review article solubility parameters of permanent gases...hildebrand solubility parameters. e values...

Review ArticleSolubility Parameters of Permanent Gases

Yizhak Marcus

Institute of Chemistry The Hebrew University of Jerusalem 91904 Jerusalem Israel

Correspondence should be addressed to Yizhak Marcus ymarcusvmshujiacil

Received 14 August 2016 Accepted 9 October 2016

Academic Editor Tomokazu Yoshimura

Copyright copy 2016 Yizhak Marcus This is an open access article distributed under the Creative Commons Attribution Licensewhich permits unrestricted use distribution and reproduction in any medium provided the original work is properly cited

The solubility parameters 120575H(119879b) of nonreactive permanent gases at their boiling points 119879b (lt290K) are calculated fromindividually discussed values of their molar enthalpies of vaporization and densities obtained from the literature These valuesare tabulated and where available the coefficients of the temperature dependence expression 120575H(119879) are also tabulated The trendsnoted in the 120575H(119879b) values are dealt with and the values are compared with those reported in the literature and derived from thesolubilities of the gases in various solvents The 120575H(119879b) values are shown to correlate linearly with the depths of the potential wells(attractive interaction energies 120576119896B) for binary collisions of the gaseous molecules and with the surface tensions 120590(119879b) of theliquefied gases

1 Introduction

The solubility of gases in liquid solvents is an important issuein many fields of chemistry and chemical engineering fromprocessing to environmental elimination In this review thesolubility of permanent nonreactive gases is dealt with interms of their solubility parameters at the normal boilingpoints of the liquefied gases and their temperature depen-dence Permanent gases are those substances that are gaseousat ambient conditions that is at atmospheric pressure andle290K Nonreactive gases include those that dissolve intheir molecular (atomic for noble gases) form in the sol-vents without causing chemical changes in them This limitexcludes gases like F2 Cl2 the hydrogen halides NO2 anda few others Still this review is not exhaustive but attemptsto include practically all the inorganic gases and most ofthe organic ones up to butane The normal boiling points119879b of the liquefied gases are selected because the requireddata mainly pertain to these conditions (at which the vaporpressures of the saturated liquefied gases reach 101325 kPa orone atm) 119879b are also considered to be ldquocorresponding statesrdquoas is indicated by the Trouton constant (the molar entropyof vaporization at 119879b) being the same ΔV119878(119879b) = 105119877 forordinary (nonassociating) liquids

11 Gas Solubility from Regular Solution Theory The gasesdealt with here are generally non- or only mildly polar and

their solubilities can be described by means of the regularsolution theory of Hildebrand [1] This states that the molefraction solubility 119909G of the solute gas (subscript G) in theliquid solvent (subscript S) is as follows

ln119909G = ln119909Gid minus (119881G119877119879) (120575HG minus 120575HS)2 (1)

where 119881G is the molar volume and the two 120575Hrsquos are the total(Hildebrand) solubility parametersThe ideal solubility at thetemperature 119879 119909Gid is given by

ln119909Gid = (ΔV119867G (119879b)119877 ) (119879bminus1 minus 119879minus1) (2)

where ΔV119867G(119879b) is the molar enthalpy of vaporization ofthe liquefied solute gas at its normal boiling point 119879b In thecases of polar solutes or solvents or those prone to hydrogenbonding the partial (Hansen) solubility parameters [2] ofsuch solvents should be used instead for the prediction of thegas solubilities but this needs not concern much the presentreview The solubility parameters of liquid solvents 120575HS areavailable in compilations for molecular [3 4] and ionic [5 6]solvents

The solubility of a gas in a liquid is often expressed as theHenry constant 119867G(S) which is related to the mole fractionsolubility in the solvent 119909G(S) as follows

Hindawi Publishing CorporationJournal of ChemistryVolume 2016 Article ID 4701919 18 pageshttpdxdoiorg10115520164701919

2 Journal of Chemistry

119867G(S) = 119901G119909G(S) (3)

where 119901G is the partial pressure of the gas that is at equilib-rium with its saturated solution Hence the larger the mea-sured Henry constant the smaller the actual (mole fraction)solubility The solubility of a permanent gas is generally notneeded at its normal boiling point but 120575HG(119879b) is a referencevalue from which the temperature dependence of 120575HG canbe used to obtain the value at the desired temperature Suchtemperature dependence data unfortunately are available foronly a minority of gaseous solutes

12 Hildebrand Solubility Parameters The values of the total(Hildebrand) solubility parameter of the gases dealt withhere 120575HG are obtained as the square roots of the cohesiveenergy densities 119888119890119889GThe latter are obtained from themolarenthalpies of vaporization and the molar volumes assumingthe liquefied gas vaporizes without association or dissociationto an ideal gas at 119879b that is at 101325 kPa as follows

119888119890119889G = 120575HG2 = (ΔV119867G (119879b) minus 119877119879b)119881G (119879b) (4)

2 The Required Data

In the following the subscript G is dropped because onlythe solute gases are being dealt with The required data forobtaining the solubility parameters 120575H are the normal boilingpoints of the liquefied gases 119879b their molar enthalpies ofvaporizationΔV119867(119879b) and their molar volumes119881(119879b) at theboiling point The molar volumes 119881 are obtained from theratios of the molar masses119872 and the densities 120588 119881 = 119872120588The molar volume is also the reciprocal of the concentration119888 119881cm3molminus1 = 1000(119888mol dmminus3) The molar masses andboiling points are taken from the Handbook [7] The otherquantities are obtained from the literature from primarysources as noted below when readily available or else fromsecondary sources (compilations) such as [8ndash11]

Following are details of the data used and the results ofthe application of (2) yielding 120575H(119879b)MPa12 values

21 Specific Data for Each Gas

211 Helium The earliest report of the solubility parameterof helium is that of Clever et al [20] derived from itssolubility in hydrocarbons and fluorocarbons and is tabu-lated at the normal boiling point as 05 cal12 cmminus32 (ie102MPa12) However the text above the table states that06 cal12 cmminus32 (ie 123MPa12) is ldquomore compatible withthe solubility parameter at the gas bprdquo The subsequentreport by Yosim andOwens [21] evaluated themolar enthalpyof vaporization using the scaled particle theory but reportedalso its experimental value and the density at the boilingpoint [22] fromwhich the value 120MPa12 is derivableThemost recent report is by Donnelly and Barenghi [23] whopresented density and vapor pressure data at 005 K intervalsaround the boiling point that interpolate to 119879b = 422K and

120588(119879b) = 01250 g cmminus3 They also presented four reports forΔV119867 at 4207K that average at 8304 plusmn 037 Jmolminus1 fromwhich the solubility parameter 120575H(119879b) = 122 plusmn 001MPa12is derived and represents the selected value

212 Neon The 120575H(119879b) value tabulated by Clever et al[20] obtained as described for He is 49 cal12 cmminus32 (ie1002MPa12) The value 120575H(119879b) = 949MPa12 is derivedfrom the [22] data reported byYosim andOwens [21] Linfordand Thornhill [24] reported the energy of vaporization asΔV119864(119879b) (presumably ΔV119867 minus 119877119879b) = 037 kcalmolminus1 andwith the density from Gladun [25] 006093mol cmminus3 thevalue 120575H(119879b) = 898MPa12 is derived Leonhard and Deiters[26] reported the densities and the molar enthalpy of thegas and liquid at 5 K intervals between 25 and 40K Thedifference in the latter yields ΔV119867 values so the expressionshown in Table 3 results fromwhich follows the value 120575H(119879b)= 1001MPa12 The value 120575H(119879b) = 1001MPa12 from [26]agreeing with that of [20] is adopted as the selected value forNe

213 Argon The 120575H(119879b) value tabulated by Clever et al[20] obtained as described for He is 70 cal12 cmminus32 (ie1432MPa12) The value 120575H(119879b) = 1419MPa12 is derivedfrom the data of [22] reported by Yosim and Owens [21]Much lower values were reported by Prausnitz and Shair[27] at an unspecified temperature 533 (calcm3)12 (ie1090MPa12) that was quoted by LaPack et al [28] Chenet al [29] presented the molar volumes and the molarenthalpies of vaporization or Ar at 17 temperatures betweenthe triple and boiling points from which the expressionfor the solubility parameter shown in Table 3 results and120575H(119879b) = 1407MPa12 Linford and Thornhill [24] reportedthe energy of vaporization as ΔV119864(119879b) = 1385 kcalmolminus1and with the molar volume from Terry et al [30] 119881(119879b) =28713 cm3molminus1 the value 120575H(119879b) = 1421MPa12 is derivedThe average of the four agreeing values 1421 plusmn 010MPa12is adopted as the representative value for 120575H(119879b)214 Krypton The 120575H(119879b) value tabulated by Clever et al[20] obtained as described for He is 75 cal12 cmminus32 (ie1534MPa12) The value 120575H(119879b) = 1521MPa12 is derivedfrom the data of [22] reported by Yosim and Owens [21]Much lower values were reported by Prausnitz and Shair[27] at an unspecified temperature 64 (calcm3)12 (ie1309MPa12) Chen et al [29] presented the molar vol-umes and the molar enthalpies of vaporization of Kr at 19temperatures between the triple and boiling points fromwhich the expression for the solubility parameter shown inTable 3 results and 120575H(119879b) = 1518MPa12 Linford andThorn-hill [24] reported the energy of vaporization as ΔV119864(119879b)= 200 kcalmolminus1 and with the molar volume from Terryet al [30] 119881(119879b) = 34731 cm3molminus1 the value 120575H(119879b) =1457MPa12 is derived The average of the three agreeingvalues 1524 plusmn 009MPa12 is adopted as the representativevalue for 120575H(119879b)

Journal of Chemistry 3

215 Xenon The 120575H(119879b) value tabulated by Clever et al[20] obtained as described for He is 80 cal12 cmminus32 (ie1636MPa12) The value 120575H(119879b) = 1619MPa12 is derivedfrom the data of [22] reported by Yosim and Owens [21]Chen et al [29] presented the molar volumes and the molarenthalpies of vaporization of Xe at 17 temperatures betweenthe triple and boiling points from which the expression forthe solubility parameter shown inTable 3 results and 120575H(119879b)=1579MPa12 Linford andThornhill [24] reported the energyof vaporization as ΔV119864(119879b) = 269 kcalmolminus1 and with themolar volume fromTerry et al [30]119881(119879b)= 4468 cm3molminus1

(interpolated) the value 120575H(119879b) = 1487MPa12 is derivedThe average of the three largest values 161 plusmn 03MPa12 isadopted as the representative value for 120575H(119879b)216 Radon Prausnitz and Shair [27] reported a low value(compared with the other noble gases) at an unspecifiedtemperature 683 (calcm3)12 (ie 1397MPa12) A valuebetter compatible with the other noble gases was reportedby Lewis et al [31] 842 plusmn 011 cal12 cmminus32 (ie 1722 plusmn023MPa12) at an unspecified temperature derived from thesolubility of Rn in fluorocarbon solvents The molar enthalpyof vaporization ΔV119867 = 1636 kJmolminus1 and the liquid density120588 = 4329 kgmminus3 reported recently by Mick et al [32] at theboiling point of 222Rn 2105 K were obtained from MonteCarlo simulations leading to 120575H(119879b) = 1688MPa12 Micket al quoted experimental values obtained more than 100years ago for the enthalpy of vaporization ΔV119867kJmolminus1 =1659 and 1678 but not highly accurate liquid densities Withthe density from the simulation these two enthalpy valuesyield 120575H(119879b)kJmolminus1 = 1701 and 1712MPa12 The averageof the four agreeing values 1706 plusmn 015 is selected here asrepresentative

217 Hydrogen Yosim and Owens [21] quoted ΔV119867 datafrom Stull and Sinke [33] leading to 120575H(119879b) = 508MPa12Linford and Thornhill [24] reported the energy of vapor-ization as ΔV119864(119879b) = 0175 kcalmolminus1 and with the molarvolume from Van Itterbeek et al [34] interpolated to 119879b119881(119879b) = 28375 cm3molminus1 the value 120575H(119879b) = 508MPa12 isderived The reference data by Leachman et al [35] showedliquid density and gas and liquid molar enthalpy values attemperatures between 14 and 21 K that yield the expressionshown in Table 3 and 120575H(119879b) = 508MPa12 Sistla et al [36]quote Hansen [2] and report 120575d = 51MPa12 at 298K and1 atm for the dispersion partial solubility parameter The wellagreeing value from three authors 120575H(119879b) = 508MPa12 isthe selected value

218 Nitrogen Gjaldbaek and Hildebrand [37] assigned tonitrogen the value 120575H = 53 cal12 cmminus32 (1084MPa12) inorder to fit its solubility in several solvents at 298KYosim andOwens [21] quoted ΔV119867 data from Rossini et al [9] leadingto 120575H(119879b)= 1196MPa12 Linford andThornhill [24] reportedthe energy of vaporization as ΔV119864(119879b) = 118 kcalmolminus1 andwith the molar volume from Terry et al [30] 3491 cm3molminus1

the value 120575H(119879b) = 1189MPa12 is derived Jordan et al [38]reported the molar enthalpy of vaporization from the Hand-book [7] 5569 Jmolminus1 and the density 120588 = 08801 g cmminus3at 119879b = 7735 K yielding 120575H(119879b) = 1192 The experimentallatent heat of vaporization (at an unspecified temperaturepresumably119879b) of 2012 J gminus1 yieldswith 120588=08801 g cmminus3 thevalue 120575H(119879b) = 1202 Sistla et al [36] quote Hansen [2] andreport 120575d = 119MPa12 at 298K and 1 atm for the dispersionpartial solubility parameter The mean value from the fivemutually agreeing reports 120575H(119879b) = 1195 is selected here

219 Oxygen Suyama and Oishi [39] quoted earlier-published molar enthalpies of vaporization at the boilingpoint that agree with their own value 68227 Jmolminus1 Thisvalue is somewhat larger than that used by Yosim and Owens[21] from Kelley and King [40] 6812 Jmolminus1 These twovalues with the molar volume interpolated in Terry et al[30] data 28135 cm3molminus1 yield the solubility parameters120575H(119879b)MPa12 = 1469 and 1468 respectively A muchlower value at an unspecified temperature was reported byPrausnitz and Shair [27] 120575H = 40 (calcc)12 818MPa12quoted by LaPack et al [28] A value was also derivedfrom the molar energy of vaporization at the boiling pointreported by Linford andThornhill [24] 145 kcalmolminus1 yield-ing 120575H(119879b)MPa12 = 1469 Molecular dynamics simulationsby Zasetsky and Svishchev [41] yielded ΔV119867Jmolminus1 = 69346232 and 5083 at 119879K = 84 100 and 120 respectively Theseyield with the density data the following solubility parametervalues 120575H(119879)MPa12 = 1511 1356 and 1113 at these threetemperatures interpolating to 120575H(119879b)MPa12 = 1455 andyielding the data shown in Table 3 Sistla et al [36] quoteHansen [2] and report 120575d = 119MPa12 at 298K and 1 atmfor the dispersion partial solubility parameter From the fouragreeing values at the boiling point the average 120575H(119879)MPa12= 1464 plusmn 007 is taken as selected

2110 Boron Trifluoride No data regarding the molarenthalpy of vaporization of liquid BF3 were found exceptfor the entry in the Handbook [7] that was not traced toa definite reference of ΔV119867Jmolminus1 = 19330 The boilingpoint was given there as minus101∘C that is 1722 K The densityof liquid BF3 was obtained from Fischer and Weidemann[42] as 120588(119905∘C)g cmminus3 = 168[1 minus 00023(119905 + 128)] that is15757 g cmminus3 at 119879b These data yield 120575H(119879b)MPa12 = 2039but there is no corroboration of this value from any othersource

