Editing Propane (section)

{{short description|Hydrocarbon compound}}
{{SM|Liquefied petroleum gas|discuss=Talk:Propane#Proposed move of content from Propane article to LPG article|date=August 2024}}
{{Distinguish|propene|propyne}}
{{Chembox
| Watchedfields  = changed
| verifiedrevid  = 464375285
| ImageFileL1    = Propane-2D-Skeletal.svg
| ImageClassL1 = skin-invert-image
| ImageFileL1_Ref = {{chemboximage|correct|??}}
| ImageNameL1    = Skeletal formula of propane
| ImageFileR1    = PropaneFull.png
| ImageClassR1 = skin-invert-image
| ImageFileR1_Ref = {{chemboximage|correct|??}}
| ImageNameR1    = Skeletal formula of propane with all implicit carbons shown, and all explicit hydrogens added
| ImageFileL2    = Propane-3D-balls-B.png
| ImageClassL2 = bg-transparent
| ImageFileL2_Ref = {{chemboximage|correct|??}}
| ImageNameL2    = Ball and stick model of propane
| ImageFileR2    = Propane-3D-vdW-B.png
| ImageClassR2 = bg-transparent
| ImageFileR2_Ref = {{chemboximage|correct|??}}
| ImageNameR2    = Spacefill model of propane
| PIN            = Propane<ref name=iupac2013>{{cite book | title =  Nomenclature of Organic Chemistry : IUPAC Recommendations and Preferred Names 2013 (Blue Book) | chapter = General Principles, Rules, and Conventions | publisher = [[Royal Society of Chemistry|The Royal Society of Chemistry]] | date = 2014 | location = Cambridge | at = P-12.1 | doi = 10.1039/9781849733069-00001 | isbn = 978-0-85404-182-4 | quote = Similarly, the retained names 'ethane', 'propane', and 'butane' were never replaced by systematic names 'dicarbane', 'tricarbane', and 'tetracarbane' as recommended for analogues of silane, 'disilane’; phosphane, 'triphosphane'; and sulfane, 'tetrasulfane'.}}</ref>
| SystematicName = Tricarbane (never recommended<ref name=iupac2013 />)
| Section1       = {{Chembox Identifiers
| CASNo = 74-98-6
| CASNo_Ref = {{cascite|correct|CAS}}
| PubChem = 6334
| ChemSpiderID = 6094
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
| UNII = T75W9911L6
| UNII_Ref = {{fdacite|correct|FDA}}
| EINECS = 200-827-9
| UNNumber = 1978
| KEGG = D05625
| KEGG_Ref = {{keggcite|correct|kegg}}
| ChEBI = 32879
| ChEBI_Ref = {{ebicite|correct|EBI}}
| ChEMBL = 135416
| ChEMBL_Ref = {{ebicite|correct|EBI}}
| RTECS = TX2275000
| Beilstein = 1730718
| Gmelin = 25044
| SMILES = CCC
| StdInChI = 1S/C3H8/c1-3-2/h3H2,1-2H3
| StdInChI_Ref = {{stdinchicite|correct|chemspider}}
| StdInChIKey = ATUOYWHBWRKTHZ-UHFFFAOYSA-N
| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
}}
| Section2       = {{Chembox Properties
| Properties_ref = <ref name="GESTIS">{{GESTIS|ZVG=10020|Name=Propane}}</ref>
| C=3 | H=8
| Appearance = Colorless gas
| Odor = Odorless
| Density = 2.0098&nbsp;kg/m<sup>3</sup> (at 0&nbsp;°C, 101.3&nbsp;kPa)
| MeltingPtK = 85.5
| BoilingPtK = 230.9 to 231.11
| CriticalTP = {{cvt|370|K}}, {{cvt|4.23|MPa|atm}}
| Solubility = 47&nbsp;mg⋅L<sup>−1</sup> (at 0&nbsp;°C)
| LogP = 2.236
| VaporPressure = 853.16&nbsp;kPa (at {{convert|21.1|C}})
| HenryConstant = 15&nbsp;nmol⋅Pa<sup>−1</sup>⋅kg<sup>−1</sup>
| MagSus = −40.5&nbsp;×&nbsp;10<sup>−6</sup>&nbsp;cm<sup>3</sup>/mol
| ConjugateAcid = [[Propanium]]
| Dipole = 0.083&nbsp;D<ref>{{cite journal |title= Microwave Spectrum, Structure, and Dipole Moment of Propane |journal= J. Chem. Phys. |volume= 33 |issue= 5 |pages= 1514–1518 |year= 1960 |doi= 10.1063/1.1731434 |first= David R. Jr. |last= Lide |bibcode= 1960JChPh..33.1514L }}</ref>
}}
| Section3       = {{Chembox Thermochemistry
| DeltaHf = −105.2–104.2&nbsp;kJ⋅mol<sup>−1</sup>
