Solubilities of hydrofluorocarbons in ionic liquids: Experimental and modelling study

Sousa, José M.M.V.; Granjo, José F.O.; Queimada, António J.; Ferreira, A.G.M.; Oliveira, Nuno M.C.; Fonseca, I.M.A.

doi:10.1016/j.jct.2013.07.013

Cited by 32 publications

(28 citation statements)

References 55 publications

(46 reference statements)

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“…This result may be caused by two reasons:14,26 one is the longer alkyl chains on the cation which will increase the free volume in the ionic liquid, another is that the hydrogen bond (H−F) plays an important role between the hydrogen atoms in the HFCs and the fluorine atoms on the anion, as well as the fluorine atoms of the HFCs and the hydrogen atoms on the cation. [HMIM][Tf 2 N] has longer alkyl chains on the cation and more fluorine atoms on the anion than [BMIM][PF 6 ], [EMIM][TfO], and [BMIM][TfO], so it has higher solubilities for R-152a.…”

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confidence: 99%

Vapor–Liquid Equilibrium of Three Hydrofluorocarbons with [HMIM][Tf₂N]

Liu

et al. 2015

J. Chem. Eng. Data

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New experimental data for the vapor−liquid equilibrium of 1-hexyl-3-methylimidazolium bis(trifluoromethylsulfonyl)imide ([HMIM][Tf 2 N]) with difluoromethane (R-32), 1,1-difluoroethane (R-152a), and pentafluoroethane (R-125) were presented. Measurements were performed using an isochoric saturation method at temperatures from (302.3 to 344.1) K and at pressures between (0.03 to 1.22) MPa. The relative expanded uncertainty in solubility measurement is less than 4 %. Within the investigated temperature and pressure range, the order of the solubilities for R-32, R-152a, and R-125 in [HMIM][Tf 2 N] is R-152a > R-32 > R-125. The experimental results were successfully correlated with the Krichevsky−Kasarnovsky equation. The AAD between the experimental data and calculated values for the solubilities of R-152a, R-32, and R-125 in [HMIM][Tf 2 N] are 1.4 %, 1.5 %, and 0.8 %, respectively.

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confidence: 99%

Vapor–Liquid Equilibrium of Three Hydrofluorocarbons with [HMIM][Tf₂N]

Liu

et al. 2015

J. Chem. Eng. Data

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“…3 due to the limited solubility data for R143a, R125, R152a and R161 in ionic liquids. Longer alkyl chains on the cation and larger anion, which will increase the free volume in the ionic liquid, is believed to improve the absorption capacity of ionic liquid [23]. Fig.…”

Section: Resultsmentioning

confidence: 99%

“…Shiflett et al [9] reported the solubilities of R134a in trihexyltetradecylphosphonium 1,1,2-trifluoro-2-(perfluoroethoxy) ethanesulfonate ([P14666] [TPES]) and tributyltetradecyl phosphonium 1,1,2,3,3,3-hexafluoropropanesulfonate ([P14444][HFPS]). Sousa et al [23,24] studied the solubilities of trifluoromethane, difluoromethane and fluoromethane in trihexyltetradecylphosphonium bis (trifluoromethylsulfonyl) amid ( PO 4 ].…”

Section: Introductionmentioning

confidence: 99%

Gaseous absorption of fluorinated ethanes by ionic liquids

Liu

et al. 2015

Fluid Phase Equilibria

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“…Namely, the solubility data should be known when the performance of an absorption cycle was analyzed. For phosphonium ILs, Sousa et al 22,23 studied the solubilities of HFCs (R41, R32, or R23) in phosphonium ILs ([P 66614 ]Cl, [P 66614 ][Tf 2 N], [P 4441 ][C 1 SO 4 ], and [P 4442 ]-[(C 2 ) 2 PO 4 ]) from 288 to 308 K at atmospheric pressure. Shiflett et al 24 measured the solubility and diffusivity of R134a in [P 66614 ][TPES] and in [P 4441 ][HFPS] from 283 to 348 K and pressure up to 0.35 MPa.…”

Section: Introductionmentioning

confidence: 99%

Solubility for Propane and Isobutane in [P₆₆₆₁₄]Cl from 278.15 to 348.15 K

et al. 2021

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Absorption-cycle technology driven by low-grade thermal energy has attracted significant attention. Environment-friendly refrigerant/ionic-liquid absorbents have been currently proposed as promising candidates to traditional H2O/LiBr and NH3/H2O working pairs. The properties of refrigerant/absorbent pairs have a large impact on the performance of an absorption–refrigeration cycle, especially the solubility of the gaseous refrigerant in an absorbent. In this work, solubilities (vapor–liquid phase equilibrium) were measured for two new working pairs (isobutane/[P66614]Cl and propane/[P66614]Cl) from 278.15 to 348.15 K by an isochoric saturation method. Solubilities increase with a decrease in temperature and an increase in pressure. The new data were correlated by the nonrandom two-liquid (NRTL) equation. Results show that the NRTL model provides small deviations distributed as a function of pressure. Furthermore, the enthalpy, entropy, and Gibbs energy of dissolution were estimated. Calculated enthalpies are negative indicating that the process of dissolution is exothermic. The Gibbs energy accords with the classical thermodynamics theory: the lower is the value, the more favorable is the dissolution capacity.

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Solubilities of hydrofluorocarbons in ionic liquids: Experimental and modelling study

Cited by 32 publications

References 55 publications

Vapor–Liquid Equilibrium of Three Hydrofluorocarbons with [HMIM][Tf₂N]

Vapor–Liquid Equilibrium of Three Hydrofluorocarbons with [HMIM][Tf₂N]

Gaseous absorption of fluorinated ethanes by ionic liquids

Solubility for Propane and Isobutane in [P₆₆₆₁₄]Cl from 278.15 to 348.15 K

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Solubilities of hydrofluorocarbons in ionic liquids: Experimental and modelling study

Cited by 32 publications

References 55 publications

Vapor–Liquid Equilibrium of Three Hydrofluorocarbons with [HMIM][Tf2N]

Vapor–Liquid Equilibrium of Three Hydrofluorocarbons with [HMIM][Tf2N]

Gaseous absorption of fluorinated ethanes by ionic liquids

Solubility for Propane and Isobutane in [P66614]Cl from 278.15 to 348.15 K

Contact Info

Product

Resources

About

Vapor–Liquid Equilibrium of Three Hydrofluorocarbons with [HMIM][Tf₂N]

Vapor–Liquid Equilibrium of Three Hydrofluorocarbons with [HMIM][Tf₂N]

Solubility for Propane and Isobutane in [P₆₆₆₁₄]Cl from 278.15 to 348.15 K