Calorimetric studies of binary systems of 1,3,5-trinitrobenzene with naphthalene, anthracene and carbazole. II. Phase diagrams

Radomska, M.; Radomski, R.

doi:10.1016/0040-6031(80)80083-9

Cited by 8 publications

(6 citation statements)

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“…The fundamental relationship expressed by eq can be used to calculate the solubility of a solid solute in equilibrium with a fluid at high pressure: y 2 = P 2 vap P · 1 φ 2 F · exp true( v 2 sat · ( P − P 2 vap ) R · T true) where y 2 is the mole fraction of the solute, P 2 vap and v 2 sat denote its saturated vapor pressure and solid-state molar volume, respectively, P and T are the equilibrium pressure and temperature, respectively, R is the universal gas constant, and φ 2 F is the fugacity coefficient of the fluid phase (which is indicative of the nonideal behavior of the fluid phase). As indicated above, the saturated vapor pressure of 9 H -carbazole was estimated using eq , and a value of 1.51·10 −4 m 3 ·mol −1 was used for the solid molar volume . For the calculation of the fugacity coefficient φ 2 F , cubic equations of state are often used, as these semiempirical equations offer simplicity and accuracy.…”

Section: Resultsmentioning

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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Section: Resultsmentioning

confidence: 99%

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

et al. 2011

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“…According to the regular solution theory, the deviations from ideality can be described by the expression RTlny1 =Ax~ 2 (1) where A is a parameter ("heat of mixing"), y is the activity coefficient and x is the mole fraction. The subscripts 1 and 2 refer to the components of the binary system.…”

Section: Calculation Of Liquidus Linesmentioning

confidence: 99%

“…The excess free energy of mixing of the liquid phase was estimated by fitting the modified van Laar equation to the measured liquidus lines. The enthalpy and the entropy of complex formation were used as the fitting parameters.The object of this study was to explore the applicability of a previously presented model for calculation of the liquidus lines in binary systems involving a charge-transfer (CT) complex [1,2]. The model is based on the assumption that, in a system involving an addition compound, the excess Gibbs energy for the liquid phase is the sum of two parts, related to complexing and non-complexing interactions.…”

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confidence: 99%

Phase diagrams in the binary systems of tetracyanoethylene with mesitylene, durene and pentamethylbenzene

Radomska

Radomski

1991

Journal of Thermal Analysis

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The phase diagrams of the binary systems of tetracyanoethylene (TCNE) with some methylbenzenes were determined by differential scanning calorimetry. In the durene-TCNE system a 1:1 complex was observed. The other two pairs of components form both 1:1 and 1:2 complexes. In all the systems, the complexes melted incongruently. Solid -solid phase transitions were found in the complexes in the pentamethylbenzene-TCNE system. The excess free energy of mixing of the liquid phase was estimated by fitting the modified van Laar equation to the measured liquidus lines. The enthalpy and the entropy of complex formation were used as the fitting parameters.The object of this study was to explore the applicability of a previously presented model for calculation of the liquidus lines in binary systems involving a charge-transfer (CT) complex [1,2]. The model is based on the assumption that, in a system involving an addition compound, the excess Gibbs energy for the liquid phase is the sum of two parts, related to complexing and non-complexing interactions.Our earlier investigations concerned systems with 1,3,5-trinitrobenzene (TNB) as an accepter (A) and polycyclic aromatic hydrocarbons as donors (D). The complexes observed in those systems were relatively weak, and the experimental liquidus lines differed from those calculated for the ideal ease only insignificantly. This paper details further refinement of this model, and its application to systems involving strong complexes. Tetracyanoethylene (TCNE) was chosen as an accepter because complexes with TCNE are known to be stronger than those with TNB [3a]. For the sake of comparison of the properties in a homologous series, the methylbenzenes were selected John grtley & Sons, Limite~ Chiche~ter Akad~niai Kiad6, Budapest

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“…The C-5 derivatives are thermally stable (112). Phase diagrams for binary systems of 1,3,5-(03N)3C6H3 with naphthalene, anthracene, and carbazole were determined by DSC and optical microscopy from 180 K to just above the melting point (180). Temperatures and heats of transition were determined for the solid-solid phase transition in where R = R1 = H; R, R1 = CH2, and Me3CZCMe3 (Z = N:N(0), N:N, and CH:CH) (26).…”

Section: Differential Thermal Analysis and Differential Scanning Calo...mentioning

confidence: 99%

Thermal analysis

Wendlandt¹

1982

Anal. Chem.

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after 22 years of editing this review (160), has decided to turn the job over to another author. It is with a deep sense of responsibility and dedication that I hereby accept this challenge. The workers in the field of thermal analysis, as well as myself, should be eternally grateful to Dr. Murphy for his devoted and accurate reporting of thermal analysis activities as they occurred through the years. I only hope that I can continue this tradition in the manner and spirit that he did.As usual, this review covers the almost 2-year period from January 1980 through November 1981. Unfortunately, not all of the thermal analysis papers can be described here, due to their magnitude. An attempt has been made, however, to include representative studies in all of the thermal analysis areas as well as, in my judgement, new and novel ideas and developments. Due to space limitations, very few review articles (of which there are many), books, and meetings are included here.

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Calorimetric studies of binary systems of 1,3,5-trinitrobenzene with naphthalene, anthracene and carbazole. II. Phase diagrams

Cited by 8 publications

References 9 publications

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

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

Phase diagrams in the binary systems of tetracyanoethylene with mesitylene, durene and pentamethylbenzene

Thermal analysis

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