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nks toggle the table of contents boiling point 96 languages afrikaans alemannisch aragonés العربية asturianu azərbaycanca bikol central беларуская тарашкевіца беларуская български বাংলা bosanski català čeština чӑвашла cymraeg dansk deutsch ελληνικά esperanto español eesti euskara فارسی suomi français frysk gaeilge galego gaelg עברית हिन्दी hrvatski kreyòl ayisyen magyar հայերեն interlingua jaku iban bahasa indonesia íslenska italiano 日本語 la lojban ქართული қазақша 한국어 kurdî кыргызча latina lombard lietuvių latviešu македонски മലയാളം монгол मराठी bahasa melayu မြန်မာဘာသာ plattdüütsch नेपाल भाषा nederlands norsk nynorsk norsk bokmål occitan oromoo ਪੰਜਾਬੀ polski پنجابی پښتو português runa simi română русский سنڌي srpskohrvatski српскохрватски සිංහල simple english slovenčina slovenščina shqip српски srpski sunda svenska kiswahili தமிழ் తెలుగు ไทย türkçe українська اردو oʻzbekcha ўзбекча tiếng việt 吴语 閩南語 bân lâm gí 粵語 中文 edit links article talk english read edit view history tools tools move to sidebar hide actions read edit view history general what links here related changes upload file permanent link page information cite this page get shortened url print export download as pdf printable version in other projects wikidata item appearance move to sidebar hide from wikipedia the free encyclopedia characteristic temperature for a substance this article is about the boiling point of liquids for other uses see boiling point disambiguation water boiling at 99 3 c 210 8 f at 215 m 705 ft elevation the boiling point of a substance is the temperature at which the vapor pressure of a liquid equals the pressure surrounding the liquid 1 2 and the liquid changes into a vapor the boiling point of a liquid varies depending upon the surrounding environmental pressure a liquid in a partial vacuum i e under a lower pressure has a lower boiling point than when that liquid is at atmospheric pressure because of this water boils at 100 c or with scientific precision 99 97 c 211 95 f under standard pressure at sea level but at 93 4 c 200 1 f at 1 905 metres 6 250 ft 3 altitude for a given pressure different liquids will boil at different temperatures the normal boiling point also called the atmospheric boiling point or the atmospheric pressure boiling point of a liquid is the special case in which the vapor pressure of the liquid equals the defined atmospheric pressure at sea level one atmosphere 4 5 at that temperature the vapor pressure of the liquid becomes sufficient to overcome atmospheric pressure and allow bubbles of vapor to form inside the bulk of the liquid the standard boiling point has been defined by iupac since 1982 as the temperature at which boiling occurs under a pressure of one bar 6 the heat of vaporization is the energy required to transform a given quantity a mol kg pound etc of a substance from a liquid into a gas at a given pressure often atmospheric pressure liquids may change to a vapor at temperatures below their boiling points through the process of evaporation evaporation is a surface phenomenon in which molecules located near the liquid s edge not contained by enough liquid pressure on that side escape into the surroundings as vapor on the other hand boiling is a process in which molecules anywhere in the liquid escape resulting in the formation of vapor bubbles within the liquid saturation temperature and pressure edit demonstration of the lower boiling point of alcohol at lower pressure achieved by using a vacuum pump main article vapor liquid equilibrium a saturated liquid contains as much thermal energy as it can without boiling or conversely a saturated vapor contains as little thermal energy as it can without condensing saturation temperature means boiling point the saturation temperature is the temperature for a corresponding saturation pressure at which a liquid boils into its vapor phase the liquid can be said to be saturated with thermal energy any addition of thermal energy results in a phase transition if the pressure in a system remains constant isobaric a vapor at saturation temperature will begin to condense into its liquid phase as thermal energy heat is removed similarly a liquid at saturation temperature and pressure will boil into its vapor phase as additional thermal energy is applied the boiling point corresponds to the temperature at which the vapor pressure of the liquid equals the surrounding environmental pressure thus the boiling point is dependent on the pressure boiling points may be published with respect to the nist usa standard pressure of 101 325 kpa 1 atm or the iupac standard pressure of 100 000 kpa 1 bar at higher elevations where the atmospheric pressure is much lower the boiling point is also lower the boiling point increases with increased pressure up to the critical point where the gas and liquid properties become identical the boiling point cannot be increased beyond the critical point likewise the boiling point decreases with