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The solubility of CO2, CH4, N2, and CO was measured in a broad number of ionic liquids using a pressure drop set-up. A successful correlation of the Henry's law constants at 60 °C was made to two empirical models already described in literature (Camper et al. [13] and Moganty and Baltus [25] ). Subsequently, a new empirical model was proposed, which describes the Henry's law constant as a function of the molar mass of the ionic liquid, as long as physical interactions between gas and ionic liquid are dominant. Additionally, the entropy and enthalpy of solvation was studied by means of the temperature influence to the Henry's law constant. |
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