2111 Boron Trichloride Thevapor pressure of liquefied BCl3was reported by Fetisov et al [43] as log119901 = 74311 minus12980119879 from which by the Clausius-Clapeyron expressionΔV119867 = 1198771198792(119889 ln119901119889119879) = 24840 Jmolminus1 at 119879b = 1265∘C[7] = 2858 K (119879b = 121∘C was given in [43] and ΔV119867(119879b) =2377 kJmolminus1 was given in [7])The density of liquefied BCl3was reported by Ward [44] from minus44 to +5∘C being linearwith the temperature and a brief extrapolation to119879b = 1265∘Cyields 120588(119905∘C)g cmminus3 = 13472 (extrapolation to 110∘C yields120588g cmminus3 = 13493 in agreement with the value reported


by Briscoe et al [45]) These data yield 120575H(119879b)MPa12= 1607

2112 Carbon Monoxide Prausnitz and Shair [27] reported120575H = 313 (calcc)12 that is 640MPa12 a very low valuecompared to other reports Yosim and Owens [21] used theΔV119867 data of Kelley and King [40] from which the value120575H(119879b)MPa12 = 1237 is derived Goodwin [46] presentedenthalpy of vaporization and density data from the meltingto the boiling points that yield the expression shown inTable 3 and 120575H(119879b)MPa12 = 1229 Linford andThornhill [24]reported 128 kcalmolminus1 for the molar energy of vaporizationat the boiling point yielding with the molar volume dataof Terry et al [30] interpolated to 119879b 119881 = 3553 cm3molminus1

and the value 120575H(119879b)MPa12 = 1227 Barreiros et al [47]reported the molar enthalpy of vaporization and the molarvolume at 80 to 125K and at the boiling point 5991 kJmolminus1

and 35373 cm3molminus1 from which 120575H(119879b)MPa12 = 1226 isderived The temperature dependence at temperatures abovethose in Goodwinrsquos paper [46] is shown in Table 3 Prausnitzand Shair [27] quote Hansen [2] and report 120575d = 115MPa12at 298K and 1 atm for the dispersion partial solubilityparameter but the total Hildebrand solubility parameterincluded a contribution from the polar interactions of thesegas molecules adding up to 120575H(298K)MPa12 = 1250 Theaverage of the four agreeing values 120575H(119879b)MPa12 = 1230 plusmn005 is taken as selected

2113 Carbon Dioxide Carbon dioxide sublimes from thesolid to the gas without passing at ambient pressures througha liquid phase Prausnitz and Shair [27] reported 120575H =60 (calcc)12 that is 1237MPa12 quoted as 123MPa12by LaPack et al [28] at an unspecified temperature avalue comparable to some other reports Span and Wagner[48] reported data over a wide temperature range for boththe molar enthalpy and the density of the condensed andgaseous phases from which the expression shown in Table 3is derived for temperatures between the triple point 119879t =21659 K and 119879 = 29815 K from which 120575H(119879t)MPa12 =1910 and 120575H(29815 K)MPa12 = 678 result a wide spanof values Politzer et al [49] predicted from ab initiocomputations for CO2 the heats of formation at 29815 Kas Δ f119867kcalmolminus1 = minus923 for the gas and minus966 for theliquid yielding ΔV119867Jmolminus1 = 17991 for the difference thatis for vaporization of the liquid With the density at 119879t =117846 g cmminus3 this yields 120575H(119879t)MPa12 = 2082 Prausnitzand Shair [27] quote Hansen [2] and report 120575d = 157MPa12at 298K and 1 atm for the dispersion partial solubility param-eter but the total Hildebrand solubility parameter includeda contribution from the polar interactions and hydrogenbonding of this gasmolecules adding up to120575H(298K)MPa12= 1785 This value is incompatible with that resulting fromthe Span and Wagner data It appears that the compilationof Span and Wagner [48] results in the most reliable valuesof 120575H(119879) and that 120575H(119879t)MPa12 = 1910 may be selectedhere

2114 Phosgene The normal boiling point of COCl2 wasestablished as 28066K by Giauque and Jones [50] andwas listed in the Handbook [7] as 8∘C that is 2812 Kand the most recently reported vapor pressure data ofHuang et al [51] lead to 119879bK = 28295 at which thepressure equals 0101325MPa (ie 1 atm)Themolar enthalpyof vaporization at the boiling point was reported asΔV119867(119879b)calmolminus1 = 5832 plusmn 6 that is 24401 Jmolminus1 [50]The more recent value [51] is larger 25565 Jmolminus1 derivedfrom the vapor pressure curve The density of liquid phos-gene was reported by Davies [52] as 120588g cm3 = 142014 minus00023120(119905∘C) minus 0000002872(119905∘C)2 that is 120588(119879b)g cm3= 140146 and 119881(119879b)cm3molminus1 = 7059 A slightly smallervalue 7013 cm3molminus1 results from the interpolated liquiddensity data in [51] The solubility parameter resulting fromthe more recent ΔV119867 is 120575H(119879b)MPa12 = 1813 and thetemperature dependence is shown in Table 3

2115 Nitrogen Trifluoride There are conflicting reportsregarding the boiling point of liquid NF3 the older value isminus119∘C by Ruff et al [53] and a more recent one is 1442 Kby Sladkov and Novikova [54] confirmed as minus12875∘C [7]that is 119879b = 14440K that is taken to be the valid oneAlso the reported ΔV119867 values differ 2400 calmolminus1 that is10042 Jmolminus1 [53] and 11600 Jmolminus1 [54] or 11560 Jmolminus1 [7]and again the latter value is used The molar volume at theboiling point is listed as 119881(119879b) = 461 cm3molminus1 [54] so that120575H(119879b)MPa12 = 150

2116 Nitrous Oxide Yosim and Owens [21] used the ΔV119867data of Kelley and King [40] for N2O from which the value120575H(119879b)MPa12 = 2041 is derived Atake and Chihara [55]reported ΔV119867Jmolminus1 = 16544 and with the density dataof Leadbetter et al [56] yielding 119881(119879b) = 3564 cm3molminus1

this produced 120575H(119879b)MPa12 = 2052 Sistla et al [36] quoteHansen [2] and report 120575d = 115MPa12 at 298K and 1 atmfor the dispersion partial solubility parameter but the totalHildebrand solubility parameter included a contributionfrom the polar interactions of these gas molecules adding upto 120575H(298K)MPa12 = 2081 The average of these agreeingvalues 2058 plusmn 020 is selected here

2117 Nitrogen Monoxide Monomeric nitrogen oxide NOhas received very little attention in the literature regardingits molar enthalpy of vaporization A very early ldquocalcu-latedrdquo value of 3412 calmolminus1 due to Bingham [57] that is14276 Jmolminus1 differs from the value 3293 calmolminus1 that is13778 Jmolminus1 of Kelley and King [40] quoted by Yosim andOwens [21] From the latter with the supplied density of1269 g cmminus3 at the boiling point of 1214 K the solubilityparameter 120575H(119879b)MPa12 = 2324 is derived There seems tobe no more modern value for this quantity in the literature

2118 Silicon Tetrafluoride The liquid range of SiF4 (alsocalled tetrafluorosilane) is quite narrow and its normalboiling point has been reported differently by various authors1775 le 119879bK le 1872 [58] and its triple point 119879tK = 18635


[59] hence the lower values appear not to be valid Thehigher values 187 [60] and 1872 [7] appear to be more nearlycorrect The molar enthalpy of vaporization was reported byLyman and Noda [61] as 15802 kJmolminus1 (but they report 119879b= 17783 K below 119879t of 18635 K but discuss properties of theliquid) The density of liquid SiF4 was reported by Pace andMosser [59] as 120588g cmminus3 = 2479 minus 0004566119879 at 186 le 119879K le195 extrapolating to 1624 g cmminus3 at 119879b = 1872 K and a molarvolume119881(119879b) = 6408 cm3molminus1The solubility parameter ofSiF4 is therefore 120575H(119879b)MPa12 = 1491

2119 Sulfur Tetrafluoride The data needed for obtainingthe solubility parameter of SF4 at its boiling point are allavailable from Brown and Robinson [68] The boiling pointis minus404∘C that is 119879b = 23275 K the molar enthalpy ofvaporization is 6320 calmolminus1 that is 26443 Jmolminus1 and thedensity of the liquid follows 120588g cmminus3 = 25471 minus 000314119879 (at170 le 119879K le 200) assumed to be valid up to 119879b yielding120588(119879b)g cmminus3 = 18164 Hence 120575H(119879b)MPa12 = 2031 Asomewhat larger value of 119879b = 236K was reported later byStreng [69] with 120588(119879b)g cmminus3 = 18061 but with no otherlatent heat of vaporization The resulting 120575H(119879b)MPa12 =2022 does not differ much from the value selected here

2120 Sulfur Hexafluoride Since SF6 sublimes and does notform a liquid on heating the solid it is difficult to specifya temperature at which the solubility parameter should beobtained The triple point has been reported as 119879t = 22356Kby Funke et al [70] but the molar enthalpy of vaporizationand the density have been reported at other temperaturesLinford and Thornhill [24] reported the molar energy ofvaporization as 408 kcalmolminus1 that is 17071 Jmolminus1 at anunspecified temperatureA so-called ldquoboiling temperaturerdquo of204Kwas reported byGorbachev [71] at which themolar vol-ume of SF6 was 753 cm

3molminus1 The value 120575H(204K)MPa12= 1429 results from this pair of data Funke et al [70] reportedvapor pressures and liquid densities over the temperaturerange 224 to 314K From these data the molar enthalpy ofvaporization is ΔV119867 = 17375 Jmolminus1 and the molar volumeis119881 = 7916 cm3molminus1 at 224K yielding 120575H(224K)MPa12 =1482 However a considerably larger ΔV119867 = 56 kcalmolminus1was quoted from Langersquos Handbook of Chemistry for SF6 byAnderson et al [72] that is 23430 Jmolminus1 This value is nearthe molar enthalpy of sublimation Δ subl119867 = 23218 Jmolminus1 at186K reported by Ohta et al [73] However no density dataat this temperature lower than the triple point are availableA tentative value based on the data in [70] is suggested here120575H(224K)MPa12 = 1482 as representative

2121 Diborane Themolar enthalpy of vaporization of B2H6at the boiling point 119879b = 18032 K was reported by Clarkeet al [74] as ΔV119867calmolminus1 = 3412 in the text and as 3422as the average of four runs in a table that is 14297 plusmn21 Jmolminus1 The density was reported by Laubengayer et al[75] as 120588g cmminus3 = 03140 minus 0001296(119905∘C) being accordingly04343 at 119879b yielding a molar volume of 6371 cm3molminus1 anda solubility parameter of 120575H(119879b)MPa12 = 1417 A subsequent

study by Wirth and Palmer [76] reported 119879b = 18063 Kand ΔV119867calmolminus1 = 3413 that is 14280 Jmolminus1 The molarvolume at the boiling point 119879b = 18066K was quoted byJhon et al [77] from the Landoldt-Bornstein compilation as6336 cm3molminus1 This pair of values yields 120575H(119879b)MPa12 =1420 The average between the two values 14185 is selectedhere

2122 Silane The boiling point and molar heat of vapor-ization of liquid SiH4 were quoted by Taft and Sisler [78]from secondary sources as 161 K and 298 kcalmolminus1 that is12470 Jmolminus1 and listed in [7] as minus1119∘C that is 1613 Kand 121 kJmolminus1 The molar volume at the boiling pointwas reported by Zorin et al [79] from experimental den-sity measurements as 119881(119879b) = 5504 cm3molminus1 and frommolecular dynamics simulations of the density reported bySakiyama et al [80] interpolated to the boiling point as119881(119879b)= 5727 cm3molminus1 but the experimental value is preferredThe resulting solubility parameter is 120575H(119879b)MPa12 = 1422

2123 Germane The boiling point and molar heat ofvaporization of liquid GeH4 were quoted in [78] fromsecondary sources as 184K and 365 kcalmolminus1 that is15270 Jmolminus1 reported by Devyatykh et al [81] as minus8851∘Cand 3608 calmolminus1 that is 15096 Jmolminus1 and listed in [7]as minus881∘C that is 18505 K and 1406 kJmolminus1 The molarvolume at the boiling point was reported in [79] from exper-imental density measurements as 119881(119879b) = 5591 cm3molminus1Hence 120575H(119879b)MPa12 = 1497 results from the more recentdata

2124 Stannane There are only the older data for liquidSnH4 the boiling point and molar heat of vaporization werereported by Paneth et al [82] as minus52∘C and 455 kcalmolminus1and were quoted in [78] from secondary sources as 221 Kand 45 kcalmolminus1 that is 18800 Jmolminus1 The molar volumeat the boiling point was reported in [79] from experimentaldensity measurements as 119881(119879b) = 6318 cm3molminus1 Hence120575H(119879b)MPa12 = 1640 results

2125 Phosphine The paper by Durrant et al [83] reportsall the required data for the group V hydrides For PH3 theboiling points minus874 minus85 and minus862∘C were quoted in [83]from previous publications 187 K is listed in [78] minus879∘Cis reported by Devyatykh et al [81] and minus8775∘C is listedin [7] that is 119879b = 18540K which is taken as the validvalueThemolar enthalpy of vaporization at the boiling pointis reported as ΔV119867(119879b) = 385 kcalmolminus1 in [83] that is16110 Jmolminus1 as 379 kcalmolminus1 in [55] that is 15860 Jmolminus1as 3949 kcalmolminus1 in [81] that is 16520 Jmolminus1 Howeverconsiderably lower values were reported more recently14600 Jmolminus1 in [7] and 13440 Jmolminus1 in [84] as themeasuredvalue (Note that Ludwig [84] reports for H2S an experi-mental ΔV119867 value in accord with other reports so that it isunclear why for PH3 such a low value is reported) The meanof the earlier reported values namely ΔV119867(119879b)Jmolminus1 =16160 is taken as validThe density of PH3 at the boiling point


is interpolated in the data of [83] as 120588(119879b) = 07653 g cmminus3yielding 119881(119879b) = 4443 cm3molminus1 A somewhat larger value119881(119879b) = 4572 cm3molminus1 was reported in [79] The solubilityparameters 120575H(119879b)MPa12 = 1813 and 1788 result from thesetwo molar volume values and the mean 1800 is selectedhere

2126 Arsine Durrant et al [83] report the boiling pointof liquid AsH3 as 2145 K in agreement with some earlierdata but somewhat lower than a much older value 2182quoted also in [78] and larger than the value 2111 K (fromminus621∘C) reported in [81] Sherman and Giauque [85] report119879b = 21068K listed as minus625∘C in [7] that is 21065 K anda mean ΔV119867(119879b) = 3988 calmolminus1 that is 16686 Jmolminus1The molar enthalpy of vaporization at the boiling pointis reported as ΔV119867(119879b) = 434 kcalmolminus1 in [83] that is18160 Jmolminus1 as 427 kcalmolminus1 in [78] that is 17870 Jmolminus1as 4100 kcalmolminus1 in [81] that is 17150 Jmolminus1 Again alower value 16690 Jmolminus1 is listed in [7] but the averageof the former three values 17730 Jmolminus1 is taken here asvalid The density of AsH3 at the boiling point is interpolatedin the data of [83] as 120588(119879b) = 16320 g cmminus3 yielding 119881(119879b)= 4776 cm3molminus1 A very similar value 4782 cm3molminus1was reported in [79] The resulting solubility parameter is120575H(119879b)MPa12 = 1827

2127 Stibine Durrant et al [83] report the boiling point ofliquid SbH3 as minus170∘C that is 2562 K in agreement with256K in [78] The molar enthalpy of vaporization at theboiling point is reported as ΔV119867(119879b) = 5067 kcalmolminus1 in[83] that is 21200 Jmolminus1 and as 49 to 50 kcalmolminus1 in[78] that is 20700 Jmolminus1 and is listed as 21300 Jmolminus1 in[7] the latter is taken as valid The density of AsH3 at theboiling point is interpolated in the data of [83] as 120588(119879b)= 22039 g cmminus3 yielding 119881(119879b) = 5662 cm3molminus1 A largervalue 5783 cm3molminus1 was reported in [79] The resultingsolubility parameters are 120575H(119879b)MPa12 = 1840 and 1820their mean 1830 being selected here