decreasing pressure until the triple point is reached the boiling point cannot be reduced below the triple point if the heat of vaporization and the vapor pressure of a liquid at a certain temperature are known the boiling point can be calculated by using the clausius clapeyron equation thus t b 1 t 0 r ln p p 0 δ h vap 1 displaystyle t_ text b left frac 1 t_ 0 frac r ln frac p p_ 0 delta h_ text vap right 1 where t b displaystyle t_ text b is the boiling point at the pressure of interest r displaystyle r is the ideal gas constant p displaystyle p is the vapor pressure of the liquid p 0 displaystyle p_ 0 is some pressure where the corresponding t 0 displaystyle t_ 0 is known usually data available at 1 atm or 100 kpa 1 bar δ h vap displaystyle delta h_ text vap is the heat of vaporization of the liquid t 0 displaystyle t_ 0 is the boiling temperature ln displaystyle ln is the natural logarithm saturation pressure is the pressure for a corresponding saturation temperature at which a liquid boils into its vapor phase saturation pressure and saturation temperature have a direct relationship as saturation pressure is increased so is saturation temperature if the temperature in a system remains constant an isothermal system vapor at saturation pressure and temperature will begin to condense into its liquid phase as the system pressure is increased similarly a liquid at saturation pressure and temperature will tend to flash into its vapor phase as system pressure is decreased there are two conventions regarding the standard boiling point of water the normal boiling point is commonly given as 100 c 212 f actually 99 97 c 211 9 f following the thermodynamic definition of the celsius scale based on the kelvin at a pressure of 1 atm 101 325 kpa the iupac recommended standard boiling point of water at a standard pressure of 100 kpa 1 bar 7 is 99 61 c 211 3 f 6 8 for comparison on top of mount everest at 8 848 m 29 029 ft elevation the pressure is about 34 kpa 255 torr 9 and the boiling point of water is 71 c 160 f 10 the celsius temperature scale was defined until 1954 by two points 0 c being defined by the water freezing point and 100 c being defined by the water boiling point at standard atmospheric pressure relation between the normal boiling point and the vapor pressure of liquids edit a log lin vapor pressure chart for various liquids the higher the vapor pressure of a liquid at a given temperature the lower the normal boiling point i e the boiling point at atmospheric pressure of the liquid the vapor pressure chart to the right has graphs of the vapor pressures versus temperatures for a variety of liquids 11 as can be seen in the chart the liquids with the highest vapor pressures have the lowest normal boiling points for example at any given temperature methyl chloride has the highest vapor pressure of any of the liquids in the chart it also has the lowest normal boiling point 24 2 c which is where the vapor pressure curve of methyl chloride the blue line intersects the horizontal pressure line of one atmosphere atm of absolute vapor pressure the critical point of a liquid is the highest temperature and pressure it will actually boil at see also vapour pressure of water boiling point of chemical elements edit further information list of chemical elements and boiling points of the elements data page the element with the lowest boiling point is helium both the boiling points of rhenium and tungsten exceed 5000 k at standard pressure because it is difficult to measure extreme temperatures precisely without bias both have been cited in the literature as having the higher boiling point 12 boiling point as a reference property of a pure compound edit as can be seen from the above plot of the logarithm of the vapor pressure vs the temperature for any given pure chemical compound its normal boiling point can serve as an indication of that compound s overall volatility a given pure compound has only one normal boiling point if any and a compound s normal boiling point and melting point can serve as characteristic physical properties for that compound listed in reference books the higher a compound s normal boiling point the less volatile that compound is overall and conversely the lower a compound s normal boiling point the more volatile that compound is overall some compounds decompose at higher temperatures before reaching their normal boiling point or sometimes even their melting point for a stable compound the boiling point ranges from its triple point to its critical point depending on the external pressure beyond its triple point a compound s normal boiling point if any is higher than its melting point beyond the critical point a compound s liquid and vapor phases merge into one phase which may be called a superheated gas at any given temperature if a compound s normal boiling point is lower then that compound will generally exist as a gas at atmospheric external pressure if the compound s normal boiling point is higher then that compound