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11%, and the viscosity decreased by 40%. Thus the viscosity is more sensitive to the temperature in comparison to the density, especially for a mixture with a low water concentration. Table 1. Experimental density and viscosity of aqueous [Amim][HCOO] ( mw is mass fraction of water). mw ρ / g·cm-3 0 0.10 0.19 0.37 η / mPa·s 0.19 0.37 0.73 15.9 10.1 7.48 14.2 9.83 7.05 13.1 9.71 6.73 12.7 9.58 6.67 12.4 9.32 6.48 12.1 9.02 6.33 11.9 8.96 6.15 11.6 8.70 5.96 11.4 8.59 5.74 T/K 293.15 1.171 298.15 1.168 303.15 1.165 308.15 1.162 313.15 1.159 318.15 1.156 323.15 1.153 328.15 1.150 333.15 1.147 1.164 1.148 1.112 1.160 1.145 1.109 1.157 1.142 1.106 1.154 1.139 1.103 1.151 1.136 1.100 1.148 1.132 1.096 1.145 1.129 1.093 1.142 1.126 1.090 1.139 1.123 1.087 0.73 1.041 1.039 1.037 1.035 1.032 1.030 1.027 1.024 1.021 0 0.10 128 30.0 91.5 24.3 65.5 21.0 50.2 19.1 38.9 18.1 30.4 16.0 25.2 15.2 21.2 14.3 18.2 14.1 2.3.2 Gas solubility The solubility of both CO2 and CH4 in dry [Amim][HCOO] was measured at pressures up to 1.8 MPa and at temperatures of 298.2, 313.2 and 333.2 K. It was assumed that only CO2 or CH4 exit in the vapor phase because of the low vapor pressure of the IL. The experimental results are listed in Table 2. The CO2 solubility in dry [Amim][HCOO] was much higher than that of CH4. For example, at 1 MPa and 298.2 K, the mole fraction of CO2 in [Amim][HCOO] was 0.226, while the mole fraction of CH4 only reached 0.016. Moreover, the mole fractions of CO2 and CH4 at the investigated temperatures and pressures were up to 0.288 and 0.026, respectively. The CO2 solubility in aqueous [Amim][HCOO] was measured at different pressures up to 1.8 MPa and temperatures of 298.2, 313.2 and 333.2 K. The mass fraction of water in the mixture solvent was varied at 0.10, 0.19, 0.37 and 0.73. The measured results are illustrated in Table 3. For the aqueous system studied in the experimental work, it was assumed that the vapor pressures of [Amim][HCOO] and H2O were negligible. As described in our previous work [9], the water content in the vapor phase was very low and could be neglected for the CO2-H2O systems under investigation. In fact, the strong interaction between H2O and [Amim][HCOO] further decreased the content of water in the vapor pressure. Therefore, during the experimental measurements, it was reasonable to assume that only CO2 existed in the vapor phase.PDF Image | CO2 Separation with Ionic Liquids
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