2128 Hydrogen Sulfide Themolar enthalpy of vaporizationof H2S was reported by Cubitt et al [86] from experimentaldata as ΔV119867 = 18701 Jmolminus1 and the molar volume as V= 3583 cm3molminus1 (interpolated) at the boiling point 119879b= 21285 K The value 120575H(119879b)MPa12 = 2174 results fromthese values The temperature dependence of 120575H is shown inTable 3 A less precise value of ΔV119867 = 1836 kJmolminus1 anda density of 120588 = 934 kgmminus3 were reported as experimentalvalues at 2202 K from an undisclosed source by Kristof andLiszi [87] The value 120575H(2202 K)MPa12 = 2128 is derivedfrom these data ΔV119867 = 1867 kJmolminus1 at the boiling pointwas reported by Ludwig [84] as the experimental value Avalue ΔV119867 = 446 kcalmolminus1 that is 18661 Jmolminus1 at theboiling point was reported by Riahi and Rowley [88] aswell as by Orabi and Lamoureux [89] attributed to Clarkeand Glew [90] and the density 949 kgmminus3 and a densityof 940 kgmminus3 result from the data of [79] These valuesyield 120575H(119879b)MPa12 = 2169 Sistla et al [36] quote Hansen

[2] and report 120575d = 170MPa12 at 298K and 1 atm for thedispersion partial solubility parameter but the total Hilde-brand solubility parameter included a contribution fromthe polar interactions of these gas molecules adding up to120575H(298K)MPa12 = 2071The average of the values resultingfrom [86 89] 120575H(119879b)MPa12 = 2072 nearly coincides withthe latter value (for 298K)

2129 Hydrogen Selenide The boiling point of H2Se wasreported as minus415∘C by Robinson and Scott [91] 231 K in[78] taken from secondary sources and as minus4125∘C in [7]that is 23190KThe very early ΔV119867(119879b) = 4740 calmolminus1 byForcrand and Fonzes-Diacon [92] at the boiling point minus42∘Cthat is 19830 Jmolminus1 is confirmed by the value 19790 Jmolminus1derived from the Trouton constant of 204 cal Kminus1molminus1reported in [91] leading to 478 kcalmolminus1 in [78] thatis 20000 Jmolminus1 The 120588(119879b) = 2004 g cmminus3 [91] yields119881(119879b) = 4042 cm3molminus1 The density data of [79] yieldthe reported 119881(119879b) = 4121 cm3molminus1 hence the solubilityparameter 120575H(119879b)MPa12 = 2097 results from the means ofthe ΔV119867(119879b) and 119881(119879b) values2130 Hydrogen Telluride Robinson and Scott [91] reportedboiling points of minus4 and minus5∘C definitely lower than pre-vious reports leading to 272K in [78] and minus2∘C in [7]For the present purpose 119879b = 270K is used Troutonrsquosconstant 167 cal Kminus1molminus1 reported in [91] yields ΔV119867(119879b)= 18870 Jmol much lower than 23430 Jmolminus1 (from56 kcalmolminus1) from [78] but confirmed by 192 kJmolminus1listed in [7] The mean 19040 Jmolminus1 of the better agree-ing values is used here The density at the boiling pointis 2650 g cmminus3 according to [91] yielding 119881(119879b) =489 cm3molminus1 much lower than 5514 cm3molminus1 resultingfrom the density data in [79] The minimal value of 120575H(119879b)MPa12 from these data is 175 and the maximal value is 208The value 184MPa12 from the old data of [91] may representthe true value but the trend with the molar mass of thegaseous substances points to the maximal value 208MPa12as possibly better

2131 Methane Yosim and Owens [21] used the ΔV119867 dataof Kelley and King [40] from which the value 120575H(119879b)MPa12= 1383 is derived Prausnitz and Shair [27] reported 120575H =568 (calcc)12 that is 1162MPa12 (reported as 116 in [28])a low value compared to other reports Linford andThornhill[24] reported the energy of vaporization as ΔV119864(119879b) =173 kcalmolminus1 and with the molar volume from Terry et al[30]119881(119879b) = 381 cm3molminus1 the value 120575H(119879b) = 1287MPa12is derived Jorgensen et al [93] quoted experimental data atthe boiling point from compilations ΔV119867kcalmolminus1 = 196and VA3moleculeminus1 = 628 from which 120575H(119879b)MPa12 =1386 is calculated Daura et al [94] quoted experimental dataat the boiling point from compilations ΔV119867kJmolminus1 = 819and density 120588kgmminus3 = 424 from which 120575H(119879b)MPa12 =1387 is calculated Prausnitz and Shair [27] quote Hansen[2] and report 120575d = 140MPa12 at 298K and 1 atm for the


dispersion partial solubility parameter which for methaneis the total solubility parameter The mean of the agreeingvalues 120575H(119879b)MPa12 = 1387 is selected here

2132 Fluoromethane Oi et al [95] provided the coefficientsof the vapor pressure expression log(119901torr) = 119860 minus 119861(119862 +119905∘C) for CH3F from which ΔV119867(119879b) = 15764 Jmolminus1 isderived Fonseca and Lobo [96] provided the molar volumeof CH3F at 16139 K and at 19548K from which 119881(119879b =1948K) = 3861 cm3molminus1 is interpolated The resultingsolubility parameter is 120575H(119879b)MPa12 = 1914

2133 Difluoromethane Potter et al [97] provided the need-ed data for the calculation of the solubility parameter119901(119879)bar 120588(119879)g cmminus3 and ΔV119867(119879)kJmolminus1 from the for-mer of which 119879b = 2216 K is interpolated for pbar =101325 (= 1 atm for the normal boiling point) The resultingvalues 120588(119879b)g cmminus3 = 1268 and ΔV119867(119879b)kJmolminus1 = 1997yield 120575H(119879b)MPa12 = 2102 for CH2F2 The temperaturedependence of 120575H is shown in Table 3

2134 Trifluoromethane Potter et al [97] provided the need-ed data for the calculation of the solubility parameter119901(119879)bar 120588(119879)g cmminus3 and ΔV119867(119879)kJmolminus1 from the for-mer of which 119879b = 1911 K is interpolated The resultingvalues 120588(119879b)g cmminus3 = 1467 and ΔV119867(119879b)kJmolminus1 = 1614yield 120575H(119879b)MPa12 = 1746 for CHF3 The temperaturedependence of 120575H is shown in Table 3

2135 Tetrafluoromethane Gilmour et al [98] reportedthe values of 119879b = 1451 K ΔV119867(119879b)kcalmolminus1 = 301(= 1259 kJmolminus1) and 119881(119879b)cm3molminus1 = 549 fromwhich 120575H(119879b) = 1440MPa12 results Linford and Thornhill[24] reported the energy of vaporization as ΔV119864(119879b) =272 kcalmolminus1 at 119879b = 1452 K and with the molar volumefrom Terry et al [30] 119881(119879b) = 544 cm3molminus1 the value120575H(119879b) = 1446MPa12 is derived The values resulting fromthe Potter et al [97] data are 120588(119879b)g cmminus3 = 1563 andΔV119867(119879b)kJmolminus1 = 1172 yielding 120575H(119879b)MPa12 = 1466The most recent report is of Monte Carlo computer simula-tion results byWatkins and Jorgensen [99] that compare wellwith the experimental values for the enthalpy of vaporizationand the density yielding 120575H(119879b)MPa12 = 1448 The meanof the three closely agreeing reported values 1443MPa12is taken to represent the solubility parameter of CF4 Thetemperature dependence of 120575H is shown in Table 3

2136 Chloromethane Meyer et al [100] reported the coeffi-cients of the Antoine vapor pressure expression [missing theminus sign between 119860 and 119861(119862 + 119905) for log119901] from whichwas obtained ΔV119867kJmolminus1 = 22803 over the range minus75 le119905∘C le minus25 that is up to the boiling point of minus2414∘C thatis 2490 K Kumagai and Iwasaki [101] reported the specificvolumes of CH3Cl at the saturated vapor pressures at fourtemperatures above minus20∘C extrapolating to 0988 cm3 gminus1at 119879b and a molar volume of 4940 cm3molminus1 The value120575H(119879b)MPa12 = 2038 results from these data Freitas et

al [102] quoted ΔV119867(119879b)kJmolminus1 = 215 and the density120588g cmminus3 = 0985 from a secondary source taking 119879b =23939KThe resulting solubility parameter is 120575H(119879b)MPa12

= 1947 The mean of the two values 199MPa12 is taken forthe solubility parameter for CH3Cl

2137 Bromomethane The boiling point 119879b = 27670K ofCH3Br and its molar enthalpy of vaporization at this tem-perature ΔV119867(119879b) = 576 kcalmolminus1 (= 2410 kJmolminus1) werereported by Kudchadker et al [103] The specific volumes atminus20 0 20 and 40∘C and saturation pressures were reportedby Kumagai and Iwasaki [101] yielding a linear relationshipFrom which the density 120588(119879b)g cmminus3 = 17196 and themolar volume119881(119879b)cm3molminus1 = 5521 could be derivedTheresulting solubility parameter is 120575H(119879b)MPa12 = 1987

2138 Formaldehyde The boiling point of liquid HCHOwasreported as minus215∘C by Mali and Ghosh [104] that is 252KThe density at minus20∘C of 0815 g cmminus3 is available in [7] Thelatent heat of evaporation was reported as 5600 calmolminus1 in[104] The resulting solubility parameter is 120575H(119879b)MPa12= 2406 These are the only data found for this gaseoussubstance in the neat liquid form hence the value of 120575H mustbe considered as tentative

2139 Methylthiol The molar enthalpy of vaporization ofCH3SH was reported by Russell et al [105] as 5872 calmolminus1that is 24568 Jmolminus1 at the normal boiling point 119879b =27912 K The density was reported by Kaminski et al [106]presumably at 119879b (for which the above-noted reference isappropriate) as 0888 g cmminus3 Hence the solubility parameteris 120575H(119879b)MPa12 = 2026

2140 Acetylene This substance sublimes and has no definiteliquid phase at ambient pressures hence no boiling pointThe triple point 119879t was reported as 1924 K by Tan et al[107] and the molar volume at 1919 K was reported as4206 cmminus3molminus1 from molecular dynamics computation byKlein and McDonald [108] These authors also deduced themolar enthalpy of vaporization over the temperature rangeof 191 to 223K from vapor pressure data of Kordes [109]as 166 kJmolminus1 who also reported the density at 1915 K as0613 g cmminus3 that is 119881(119879b) = 4248 cm3molminus1 The resultingsolubility parameter ofHCequivCH is thus 120575H(119879t)= 1889MPa12According to Vitovec and Fried [65] quoting from a sec-ondary source under pressure (48 atm) at 25∘C the enthalpyof vaporization of the saturated acetylene is 3737 kcalmolminus1and the molar volume is 6914 cm3molminus1 yielding 120575H(298K)= 675 cal12 cmminus32 that is 1381MPa12 The solubility ofacetylene in benzene toluene and p-xylene at 25∘C [65] andapplication of the regular solution expression ln119909HCCH =minus(119881HCCH119877119879)[120575H(HCCH) minus 120575H(solvent)]2 yielded the meanvalue 686 cal12 cmminus32 that is 1403MPa12 for 120575H(HCCH)in fair agreement with their value from the enthalpy of vapor-ization Sistla et al [36] quote from Hansen [2] values forthe dispersion polar and hydrogen bonding partial solubilityparameters of 144 42 and 119MPa12 respectively adding


up to the total 120575H(298K 1 atm) = 1915MPa12 an unlikelyvalue in view of the nonexistence of liquid acetylene at 298Kand 1 atm

2141 Ethylene Prausnitz and Shair [27] reported 120575H =66 (calcc)12 that is 135MPa12 a low value comparedto other reports Michels and Wassenaar [110] reported anexpression for the temperature dependence of the vapor pres-sure leading to ΔV119867(119879) = 14641 kJmolminus1 (148 le 119879K le 281)Yosim and Owens [21] used the density and ΔV119867 data froma secondary source from which the value 120575H(119879b)MPa12 =1564 is derived Calado et al [111] reported liquid molarvolumes and enthalpies of vaporization over the temperaturerange 110 le 119879 le 250 from which the values at theboiling point of C2H4 119879b = 1695 K of 119881(119879b)cm3molminus1 =4948 and ΔV119867(119879b)Jmolminus1 = 13447 are deduced yielding120575H(119879b)MPa12 = 1560 The temperature dependence of 120575His shown in Table 3 Sistla et al [36] quote from Hansen [2]values for the dispersion polar and hydrogen bonding partialsolubility parameters of 150 27 and 27MPa12 respectivelyadding up to the total 120575H(298K 1 atm) = 1548MPa12 Thevalue from Calado et al [111] is selected here as valid

2142 Ethane Prausnitz and Shair [27] reported 120575H =66 (calcc)12 that is 135MPa12 repeated in [28] a lowvalue compared to other reports Yosim and Owens [21] usedthe density and ΔV119867 data from a secondary source fromwhich the value 120575H(119879b)MPa12 = 1456 is derived Bradfordand Thodos [66] reported expressions and parameters fromwhich the solubility parameter was supposed to be calculatedbut the resulting value (79MPa12) is too small Gilmouret al [98] reported density and ΔV119867 data from an undis-closed source from which the value 120575H(119879b)MPa12 = 155is deduced Linford and Thornhill [24] reported the energyof vaporization as ΔV119864(119879b) = 315 kcalmolminus1 and with thedensity of 120588(119879b) = 05481 g cmminus3 extrapolated from the dataof Chui and Canfield [112] the value 120575H(119879b) = 1550MPa12is derived Jorgensen et al [93] reported the molecularvolume in A3moleculeminus1 of ethane at its boiling point fromwhich the molar volume 551 cm3molminus1 is obtained thatwith the ΔV119867(119879b) = 352 kcalmolminus1 that they report yields120575H(119879b)MPa12 = 1548 Daura et al [94] report ΔV119867(119879b) =1470 kJmolminus1 and the density 120588(119879b) = 0546 kgmminus3 fromwhich 120575H(119879b)MPa12 = 1548 results Sistla et al [36] quoteHansen [2] and report 120575d = 156MPa12 at 298K and 1 atmfor the dispersion partial solubility parameter which forethane is the total solubility parameter The value 120575H(119879b) =1550MPa12 is selected here

2143 Chloroethane The boiling point of C2H5Cl is some-what below ambient 1226∘C = 2854 K and the coefficientsof the Antoine vapor pressure expression [missing the minussign between 119860 and 119861(119862 + 119905) for log119901] were reported byMeyer et al [100] from which ΔV119867kJmolminus1 = 26615 wasobtained over the range minus56 le 119905∘C le 13 A somewhatsmaller ΔV119867kJmolminus1 = 2473 was quoted by Smith [113]from a secondary sourceThemolar volumewas estimated by

Taft et al [114] (for an unspecified temperature presumably25∘C) as 119881 = 715 cm3molminus1 whereas the Handbook [7]specifies the density as 120588(25∘C) = 08902 g cmminus3 from whichthe molar volume is 119881(25∘C) = 691 cm3molminus1 Averagingthe ΔV119867 and 119881 values the tentative solubility parameter is182MPa12 near the boiling point

