A versatile apparatus to study the vapor pressures and heats of vaporization of carbazole, 9-fluorenone and 9-hydroxyfluorene at elevated temperatures

Sivaraman, A.; Martin, Raymond J.; Kobayashi, Riki

doi:10.1016/0378-3812(83)85019-5

Cited by 18 publications

(11 citation statements)

References 10 publications

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“…Deviations from the results of the present research are very large and reach 40% at the low-temperature extreme, as shown in figure 3. Sivaraman et al [46] also calculated enthalpies of vaporization with their results that agree poorly with the values given in table 9. Thermodynamic consistency was demonstrated earlier for the results of the present research, and consequently, we conclude that the results of Sivaraman et al [46] are in error.…”

Section: Comparisons With Experimental Property Values From the Litercontrasting

confidence: 43%

“…These values are in general accord with those of this research, but with much larger uncertainties than those reported here. The enthalpy of fusion D 1 cr H for 9-fluorenone was reported by Sabbah et al [ [46] for the temperature range 426 < (T/K) < 623 with a stated relative uncertainty of 0.01%. Deviations from the results of the present research are very large and reach 40% at the low-temperature extreme, as shown in figure 3.…”

Section: Comparisons With Experimental Property Values From the Litermentioning

confidence: 70%

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Thermodynamic properties of 9-fluorenone: Mutual validation of experimental and computational results

Chirico

Kazakov

Steele

2012

The Journal of Chemical Thermodynamics

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a b s t r a c tMeasurements leading to the calculation of thermodynamic properties for 9-fluorenone (IUPAC name 9H-fluoren-9-one and Chemical Abstracts registry number [486-25-9]) in the ideal-gas state are reported. Experimental methods were adiabatic heat-capacity calorimetry, inclined-piston manometry, comparative ebulliometry, and combustion calorimetry. Critical properties were estimated. Molar entropies for the ideal-gas state were derived from the experimental studies at selected temperatures T between T = 298.15 K and T = 600 K, and independent statistical calculations were performed based on molecular geometry optimization and vibrational frequencies calculated at the B3LYP/6 À 31 + G(d,p) level of theory. Values derived with the independent methods are shown to be in excellent accord with a scaling factor of 0.975 applied to the calculated frequencies. This same scaling factor was successfully applied in the analysis of results for other polycyclic molecules, as described in recent articles by this research group. All experimental results are compared with property values reported in the literature. Thermodynamic consistency between properties is used to show that several studies in the literature are erroneous.Published by Elsevier Ltd.

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Section: Comparisons With Experimental Property Values From the Litercontrasting

confidence: 43%

Section: Comparisons With Experimental Property Values From the Litermentioning

confidence: 70%

Thermodynamic properties of 9-fluorenone: Mutual validation of experimental and computational results

Chirico

Kazakov

Steele

2012

The Journal of Chemical Thermodynamics

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“… a Value taken from ref . b Value taken from ref . c Value taken from ref . d Value taken from refs and . e Value taken from ref . f Value taken from ref . g Value taken from ref . …”

Section: Methodsmentioning

confidence: 99%

Measurement and Modeling of the Solubility of 9H-Carbazole in Sub- and Supercritical Propane

et al. 2011

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The solubility of 9H-carbazole in sub- and supercritical propane has been measured using a static view cell at pressures from (4.3 to 10.0) MPa and temperatures from (323 to 405) K. The mole fraction of 9H-carbazole varied from 4·10−5 to 4·10−4 over the experimental range studied. The solubility of 9H-carbazole in propane is 1 order of magnitude higher than that of 9H-carbazole in CO2 for similar values of the reduced pressure and temperature, which highlights the excellent solvent properties of propane relative to CO2 for the extraction of polyaromatic compounds. The experimental solubility data were correlated with the Peng−Robinson equation of state using six different sets of mixing rules for the estimation of the mixture parameters a M and b M. Good fits of the experimental results were obtained for all of the mixing rules tested, especially for those involving two adjustable parameters; the absolute average percentage deviation (AAPD) was 16.4 % for the best fit. In addition, the empirical equation of Chrastil was used to model the experimental solubility, and a similar AAPD (16.6 %) was obtained. In this case, because of the simplicity of the empirical model, three adjustable parameters were required for the adjustment. Both of the mathematical expressions evaluated (Peng−Robinson and Chrastil) can be used for the prediction of the solubility of 9H-carbazole in propane.

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“… a Value taken from ref . b Value taken from ref . c Value taken from ref . d Value taken from ref . e Value taken from ref . Other values are reported for ω anthracene in ref and . f Value taken from ref : g Value taken from ref : h Value taken from ref : i Value taken from ref : j Value taken from ref : k Value taken from ref : l Value taken from ref : m Value taken from ref : n Value taken from ref : o Value taken from ref : …”

Section: Resultsmentioning

confidence: 99%

Measurement and Modeling of the Solubility of Anthracene and Carbazole in Compressed Isobutane

2012

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The solubilities of anthracene and carbazole in liquid and supercritical isobutane have been experimentally determined in a static view cell, at temperatures from (367 to 418 K) and pressures from (3.2 to 8.6) MPa. The solubilities of anthracene varied from (7.3 to 51.8) mg of solute per gram of isobutane, whereas those of carbazole were from (1.4 to 9.9) mg of solute per gram of isobutane within the experimental range studied. These differences in solute solubilities have been explained attending to the higher vapor pressures of anthracene and its smaller dipole moment (and so stronger affinity to isobutane). The experimental solubilities have been compared to those of these solutes in propane and CO 2 . At similar reduced temperature and pressure conditions, it has been found that solute mole fractions are higher in isobutane than in the other two fluids (3 to 15 times and 160 to 270 times higher than in propane and CO 2 , respectively). Anthracene and carbazole solubilities in isobutane have been modeled by the Peng−Robinson equation of state. Good fit of the experimental results has been obtained (APD values of 6.7 % for anthracene and 9.7 % for carbazole).

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A versatile apparatus to study the vapor pressures and heats of vaporization of carbazole, 9-fluorenone and 9-hydroxyfluorene at elevated temperatures

Cited by 18 publications

References 10 publications

Thermodynamic properties of 9-fluorenone: Mutual validation of experimental and computational results

Thermodynamic properties of 9-fluorenone: Mutual validation of experimental and computational results

Measurement and Modeling of the Solubility of 9H-Carbazole in Sub- and Supercritical Propane

Measurement and Modeling of the Solubility of Anthracene and Carbazole in Compressed Isobutane

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