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The solubilities of sulfuryl fluoride (SO 2 F 2 ) in propylene carbonate (PC), tributyl phosphate (TBP) and N-methylpyrrolidone (NMP) was measured by isochoric saturation method at the pressure of up to 600 kPa and temperatures ranging from (293.15 to 313.15) K. Results showed that SO 2 F 2 solubility increased with increasing pressure and decreased with increasing temperature in the three solvents, and the dissolution of SO 2 F 2 in the solvents was a physical process. Moreover, Henry’s law constants and thermodynamic properties such as standard Gibbs free energy, enthalpy, and entropy changes of SO 2 F 2 solvation were further calculated according to the experimental solubility data. The solubility of SO 2 F 2 in these three solvents followed the order of TBP > PC > NMP. The results illustrated that TBP possessed the potentiality to capture SO 2 F 2 among the present absorbents due to the relatively large solubility and low absorption enthalpy for SO 2 F 2 . [ABSTRACT FROM AUTHOR]

The solubility of sulfuryl fluoride in water was experimentally measured over the pressure from P = (0 to 600) kPa and T = (283.15 to 308.15) K using isochoric saturation method. Results show that SO 2 F 2 solubility increases with increasing pressure and decreases with increasing temperature. Using the experimental solubility data, Henry’s law constants and the thermodynamic properties such as the standard Gibbs free energy, enthalpy, and entropy changes of SO 2 F 2 solvation were obtained. Henry’s law constant based on mole fraction and molality of SO 2 F 2 in water vary from (432.21 to 1052.96) MPa and (7.78 to 18.96) MPa at T = (283.15 to 308.15) K, respectively. [ABSTRACT FROM AUTHOR]