2144 Hexafluoroethane Gilmour et al [98] provided themolar enthalpy of vaporization (from vapor pressure mea-surements) and the molar volume of C2F6 at the boilingpoint 1949 K yielding the value 120575H(119879b) = 1300MPa12 andreported 120575Hcal12 cmminus32 = 64 that is 131MPa12 (withthe error of inverting the signs on the units) SubsequentlyWatkins and Jorgensen [99] quoted literature values of themolar enthalpy of vaporization and the density of C2F6at the boiling point 19505 K yielding the value 120575H(119879b)= 1294MPa12 Sharafi and Boushehri [115] reported thefollowing values 119879b = 19495 K 120588(119879b) 1605 kgmminus3 andΔV119867(119879b)119877 = 19422K from which 120575H(119879b) = 1300MPa12

is derived The mean 1298MPa12 is selected here

2145 Ethylene Oxide Maass and Boomer [116] measuredthe vapor pressure and density of c-C2H4O over a consid-erable temperature range and reported the molar enthalpyof vaporization at the boiling point minus1073∘C (28388K) asΔV119867(119879b)kcal Kminus1molminus1 = 600 that is 25104 Jmolminus1 At thistemperature (interpolated) the density is 08823 g cmminus3 andthe molar volume is 4993 cm3molminus1 The resulting solubilityparameter is 120575H(119879b) = 2134MPa12 Giauque and Gordon[117] obtained ΔV119867(119879b)kcalmolminus1 = 6101 calorimetrically(6082 from the vapor pressures) that is 25527 Jmolminus1Olson [118] reported the density at three temperatures 025 and 50∘C interpolated to 120588(119879b) = 088266 g cmminus3 and119881(119879b) = 4991 cm3molminus1 These two data yield 120575H(119879b) =2155MPa12 Eckl et al [119] recently reported the densityand molar enthalpy of vaporization at 235 270 305 and340K from which the interpolated values for 119879b = 2835 Kare ΔV119867(119879b)kJmolminus1 = 25659 and 120588(119879b)mol Lminus1 = 2007that is 119881(119879b) = 4983 cm3molminus1 resulting in 120575H(119879b) =2162MPa12 and the temperature dependence is shown inTable 3 The mean of the latter two mutually agreeingestimates is selected here 2159MPa12

2146 Dimethyl Ether Maass and Boomer [116] measuredthe vapor pressure and density of (CH3)2O over a consid-erable temperature range and reported the molar enthalpyof vaporization at the boiling point minus249∘C (24825 K) asΔV119867(119879b)kcal Kminus1molminus1 = 531 that is 22220 Jmolminus1 At thistemperature the (interpolated) density is 07345 g cmminus3 andthe molar volume is 6272 cm3molminus1 The resulting solubilityparameter is 120575H(119879b) = 1793MPa12 Kennedy et al [120] mea-sured the vapor pressure and reported the molar enthalpy ofvaporization at the boiling point as ΔV119867(119879b)cal Kminus1molminus1= 51410 that is 21510 Jmolminus1 Staveley and Tupman [121]reported themolar entropy of vaporization at the temperatureat which the vapor pressure is 760mmHg that is the boiling


point 119879b = 2484 K ΔV119878cal Kminus1molminus1 = 2073 Hence themolar enthalpy of vaporization is ΔV119867kJmolminus1 = 119879bΔV119878 =21680 near that reported in [120] and quoted by Briggs et al[122] who reported the boiling point as minus248∘C The meanof the latter two ΔV119867 values and the Maass and Boomer[116] molar volume yield the solubility parameter 120575H(119879b) =1765MPa12 selected here instead of the slightly larger earliervalue

2147 Propene Powell and Giauque [123] reported vaporpressure data for C3H6 from which they derived the molarenthalpy of vaporization 4402 calmolminus1 that is 18418 Jmolminus1and reported the boiling point as 22535 K Jorgensen et al[124] adopted this value for ΔV119867(119879b)cal Kminus1molminus1 at 119879b= 2255 K The densities for propene under pressure werereported by Parrish [125] between 5 and 25∘C that wereextrapolated to 2255 K as 120588(119879b)g cmminus3 = 060049 yielding119881(119879b) = 7008 cm3molminus1 The resulting solubility parameteris 120575H(119879b) = 1536MPa12

2148 Cyclopropane Ruehrwein and Powell [126] measuredthe vapor pressures of c-C3H6 and derived the molarenthalpy of vaporization ΔV119867(119879b)calmolminus1 = 4793 that is20054 Jmolminus1 at the boiling point 119879b = 24030K Lin et al[127] reported the molar enthalpy of vaporization at temper-atures ge 20∘C obtained from the vapor pressures extrap-olating to ΔV119867(119879b)cal gminus1 = 11903 that is 20956 Jmolminus1Calado et al [111] reported a vapor pressure expressionfrom which ΔV119867(119879)kcalmolminus1 = 22200 Jmolminus1 is calcu-lated for 170 le TK le 225 Helgeson et al [128] reportedΔV119867(119879b)kcalmolminus1 = 479 that is 20041 Jmolminus1The agree-ment between these values is only fair and their mean20810 Jmolminus1 is adopted here The densities reported by Linet al [127] at temperatures ge 20∘ extrapolate to 07119 g cmminus3at 119879b Helgeson et al [128] reported 0705 g cmminus3 at 119879band Costa Gomes et al [129] report data up to 175K thatextrapolate to 6894 kgmminus3 at 119879b Again the mean of thesethree values is adopted here 07021 g cmminus3 The resultingsolubility parameter is 120575H(119879b) = 177MPa12

2149 Propane Linford and Thornhill [24] reported theenergy of vaporization as ΔV119864(119879b) = 403 kcalmolminus1that is 16845 Jmolminus1 and with the molar volume 119881(119879b)A3moleculeminus1 = 1260 that is 7588 cm3molminus1 from Jorgen-sen et al [93] the value 120575H(119879b) = 1490MPa12 is derivedThe latter authors provided ΔV119867(119879b)kcalmolminus1 = 449 thatis 18686 Jmolminus1 at the boiling point 119879b = 23188K so thatthe same value 120575H(119879b) = 1490MPa12 is derived Bradfordand Thodos [66] reported the parameters of the followingexpression

120575H = 120575c + 119896 (1 minus 119879R)119898 (5)

where 120575c = 2362 (calcm3)12 is the solubility parameter atthe critical point 119896 = 745 119898 = 0446 and 119879R = 119879119879cis the reduced temperature the critical temperature being119879c = 36980K according to Goodwin [130] The value 120575H(119879b)

= 1467MPa12 results Gilmour et al [98] reported the valuesΔV119867(230K)kcalmolminus1 = 448 and 119881(230K)cm3molminus1 =753 fromwhich120575H(119879b)= 1494MPa12 is derivedHelpenstilland van Winkle [67] reported 120575H(119879)(calcm3)12 = 692 at0∘C and 654 at 25∘C that is 120575H(273K)MPa12 = 1415 and120575H(298K)MPa12 = 1338 the latter value being near that ofLaPack et al [28] at an unspecified temperature (presumably25∘C) of 136MPa12 Daura et al [94] reported data obtainedfrom their GROMOSC96modelΔV119867(119879)kcalmolminus1 = 1479and 120588(T) = 493 kgmminus3 at 119879 = 298K from which120575H(298K)MPa12 = 1230 The value at the boiling point120575H(119879b) = 1490MPa12 is selected here Then temperaturedependence of 120575H is shown in Table 3

2150 Octafluoropropane Gilmour et al [98] reported datafor C3F8 at several temperatures from 230 to 237K fromwhich the values at119879b = 2365 K are readily derivedΔV119867(119879b)= 470 kcalmolminus1 (= 1979 kJmolminus1)119881(119879b) = 1168 cm3molminus1and 120575H(119879b)MPa12 = 1228 The computer simulations ofWatkins and Jorgensen [99] agree with experimental valuesyieldingΔV119867(119879b) = 473 kcalmolminus1 (= 1966 kJmolminus1)119881(119879b)= 1171 cm3molminus1 and 120575H(119879b)MPa12 = 1226 Sharafi andBoushehri [115] reported the following values 119879b = 23665 K120588(119879b) 1603 kgmminus3 and ΔV119867(119879b)119877 = 23519K fromwhich 120575H(119879b) = 1224MPa12 is derived The mean value120575H(119879b)MPa12 = 1226 is selected here Then temperaturedependence of 120575H is shown in Table 3

2151 EthylMethyl Ether Themolar enthalpy of vaporizationof CH3OC2H5 at its boiling point of 735∘C (119879b = 2805K)was reported by Ambrose et al [131] as 251 kJmolminus1 Aslightly lower value 591 kcalmolminus1 that is 2473 kJmolminus1was reported by Maass and Boomer [116] These authorsquoted Aronovich et al [132] for the density 120588(119879b) =07205 g cmminus3 so that the solubility parameters resulting fromthe above two values of ΔV119867(119879b) are 120575H(119879b)MPa12 = 1652and 1638 The mean 1645 is selected here as representative

2152 1-Butene Helpenstill and van Winkle [67] reported120582(119879)(calcm3)12 = 724 at 0∘C and 690 at 25∘C and120591(119879)(calcm3)12 = 143 at 0∘C and 132 at 25∘C where120582 pertains to the dispersion aspect and 120591 to the polarityaspects (120591 = 0 for the saturated hydrocarbons) The totalsolubility parameter for 1-C4H8 is 120575H(119879) = (1205822 + 1205912)12that is 1510MPa12 at at 0∘C and 1437MPa12 at 25∘CJorgensen et al [93] reported ΔV119867(298K)kcalmolminus1 = 487andV(298K)A3moleculeminus1 = 1582 that is 9527 cm3molminus1resulting in 120575H(298K)MPa12 = 1381 Spyriouni et al [133]reported results from molecular dynamics simulations overthe temperature range 290 to 390K extrapolating to 119879b =2675 K as ΔV119867(119879b)Jmolminus1 = 20480 and 120588(119879b)g cmminus3 =05738 resulting in 120575H(119879b) = 1366MPa12 and the temper-ature dependence is shown in Table 3 The Handbook [7]reports 119879b = 2669 K and ΔV119867(119879b)kJmolminus1 = 2207 andwith the extrapolated molar volumes from [67] 119881(119879b) =


8907 cm3molminus1 the resulting solubility parameter is 120575H(119879b =2669 K)MPa12 = 1493 being selected here

2153 Cyclobutane Only scant relevant data are availa-ble for c-C4O8 namely from Helgeson et al [128] ΔV119867(119879b)kcalmolminus1 = 578 and 120588(119879b)g cmminus3 = 0732 the boiling pointbeing [7]minus126∘C that is119879b = 2606 KThe resulting 120575H(119879b)=1695MPa12ΔV119867(119879b)kJmolminus1 = 2419 in theHandbook [7]yields practically the same solubility parameter The densityin the Handbook pertaining to 25∘C 120588(298)g cmminus3 = 06890and the molar volume 119881(18234 K) = 6962 cm3molminus1 fromMartins et al [134] are irrelevant here

2154 Octafluorocyclobutane The computer simulations ofWatkins and Jorgensen [99] do not agree very well withexperimental values (translated from the engineering valuesof Martin [135] in psi and ft3lb) ΔV119867(119879b) = 469 kcalmolminus1(= 1962 kJmolminus1) and 120588(119879b) = 1753 g cmminus3 and there isalso a misprint in their 119879b minus4020 instead of minus420∘C thecorrect value being 119879b = 2673 K The experimental data yield120575H(119879b) = 1367MPa12 whereas the computed data yield1414MPa12 the former value being preferred

2155 n-Butane Yosim and Owens [21] reported data fromsecondary sources ΔV119867(119879b)calmolminus1 = 5352 and 120588(119879b)g cmminus3 = 0601 at 119879b = 2727 K from which 120575H(119879b)MPa12= 1443 is derived Bradford and Thodos [66] reported theparameters of the expression (5) where 120575c = 2259 (calcm3)12 119896 = 742 119898 = 0446 and 119879R = 119879119879c 119879c = 42514KfromKratzke et al [136] with the value 120575H(119879b)= 1424MPa12resulting Gilmour et al [98] reportedΔV119867(119879b)kcalmolminus1 =535 and119881(119879b)cm3molminus1 = 964 from which 120575H(119879b)MPa12= 1445 is derived Helpenstill and van Winkle [67] reported120575H(119879)(calcm3)12 = 725 at 0∘C and 6954 at 25∘C and677 at 45∘C extrapolating to 120575H(119879b)MPa12 = 1482 Daset al [137] reported the molar enthalpies and volumes ofliquid and gaseous butane over the temperatures from 119879bto 119879c from which the expression in Table 3 is derived and120575H(119879b)MPa12 = 1443 as from the previous authors Anappreciably smaller value 120575HMPa12 = 139 at an unspecifiedtemperature (presumably 298K) was reported by LaPacket al [28] This value is near that 1375 derived from theΔV119867(298) and 120588(298) obtained from GROMOSC96 modelof Daura et al [94]Themean of themutually agreeing values120575H(119879b)MPa12 = 1447 is selected here

2156 n-Decafluorobutane Brown andMears [138] providedthe required data for 119899-C4F10 119879b = ndash200∘C (119879b = 27115 K)ΔV119867(119879b)kcalmolminus1 = 5480 (= 2293 kJmolminus1) and thedensity interpolated in the reported data 120588(119879b)g cmminus3 =15925 yielding 120575H(119879b)MPa12 = 1176 The data provided byGilmour et al [98] lead to a similar value 120575H(119879b)MPa12= 1178 whereas the simulation of Watkins and Jorgensen[99] yielded a slightly lower value 120575H(119879b)MPa12 = 1169The mean of the two agreeing values is selected here1177MPas12

Table 1 Selected solubility parameters of liquefied inorganic gasesat their boiling points

Gas 119879bK 120575HMPa12

He 422 122Ne 2707 1001Ar 8730 1421Kr 1199 1524Xe 1650 161Rn 2115 171H2 2028 508N2 7736 1195O2 9020 1464BF3 1722 204BCl3 2858 161CO 8165 1230CO2 Sublimes 1910(119879t)COCl2 2812 1813NF3 14440 150N2O 1847 2058NO 1214 2324SF4 23270 2031SF6 Sublimes 1482(119879t)B2H6 1806 1419SiH4 1613 1422GeH4 18505 1497SnH4 2165 1640PH3 18540 1800AsH3 21065 1827SbH3 2562 1830H2S 2136 2072H2Se 23190 2097H2Te 270 208

2157 Isobutane Gilmour et al [98] reported 2-methylpro-pane (isobutane) ΔV119867(119879b)kcalmolminus1 = 509 and 119881(119879b)cm3molminus1 = 978 at 119879b = 2614 K from which 120575H(119879b)MPa12= 1398 is derived Jorgensen et al [93] reported similar valuesfor ΔV119867(298)kcalmolminus1 = 457 and 119881(119879b)A3moleculeminus1 =1751 from secondary sources as the previous authors result-ing in 120575H(298)MPa12 = 1256 Daura et al [94] reporteddata obtained from their GROMOSC96 model ΔV119867(119879)kcalmolminus1 = 1954 and 120588(T) = 551 kgmminus3 at 119879 = 298Kfrom which 120575H(298K)MPa12 = 1283 results The value atthe boiling point 120575H(119879b)MPa12 = 1398 is selected here

22 Results The resulting selected 120575H(119879b) values are shownin Table 1 for inorganic liquefied gases and in Table 2 fororganic ones (carbon compounds)

As the temperature is increased the molar enthalpy ofvaporization ΔV119867(119879) diminishes towards its disappearanceat the critical point Over a temperature range near thenormal boiling point 119879b the function ΔV119867(119879) is linearwith the temperature Also as the temperature is increased


Table 2 Selected solubility parameters of liquefied organic gases attheir boiling points

