Solubility of the Single Gases Methane and Xenon in the Ionic Liquid [bmim][CH₃SO₄]

Abstract

Solubility measurements of methane and of xenon in the ionic liquid 1-n-butyl-3-methylimidazolium methyl sulfate ([bmim][CH 3 SO 4 ]) were performed with a high-pressure view-cell technique based on the synthetic method. The temperature ranged from 293.1 K to 413.2 K, and the maximum pressure (the maximum gas molality) was 8.9 MPa (0.19 mol‚kg -1 ) for methane and 11.3 MPa (0.65 mol‚kg -1 ) for xenon. Both gases become less soluble in [bmim][CH 3 SO 4 ] with rising temperature, but xenon shows a significantly higher solubility at all conditions investigated. An extension of Henry's law is employed to correlate the solubility pressures in both cases. The final results for the Henry's constant (at zero pressure) of methane and xenon in [bmim][CH 3 SO 4 ] (on the molality scale) are correlated within the experimental uncertainty (about ( 1.3 %) by ln(k H,CH 4 (0) /MPa) ) 6.216 -564.5/ (T/K) -0.002566(T/K) and ln(k H,Xe (0) /MPa) ) 5.5906 -928/(T/K) -0.00141(T/K), respectively.

Experimental Study on the Solubility of Carbon Dioxide in Nitrate and Thiocyanate-Based Ionic Liquids

“…As Figure shows, the pressure above the solution of CO 2 + IL increases linearly with an increase in CO 2 molality. This behavior is observed for the solubility of CO 2 in other types of ILs. − Furthermore, the solubility of CO 2 in studied ILs decreases with an increase in temperature.…”

“…In the studied ILs, the experimental results for the gas solubility are correlated with the extended Henry’s law. The Henry’s constant for CO 2 in ILs are calculated similar to the procedure that was described by Kumelan et al − and Perez-Salado et al As Perez-Salado et al have pointed out, the vapor–liquid equilibrium condition for CO 2 + ILs systems results in the extended Henry’s law where K H′CO 2 0 ( T ′ P ) is Henry’s constant of CO 2 in IL based on the molality scale, a CO 2 ( T ′ m C O 2 ) is the activity of CO 2 in the IL, and f CO 2 ( T ′ P ) is the fugacity of CO 2 in the vapor phase. The Henry’s constant of CO 2 in IL is expressed as where K H′CO 2 0 ( T ) is the Henry’s constant of CO 2 in IL at zero pressure, and V m′CO 2 ∞ is the partial molar volume of CO 2 in IL at infinite dilution.…”

“…According to their results, the solubility of ILs decreases with increasing temperature and increases with increasing pressure . Kumelan et al − studied the solubility of different single gases in ILs. In recent years, the amount of experimental data in literature for these systems has considerably increased. − Most of the experimental data in literature shows the superiority of ILs over various conventional solvents …”

Thermodynamic and molecular insights into the absorption of H2S, CO2, and CH4 in choline chloride plus urea mixtures

“…Tables S6 and S7 in the Supporting Information summarizes the Henry's constants of gases and ideal selectivities of gas pairs in other physical solvents reported in the literature, including normal ILs and traditional organic solvents . It is found that the solubilities of H 2 S and CO 2 in ChCl + urea mixtures are similar to those in PC but inferior to most other physical solvents.…”

Screening ionic liquids as candidates for separation of acid gases: Solubility of hydrogen sulfide, methane, and ethane

“…Experimental data for CH 4 ‐IL systems are summarized in Table . The cations included in the database are bmim and hmim, whereas the anions are BF 4 , CH 3 SO 4 , PF 6 , and Tf 2 N. Experimental data for four ILs with C 2 H 6 , summarized in Table . The cations included in the database are bmim and hmim, whereas the anions are BF 4 , PF 6 , and Tf 2 N.…”