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The excess part of Henry’s constant was expressed as: 1 the Henry’s constant for gas in the mixture. Bn,1 and Bn,2 are the parameters fitted to the Hmix obtained from the experimental gas solubility in the aqueous ILs. The activity coefficient of component i ( i) in the liquid phase was calculated with NRTL model (eqs. 3.24-3.26). The fugacity coefficient of component i (φi) was calculated with the RK equation. For gas mixtures, the mixing rules for a and b in eq. 3.19 are a yi ai i and b yibi . i 3.2 Energy analysis The enthalpy of CO2 absorption in aqueous ILs can be further calculated from the Henry’s constant and activity coefficients of CO2, as shown in the following equations: n 0 lnHE x (1 x ) (B B T)(1 2x )n (3.30) where Hw and HIL are the Henry’s constants for gas in water and dry ILs, respectively. Hmix is ww n,1 n,2 w H H (1 m)Hex abs dis H RT2( lnHi(T,P)) dis T where H is the absorption enthalpy, H (3.31) (3.32) T Hex RT2 x ln i i (3.33) is the is the enthalpy of gas dissolution, H ex excess enthalpy, and m is the moles of solution at saturation state (equilibrium state) to absorb 1 mole of gas. abs dis Based on the CO2 absorption enthalpy and other thermodynamic properties, the energy demand for CO2 separation process can be estimated. As IL is a liquid absorbent, the conventional separation process was used to conduct energy demand for solvent regeneration. The schematic is illustrated in Figure 3.1. The CO2 separation process includes absorber, 16PDF Image | CO2 Separation with Ionic Liquids
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