Gas 119879bK 120575HMPa12

CH4 1117 1387CH3F 1948 1914CH2F2 2216 2102CHF3 1911 1746CF4 1462 1443CH3Cl 24906 199CH3Br 27670 199HCHO 252 2406CH3SH 2791 2026C2H2 Sublimes 189(119879t)C2H4 1695 1560C2H6 1845 1550C2H5Cl 2854 182C2F6 1951 1298c-C2H4O 2839 2159(CH3)2O 2484 1765C3H6 2254 1536c-C3H6 2403 177C3H8 2311 1490C3F8 2365 1226CH3OC2H5 2805 16451-C4H8 26689 149c-C4H8 2606 1695c-C4F8 2673 1367n-C4H10 2727 1447n-C4F10 27115 1177i-C4H10 2614 1398

the density 120588(119879) diminishes and the molar volume 119881(119879)increases both linearly over a temperature range near thenormal boiling point 119879b Therefore the solubility parameter120575H(119879) = [(ΔV119867(119879) minus 119877119879)119881(119879)]05 necessarily diminishesas the temperature is increased For several of the gaseoussolutes for which there are data over a sufficient temperaturerange (excluding the noble gases) the decrease in 120575H(119879) islinear with 119879 with a slope of minus006 plusmn 002Kminus1 as is seenin Table 3 This slope may be used for the approximateestimation from the 120575H(119879b) values in Tables 1 and 2 of theapplicable solubility parameter of the solute gases at thetemperatures at which their solubility is needed

3 Discussion

31 Trends in the Solubility Parameters The following trendsmay be seen in the data of Tables 1 and 2 remembering thatthe normal boiling points may be considered as ldquocorrespond-ing temperaturesrdquo for the comparison of thermophysical data120575H(119879b) of the noble gases and of the hydrides of group IVand V elements increase with increasing molar masses of thegases The opposite appears to be the case for homologousorganic compounds Polarity adds to the value arising fromdispersion forces only as among others Sistla et al [36]

pointed out Meyer et al [100] calculated the contributionof the dispersion polarity and orientation to the cohesiveenergy the dispersion part being 73 and 80 of the totalfor CH3Cl and C2H5Cl respectively but did not obtain thesolubility parameters

32 Solubility Parameters Derived from Solubilities In viewof the concern with the solubility of gases in a variety ofsolvents many authors have presented values of the solubilityparameters of gases Clever et al [20] reported values of120575H(119879b)(cal cmminus3)12 of the noble gases helium to xenon toone decimal digit that correspond well to the selected valuesin Table 1 These values however are larger (except forhelium) than those derived from the relative solubilities incyclohexane and perfluorocyclohexane Vitovec and Fried[65] derived a value for 120575H(298K)(cal cmminus3)12 = 675 foracetylene that is as expected smaller than the value atthe triple point 1915 K but agrees with the mean valuederived from the solubility in benzene toluene and p-xylene686 (cal cmminus3)12 Prausnitz and Shair [27] reported values of120575H(cal cmminus3)12 for Ar Kr Rn N2 O2 CO CO2 CH4 C2H4and C2H6 suggested to be valid over a range of temperaturesmuch larger than the boiling points As expected these valuesare smaller than 120575H(119879b) Similarly Blanks and Prausnitz [64]reported values of 120575H(298K)(cal cmminus3)12 from undisclosedsources for CH4 C2H4 C2H6 C3H6 C3H9 and C4H10shown in Table 4 Bradford and Thodos [66] provided theparameters for equation (5) for CH4 C2H6 C3H8 andC4H10from which solubility parameters at any temperature maybe evaluated The values at 298K are shown in Table 4except for methane for which 119879c lt 298K Gilmour etal [98] reported 120575H(119879b)(cal cmminus3)12 values for CF4 C2F6CH4 C2H6 C3H8 and C4H10 that agree well with thevalues in Table 2 Helpenstill and van Winkle [67] reportedthe dispersion and polarity partial solubility parameters ofhydrocarbons which in the cases ofC3H8 andC4H10 are onlythe dispersion ones equaling 120575H(cal cmminus3)12 and shown inTable 4 for 298K

Lawson [62] reported values of 120575H(298K)(cal cmminus3)12for eight gases obtained indirectly from their solubilities andare shown in Table 4 LaPack et al [28] quoted previouslyreported values as shown in Table 4 Sistla et al [36] quotedthe partial solubility parameters given by Hansen [2] for298K and the total (Hildebrand) solubility parameters shownin Table 4

It should be remembered that at ambient conditionsthat pertain to Table 4 the solutes are gases If the criticaltemperature is 119879c gt 298K they are liquid only under con-siderable pressure Still it has been tempting to take (1) to bevalid at ambient conditions for these gaseous solutes so thatsolubility parameters might be evaluated from the solubilitydata In some cases the authors find lower solubility param-eters of the solutes than from the relevant thermodynamicdata at the boiling points of the liquefied gaseous solutesfor example by Clever et al [20] for noble gases and byPrausnitz and Shair [27] for these and other gases In anothercase in acetylene according to Vitovec and Fried [65] thenonideality of the gas had to be taken into account to obtain


Table 3The temperature dependence of the solubility parameters of gaseous solutes 120575HMPa12 =119860+119861(119879K)+119862(119879K)2 over the temperaturerange shown The average uncertainties of 119860 are plusmn10 of 119861 are plusmn26 and of C are plusmn50

Gas Temperature range 119879K 119860 119861 119862Neon 25ndash40 8036 03382

minus00098Argon 84ndash87 2195 minus009028Krypton 116ndash120 2272 minus00629Xenon 161ndash165 2539 minus005813

minus0004784Hydrogen 14ndash21 511 009611Oxygen 84ndash120 2452 minus01110Carbon monoxide 68ndash81 1913 minus00837Carbon monoxide 80ndash110 2147 minus01121Carbon dioxide 217ndash290 minus3381 05243

minus0001297

Phosgene 230ndash349 2984 minus00421Hydrogen sulfide 188ndash270 3327 minus005438Difluoromethane 200ndash280 4956 minus005606Trifluoromethane 180ndash260 3011 minus006632Tetrafluoromethane 120ndash200 2279 minus006299Ethylene 110ndash220 2445 minus005273Ethylene oxide 235ndash375 3544 minus004894Cyclopropane 293ndash323 3235 minus005976Propane 210ndash230 2385 minus003870Octafluoropropane 200ndash237 2024 minus0033591-Butene 290ndash370 2622 minus004482Butane 280ndash350 2586 minus004133

agreement between the solubility and thermodynamic valuesLinford andThornhill [24] related the solubilities of a varietyof solvents in many solvents to the cohesive energy of thesolute gases but did not use the solubility parameters Lawson[62] used the solubility parameters of solute gases listed inTable 4 to calculate their solubilities in hydrocarbons andperfluorohydrocarbons Lewis et al [31] fitted the solubilityof radon in selected perfluorocarbon solvents at 278 to 313 Kby assigning it the value 842 cal12 cmminus32 (1722MPa12)

Vetere [63] used solubility data of ten gases H2 O2 N2CH4 C2H4 C2H6 C3H8 CO CO2 and H2S in a variety ofpolar and nonpolar solvents and theNRTL (nonrandom two-liquid) model to obtain the (absolute) values of 120575HS minus 120575HGFrom these with known values of the solvent 120575HS valuesthose for the solute gases could be estimated The presented120575HSminus120575HG data pertained to a variety of temperatures for eachsolute gas and it is difficult to obtain values for a definitetemperature for all the solvents employed for a given gasThemean values pertaining to 303 plusmn 5K are listed in Table 4Shamsipur et al [139] dealt with the solubilities of gases invarious solvents and reported ldquo120575Hrdquo values for the alkanesC119899H2119899+2 (1 le 119899 le 8) When these are related to their knownHildebrand solubility parameters as solvents the relationship120575HMPa12 = 765ldquo120575Hrdquo02 results When this relationship isapplied to ldquo120575Hrdquo = 01402 for Ne this yields 120575H = 108MPa12Note that for He the resulting value is too large 106MPa12so the approximate agreement for Ne should not be taken asvalid

As is seen in Table 4 the agreement between the entriesfor a given gas by diverse authors at a given temperature

near ambient is rather poor This arises from the meansused by the authors to calculate the values from solubil-ities via (1) or equivalent expressions or based on otherpremises

On the other hand the miscibility of the liquefied gasesamong themselves should be directly related to their solubil-ity parameters according to (1) Some data on the miscibilityof gases were presented by Streng [69]

33 Correlations The cohesive energies of permanent gasesat their boiling points should be related to the attractiveinteractions of the particles These in turn are relatedto the depths 120576 of the potential wells arising from theenergetics of the collisions of the particles in the gas phase Acommonmeasure of the energetics is the 12-6 Lennard-Jonesrelationship

119906 = 120576 [( 119903120590)12 minus ( 119903120590)

6] (6)

where 119903 is the distance apart of the two colliding particles 120590is the distance of their centers at contact and 120576 reported inunits of the Boltzmann constant in Kelvins that is (120576119896B)Kis theminimum of the interaction potential energy 119906 Indeedthe cohesive energy densities [120575H(119879b)]2 are linearly related tothe (120576119896B) values of the gases for which values were found seeFigure 1 It should be noted that the (120576119896B) reported by variousauthors like De Ligny and Van der Veen [14] Teplyakov andMeares [13] Leites [12] and Churakov and Gottschalk [15]


Table 4 Literature values of solubility parameters of gases nearambient temperatures

Gas 119879K 120575HMPa12 RefHe 298 10 [36]Ar 273ndash333 109 [27 28]Kr 289ndash314 131 [27]

Rn 273ndash313 140 [27]298 172 [31]

H2298 45 [62]298 51 [36]

N2

253ndash435 53 [27 28]298 106 [62]298 119 [36]303 143 [63]

O2

273ndash333 82 [27 28]298 117 [62]298 147 [36]303 102 [63]

CO253ndash333 64 [27]298 119 [62]298 125 [36]

CO2

298 68 [62]298 123 [28]298 179 [36]313 225 [63]

NO 298 208 [36]

H2S298 207 [36]303 317 [63]

CH4

253ndash444 116 [27 28]298 96 [64]298 127 [62]298 140 [36]303 147 [63]

CH3Cl 298 198 [28]

C2H2298 138 [65]298 192 [36]

C2H4273ndash398 135 [27]298 113 [64]298 155 [36]

C2H6

255ndash422 135 [27 28]298 116 [64]298 80 [66]298 135 [62]298 156 [36]303 90 [63]

C3H6 298 125 [64]

C3H8

298 127 [64]298 122 [66]298 134 [67]298 136 [28 62]412 117 [63]

Table 4 Continued

Gas 119879K 120575HMPa12 Ref

C4H10

298 135 [64]298 135 [66]298 142 [67]298 139 [28]

0

100

200

300

400

0 200100 400 500300

120575H2 (MPa)

(120576k

B)(K

)

Figure 1 The depth of the collision potential well of gas molecules(120576119896B)K plotted against their cohesive denisty energy at the boilingpoint 120575H2MPaThe symbols are for (120576119896B)K from [12]e from [13]998787 from [14] 998771 and from [15] ⧫

among others vary considerably as the figure shows Still acorrelation

( 120576119896B) K = (104 plusmn 107)

+ (065 plusmn 005) [120575H (119879b) MPa12]2(7)

with a correlation coefficient 09194 is foundAnother conceivable correlation of the solubility parame-

ters of the liquefied gaseswould bewith their surface tensions120590 Data for the latter quantities are not plentiful but werefound for a representative group of the gases treated hereIndeed for the 17 liquefied gases for which surface tensiondata were found [16ndash19 140] there is a linear relationshipbetween the surface tension and the solubility parameter atthe boiling point as follows

120590 (119879b) mNmminus2 = (minus166 plusmn 16)+ (214 plusmn 011) (120575H (119879b) MPa12) (8)

with a correlation coefficient of 09797 see Figure 2The value[18] for dimethyl ether is an outlier

Koenhen and Smolders [141] reported the relationshipbetween the dispersion solubility parameter and the index of


0

10

20

30

40

120590(m

N m

minus1)

0 2010 30

120575H (MPa12)

Figure 2 The surface tension of liquefied gases at their boilingpoints 120590mNmminus2 plotted against their solubility parameters 120575HMPa12The symbols are for the surface tension from [16 17]e from[18] 998771 and [19] 998787 and for the outlier (CH3)2O998810 [18]

refraction 119899D for many substances that are liquid at ambienttemperatures but not for those that are gasesThe expression

120575H (cal cmminus3)12 = 955119899D minus 555 (9)

at an unspecified temperature (presumably 298K) was foundand may be applicable also for gaseous solutes

4 Conclusions

The solubility parameters 120575H(119879b) of nonreactive permanentgases at their boiling points 119879b (lt290K) including mostinorganic gases (excluding reactive ones such as halogensand hydrogen halides) and organic ones up to butane arepresented They have been calculated from individuallydiscussed values of their molar enthalpies of vaporizationand densities obtained from the literature Where availablethe coefficients of the temperature dependence expression120575H(119879) are also tabulated The 120575H(119879b) values of representativeinorganic gases increase with their molar masses but thoseof organic solutes (hydrocarbon) tend to diminish withincreasing molar masses The 120575H values generally diminishwith increasing temperatures Values of the solubility param-eters reported in the literature that were derived from thesolubilities of the gases in various solvents are inconsistentamong various authors The 120575H(119879b) values correlate linearlywith the attractive interaction energies of binary collisions ofthe gas molecules the depths of the potential wells 120576119896B andwith the surface tensions 120590(119879b) of the liquefied gases

Competing Interests

The author declares that there are no competing interestsregarding the publication of this paper

References

[1] J H Hildebrand and R L Scott Solubility of Non-ElectrolytesReinhold New York NY USA 3rd edition 1949

[2] C M Hansen Hansen Solubility Parameters CRC Press BocaRaton Fla USA 2007

[3] J A Riddick W B Bunger and T K Sakano Organic SolventsJohn Wiley amp Sons New York NY USA 4th edition 1986

[4] Y Marcus The Properties of Solvents John Wiley amp SonsChichester UK 1998

[5] Y Marcus ldquoSurface tension and cohesive energy density ofmolten saltsrdquoThermochimica Acta vol 571 pp 77ndash81 2013

[6] Y Marcus Ionic Liquid Properties Springer Dordrecht TheNetherlands 2016

[7] D R Lide EdHandbook of Chemistry and Physics CRC PressBoca Raton Fla USA 82nd edition 2001-2002

[8] International Critical TablesMcGraw-Hill NewYorkNYUSA1926

[9] F D Rossini K S Pitzer W J Taylor et al Selected Values ofProperties of Hydrocarbons vol 461 of United States NationalBureau of Standards Circular 1947

[10] R Gallant Physical Properties of Hydrocarbons Gulf PublishingCompany Houston Tex USA 1968

[11] Selected Values of Properties of Chemical Compounds TexasAampM University College Station Tex USA 1980

[12] I L Leites ldquoSome trends and a prediction of the solubility ofgases in liquids and the heat of dissolutionrdquo Separation andPurification Technology vol 12 no 3 pp 201ndash213 1997

[13] V Teplyakov and PMeares ldquoCorrelation aspects of the selectivegas permeabilities of polymeric materials andmembranesrdquoGasSeparation and Purification vol 4 no 2 pp 66ndash74 1990

[14] C L De Ligny and N G Van der Veen ldquoA test of Pierottirsquostheory for the solubility of gases in liquids bymeans of literaturedata of solubility and entropy of solutionrdquoChemical EngineeringScience vol 27 no 2 pp 391ndash401 1972

[15] S V Churakov and M Gottschalk ldquoPerturbation theory basedequation of state for polar molecular fluids I Pure fluidsrdquoGeochimica et Cosmochimica Acta vol 67 no 13 pp 2397ndash24142003

[16] W Porteous ldquoCalculating surface tension of light hydrocarbonsand their mixturesrdquo Journal of Chemical and Engineering Datavol 20 no 3 pp 339ndash343 1975

[17] P Dashora P Karnawat and U Parnami ldquoA study of thetemperature dependence of topological short-range-order andsurface tension of liquid elementsrdquo Physica Scripta vol 64 no6 pp 554ndash562 2001

