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where Vi is the liquid molar volume, Mi is the molecular weight, Vmix and ηmix are the liquid molar volume and viscosity of the mixture. xi is the mole fraction of each component, kij and lij are the binary parameters, and they were correlated from the corresponding experimental properties. ViE is the excess molar volume, Δηi is the viscosity deviation, and AiE is excess molar energy of activation. The excess property (i.e. VE, AE) was fitted to Redlich–Kister equation [47]: V E x x 4 A x x n ( 3 . 1 5 ) ( 3 . 1 6 ) i12 n 0 n12 A 1 a T i n i 0 i where ai is the parameter in fitting. 3.1.2 Modeling phase equilibria (a) Pure-gas solubility in dry ILs Due to the low vapor pressure of ILs, it was assumed that IL only exists in the liquid phase. The vapor-liquid equilibrium can be expressed as: P Hx (3.17) i iii where P is the system pressure, φi is the fugacity coefficient of gas i in the vapor phase, Hi is the Henry’s constant of gas i in dry IL, xi is the mole fraction of gas i in the liquid phase, γi* is the activity coefficient of gas i in the liquid phase at the infinite dilution reference state. The fugacity coefficient of gas i was calculated by the Redlich–Kwong (RK) equation [48]: a/R2T2.5 ln i Z 1 ln(Z bP/RT) b/RT ln(1 bP/ZRT) (3.18) 13PDF Image | CO2 Separation with Ionic Liquids
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