Thermal and volumetric properties of chloroform+benzene mixtures and the ideal associated solution model of complex formation

Grolier, J.-P.E.; Roux-Desgranges, G.; Kooner, Z. S.; Smith, J. F.; Hepler, Loren G.

doi:10.1007/bf00652577

Cited by 25 publications

(16 citation statements)

References 14 publications

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“…Chloroform (Caledon Lab Ltd.) was purified and stored as described previously (5). Ammonia (Medigas Ltd.) was used without further purification.…”

Section: Methodsmentioning

confidence: 99%

“…[2]- [5] with xA = 1 -xB, we obtain an expression for the equilibrium constant in terms of xB (the mole fraction solubility of B in A) and r:…”

Section: Derivation Of Equationsmentioning

confidence: 99%

“…Several studies (4)(5)(6)(7)(8)(9) have shown that the ideal associated solution model can be applied successfully to many associated systems (A + B = AB) in which A and B are liquids. This success suggests the possibility that the model may be useful inthe investigation of systems in which a dissolved gas, B, interacts chemically with the solvent, A, to form an associated complex, AB.…”

Section: Introductionmentioning

confidence: 99%

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Solubility of ammonia in chloroform: analysis in terms of Henry's law and the equilibrium constant for hydrogen-bonded complex formation

Smith¹,

Li²,

Roth³

et al. 1989

Can. J. Chem.

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. 67,2213 (1989). We have measured the solubility of ammonia in chloroform at several pressures and at three temperatures (25,30, and 35°C). Results of these measurements have been analysed in terms of the Henry's law constant that applies to "simple" dissolution of the type B(g) = B(disso1ved) and the equilibrium constant K for the liquid phase complex-forming equilibrium represented by A + B = AB where A and B represent chloroform and ammonia, respectively. As expected on the basis of this analysis, ammonia is more soluble (same pressure and temperature) in chloroform than in carbon tetrachloride, where no hydrogen-bonded complex can be formed.Key words: gas solubility, hydrogen-bonded complexes, Henry's law constant, ammonia-chloroform complex, chloroformammonia complex. Mots clks : solubilit6 des gaz, complexes par liaisons hydrogknes, constante de la loi de Henry, complexe ammoniac-chloroforme, complexe chlorofome-ammoniac.[Traduit par la revue] Introduction Analyses of the thermodynamic properties of non-electrolyte solutions are generally made by comparing the measured properties with the properties the solution would have if it were ideal. Attempts are then made to explain the observed deviations in terms of some model (or theory) of solutions. As a first step in the development of such a model it is often convenient to separate the deviations from ideality into "physical" and

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“…Chloroform (Caledon Lab Ltd.) was purified and stored as described previously (5). Ammonia (Medigas Ltd.) was used without further purification.…”

Section: Methodsmentioning

confidence: 99%

“…[2]- [5] with xA = 1 -xB, we obtain an expression for the equilibrium constant in terms of xB (the mole fraction solubility of B in A) and r:…”

Section: Derivation Of Equationsmentioning

confidence: 99%

Section: Introductionmentioning

confidence: 99%

See 1 more Smart Citation

Solubility of ammonia in chloroform: analysis in terms of Henry's law and the equilibrium constant for hydrogen-bonded complex formation

Smith¹,

Li²,

Roth³

et al. 1989

Can. J. Chem.

Self Cite

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“…30 Particularly, in the case of the chloroform + benzene system, some influences can be mentioned as an explanation of the V E -composition behaviour, for example: (a) the difference between van der Waals volumes 31 of the constituents, (b) the formation of a weak complex between benzene and chloroform 32,33 and (c) the presence of steric hindrance effects in the mixture. 30 Particularly, in the case of the chloroform + benzene system, some influences can be mentioned as an explanation of the V E -composition behaviour, for example: (a) the difference between van der Waals volumes 31 of the constituents, (b) the formation of a weak complex between benzene and chloroform 32,33 and (c) the presence of steric hindrance effects in the mixture.…”

Section: Ternary Systemsmentioning

confidence: 99%

Modelling of volumetric properties of binary and ternary mixtures by CEOS, CEOS/Ge and empirical models

Djordjević¹,

Šerbanović²,

Radović³

et al. 2007

JSCS

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Although many cubic equations of state coupled with van der Waals-one fluid mixing rules including temperature dependent interaction parameters are sufficient for representing phase equilibria and excess properties (excess molar enthalpy H E , excess molar volume V E , etc.), difficulties appear in the correlation and prediction of thermodynamic properties of complex mixtures at various temperature and pressure ranges. Great progress has been made by a new approach based on CEOS/G E models. This paper reviews the last six-year of progress achieved in modelling of the volumetric properties for complex binary and ternary systems of non-electrolytes by the CEOS and CEOS/G E approaches. In addition, the vdW1 and TCBT models were used to estimate the excess molar volume V E of ternary systems methanol + chloroform + benzene and 1-propanol + chloroform + benzene, as well as the corresponding binaries methanol + chloroform, chloroform + benzene, 1-propanol + chloroform and 1-propanol + benzene at 288.15-313.15 K and atmospheric pressure. Also, prediction of V E for both ternaries by empirical models (Radojković, Kohler, Jackob-Fitzner, Colinet, Tsao-Smith, Toop, Scatchard, Rastogi) was performed.

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“…of benzene and is an indirect evidence of the equimolecular complex formation [14,15]. Thermal and volumetric properties of a benzene-chloroform solution were described quantitatively within a model of ideal associated solution, which took the complex formation into account [16].…”

Section: Introductionmentioning

confidence: 99%

Formation of Molecular Complexes in Liquid Benzene-Chloroform Mixtures Examined by Mid-IR 2D Correlation Spectroscopy and Multivariate Curve Resolution

et al. 2016

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Mid-IR spectroscopy is used for the investigation of the formation of molecular complexes in a liquid benzene-chloroform solution. Spectra are measured in the spectral interval 2950-3100 cm −1 , which corresponds to CH stretching vibrations of benzene and chloroform. The 2D correlation analysis of spectral data indicates the presence of molecular complexes in the solution. The analysis of residual spectra also supports this conclusion. Model-free and model-based analyses are applied for the decomposition of spectral data. The concentration and spectral profiles of molecular complexes are determined. The analysis shows that a complex consists of one molecule of benzene and one molecule of chloroform.

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Thermal and volumetric properties of chloroform+benzene mixtures and the ideal associated solution model of complex formation

Cited by 25 publications

References 14 publications

Solubility of ammonia in chloroform: analysis in terms of Henry's law and the equilibrium constant for hydrogen-bonded complex formation

Solubility of ammonia in chloroform: analysis in terms of Henry's law and the equilibrium constant for hydrogen-bonded complex formation

Modelling of volumetric properties of binary and ternary mixtures by CEOS, CEOS/Ge and empirical models

Formation of Molecular Complexes in Liquid Benzene-Chloroform Mixtures Examined by Mid-IR 2D Correlation Spectroscopy and Multivariate Curve Resolution

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