Abstract
The solubility of carbon dioxide was determined in dimethyl sulfoxide, ethylene glycol, and their binary mixtures at the temperatures ranging from 298.15 Kto 328.15 K and the pressures ranging from (0 to 6) bar (0 to 0.6 MPa). It was shown that the solubility of CO2 increased with the increasing of pressure while decreased with the increasing of temperature. The Henry’s constants and thermodynamic properties of solution were calculated from the solubility data. The solubility and Henry’s constant of CO2 in the solvent mixtures increased with increasing the mole fraction of dimethyl sulfoxide. Finally, the dependence of CO2 solubility on solvent properties was investigated using the linear Gibbs energy relationship method. Results showed that solute-solvent interactions in the scale of polarity/polarizability and hydrogen bond acceptor ability of the solvent were the main parameters which control the solubility of CO2 in the solvents.
Talk to us
Join us for a 30 min session where you can share your feedback and ask us any queries you have
Schedule a callDisclaimer: All third-party content on this website/platform is and will remain the property of their respective owners and is provided on "as is" basis without any warranties, express or implied. Use of third-party content does not indicate any affiliation, sponsorship with or endorsement by them. Any references to third-party content is to identify the corresponding services and shall be considered fair use under The CopyrightLaw.
