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Solubilitiesof SO2in binary mixtures of urea and ethyleneglycol were determined by gas–liquid equilibrium experimentsat the temperatures from (298.15 to 318.15 K) and 122.7 kPa, withSO2partial pressure in gas phase in the range of (0 to130) Pa. Henry’s law constants were calculated based on thesolubility data. It indicated that the mixture with urea molalityof 6.65 mol·kg–1has the most desirable capacity.More than 90 % SO2can be regenerated by bubbling N2at 338.15 K. Density and viscosity data for the binary mixtureswere also measured. In addition, UV, IR, and NMR experiments wereconducted to investigate the interaction between ethylene glycol,urea, and SO2. The result demonstrated that SO2can interact with the mixture by both the charge-transfer interactionbetween S (SO2)···N (urea) and the hydrogenbond between O (SO2)···H (ethylene glycol). [ABSTRACT FROM AUTHOR]

Abstract: In this paper, isothermal gas–liquid equilibrium data were measured for the system SO2 +N2 in N,N-dimethylformamide (DMF)+diethylene glycol (DEG) at T =(298.15, 303.15, 308.15, 313.15, and 318.15)K and p =122.66kPa. Based on these data, Henry's law constants were obtained by fitting the linear slope of GLE data. The results indicated the solubility of dilute SO2 in the system DMF+DEG increases with increasing DMF concentration. From the GLE data of dilute SO2 in pure DMF and pure DEG, the thermal parameter of dissolving SO2 in pure DMF and pure DEG was obtained. Meanwhile, density, ρ, and viscosities, ν, for the binary mixtures of DMF+DEG were measured over the whole concentration range at T =(298.15, 303.15, 308.15, 313.15, and 318.15)K. From the experimental density and viscosity data, the excess molar volume, V m E , and viscosity deviations, Δν, were calculated and the calculated results were fitted to a Redlich–Kister equation to obtain the coefficients and estimate the standard deviations between the experimental and calculated quantities. The values of V m E and Δν were negative at all experimental temperatures and components. From the kinematic viscosity data, enthalpy of activation for viscous flow (ΔH *), entropy of activation for the viscous flow (ΔS *), and Gibbs free energy of activation for viscous flow (ΔG *) were calculated. [Copyright &y& Elsevier]

Abstract: This work reports the solubility data of dilute sulfur dioxide in 1,4-dioxane, 15-crown-5 ether, polyethylene glycol 200 (PEG 200), polyethylene glycol 300 (PEG 300), and their binary mixtures at 308.15K and 122.66kPa with the SO2 partial pressure ranging between (7.35 and 118Pa). From the solubility data, Henry''s law constants of SO2 in pure solvents were calculated. The results show that the solubilities of SO2 in these four solvents increase linearly with the enhancement of the equilibrium partial pressure of SO2 in the gas phase within the studied regions. Furthermore, the absorption of SO2 in pure 1,4-dioxane, 15-crown-5 ether, PEG 200 are typical physical processes, and the solubility of SO2 in the three solvents decreases in the order: 1,4-dioxane>15-crown-5 ether>PEG 200. But the SO2 absorption in PEG 300 is a physical process accompanied by a chemical process. [Copyright &y& Elsevier]

In this work, isothermal (gas+liquid) equilibrium (GLE) data were measured for the system SO2 +N2 +N,N-dimethylformamide (DMF)+Ethylene Glycol (EG) at T =308.15K and p =122.66kPa. Based on these data, Henry’s law constants were obtained by fitting the linear slope of the GLE data. The results show the solubility of dilute SO2 in the DMF+EG solutions increases with the increasing DMF concentration, and the solubility values range from 2.38 mol·m−3 (pure EG) to 47.2mol·m−3 (pure DMF) when SO2 concentration in the gas phase is designed at =5·10−4. Meanwhile, the densities, ρ, and viscosities, ν, for the binary mixtures of DMF+EG were measured over the whole concentration range at T =(298.15, 303.15, 308.15, 313.15 and 318.15)K. The experimental results were compared with reported data in literatures. From the experimental density and viscosity data, the excess molar volumes, , and viscosity deviations, Δν, were calculated and the calculated results were fitted to a Redlich–Kister equation to obtain the coefficients and estimate the standard deviations between the experimental and calculated quantities. The values of and Δν are shown to be negative at all experimental temperatures and compositions. From the kinematic viscosity data, Gibbs energies of activation of viscous flow (ΔG ∗), enthalpy of activation for viscous flow (ΔH ∗) and entropy of activation for the viscous flow (ΔS ∗) were also calculated. [ABSTRACT FROM AUTHOR]