(Vapour+liquid) equilibria of (methanethiol or ethanethiol or propan-1-thiol or butan-1-thiol+ n-hexane or n-decane or toluene or water) for mole fractions x = 0 to 0.2 of thiol at temperatures between 323 and 373 K

(Vapour+liquid) equilibria of (alkoxyalkanes+alkanes, oro-xylene, or water, or methanol) for ether mole fractions 0 to 0.5, between temperatures 293 K and 323 K

“…The technique, as described previously, (11) involves the quantitative mass transfer by vacuum distillation of the components into a cell that can be held at constant temperature and is connected to a sensitive capacitance pressure measuring device.…”

Solubility of Ethanethiol in Water

“…New VLE and VLLE data for the ethanethiol + water system (with methane as overburden pressure) are shown in Table . Similar to Jou et al (2021), the Peng and Robinson (1976) equation of state (EoS), shown in eqs –, was used to correlate the new data and the VLE and LLE data of Gillespie and Wilson and the VLE of Kilner et al The Peng-Robinson EoS with the original quadratic mixing rules has been widely used in process simulators and can be considered a base model for which to compare other modeling approaches. As this investigation was focused on the VLE region of this system, the VLLE data of Awan et al were not considered in this correlation.…”

“…The new data were correlated to an average absolute percentage deviation (AAPD) of 4.1% in pressure and 7.8% in ethanethiol mole fraction (1.3% and 8.1% respectively for the VLE data). The data of Kilner et al were correlated to an average absolute percentage deviation (AAPD) of 10.0% in pressure and the data of Gillespie and Wilson were correlated to 23.2% (vapor or L 2 ethanethiol mole fraction) and an AAPD of 34.2% (aqueous phase ethanethiol mole fraction). Overall, this modeling approach reproduces both the experimental VLE and the LLE over the 291 K span of temperature and the large range of partial pressures reasonably well.…”

Addition of the sulfhydryl group (–SH) to the PPR78 model (predictive 1978, Peng–Robinson EOS with temperature dependent kij calculated through a group contribution method)

“…The DIPPR database was chosen. Table 3 details the sources of the binary experimental data used in our evaluations [27][28][29][30][31][32][33][34][35][36][37][38] along with the temperature, pressure, and composition ranges for each binary system. Most of the data available in the open literature (731 bubble points + 320 dew points + 58 azeotropic points) were collected.…”

“…Prediction of phase equilibria for systems containing hydrocarbons, CO 2 , N 2 , H 2 S, and mercaptans: A general overview 3.1. A priori reflections regarding the study By looking at the experimental data [27][28][29][30][31][32][33][34][35][36][37][38] of binary systems containing mercaptans and a hydrocarbon or CO 2 or N 2 or H 2 S, we can notice that the only particularity likely to arise on these phase diagrams is the presence of a homogeneous azeotropic point [39] (for instance, (liquid À liquid) equilibrium has never been noticed experimentally). It thus seems logical to consider that binary systems with mercaptans essentially exhibit type I behavior in the classification scheme of van Konynenburg and Scott [40].…”