites and has scientific importance in solar nebula research. Burning of the coal dumps can also produce such compound. |
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] is the name for mineralogical form of CaS. It is a rare component of some meteorites and has scientific importance in solar nebula research.<ref>{{Cite web|url=https://www.mindat.org/min-2970.html|title=Oldhamite}}</ref><ref>{{Cite web|url=https://www.ima-mineralogy.org/Minlist.htm|title=List of Minerals|date=21 March 2011}}</ref> Burning of coal dumps can also produce the compound.<ref name="Kruszewski">{{cite journal |last1=Kruszewski|first1=Ł. |date=January 2006 |url=https://www.researchgate.net/publication/285329328 |title=Oldhamite-periclase-portlandite-fluorite assemblage and coexisting minerals of burnt dump in Siemianowice Ślaskie-Dabrówka Wielka area (Upper Silesia, Poland) - preliminary report |journal=Mineralogia Polonica - Special Papers |volume=28 |pages=118–120}}</ref> |
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==See also== |
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* ] |
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==References== |
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==References== |
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{{Reflist}} |
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<references/> |
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{{Calcium compounds}} |
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{{Calcium compounds}} |
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{{Sulfides}} |
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{{Meteorites}} |
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