Vapor−Liquid Equilibrium Data of the Carbon Dioxide + Ethyl Butyrate and Carbon Dioxide + Propylene Carbonate Systems at Pressures from (1.00 to 13.00) MPa and Temperatures from (313.0 to 373.0) K

Abstract

High-pressure vaporÀliquid equilibrium data for the binary systems of ethyl butyrate (EB) þ carbon dioxide and propylene carbonate (PC) þ carbon dioxide were measured. The experimental pressure range was from (1.00 to 13.00) MPa and the temperature range from (313.0 to 373.0) K. Experimental results were correlated with the PengÀRobinson equation of state with the two-parameter van der Waals mixing rule. At the same time, the Henry's coefficient and solution enthalpy and solution entropy of CO 2 during dissolution at different temperature were also calculated.

Low pressure carbon dioxide solubility in pure electrolyte solvents for lithium-ion batteries as a function of temperature. Measurement and prediction

“…These reported CO 2 solubility data can be also compared with those reported in the literature by our group previously [18] as well as by others [19][20][21][22][23][24][25][26][27][28][29][30][31][32][33]. From table 4 and figure 4, it can be seen that the values of CO 2 solubility in PC are in excellent agreement with published data by Blanchard et al [18].…”

“…Figure 3 represents the CO 2 solubility data, expressed in mole fraction of CO 2 (a) as well as in Henry's Law constants (b) at the atmospheric pressure, in the selected pure solvents as a function of temperature. It can be observed that the CO 2 is more soluble in linear solvents than in cyclic carbonates, as already described in the literature by our group [18] and others [23,33].…”

“…Issacs et al [20], Zubchenko et al [21], Xu et al [27] and Schmack and Bittrich [28] within a per cent RAAD close to (1.8, 3.2, 8.7, 8.5, and 7.9)%, respectively. Nevertheless, higher deviations were found with the published data of Murrieta-Guevara et al [25,26] (14%), Mantor et al [19] (16%), Rivas and Prausnitz [22] (14%), Hongling et al [23] (20%), and Lenoir et al [24] (up to 30%). Even if the origin of such differences is difficult to understand clearly, such deviations could come from the difference of experimental techniques used by each group, the solvent-purity and water content in each sample.…”

“…An experimental procedure based on chemical titration methodology has been used during this work. These selections of solvents and experimental techniques were chosen first to confirm previous data published by our group [18], and to evaluate these data with those already published by other groups [19][20][21][22][23][24][25][26][27][28][29][30][31][32][33]. Secondly, an attempt was made to estimate from the solubility data as a function of temperature the Henry's law constants and dissolution properties like the Gibbs energy, the standard enthalpy and entropy of dissolution, as well as the mixing enthalpy of the solvent with CO 2 in its hypothetical liquid state.…”

“…Thirdly, we have tried to cover different families of solvents that could best illustrate solvent effects on the CO 2 solubility like the size of the molecule (DMC versus EMC versus DEC) or its basic structure (linear versus cyclic), which can drive different dissolution pathways. Furthermore, based on their relatively low vapour pressure and their cost, these solvents are sometimes referred to as a ''green adsorbents'' for CO 2 capture which present high CO 2 solubility in comparison with molecular solvents, like water or alcohols [23,30,34]. In order to analyse their CO 2 capture capability in greater detail, a comparison has been realised between CO 2 solubility data presented herein with those reported for another family of designer solvents like ionic liquids [35].…”