can exist as a liquid or solid at that given temperature at atmospheric external pressure and will so exist in equilibrium with its vapor if volatile if its vapors are contained if a compound s vapors are not contained then some volatile compounds can eventually evaporate away in spite of their higher boiling points boiling points of alkanes alkenes ethers halogenoalkanes aldehydes ketones alcohols and carboxylic acids as a function of molar mass in general compounds with ionic bonds have high normal boiling points if they do not decompose before reaching such high temperatures many metals have high boiling points but not all very generally with other factors being equal in compounds with covalently bonded molecules as the size of the molecule or molecular mass increases the normal boiling point increases when the molecular size becomes that of a macromolecule polymer or otherwise very large the compound often decomposes at high temperature before the boiling point is reached another factor that affects the normal boiling point of a compound is the polarity of its molecules as the polarity of a compound s molecules increases its normal boiling point increases other factors being equal closely related is the ability of a molecule to form hydrogen bonds in the liquid state which makes it harder for molecules to leave the liquid state and thus increases the normal boiling point of the compound simple carboxylic acids dimerize by forming hydrogen bonds between molecules a minor factor affecting boiling points is the shape of a molecule making the shape of a molecule more compact tends to lower the normal boiling point slightly compared to an equivalent molecule with more surface area comparison of butane c 4 h 10 isomer boiling points common name n butane isobutane iupac name butane 2 methylpropane molecular form boiling point c 0 5 11 7 comparison of pentane isomer boiling points common name n pentane isopentane neopentane iupac name pentane 2 methylbutane 2 2 dimethylpropane molecular form boiling point c 36 0 27 7 9 5 binary boiling point diagram of two hypothetical only weakly interacting components without an azeotrope most volatile compounds anywhere near ambient temperatures go through an intermediate liquid phase while warming up from a solid phase to eventually transform to a vapor phase by comparison to boiling a sublimation is a physical transformation in which a solid turns directly into vapor which happens in a few select cases such as with carbon dioxide at atmospheric pressure for such compounds a sublimation point is a temperature at which a solid turning directly into vapor has a vapor pressure equal to the external pressure impurities and mixtures edit in the preceding section boiling points of pure compounds were covered vapor pressures and boiling points of substances can be affected by the presence of dissolved impurities solutes or other miscible compounds the degree of effect depending on the concentration of the impurities or other compounds the presence of non volatile impurities such as salts or compounds of a volatility far lower than the main component compound decreases its mole fraction and the solution s volatility and thus raises the normal boiling point in proportion to the concentration of the solutes this effect is called boiling point elevation as a common example salt water boils at a higher temperature than pure water in other mixtures of miscible compounds components there may be two or more components of varying volatility each having its own pure component boiling point at any given pressure the presence of other volatile components in a mixture affects the vapor pressures and thus boiling points and dew points of all the components in the mixture the dew point is a temperature at which a vapor condenses into a liquid furthermore at any given temperature the composition of the vapor is different from the composition of the liquid in most such cases in order to illustrate these effects between the volatile components in a mixture a boiling point diagram is commonly used distillation is a process of boiling and usually condensation which takes advantage of these differences in composition between liquid and vapor phases boiling point of water with elevation edit following is a table of the change in the boiling point of water with elevation at intervals of 500 meters over the range of human habitation the dead sea at 430 5 metres 1 412 ft to la rinconada peru at 5 100 m 16 700 ft then of 1 000 meters over the additional range of uninhabited surface elevation up to mount everest at 8 849 metres 29 032 ft along with a similar range in imperial boiling point of water elevation m boiling point c elevation ft boiling point f 500 101 6 1 500 214 7 0 100 0 0 212 0 500 98 4 1 500 209 3 1 000 96 7 3 000 206 6 1 500 95 1 4 500 203 9 2 000 93 4 6 000 201 1 2 500 91 7 7 500 198 3 3 000 90 0 9 000 195 5 3 500 88 2 10 500 192 6 4 000 86 4 12 000 189 8 4 500 84 6 13 500 186 8 5 000 82 8 15 000 183 9...