[18] V A M Soares B J V S de Almeida I A McLure and R AHiggins ldquoSurface tension of pure and mixed simple substancesat low temperaturesrdquo Fluid Phase Equilibria vol 32 no 1 pp9ndash16 1986

[19] M Y Gorbachev ldquoDependence of surface tension of near-boiling non-associated liquids on their molar volume and somecritical constantsrdquo Physics and Chemistry of Liquids vol 39 no3 pp 315ndash325 2001

[20] H L Clever J H Saylor and P M Gross ldquoThe solubility ofhelium neon argon krypton and xenon in methylcyclohexaneand perfluoromethylcyclohexanerdquo Journal of Physical Chem-istry vol 62 no 1 pp 89ndash91 1958

[21] S J Yosim and B B Owens ldquoCalculation of heats of vapor-ization and fusion of nonionic liquids from the rigidminussphere


equation of staterdquoThe Journal of Chemical Physics vol 39 no 9pp 2222ndash2226 1963

[22] G A Cook Argon Helium and the Rare Gases IntersciencePublishers New York NY USA 1961

[23] R J Donnelly and C F Barenghi ldquoThe observed propertiesof liquid helium at the saturated vapor pressurerdquo Journal ofPhysical and Chemical Reference Data vol 27 no 6 pp 1217ndash1274 1998

[24] R G Linford and D G Thornhill ldquoUse of Hildebrand andLamoreauxrsquos theory to predict solubility and related propertiesof gas-liquid systemsrdquo Journal of Applied Chemistry andBiotech-nology vol 27 no 3 pp 479ndash497 1977

[25] CGladun ldquoThe specific heat at constant volumeof liquid neonrdquoCryogenics vol 6 no 1 pp 27ndash30 1966

[26] K Leonhard and U K Deiters ldquoMonte Carlo simulations ofneon and argon using ab initio potentialsrdquo Molecular Physicsvol 98 no 20 pp 1603ndash1616 2000

[27] JM Prausnitz and FH Shair ldquoA thermodynamic correlation ofgas solubilitiesrdquo AIChE Journal vol 7 no 4 pp 682ndash687 1961

[28] M A LaPack J C Tou V L McGuffin and C G EnkeldquoThe correlation of membrane permselectivity with Hildebrandsolubility parametersrdquo Journal of Membrane Science vol 86 no3 pp 263ndash280 1994

[29] H H Chen C C Lim and R A Aziz ldquoThe enthalpy ofvaporization and internal energy of liquid argon kryptonand xenon determined from vapor pressuresrdquo The Journal ofChemical Thermodynamics vol 7 no 2 pp 191ndash199 1975

[30] M J Terry J T Lynch M Bunclark K R Mansell and L A KStaveley ldquoThe densities of liquid argon krypton xenon oxygennitrogen carbon monoxide methane and carbon tetrafluoridealong the orthobaric liquid curverdquo The Journal of ChemicalThermodynamics vol 1 no 4 pp 413ndash424 1969

[31] C Lewis P K Hopke and J J Stukel ldquoSolubility of radon inselected perfluorocarbon compounds and waterrdquo Industrial andEngineering Chemistry Research vol 26 no 2 pp 356ndash359 1987

[32] J R Mick M S Barhaghi and J J Potoff ldquoPrediction of radon-222 phase behavior by Monte Carlo simulationrdquo Journal ofChemical amp Engineering Data vol 61 no 4 pp 1625ndash1631 2016

[33] D R Stull and G C Sinke ldquoIntroductionrdquo in ThermodynamicProperties of the Elements vol 18 of Advances in ChemistrySeries chapter 1 pp 3ndash5 1956

[34] A Van Itterbeek O Verbeke F Theeuwes and V JansooneldquoThe molar volume of liquid normal hydrogen in the temper-ature range between 21∘K and 40∘K at pressures up to 150 atmrdquoPhysica vol 32 no 9 pp 1591ndash1600 1966

[35] J W Leachman R T Jacobsen S G Penoncello and E WLemmon ldquoFundamental equations of state for parahydrogennormal hydrogen and orthohydrogenrdquo Journal of Physical andChemical Reference Data vol 38 no 3 pp 721ndash748 2009

[36] Y S Sistla L Jain and A Khanna ldquoValidation and predictionof solubility parameters of ionic liquids for CO2 capturerdquoSeparation and Purification Technology vol 97 pp 51ndash64 2012

[37] J C Gjaldbaek and J H Hildebrand ldquoThe solubility of nitrogenin carbon disulfide benzene normal- and cyclo-hexane and inthree fluorocarbonsrdquo Journal of the American Chemical Societyvol 71 no 9 pp 3147ndash3150 1949

[38] P C Jordan P J vanMaaren JMavri D van der Spoel andH JC Berendsen ldquoTowards phase transferable potential functionsmethodology and application to nitrogenrdquo The Journal ofChemical Physics vol 103 no 6 pp 2272ndash2285 1995

[39] Y Suyama and J Oishi ldquoA determination of vapor pressure-temperature relation of oxygen based on latent heat measure-ments at normal boiling pointrdquo Japanese Journal of AppliedPhysics vol 15 no 6 pp 1037ndash1043 1976

[40] K K Kelley and E G King ldquoContributions to the data oftheoretical metallurgy XIV Entropies of the elements andinorganic compoundsrdquo United States Bureau of Mines Bulletinvol 592 1961

[41] A Y Zasetsky and I M Svishchev ldquoLocal order in liquid oxy-gen computer simulations with point charge modelrdquo ChemicalPhysics Letters vol 334 no 1ndash3 pp 107ndash111 2001

[42] W Fischer and W Weidemann ldquoThe gas densities of BF3 SiF4and GeF4 at room temperature and in the vicinity of the boilingpointrdquo Zeitschrift fur Anorganische und Allgemeine Chemie vol213 no 1 pp 106ndash114 1933

[43] Yu M Fetisov A A Efremov Yu I Levin and Ya DZelrsquovenskii ldquoLiquid-vapor equilibrium of dilute solutions ofphiosgen in boron trichloriderdquo Trudy InstitutamdashMoskovskiiKhimiko-Tekhnologicheskii Institut Imeni D I Mendeleeva vol67 pp 34ndash37 1970

[44] T J Ward ldquoDensity viscosity and thermal conductivity ofliquid boron trichloriderdquo Journal of Chemical and EngineeringData vol 14 no 2 pp 167ndash168 1969

[45] H V A Briscoe P L Robinson and H C Smith ldquoThe densityof boron trichloride and the suspected variation in the atomicweight of boronrdquo Journal of the Chemical Society pp 282ndash2901927

[46] R D Goodwin ldquoCarbon monoxide thermophysical propertiesfrom 68 to 1000K at pressures to 100MPardquo Journal of Physicaland Chemical Reference Data vol 14 pp 849ndash869 1965

[47] S F Barreiros J C G CaladoM N da Ponte andW B StreettldquoThe equation of state and thermnodynamic properties of liquidcarbon monoxiderdquo Advances in Cryogenic Engineering vol 27pp 903ndash910 1982

[48] R Span and W Wagner ldquoA new equation of state for carbondioxide covering the fluid region from the triple-point temper-ature to 1100K at pressures up to 800MPardquo Journal of Physicaland Chemical Reference Data vol 25 no 6 pp 1509ndash1596 1996

[49] P Politzer Y Ma P Lane and M C Concha ldquoComputationalprediction of standard gas liquid and solid-phase heats offormation and heats of vaporization and sublimationrdquo Interna-tional Journal ofQuantumChemistry vol 105 no 4 pp 341ndash3472005

[50] W F Giauque and W M Jones ldquoCarbonyl chloride EntropyHeat capacity Vapor pressure Heats of fusion and vaporizationComments on solid sulfur dioxide structurerdquo Journal of theAmerican Chemical Society vol 70 no 1 pp 120ndash124 1948

[51] Y-L Huang M Heilig H Hasse and J Vrabec ldquoVapor-liquid equilibria of hydrogen chloride phosgene benzenechlorobenzene ortho-dichlorobenzene and toluene by molec-ular simulationrdquo AIChE Journal vol 57 no 4 pp 1043ndash10602011

[52] C N Davies ldquoThe density and thermal expansion of liquidphosgenerdquoThe Journal of Chemical Physics vol 14 no 1 pp 48ndash49 1946

[53] O Ruff J Fischer and F Luft ldquoThe nitrogen trifluoriderdquoZeitschrift fur Anorganische undAllgemeine Chemie vol 172 no1 pp 417ndash425 1928

[54] I B Sladkov and N Yu Novikova ldquoPhysicochemical propertiesof some nitrogen halidesrdquoRussian Journal of Applied Chemistryvol 69 no 11 pp 1660ndash1664 1996


[55] T Atake and H Chihara ldquoA new condensed gas calorimeterThermodynamic properties of solid and liquid dinitrogenoxiderdquo Bulletin of the Chemical Society of Japan vol 47 no 9pp 2126ndash2136 1974

[56] A J Leadbetter D J Taylor and B Vincent ldquoThe densities andsurface tensions of liquid ethane and nitrous oxiderdquo CanadianJournal of Chemistry vol 42 no 12 pp 2930ndash2932 1964

[57] E C Bingham ldquoThe relation of heat of vaporization to boilingpointrdquo Journal of the American Chemical Society vol 28 no 6pp 723ndash731 1906

[58] I B Golovanov and S M Zhenodarova ldquoQuantitative struc-ture-property relationship XXIV Properties of halo derivativesof methane silane and methylsilanesrdquo Russian Journal ofGeneral Chemistry vol 75 no 12 pp 1899ndash1903 2005

[59] E L Pace and J S Mosser ldquoThermodynamic properties ofsilicon tetrafluoride from 15∘ k to its triple point The entropyfrom molecular and spectroscopic datardquoThe Journal of Chemi-cal Physics vol 39 no 1 pp 154ndash158 1963

[60] R Stoslashlevik ldquoPrediction of standard heat capacity and entropy ofinorganicXY3 XY4 andXY5 gases at 25∘Cbased on correlationwith the normal boiling pointrdquoActa Chemica Scandinavica vol43 pp 758ndash762 1989

[61] J L Lyman and T Noda ldquoThermochemical properties of Si2F6and SiF4 in gas and condensed phasesrdquo Journal of Physical andChemical Reference Data vol 30 no 1 pp 165ndash186 2001

[62] D D Lawson ldquoMethods of calculating engineering parametersfor gas separationsrdquo Applied Energy vol 6 no 4 pp 241ndash2551980

[63] A Vetere ldquoAn empirical method to evaluate the solubility ofseveral gases in polar and non-polar solventsrdquo Fluid PhaseEquilibria vol 132 no 1-2 pp 77ndash91 1997

[64] R F Blanks and J M Prausnitz ldquoThermodynamics of polymersolubility in polar and nonpolar systemsrdquo Industrial ampEngineer-ing Chemistry Fundamentals vol 3 no 1 pp 1ndash8 1964

[65] J Vitovec and V Fried ldquoSolubility of acetylene in benzenetoluene and p-xylenerdquo Collection of Czechoslovak ChemicalCommunications vol 25 no 6 pp 1552ndash1556 1960

[66] M L Bradford and G Thodos ldquoSolubility parameters ofhydrocarbonsrdquoThe Canadian Journal of Chemical Engineeringvol 44 no 6 pp 345ndash348 1966

[67] J G Helpenstill and M van Winkle ldquoPrediction of infinitedilution activity coefficients for polar-polar binary systemsrdquoIndustrial amp Engineering Chemistry Process Design and Devel-opment vol 7 no 2 pp 213ndash220 1968

[68] F Brown and P L Robinson ldquoPreparation and some physicalproperties of sulphur tetrafluoriderdquo Journal of the ChemicalSociety pp 3147ndash3151 1955

[69] A G Streng ldquoMiscibility and compatibility of some liquefiedand solidified gases at low temperaturesrdquo Journal of Chemicaland Engineering Data vol 16 no 3 pp 357ndash359 1971

[70] M Funke R Kleinrahm and W Wagner ldquoMeasurement andcorrelation of the (p120588T) relation of sulfur hexafluoride (SF6)II Saturated-liquid and saturated-vapour densities and vapourpressures along the entire coexistence curverdquo The Journal ofChemical Thermodynamics vol 34 pp 735ndash354 2001

[71] M Yu Gorbachev ldquoDependence of surface tension of near-boiling non-associated liquids on their molar volume and somecritical constantsrdquo Physics and Chemistry of Liquids vol 39 no3 pp 315ndash325 2001

[72] D R Anderson E-H Lee R H Pildes and S L BernasekldquoEnergy accommodation coefficients of internally excited

moleculesrdquo The Journal of Chemical Physics vol 75 no 9 pp4621ndash4625 1981

[73] T Ohta O Yamamuro and H Suga ldquoHeat capacity andenthalpy of sublimation of sulfur hexafluoriderdquo The Journal ofChemical Thermodynamics vol 26 no 3 pp 319ndash331 1994

[74] J T Clarke E B Rifkin and H L Johnston ldquoCondensedgas calorimetry III Heat capacity heat of fusion heat ofvaporization vapor pressures and entropy of diborane between13∘K and the boiling point (18032∘K)rdquo Journal of the AmericanChemical Society vol 75 no 4 pp 781ndash785 1953

[75] A W Laubengayer R P Ferguson and A E Newkirk ldquoThedensities surface tensions and parachors of diborane borontriethyl and boron tribromide The atomic parachor of boronrdquoJournal of the American Chemical Society vol 63 no 2 pp 559ndash561 1941

[76] H E Wirth and E D Palmer ldquoVapor pressure and dielectricconstant of diboranerdquoThe Journal of Physical Chemistry vol 60no 7 pp 911ndash913 1956

[77] M S Jhon J Grosh and H Eyring ldquoThe significant structureandproperties of liquid hydrazine and liquid diboranerdquoPhysicalChemistry vol 71 no 7 pp 2253ndash2258 1967

[78] R W Taft Jr and H H Sisler ldquoHydrogen Bonding andsome observations on the physical properties of the hydrogencompounds of the elements of groups 4a 5a 6a and 7ardquo Journalof Chemical Education vol 24 no 4 pp 175ndash181 1947

[79] A D Zorin I V Runovskaya S B Lyakhmanov and LV Yudanova ldquoĐensity of the simplest volatile hydrides ofthe elements of groups III VIrdquo Russian Journal of InorganicChemistry vol 12 pp 1335ndash1338 1967

[80] Y Sakiyama S Takagi and Y Matsumoto ldquoValidation of inter-molecular pair potential model of SiH4 molecular-dynamicssimulation for saturated liquid density and thermal transportpropertiesrdquo Journal of Chemical Physics vol 122 no 23 ArticleID 234501 2005

[81] G G Devyatykh A D Zorin T K Postnikova and V AUmilin ldquoLiquid-vapor equilibria in binary systems formedby arsine with phosphine hydrogen sulphide and hydrogenchloriderdquo Russian Journal of Inorganic Chemistry vol 17 pp851ndash854 1969

[82] F Paneth W Haken and E Rabinowitsch ldquoUber die Rein-darstellung und Eigenschaften des Zinnwasserstoffsrdquo Berichteder Deutschen Chemischen Gesellschaft B vol 57 no 10 pp1891ndash1903 1924

[83] A A Durrant T G Pearson and P L Robinson ldquoPhysical rela-tionships amongst the hydrides of elements pf the fifth groupwith special reference to association in these compoundsrdquoJournal of the Chemical Society pp 730ndash735 1934

[84] R Ludwig ldquoThe effect of hydrogen bonding on the thermody-namic and spectroscopic properties of molecular clusters andliquidsrdquo Physical Chemistry Chemical Physics vol 4 no 22 pp5481ndash5487 2002

