The Heat Capacities and Heat of Crystallization of Some Isomeric Aromatic Compounds

Andrews, Donald H.; Lynn, George; Johnston, J. E.

doi:10.1021/ja01416a022

Cited by 91 publications

(50 citation statements)

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“…Andrews, et al [19], using a drop method similar to Hess but with the receiving vessel at 22° C, obtained linear relations for th e h eat capacity of solid and liqUld benzoic acid in the temperature range 22° to 200° C. Comparing th eir work in the range of this work, th eir valu es are about 5.4 percent high er at 300° K and 6.7 percent lower at 395° K. Using a cooling m ethod Hrynakowski and Smoczkiewiczowa [20] measured th e h eat capacity at 25° C. This value is 6.5 p ercent high er than the value in table 1. Parks et al [21], using an aneroid type calorimeter, measUl:ed the heat capacities from 90° to 295° K. Th ese values are within 1 percent of the values in table 1.…”

Section: Comparison With Other Resultsmentioning

confidence: 99%

“…Mathews [24] similarly calculated th e heat of fusion from th e cryoscopic constant obtained using anthracene as a solute at different concentrations. Andrews, et al [19] obtained th eir value for the h eat of fusion from the enth alpy curves for th e solid and liquid benzoic acid determined by th e drop method. Klosky, et al [25 ] calculated the h eat of fusion from th e vapor pressure curves for solid and liquid benzoic acid.…”

Section: Comparison With Other Resultsmentioning

confidence: 99%

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Calorimetric properties of benzoic acid from 0-degrees to 410-degrees-K

Furukawa¹,

McCoskey²,

King³

1951

J. RES. NATL. BUR. STAN.

133

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Section: Comparison With Other Resultsmentioning

confidence: 99%

Section: Comparison With Other Resultsmentioning

confidence: 99%

Calorimetric properties of benzoic acid from 0-degrees to 410-degrees-K

Furukawa¹,

McCoskey²,

King³

1951

J. RES. NATL. BUR. STAN.

133

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“…il nous est possible, partir de nos essais, d'tvaluer la pression de vapeur saturante des substances ttudites en utilisant la relation: dans laquelle AP(T) est la difftrence de pression de vapeur de part et d'autre du trou d'effusion; P(T), la pression mesurte par effusion a la temperature T; dmldt, la masse de substance effusCe par unitt de temps; R , la constance des gaz parfaits; M, la masse molaire de la substance; F, le facteur de Clausing et a , l'aire de l'orifice d'effusion. (2,3,26) Nous avons essay6 d'expliquer la raison pour laquelle nos valeurs de AfUsHm et de AtISHm sont inftrieures a celles de la litttrature. Parmi les facteurs tventuellement responsables de la diffirence obsemte, nous pouvons citer :…”

Section: 3unclassified

Étude thermodynamique des trois isomères du dihydroxybenzène

Sabbah¹,

Buluku²

1991

Can. J. Chem.

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R e p le 2 octobre 1990 R. SABBAH et E. N. L. E. BULUKU. Can. J. Chem. 69,481 (1991). Le prtsent travail porte sur 1'Ctude thermodynamique des trois isomeres du dihydroxybenzene. Cette ttude a permis la dCtermination des enthalpies de combustion, de sublimation, de fusion et de transition des 1,2-, 1,3-et 1,4-dihydroxybenzenes. Les techniques utilisCes ont Ct C la calorimCtrie de combustion de faibles quantitCs de substances, la calorimCtrie de changement d'Ctat (sublimation), l'analyse thermique differentielle et la mesure des capacitts calorifiques. L'ensemble des rCsultats expCrimentaux a permis de : mettre en Cvidence l'existence d'une liaison hydrogkne intramolCculaire dans l'isomkre ortho; prkciser la stabilitk relative des trois molCcules de dihydrobenzenes; et determiner : i partir de l'enthalpie de sublimation, une valeur CnergCtique pour les liaisons intermolCculaires; 1'Cnergie de conjugaison expkrimentale et de la comparer i la valeur thtorique; l'enthalpie d'atomisation 3 partir de laquelle a Ct C calculCe I'enthalpie de la liaison intramolCculaire Cb-OH.Mots clts : thermodynamique, calorimCtrie, analyse thermique differentielle, 1,2-dihydroxybenzkne ou catCcho1; 1,3-dihydroxybenzkne ou rCsorcino1; 1,4-dihydroxybenzene ou hydroquinone ou quinol; enthalpies de combustion, de sublimation, de fusion, de transition; Cnergie de conjugaison; enthalpies d'atomisation, de liaisons inter-et intra-molCculaires; temperature du point triple et de transition.R. SABBAH and E. N. L. E. BULUKU. Can. J. Chem. 69,481 (1991). The present work is concerned with a thermodynamic study of the three isomers of dihydroxybenzene. By combustion calorimetry of small amounts of substance, sublimation calorimetry, differential thermal analysis, and heat capacity measurements, it was possible to determine the enthalpies of formation of 1,2-, 1 3 , and 1,4-dihydroxybenzene in the condensed and gaseous phases, their enthalpies of fusion and transition, and the temperature of their triple point and transition. The experimental results are used to discuss the relative stability and determine the conjugation energy of the three compounds. The values are in good agreement with the theoretical values obtained from a quantum chemical calculation. The enthalpies of atomization enabled us to determine an energy value for the intramolecular Cb-OH bond in dihydroxybenzenes and to correlate it with previous results obtained from a study of alkane-diols. The enthalpies of sublimation were discussed. An intramolecular hydrogen bond was displayed in the ortho isomer. Intermolecular hydrogen bonds associated with van der Waals interactions exist in dihydroxybenzenes. Their energy contributions were determined.Key words: thermodynamics, calorimetry, differential thermal analysis, 1,2-benzenediol or 1,2-dihydroxybenzene or catechol; 1,3-benzenediol or 1 $dihydroxybenzene or resorcinol; 1,4-benzenediol or 1,4-dihydroxybenzene or hydroquinone or quinol; enthalpies of combustion, of sublimation, of fusion, of transition, energy of conjugation, enthalp...

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“…The solubilities of three trifluoromethylbenzoic acid isomers in supercritical carbon dioxide 3-trifluoromethylbenzoic acid a) Ginnings and Furukawa [21] b) Andrews et al [22] c) This work. …”

Section: Resultsmentioning

confidence: 96%