Molar excess enthalpies of binary <i>n</i>-alcohol systems at 25 °C

Pope, Alison; Pflug, Hans D.; Dacre, B.; Benson, George C.

doi:10.1139/v67-436

Cited by 68 publications

(29 citation statements)

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“…10053. 'NRCC Postdoctorate Fellow 1965-1967 wherex2 is the mole fraction of decanol in the liquid phase and p Z 0 is the vapor pressure of decanol at the same temperature as the mixture.…”

Section: Methodsmentioning

confidence: 99%

“…The con, Oruence of the present free energy results for PrOHDeOH mixtures with those published previously (1) for MeOH-DeOH and EtOH-DeOH was investigated following the method described in ref. 12.…”

Section: (13) Congruence Calc~rlatioizsmentioning

confidence: 99%

“…In our considerations of the excess enthalpies and excess volumes of alcohol systems (12,13) a four term polynomial in reciprocal powers of the chain length was employed. A similar function could also be used in fitting the free energy data.…”

Section: (13) Congruence Calc~rlatioizsmentioning

confidence: 99%

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Vapor–liquid equilibrium studies of n-propanol–n-decanol mixtures

Singh¹,

Benson²

1968

Can. J. Chem.

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“…10053. 'NRCC Postdoctorate Fellow 1965-1967 wherex2 is the mole fraction of decanol in the liquid phase and p Z 0 is the vapor pressure of decanol at the same temperature as the mixture.…”

Section: Methodsmentioning

confidence: 99%

Section: (13) Congruence Calc~rlatioizsmentioning

confidence: 99%

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Vapor–liquid equilibrium studies of n-propanol–n-decanol mixtures

Singh¹,

Benson²

1968

Can. J. Chem.

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“…The difference in K; calculated from the assumption of ciE = 0 and aE = -2ciidVE/Vseems to be a little larger. 2 The concentration dependence of C; resembles that the CF and the C ! value at equimolar concentration is less than the CF value by 0.1 -0.5 J K-' mol-' in magnitude; the difference in C: from the values assumed for aE as described above was also small.3 Discussion A few thermodynamic studies of the methanol -isometric butanol systems have been carried out at 298.15 K. Murthy et al (13) reported values of VE for the s-BuOH system that are considerably larger than the present results.…”

Section: Resultsmentioning

confidence: 86%

“…An excess thermodynamic function, xE(vE, e , and CF) is defined by [2] x E = x -x d whereX is any thermodynamic function of solution and Xd is the ideal function, which obeys the ideal mixing law. Equations for calculation of these functions should be referred to in the previous paper (4).…”

Section: Resultsmentioning

confidence: 99%

Molar excess volumes, isentropic compressions, and isobaric heat capacities of methanol – isomeric butanol systems at 298.15 K

Okano¹,

Ogawa²,

Murakami³

1988

Can. J. Chem.

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This paper is dedicaterl to Professor James A. Morrison TSUKASA OKANO, HIDEO OGAWA, and SACHIO MURAKAM!. Can. J . Chem. 66,7 13 (1988). Molar excess volumes, molar excess isentropic compressions, and molar excess isobaric heat capacities for binary liquid mixtures of methanol with 2-methylpropanol, 2-butanol, and 2-methyl-2-propanol have been determined at 298.15 K. The concentration dependence and magnitude of these thermodynamic functions are quite different from those of the methanol -1-butanol system, which had been previously determined. Molar excess volumes for two of the present systems are positive over the whole concentration range, except for the 2-methyl-2-propanol system. For the latter system they are negative in the butanol-rich range. Molar excess isentropic compressions of these systems show slightly different concentration dependence from that of the excess volumes, but the order in magnitude resembles that of the excess volumes. Molar excess isobaric heat capacities for all systems are negative and show simple concentration dependence. The minimum values of excess heat capacities are correlated with the magnitude of molar isobaric heat capacities of the pure isomeric butanols. ' The behavior of these excess functions is discussed with reference to the differences in numbers and strength of hydrogen bonding between the pure liquid and the solution.TSUKASA OKANO, HIDEO OGAWA et SACHIO MURAKAMI. Can. J. Chem. 66,713 (1988).Operant B 298,15 K, on a dCterminC les volumes molaires en excks, les compressions molaires isentropiques en excks et les capacitts calorifiques molaires isobares en excks des melanges de liquides binaires form& d'une part de mCthanol et d'autre part de methyl-2 propanol, de butanol-2 ou de methyl-2 propanol-2. La relation avec la concentration ainsi que l'amplitude de ces fonctions thermodynamiques sont trks differentes de celles qu'on avait observCes avec le systkme mCthanol/butanol-1 qu'on avait CtudiC antkrieurement. Les volumes molaires en excks de deux systkmes, except6 celui du methyl-2 propanol-2, sont positifs B toutes les concentrations CtudiCes. Toutefois, avec ce demier systkme, ils sont nCgatifs pour les concentrations riches en butanol. Par comparaison avec les volumes an excks, les compressions molaires isentropiques en excks de ces systkmes prksentent des relations avec la concentration qui sont diffirentes; toutefois, I'ordre de grandeur resemble i celui des volumes en excks. Les capacites calorifiques molaires isobares en excks sont nCgatives pour tous les systkmes et la relation avec la concentration est simple. I1 existe une correlation entre les valeurs minimales des capacitts calorifiques en excks et I'amplitude des capacites calorifiques molaires isobares des butanols isomkres purs. On discute des comportements de ces fonctions en excks en fonction des differences dans les nombres et la force des liaisons hydrogknes entre le liquide pur et la solution.[Traduit par la revue]

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DISQUAC predictions on VLE andH^Efor ternary mixtures containing 1‐alkanols and hydrocarbons

González

Fuente

Cobos

et al. 1994

Ber Bunsenges Phys Chem

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Thermodynamic properties, vapor‐liquid equilibrium or excess enthalpy, for a set of 13 ternary mixtures including one or two 1‐alkanols and hydrocarbons are studied in the framework of the DISQUAC group contribution model. The study is extended for the binaries involved. The DISQUAC analysis is developed using interchange coefficients available in the literature. No ternary interactions are taken into account.The average relative standard deviations are 0.02 for pressure in the vapor‐liquid equilibria (4 systems); and 0.07 for the excess enthalpy (9 systems).

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Molar excess enthalpies of binary n-alcohol systems at 25 °C

Cited by 68 publications

References 0 publications

Vapor–liquid equilibrium studies of n-propanol–n-decanol mixtures

Vapor–liquid equilibrium studies of n-propanol–n-decanol mixtures

Molar excess volumes, isentropic compressions, and isobaric heat capacities of methanol – isomeric butanol systems at 298.15 K

DISQUAC predictions on VLE andH^Efor ternary mixtures containing 1‐alkanols and hydrocarbons

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Molar excess enthalpies of binary n-alcohol systems at 25 °C

Cited by 68 publications

References 0 publications

Vapor–liquid equilibrium studies of n-propanol–n-decanol mixtures

Vapor–liquid equilibrium studies of n-propanol–n-decanol mixtures

Molar excess volumes, isentropic compressions, and isobaric heat capacities of methanol – isomeric butanol systems at 298.15 K

DISQUAC predictions on VLE andHEfor ternary mixtures containing 1‐alkanols and hydrocarbons

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DISQUAC predictions on VLE andH^Efor ternary mixtures containing 1‐alkanols and hydrocarbons