Recommended vapor pressures for thiophene, sulfolane, and dimethyl sulfoxide
Research highlights
► Thiophene, sulfolane, and dimethyl sulfoxide were studied. ► Vapor pressures and liquid heat capacities were determined. ► Thermodynamic properties in the ideal gas state were calculated. ► Recommended vapor pressure equations were developed.
Introduction
Thiophene, sulfolane, and dimethyl sulfoxide are important industrial solvents produced on a large scale. Despite of this fact, their vapor pressures at ambient temperatures are not known with sufficient accuracy. Reliable vapor pressure data are indispensible for processes involving phase equilibria and for phase equilibrium studies on systems containing these compounds.
In this work, we first assessed all available literature vapor pressure data and examined their consistency with calorimetrically determined vaporization enthalpies and heat capacities of condensed phases and ideal gas. Literature review and consistency tests revealed that new vapor pressure data in the low pressure region for sulfolane and dimethyl sulfoxide and new liquid heat capacities for sulfolane were needed. These data were experimentally determined in this work. Also, heat capacities of ideal gas and thermodynamic properties in the ideal gaseous state for all the studied compounds were calculated using the methods of statistical thermodynamics. We employed both the experimental and calculated fundamental vibrational frequencies and compared the obtained results as part of our effort to assess the reliability of the calculations based purely on ab initio data. Consequently, recommended vapor pressure data for thiophene, sulfolane, and dimethyl sulfoxide were developed by the simultaneous correlation of selected vapor pressure and related thermal data [1].
Section snippets
Simultaneous treatment of vapor pressures and related thermal data (SimCor method)
Vapor pressure p, enthalpy of vaporization and the difference between ideal gas heat capacity and heat capacity of liquid are linked by exact thermodynamic relationshipswhere subscript ‘sat’ denotes a derivative along the saturation line, R is the molar gas constant (R = 8.314472 J K−1 mol−1 [2], [3]), stands for the difference between the compressibility factors of the coexisting
Materials
Sulfolane was obtained from Novasol Belgium. The mass fraction purity (determined by gas gromatography (GC)) and mass fraction of water (determined by Coulometric titration, UOP 481) were w = 0.9985 and w(H2O) = 3 × 10−4, respectively, as stated in the certificates of analysis provided by the supplier. The sample was stored over 4 Å molecular sieves for approximately 2 weeks. The mass fraction of water determined prior to taking vapor pressure and heat capacity measurements was w(H2O) = 6.5 × 10−5
Vapor pressures
The vapor pressure measurements of sulfolane and dimethyl sulfoxide were performed in the temperature interval from 253 to 308 K by varying the temperature at random to detect systematic errors caused by insufficient degassing of the sample. The experiments were carried out repeatedly at selected temperatures. When the pressure did not change with the number of measuring cycles, the sample was considered completely degassed, and the final set of data was recorded. At least two experimental
Conclusions
Recommended vapor pressure equation for thiophene, sulfolane, and dimethyl sulfoxide was developed by a multi-property fit of selected experimental vapor pressure data, calorimetrically measured enthalpies of vaporization and differences in heat capacities of condensed phases and ideal gas. New vapor pressure data for sulfolane and dimethyl sulfoxide, and liquid heat capacities for sulfolane were determined in this work. The thermodynamic properties in the ideal gaseous state for all the
List of symbols
- A
integrated values of differential heat flow
- A0, A1, A2, A3
parameters of Cox equation, Eq. (3)
- c
specific heat capacity
molar ideal gas heat capacity at constant pressure
molar heat capacity of saturated vapor at constant pressure
molar heat capacity of condensed phases (crystalline or liquid phase) at constant pressure
molar heat of crystalline phase at constant pressure
molar liquid heat capacity at constant pressure
difference between ideal gas heat capacity and
Acknowledgements
We thank Vladimir Diky and Ala Bazyleva for providing the program StatTD and for valuable and helpful discussions on statistical thermodynamic calculations of ideal gas properties, Pavel Morávek for help with the sample degassing prior to vapor pressure determinations, and Novasol Belgium for providing us free of charge with anhydrous sample of sulfolane. This work is supported by the Ministry of Education of the Czech Republic under grant MSM 604 613 7307 and the Czech science foundation
References (74)
- et al.
Fluid Phase Equilib.
(1999) - et al.
J. Chem. Thermodyn.
(1999) - et al.
Fluid Phase Equilib.
(2000) - et al.
J. Chem. Thermodyn.
(2004) - et al.
J. Chem. Thermodyn.
(2006) - et al.
Phys. B
(1997) - et al.
Fluid Phase Equilib.
(2010) - et al.
J. Chem. Thermodyn.
(1985) - et al.
Thermochim. Acta
(1981) - et al.
J. Chin. Inst. Chem. Eng.
(2007)
J. Mol. Spectrosc.
J. Mol. Struct.
J. Mol. Struct.
Spectrosc. Acta A: Mol. Biomol. Spectrom.
Spectrochim. Acta
J. Mol. Spectrosc.
Spectrosc. A: Mol. Biomol. Spectrom.
Spectrochim. Acta
J. Mol. Struct.
J. Mol. Struct.
J. Chem. Thermodyn.
AIChE J.
Rev. Modern Phys.
J. Phys. Chem. Ref. Data
Ind. Eng. Chem.
Fluid Phase Equilib.
Thermochim. Acta
J. Chem. Eng. Data
J. Chem. Eng. Data
J. Chem. Eng. Data
Heat Capacity of Liquids. Critical Review and Recommended Values
J. Therm. Anal. Calorim.
J. Phys. Chem.
J. Chem. Phys.
J. Am. Chem. Soc.
J. Phys. Chem. Ref. Data
Cited by (40)
Optimization of precipitation conditions for producing physically stable amorphous solids using pair distribution function and reduced crystallization temperature
2024, Journal of Drug Delivery Science and TechnologyA rechargeable Mg|O<inf>2</inf> battery
2022, iScienceOsmotic and activity coefficients for five lithium salts in three non–aqueous solvents
2019, Journal of Chemical ThermodynamicsCitation Excerpt :We first measured the vapor pressures of the salt–free solvents. Table 4 compares our vapor pressures with those from NIST [47] and those from the literature [26,48–56]. Agreement is very good.