[85] R H Sherman and W F Giauque ldquoArsine Vapor pressureheat capacity heats of transition fusion and vaporization Theentropy from calorimetric and from molecular datardquo Journalof the American Chemical Society vol 77 no 8 pp 2154ndash21601955

[86] A G Cubitt C Henderson L A K Staveley I M A FonsecaA GM Ferreira and L Q Lobo ldquoSome thermodynamic prop-erties of liquid hydrogen sulphide and deuterium sulphiderdquoTheJournal of ChemicalThermodynamics vol 19 no 7 pp 703ndash7101987


[87] T Kristof and J Liszi ldquoEffective intermolecular potential forfluid hydrogen sulfiderdquo Journal of Physical Chemistry B vol 101no 28 pp 5480ndash5483 1997

[88] S Riahi andC N Rowley ldquoA drude polarizablemodel for liquidhydrogen sulfiderdquo Journal of Physical Chemistry B vol 117 no17 pp 5222ndash5229 2013

[89] E A Orabi and G Lamoureux ldquoSimulation of liquid andsupercritical hydrogen sulfide and of alkali ions in the pure andaqueous liquidrdquo Journal of Chemical Theory and Computationvol 10 no 8 pp 3221ndash3235 2014

[90] E C Clarke and D N Glew ldquoDeuterium and hydrogensulfides vapor pressures molar volumes and thermodynamicpropertiesrdquo Canadian Journal of Chemistry vol 48 no 5 pp764ndash775 1970

[91] P L Robinson andW E Scott ldquo127 Some physical properties ofthe hydrides of selenium and telluriumrdquo Journal of the ChemicalSociety pp 972ndash979 1932

[92] R Forcrand and H Fonzes-Diacon ldquoOn the vapor pressures ofhydrogen selenide and the dissociation of its hydraterdquo ComptesRendus vol 134 pp 229ndash230 1902

[93] W L Jorgensen J D Madura and C J Swenson ldquoOptimizedintermolecular potential functions for liquid hydrocarbonsrdquoJournal of the American Chemical Society vol 106 no 22 pp6638ndash6646 1984

[94] X Daura A E Mark and W F Van Gunsteren ldquoParametriza-tion of aliphatic CHn united atoms of GROMOS96 force fieldrdquoJournal of Computational Chemistry vol 19 no 5 pp 535ndash5471998

[95] T Oi J Shulman A Popowicz and T Ishida ldquoVapor pressureisotope effects in liquid methyl fluoriderdquo Journal of PhysicalChemistry vol 87 no 16 pp 3153ndash3160 1983

[96] I M A Fonseca and L Q Lobo ldquoThermodynamics of liquidmixtures of xenon and methyl fluoriderdquo Fluid Phase Equilibriavol 47 no 2-3 pp 249ndash263 1989

[97] S C Potter D J Tildesley A N Burgess and S C Rogers ldquoAtransferable potential model for the liquid-vapour equilibria offluoromethanesrdquo Molecular Physics vol 92 no 5 pp 825ndash8331997

[98] J B Gilmour J O Zwicker J Katz and R L Scott ldquoFlu-orocarbon solutions at low temperatures V The liquid mix-tures C2H6 + C2F6 C3H8 +C2F6 CH4 + C3F8 C2H6 + C3F8C3H8 + C3F8 C4C10 +C3F8 iso-C4H10 +C3F8 C3H8 +C4F10n-C6H14 +C4F10 n-C7H16 +C4F10 n-CH20 + n-C4F10 and n-C10H22 + n-C4F10rdquo The Journal of Physical Chemistry vol 71no 10 pp 3259ndash3270 1967

[99] E K Watkins and W L Jorgensen ldquoPerfluoroalkanes confor-mational analysis and liquid-state properties from ab initio andmonte Carlo calculationsrdquo Journal of Physical Chemistry A vol105 no 16 pp 4118ndash4125 2001

[100] E F Meyer T A Renner and K S Stec ldquoCohesive energies inpolar organic liquids II The alkyl nitriles and the 1-chloroal-kanesrdquoThe Journal of Physical Chemistry vol 75 pp 642ndash6481975

[101] A Kumagai and H Iwasaki ldquoPressure-volume-temperaturerelationships of several polar liquidsrdquo Journal of Chemical ampEngineering Data vol 23 no 3 pp 193ndash195 1978

[102] F F M Freitas B J C Cabral and F M S S FernandesldquoComputer simulation of liquid methyl chloriderdquo Journal ofPhysical Chemistry vol 97 no 37 pp 9470ndash9477 1993

[103] A P Kudchadker S A Kudchadker R P Shukla and PR Patnaik ldquoVapor pressures and boiling points of selected

halomethanesrdquo Journal of Physical and Chemical ReferenceData vol 8 no 2 pp 499ndash517 1979

[104] S Mali and J Ghosh ldquoOn the vapour pressure and chemicalconstant of formaldehyderdquo Journal of the Indian ChemicalSociety vol 1 pp 37ndash43 1925

[105] H Russell Jr D W Osborne and D M Yost ldquoThe heatcapacity entropy heats of fusion transition and vaporizationand vapor pressures of methyl mercaptanrdquo Journal of theAmerican Chemical Society vol 64 no 1 pp 165ndash169 1942

[106] G A Kaminski R A Friesner and R Zhou ldquoA computation-ally inexpensive modification of the point dipole electrostaticpolarization model for molecular simulationsrdquo Journal of Com-putational Chemistry vol 24 no 3 pp 267ndash276 2003

[107] S P Tan H Adidharma J S Kargel and G M MarionldquoEquation of state for solid solution-liquid-vapor equilibria atcryogenic conditionsrdquo Fluid Phase Equilibria vol 360 pp 320ndash331 2013

[108] M L Klein and I R McDonald ldquoMolecular dynamics calcu-lations for solid and liquid acetylenerdquo Chemical Physics Lettersvol 80 no 1 pp 76ndash82 1981

[109] E Kordes ldquoInvestigation of the heterogeneous equilibriumliquid-vapor II Calculation of the density of liquid and vaporrdquoZeitschrift fur Elektrochemie und Angewandte PhysikalischeChemis vol 58 pp 76ndash80 1954

[110] AMichels and TWassenaar ldquoThe vapour pressure of ethylenerdquoPhysica vol 16 no 3 pp 221ndash224 1950

[111] J C G Calado P Clancy A Heintz and W B StreettldquoExperimental and theoretical study of the equation of state ofliquid ethylenerdquo Journal of Chemical and Engineering Data vol27 no 4 pp 376ndash385 1982

[112] C-H Chui and F B Canfield ldquoLiquid density and excessproperties of argon + krypton and krypton + xenon binaryliquid mixtures and liquid density of ethanerdquo Transactions ofthe Faraday Society vol 67 pp 2933ndash2940 1971

[113] D W Smith ldquoEmpirical bond additivity scheme for the calcu-lation of enthalpies of vaporisation of organic liquidsrdquo Journalof the Chemical SocietymdashFaraday Transactions vol 94 no 20pp 3087ndash3091 1998

[114] R W Taft M H Abraham G R Famini R M Doherty J LAbboud and M J Kamlet ldquoSolubility properties in polymersand biological media 5 An analysis of the physicochemicalproperties which influence octanol-water partition coefficientsof aliphatic and aromatic solutesrdquo Journal of PharmaceuticalSciences vol 74 no 8 pp 807ndash814 1985

[115] Z Sharafi and A Boushehri ldquoSaturated liquid densities for 33binary refrigerant mixtures based on the ISM equation of staterdquoInternational Journal of Thermophysics vol 26 no 3 pp 785ndash794 2005

[116] O Maass and E H Boomer ldquoVapor densities at low pressuresand over an extended temperature range I The propertiesof ethylene oxide compared to oxygen compounds of similarmolecular weightrdquo Journal of the American Chemical Societyvol 44 no 8 pp 1709ndash1728 1922

[117] W F Giauque and J Gordon ldquoThe entropy of ethylene oxideHeat capacity from 14 to 285∘K Vapor pressure Heats of fusionand vaporizationrdquo Journal of theAmericanChemical Society vol71 no 6 pp 2176ndash2181 1949

[118] J D Olson ldquoSolubility of nitrogen argon methane and ethanein ethylene oxiderdquo Journal of Chemical and Engineering Datavol 22 no 3 pp 326ndash329 1977


[119] B Eckl J Vrabec and H Hasse ldquoOn the application of forcefields for predicting a wide variety of properties ethylene oxideas an examplerdquo Fluid Phase Equilibria vol 274 no 1-2 pp 16ndash26 2008

[120] R M Kennedy M Sagenkahn and J G Aston ldquoThe heatcapacity and entropy heats of fusion and vaporization andthe vapor pressure of dimethyl ether The density of gaseousdimethyl etherrdquo Journal of the American Chemical Society vol63 no 8 pp 2267ndash2272 1941

[121] L A K Staveley and W I Tupman ldquoEntropies of vaporizationand internal order in liquidsrdquo Journal of the Chemical Societypp 3597ndash3606 1950

[122] J M Briggs T Matsui and W L Jorgensen ldquoMonte Carlosimulations of liquid alkyl ethers with the OPLS potentialfunctionsrdquo Journal of Computational Chemistry vol 11 no 8pp 958ndash971 1990

[123] T M Powell and W F Giauque ldquoPropylene The heat capacityvapor pressure heats of fusion and vaporization the third lawof thermodynamics and orientation equilibrium in the solidrdquoJournal of the American Chemical Society vol 61 no 9 pp2366ndash2370 1939

[124] W L Jorgensen D S Maxwell and J Tirado-Rives ldquoDevelop-ment and testing of the OPLS all-atom force field on conforma-tional energetics and properties of organic liquidsrdquo Journal ofthe American Chemical Society vol 118 no 45 pp 11225ndash112361996

[125] W R Parrish ldquoCompressed liquid propene densities between5 and 73∘C at pressures to 96MPardquo Journal of Chemical ampEngineering Data vol 32 no 3 pp 311ndash313 1987

[126] R A Ruehrwein and T M Powell ldquoThe heat capacity vaporpressure heats of fusion and vaporization of cyclopropaneEntropy and density of the gasrdquo Journal of the AmericanChemical Society vol 68 no 6 pp 1063ndash1066 1946

[127] D C-K Lin I H Silberberg and J J McKetta ldquoVolumetricbehavior vapor pressures and critical properties of cyclo-propanerdquo Journal of Chemical and Engineering Data vol 15 no4 pp 483ndash492 1970

[128] H C Helgeson C E Owens A M Knox and L RichardldquoCalculation of the standard molal thermodynamic propertiesof crystalline liquid and gas organic molecules at high temper-atures and pressuresrdquoGeochimica et CosmochimicaActa vol 62no 6 pp 985ndash1081 1998

[129] M F Costa Gomes J C G Calado and J M N A FareleiraldquoOrthobaric volumetric properties of liquid (propane + cyclo-propane) between T = (158 and 201) KrdquoThe Journal of ChemicalThermodynamics vol 31 no 9 pp 1183ndash1194 1999

[130] R D Goodwin ldquoSpecific heats of saturated and compressedliquid propanerdquo Journal of Research of the National Bureau ofStandards vol 83 pp 449ndash458 1983

[131] D Ambrose J H Ellender C H S Sprake and R TownsendldquoThermodynamic properties of organic oxygen compoundsXLIII Vapour pressures of some ethersrdquoThe Journal of Chemi-cal Thermodynamics vol 8 no 2 pp 165ndash178 1976

[132] Kh A Aronovich L P Kastorskii andK F Fedorova ldquoPhysico-chemical properties of methyl ethyl ether and its mixtures withdiethyl etherrdquo Zhurnal Fizicheskoi Khimii vol 41 pp 20ndash241967

[133] T Spyriouni I G Economou andDNTheodorou ldquoMolecularsimulation of 120572-olefins using a new united-atom potentialmodel vapor-liquid equilibria of pure compounds and mix-turesrdquo Journal of the American Chemical Society vol 121 no 14pp 3407ndash3413 1999

[134] L F G Martins E J M Filipe and J C G Calado ldquoLiquidmixtures involving cyclic molecules 2 xenon + cyclobutanerdquoThe Journal of Physical Chemistry B vol 105 no 44 pp 10936ndash10941 2001

[135] J J Martin ldquoThermodynamic properties of perfluorocyclobu-tanerdquo Journal of Chemical amp Engineering Data vol 7 no 1 pp68ndash72 1962

[136] H Kratzke E Spillner and SMuller ldquoThermodynamic proper-ties for n-butane 1The vapour pressure of liquid n-butanerdquoTheJournal of Chemical Thermodynamics vol 14 no 12 pp 1175ndash1181 1982

[137] T R Das C O Reed Jr and P T Eubank ldquoPVT surface andthermodynamic properties of n-butanerdquo Journal of Chemicaland Engineering Data vol 18 no 3 pp 244ndash253 1973

[138] J A Brown and W H Mears ldquoPhysical properties of n-perfluorobutanerdquo Journal of Physical Chemistry vol 62 no 8pp 960ndash962 1958

[139] M Shamsipur R Ghavami BHemmateenejad andH SharghildquoSolvatochromic Linear Solvation Energy Relationships (LSER)for solubility of gases in various solvents by target factoranalysisrdquo Journal of the Chinese Chemical Society vol 52 no 1pp 11ndash19 2005

[140] S W Mayer ldquoA molecular parameter relationship betweensurface tension and liquid compressibilityrdquo The Journal ofPhysical Chemistry vol 67 no 10 pp 2160ndash2164 1963

[141] D M Koenhen and C A Smolders ldquoThe determination ofsolubility parameters of solvents and polymers by means ofcorrelations with other physical quantitiesrdquo Journal of AppliedPolymer Science vol 19 no 4 pp 1163ndash1179 1975

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CatalystsJournal of


119867G(S) = 119901G119909G(S) (3)

where 119901G is the partial pressure of the gas that is at equilib-rium with its saturated solution Hence the larger the mea-sured Henry constant the smaller the actual (mole fraction)solubility The solubility of a permanent gas is generally notneeded at its normal boiling point but 120575HG(119879b) is a referencevalue from which the temperature dependence of 120575HG canbe used to obtain the value at the desired temperature Suchtemperature dependence data unfortunately are available foronly a minority of gaseous solutes

12 Hildebrand Solubility Parameters The values of the total(Hildebrand) solubility parameter of the gases dealt withhere 120575HG are obtained as the square roots of the cohesiveenergy densities 119888119890119889GThe latter are obtained from themolarenthalpies of vaporization and the molar volumes assumingthe liquefied gas vaporizes without association or dissociationto an ideal gas at 119879b that is at 101325 kPa as follows

119888119890119889G = 120575HG2 = (ΔV119867G (119879b) minus 119877119879b)119881G (119879b) (4)

2 The Required Data

In the following the subscript G is dropped because onlythe solute gases are being dealt with The required data forobtaining the solubility parameters 120575H are the normal boilingpoints of the liquefied gases 119879b their molar enthalpies ofvaporizationΔV119867(119879b) and their molar volumes119881(119879b) at theboiling point The molar volumes 119881 are obtained from theratios of the molar masses119872 and the densities 120588 119881 = 119872120588The molar volume is also the reciprocal of the concentration119888 119881cm3molminus1 = 1000(119888mol dmminus3) The molar masses andboiling points are taken from the Handbook [7] The otherquantities are obtained from the literature from primarysources as noted below when readily available or else fromsecondary sources (compilations) such as [8ndash11]

Following are details of the data used and the results ofthe application of (2) yielding 120575H(119879b)MPa12 values