| DeltaHc = −2.2197–2.2187&nbsp;MJ⋅mol<sup>−1</sup>
| HeatCapacity = 73.60&nbsp;J⋅K<sup>−1</sup>⋅mol<sup>−1</sup>
}}
| Section4       = {{Chembox Hazards
| GHSPictograms = {{GHS02}}
| GHSSignalWord = '''DANGER'''
| HPhrases = {{H-phrases|220}}
| PPhrases = {{P-phrases|210}}
| NFPA-H = 2
| NFPA-F = 4
| NFPA-R = 0
| NFPA-S = 
| FlashPtC = −104
| AutoignitionPtC = 470
| ExploLimits = 2.37–9.5%
| PEL = TWA 1,000&nbsp;ppm (1,800&nbsp;mg/m<sup>3</sup>)<ref name=PGCH>{{PGCH|0524}}</ref>
| IDLH = 2,100&nbsp;ppm<ref name=PGCH />
| REL = TWA 1,000&nbsp;ppm (1,800&nbsp;mg/m<sup>3</sup>)<ref name=PGCH />
}}<ref>{{cite web|url=http://cameochemicals.noaa.gov/chemical/9018|title=PROPANE – CAMEO Chemicals – NOAA|publisher=NOAA Office of Response and Restoration, US GOV|website=cameochemicals.noaa.gov}}</ref>
| Section5       = {{Chembox Related
| OtherFunction_label = alkanes
| OtherFunction = {{unbulleted list|[[ethane]]|[[butane]]|[[isobutane]]}}
| OtherCompounds = {{unbulleted list|[[propene]]|[[allene]]|[[cyclopropane]]|}}
}}
}}
[[File:Propane tank 20lb.jpg|thumb|A 20 lb ({{nowrap|9.1 kg}}) steel propane cylinder. This cylinder is fitted with an overfill prevention device (OPD) valve, as evidenced by the trilobular handwheel.]]
'''Propane''' ({{IPAc-en|ˈ|p|r|oʊ|p|eɪ|n}}) is a three-[[carbon]] [[alkane]] with the molecular formula {{Chem2|C3H8}}. It is a gas at [[standard temperature and pressure]], but compressible to a transportable liquid. A [[by-product]] of [[natural gas]] processing and [[petroleum]] refining, it is often a constituent of [[liquefied petroleum gas]] (LPG), which is commonly used as a [[fuel]] in domestic and industrial applications and in low-emissions public transportation; other constituents of LPG may include [[propene|propylene]], [[butane]], [[butene|butylene]], [[butadiene]], and [[isobutylene]]. Discovered in 1857 by the French chemist [[Marcellin Berthelot]], it became commercially available in the US by 1911.  Propane has lower volumetric energy density than gasoline or coal, but has higher gravimetric energy density than them and burns more cleanly.<ref>{{Cite web |title=Fuels |url=https://www.globalfueleconomy.org/transport/gfei/autotool/approaches/technology/fuels.asp |access-date=2022-04-12 |website=www.globalfueleconomy.org}}</ref>

Propane gas has become a popular choice for barbecues and portable stoves because its low −42&nbsp;°C [[boiling point]] makes it vaporise inside pressurised liquid containers (it exists in two phases, vapor above liquid). It retains its ability to vaporise even in cold weather, making it better-suited for outdoor use in cold climates than alternatives with higher boiling points like butane.<ref>{{cite web |title=The difference between butane and propane |url=https://www.calor.co.uk/news-and-views/the-difference-between-butane-and-propane |website=Calor Gas News and Views |publisher=Calor Gas Ltd UK}}</ref> LPG powers buses, forklifts, automobiles, outboard boat motors, and [[Ice resurfacer|ice resurfacing machines]], and is used for heat and cooking in [[recreational vehicle]]s and [[Campervan|campers]]. Propane is becoming popular as a replacement refrigerant (R290) for heatpumps also as it offers greater efficiency than the current refrigerants: R410A / R32, higher temperature heat output and less damage to the atmosphere for escaped gasses—at the expense of high gas flammability.<ref>{{Cite web |title=Propane |url=https://vasa.org.au/transition-to-latest-ghs-7-chemical-id-system-starts-in-2021/ |access-date=2024-05-11 |website=vasa.org.au}}</ref>