21 Specific Data for Each Gas

211 Helium The earliest report of the solubility parameterof helium is that of Clever et al [20] derived from itssolubility in hydrocarbons and fluorocarbons and is tabu-lated at the normal boiling point as 05 cal12 cmminus32 (ie102MPa12) However the text above the table states that06 cal12 cmminus32 (ie 123MPa12) is ldquomore compatible withthe solubility parameter at the gas bprdquo The subsequentreport by Yosim andOwens [21] evaluated themolar enthalpyof vaporization using the scaled particle theory but reportedalso its experimental value and the density at the boilingpoint [22] fromwhich the value 120MPa12 is derivableThemost recent report is by Donnelly and Barenghi [23] whopresented density and vapor pressure data at 005 K intervalsaround the boiling point that interpolate to 119879b = 422K and

120588(119879b) = 01250 g cmminus3 They also presented four reports forΔV119867 at 4207K that average at 8304 plusmn 037 Jmolminus1 fromwhich the solubility parameter 120575H(119879b) = 122 plusmn 001MPa12is derived and represents the selected value

212 Neon The 120575H(119879b) value tabulated by Clever et al[20] obtained as described for He is 49 cal12 cmminus32 (ie1002MPa12) The value 120575H(119879b) = 949MPa12 is derivedfrom the [22] data reported byYosim andOwens [21] Linfordand Thornhill [24] reported the energy of vaporization asΔV119864(119879b) (presumably ΔV119867 minus 119877119879b) = 037 kcalmolminus1 andwith the density from Gladun [25] 006093mol cmminus3 thevalue 120575H(119879b) = 898MPa12 is derived Leonhard and Deiters[26] reported the densities and the molar enthalpy of thegas and liquid at 5 K intervals between 25 and 40K Thedifference in the latter yields ΔV119867 values so the expressionshown in Table 3 results fromwhich follows the value 120575H(119879b)= 1001MPa12 The value 120575H(119879b) = 1001MPa12 from [26]agreeing with that of [20] is adopted as the selected value forNe

213 Argon The 120575H(119879b) value tabulated by Clever et al[20] obtained as described for He is 70 cal12 cmminus32 (ie1432MPa12) The value 120575H(119879b) = 1419MPa12 is derivedfrom the data of [22] reported by Yosim and Owens [21]Much lower values were reported by Prausnitz and Shair[27] at an unspecified temperature 533 (calcm3)12 (ie1090MPa12) that was quoted by LaPack et al [28] Chenet al [29] presented the molar volumes and the molarenthalpies of vaporization or Ar at 17 temperatures betweenthe triple and boiling points from which the expressionfor the solubility parameter shown in Table 3 results and120575H(119879b) = 1407MPa12 Linford and Thornhill [24] reportedthe energy of vaporization as ΔV119864(119879b) = 1385 kcalmolminus1and with the molar volume from Terry et al [30] 119881(119879b) =28713 cm3molminus1 the value 120575H(119879b) = 1421MPa12 is derivedThe average of the four agreeing values 1421 plusmn 010MPa12is adopted as the representative value for 120575H(119879b)214 Krypton The 120575H(119879b) value tabulated by Clever et al[20] obtained as described for He is 75 cal12 cmminus32 (ie1534MPa12) The value 120575H(119879b) = 1521MPa12 is derivedfrom the data of [22] reported by Yosim and Owens [21]Much lower values were reported by Prausnitz and Shair[27] at an unspecified temperature 64 (calcm3)12 (ie1309MPa12) Chen et al [29] presented the molar vol-umes and the molar enthalpies of vaporization of Kr at 19temperatures between the triple and boiling points fromwhich the expression for the solubility parameter shown inTable 3 results and 120575H(119879b) = 1518MPa12 Linford andThorn-hill [24] reported the energy of vaporization as ΔV119864(119879b)= 200 kcalmolminus1 and with the molar volume from Terryet al [30] 119881(119879b) = 34731 cm3molminus1 the value 120575H(119879b) =1457MPa12 is derived The average of the three agreeingvalues 1524 plusmn 009MPa12 is adopted as the representativevalue for 120575H(119879b)





































































120575H = 120575c + 119896 (1 minus 119879R)119898 (5)













Gas 119879bK 120575HMPa12







Gas 119879bK 120575HMPa12



3 Discussion











minus0001297








119906 = 120576 [( 119903120590)12 minus ( 119903120590)

6] (6)





Rn 273ndash313 140 [27]298 172 [31]

H2298 45 [62]298 51 [36]

N2

253ndash435 53 [27 28]298 106 [62]298 119 [36]303 143 [63]

O2

273ndash333 82 [27 28]298 117 [62]298 147 [36]303 102 [63]

CO253ndash333 64 [27]298 119 [62]298 125 [36]

CO2

298 68 [62]298 123 [28]298 179 [36]313 225 [63]

NO 298 208 [36]

H2S298 207 [36]303 317 [63]

CH4

253ndash444 116 [27 28]298 96 [64]298 127 [62]298 140 [36]303 147 [63]

CH3Cl 298 198 [28]

C2H2298 138 [65]298 192 [36]

C2H4273ndash398 135 [27]298 113 [64]298 155 [36]

C2H6

255ndash422 135 [27 28]298 116 [64]298 80 [66]298 135 [62]298 156 [36]303 90 [63]

C3H6 298 125 [64]

C3H8

298 127 [64]298 122 [66]298 134 [67]298 136 [28 62]412 117 [63]

Table 4 Continued

Gas 119879K 120575HMPa12 Ref

C4H10

298 135 [64]298 135 [66]298 142 [67]298 139 [28]

0

100

200

300

400

0 200100 400 500300

120575H2 (MPa)

(120576k

B)(K

)



( 120576119896B) K = (104 plusmn 107)

+ (065 plusmn 005) [120575H (119879b) MPa12]2(7)







0

10

20

30

40

120590(m

N m

minus1)

0 2010 30

120575H (MPa12)





4 Conclusions


Competing Interests


References






























































































































































Journal of

Chemistry


Advances in

Physical Chemistry



Journal of

Volume 2014














Journal of

Spectroscopy



Journal of


Quantum Chemistry






CatalystsJournal of





































































120575H = 120575c + 119896 (1 minus 119879R)119898 (5)













Gas 119879bK 120575HMPa12







Gas 119879bK 120575HMPa12



3 Discussion











minus0001297








119906 = 120576 [( 119903120590)12 minus ( 119903120590)

6] (6)





Rn 273ndash313 140 [27]298 172 [31]

H2298 45 [62]298 51 [36]

N2

253ndash435 53 [27 28]298 106 [62]298 119 [36]303 143 [63]

O2

273ndash333 82 [27 28]298 117 [62]298 147 [36]303 102 [63]

CO253ndash333 64 [27]298 119 [62]298 125 [36]

CO2

298 68 [62]298 123 [28]298 179 [36]313 225 [63]

NO 298 208 [36]

H2S298 207 [36]303 317 [63]

CH4

253ndash444 116 [27 28]298 96 [64]298 127 [62]298 140 [36]303 147 [63]

CH3Cl 298 198 [28]

C2H2298 138 [65]298 192 [36]

C2H4273ndash398 135 [27]298 113 [64]298 155 [36]

C2H6

255ndash422 135 [27 28]298 116 [64]298 80 [66]298 135 [62]298 156 [36]303 90 [63]

C3H6 298 125 [64]

C3H8

298 127 [64]298 122 [66]298 134 [67]298 136 [28 62]412 117 [63]

Table 4 Continued

Gas 119879K 120575HMPa12 Ref

C4H10

298 135 [64]298 135 [66]298 142 [67]298 139 [28]

0

100

200

300

400

0 200100 400 500300

120575H2 (MPa)

(120576k

B)(K

)



( 120576119896B) K = (104 plusmn 107)

+ (065 plusmn 005) [120575H (119879b) MPa12]2(7)







0

10

20

30

40

120590(m

N m

minus1)

0 2010 30

120575H (MPa12)





4 Conclusions


Competing Interests


References






























































































































































Journal of

Chemistry


Advances in

Physical Chemistry



Journal of

Volume 2014














Journal of

Spectroscopy



Journal of


Quantum Chemistry






CatalystsJournal of








Gas 119879bK 120575HMPa12







Gas 119879bK 120575HMPa12



3 Discussion











minus0001297








119906 = 120576 [( 119903120590)12 minus ( 119903120590)

6] (6)





Rn 273ndash313 140 [27]298 172 [31]

H2298 45 [62]298 51 [36]

N2

253ndash435 53 [27 28]298 106 [62]298 119 [36]303 143 [63]

O2

273ndash333 82 [27 28]298 117 [62]298 147 [36]303 102 [63]

CO253ndash333 64 [27]298 119 [62]298 125 [36]

CO2

298 68 [62]298 123 [28]298 179 [36]313 225 [63]

NO 298 208 [36]

H2S298 207 [36]303 317 [63]

CH4

253ndash444 116 [27 28]298 96 [64]298 127 [62]298 140 [36]303 147 [63]

CH3Cl 298 198 [28]

C2H2298 138 [65]298 192 [36]

C2H4273ndash398 135 [27]298 113 [64]298 155 [36]

C2H6

255ndash422 135 [27 28]298 116 [64]298 80 [66]298 135 [62]298 156 [36]303 90 [63]

C3H6 298 125 [64]

C3H8

298 127 [64]298 122 [66]298 134 [67]298 136 [28 62]412 117 [63]

Table 4 Continued

Gas 119879K 120575HMPa12 Ref

C4H10

298 135 [64]298 135 [66]298 142 [67]298 139 [28]

0

100

200

300

400

0 200100 400 500300

120575H2 (MPa)

(120576k

B)(K

)



( 120576119896B) K = (104 plusmn 107)

+ (065 plusmn 005) [120575H (119879b) MPa12]2(7)







0

10

20

30

40

120590(m

N m

minus1)

0 2010 30

120575H (MPa12)





4 Conclusions


Competing Interests


References






























































































































































Journal of

Chemistry


Advances in

Physical Chemistry



Journal of

Volume 2014














Journal of

Spectroscopy



Journal of


Quantum Chemistry






CatalystsJournal of



Gas 119879bK 120575HMPa12



3 Discussion











minus0001297








119906 = 120576 [( 119903120590)12 minus ( 119903120590)

6] (6)





Rn 273ndash313 140 [27]298 172 [31]

H2298 45 [62]298 51 [36]

N2

253ndash435 53 [27 28]298 106 [62]298 119 [36]303 143 [63]

O2

273ndash333 82 [27 28]298 117 [62]298 147 [36]303 102 [63]

CO253ndash333 64 [27]298 119 [62]298 125 [36]

CO2

298 68 [62]298 123 [28]298 179 [36]313 225 [63]

NO 298 208 [36]

H2S298 207 [36]303 317 [63]

CH4

253ndash444 116 [27 28]298 96 [64]298 127 [62]298 140 [36]303 147 [63]

CH3Cl 298 198 [28]

C2H2298 138 [65]298 192 [36]

C2H4273ndash398 135 [27]298 113 [64]298 155 [36]

C2H6

255ndash422 135 [27 28]298 116 [64]298 80 [66]298 135 [62]298 156 [36]303 90 [63]

C3H6 298 125 [64]

C3H8

298 127 [64]298 122 [66]298 134 [67]298 136 [28 62]412 117 [63]

Table 4 Continued

Gas 119879K 120575HMPa12 Ref

C4H10

298 135 [64]298 135 [66]298 142 [67]298 139 [28]

0

100

200

300

400

0 200100 400 500300

120575H2 (MPa)

(120576k

B)(K

)



( 120576119896B) K = (104 plusmn 107)

+ (065 plusmn 005) [120575H (119879b) MPa12]2(7)







0

10

20

30

40

120590(m

N m

minus1)

0 2010 30

120575H (MPa12)





4 Conclusions


Competing Interests


References






























































































































































Journal of

Chemistry


Advances in

Physical Chemistry



Journal of

Volume 2014














Journal of

Spectroscopy



Journal of


Quantum Chemistry






CatalystsJournal of






minus0001297








119906 = 120576 [( 119903120590)12 minus ( 119903120590)

6] (6)





Rn 273ndash313 140 [27]298 172 [31]

H2298 45 [62]298 51 [36]

N2

253ndash435 53 [27 28]298 106 [62]298 119 [36]303 143 [63]

O2

273ndash333 82 [27 28]298 117 [62]298 147 [36]303 102 [63]

CO253ndash333 64 [27]298 119 [62]298 125 [36]

CO2

298 68 [62]298 123 [28]298 179 [36]313 225 [63]

NO 298 208 [36]

H2S298 207 [36]303 317 [63]

CH4

253ndash444 116 [27 28]298 96 [64]298 127 [62]298 140 [36]303 147 [63]

CH3Cl 298 198 [28]

C2H2298 138 [65]298 192 [36]

C2H4273ndash398 135 [27]298 113 [64]298 155 [36]

C2H6

255ndash422 135 [27 28]298 116 [64]298 80 [66]298 135 [62]298 156 [36]303 90 [63]

C3H6 298 125 [64]

C3H8

298 127 [64]298 122 [66]298 134 [67]298 136 [28 62]412 117 [63]

Table 4 Continued

Gas 119879K 120575HMPa12 Ref

C4H10

298 135 [64]298 135 [66]298 142 [67]298 139 [28]

0

100

200

300

400

0 200100 400 500300

120575H2 (MPa)

(120576k

B)(K

)



( 120576119896B) K = (104 plusmn 107)

+ (065 plusmn 005) [120575H (119879b) MPa12]2(7)







0

10

20

30

40

120590(m

N m

minus1)

0 2010 30

120575H (MPa12)





4 Conclusions


Competing Interests


References






























































































































































Journal of

Chemistry


Advances in

Physical Chemistry



Journal of

Volume 2014














Journal of

Spectroscopy



Journal of


Quantum Chemistry






CatalystsJournal of




Rn 273ndash313 140 [27]298 172 [31]

H2298 45 [62]298 51 [36]

N2

253ndash435 53 [27 28]298 106 [62]298 119 [36]303 143 [63]

O2

273ndash333 82 [27 28]298 117 [62]298 147 [36]303 102 [63]

CO253ndash333 64 [27]298 119 [62]298 125 [36]

CO2

298 68 [62]298 123 [28]298 179 [36]313 225 [63]

NO 298 208 [36]

H2S298 207 [36]303 317 [63]

CH4

253ndash444 116 [27 28]298 96 [64]298 127 [62]298 140 [36]303 147 [63]

CH3Cl 298 198 [28]

C2H2298 138 [65]298 192 [36]

C2H4273ndash398 135 [27]298 113 [64]298 155 [36]

C2H6

255ndash422 135 [27 28]298 116 [64]298 80 [66]298 135 [62]298 156 [36]303 90 [63]

C3H6 298 125 [64]

C3H8

298 127 [64]298 122 [66]298 134 [67]298 136 [28 62]412 117 [63]

Table 4 Continued

Gas 119879K 120575HMPa12 Ref

C4H10

298 135 [64]298 135 [66]298 142 [67]298 139 [28]

0

100

200

300

400

0 200100 400 500300

120575H2 (MPa)

(120576k

B)(K

)



( 120576119896B) K = (104 plusmn 107)

+ (065 plusmn 005) [120575H (119879b) MPa12]2(7)







0

10

20

30

40

120590(m

N m

minus1)

0 2010 30

120575H (MPa12)





4 Conclusions


Competing Interests


References






























































































































































Journal of

Chemistry


Advances in

Physical Chemistry



Journal of

Volume 2014














Journal of

Spectroscopy



Journal of


Quantum Chemistry






CatalystsJournal of


0

10

20

30

40

120590(m

N m

minus1)

0 2010 30

120575H (MPa12)





4 Conclusions


Competing Interests


References






























































































































































Journal of

Chemistry


Advances in

Physical Chemistry



Journal of

Volume 2014














Journal of

Spectroscopy



Journal of


Quantum Chemistry






CatalystsJournal of









































































































































Journal of

Chemistry


Advances in

Physical Chemistry



Journal of

Volume 2014














Journal of

Spectroscopy



Journal of


Quantum Chemistry






CatalystsJournal of

review article solubility parameters of permanent gases...hildebrand solubility parameters. e values...

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