Solubility and diffusion of CO2 and H2S in the ionic liquid 1-ethyl-3-methylimidazolium ethylsulfate

Jalili, Amir Hossein; Mehdizadeh, Amir; Shokouhi, Mohammad; Ahmadi, Abbas; Hosseini-Jenab, Masih; Fateminassab, Fakhrolsadat

doi:10.1016/j.jct.2010.05.008

Cited by 179 publications

(99 citation statements)

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“…The reliability and accuracy of the method of measurement have been checked in our previous works. 10,13 The measurement temperature starts at 333.15 K, which is about the melting point of [emim][PF 6 ] claimed by the supplier (Fluka) and also reported by other researchers. 22 However, in the case of [emim][Tf 2 N], the measurement temperature starts at 303.15 K. Values of ln K h,x (0) at each temperature T were obtained from the intercept of the plots of ln(f 2 0 /x 2 ) versus P at the specified temperature.…”

Section: Introductionmentioning

confidence: 66%

Solubility of H₂S in Ionic Liquids 1-Ethyl-3-methylimidazolium Hexafluorophosphate ([emim][PF₆]) and 1-Ethyl-3-methylimidazolium Bis(trifluoromethyl)sulfonylimide ([emim][Tf₂N])

et al. 2010

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The solubility of hydrogen sulfide gas in ionic liquids (ILs) 1-ethyl-3-methylimidazolium hexafluorophosphate ([emim][PF 6 ]) at temperatures from (333.15 to 363.15) K and 1-ethyl-3-methylimidazolium bis(trifluoromethyl)sulfonylimide ([emim][Tf 2 N]) at temperatures ranging from (303.15 to 353.15) K and pressures up to about 2.0 MPa was measured using a volumetric based static apparatus. The solubility data were correlated using two models: the Krichevsky-Kasarnovsky (KK) equation, and the extended Henry's law combined with the Pitzer's virial expansion for the excess Gibbs energy. Henry's law constants (at zero pressure) were obtained at different temperatures from the obtained experimental solubility data. Using the solubility data, the partial molar thermodynamic functions of solution, that is, Gibbs energy, enthalpy, and entropy were calculated. A comparison showed that the solubility of H 2 S in [emim][Tf 2 N] is greater than [emim] [PF 6 ].

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Section: Introductionmentioning

confidence: 66%

Solubility of H₂S in Ionic Liquids 1-Ethyl-3-methylimidazolium Hexafluorophosphate ([emim][PF₆]) and 1-Ethyl-3-methylimidazolium Bis(trifluoromethyl)sulfonylimide ([emim][Tf₂N])

et al. 2010

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“…The thermogravimetric method measures the solute uptake in the investigated solvent by means of a microbalance. Buoyancy corrections must be taken into account in order to correct the expansion of the solvent during the solute absorption [27,32,36]. The manometric method measures the pressure decay in a thermo-controlled cell chamber which contains a layer of solvent [35,37].…”

Section: Introductionmentioning

confidence: 99%

Assessment of VOC absorption in hydrophobic ionic liquids: Measurement of partition and diffusion coefficients and simulation of a packed column

Castillo

Biard

Guihéneuf

et al. 2019

Chemical Engineering Journal

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deltif Amrane, et al.. Assessment of VOC absorption in hydrophobic ionic liquids: Measurement of partition and diffusion coefficients and simulation of a packed column. Chemical Engineering Journal, Elsevier, 2019, 360, pp. AbstractPartition coefficients of toluene and dichloromethane (DCM) in 23 hydrophobic ionic liquids (ILs), which can be used potentially for the physical absorption of volatile organic compounds (VOCs), were measured at 298 K. The partition coefficients, expressed as Henry's law constants, were 400 to 1300 times for toluene and 10 to 47 times for DCM lower in the selected ILs than in water. Thus, the toluene and DCM diffusion coefficients were measured in three high potential hydrophobic ILs and in [Bmim][NTf 2 ] using a thermogravimetric microbalance. Diffusivity measurements were performed at 298K for toluene and between 278 and 308K for DCM. Diffusion coefficients in ILs, ranging between 1 and 4×10 -11 m 2 s -1 , were from 18 to 90 times lower than in water at 298 K. The diffusion coefficients were correlated to the temperature, the solute molar volume, the IL viscosity and molar volume with an average error of 4.2%. Finally, a 3 m industrial packed column was simulated for the removal of DCM and toluene in [AllylEt 2 S][NTf 2 ] and [bmim][NTf 2 ], which both present moderate viscosities of nearly 50 mPa s at 293K. The overall mass-transfer coefficient, the removal efficiency and the pressure drop were calculated and compared to those obtained using other heavy solvents (a silicon * Corresponding author : pierre-francois.biard@ensc-rennes.fr, Tel: + 33 2 23 23 81 49 2 oil and di-(2-ethylhexyl) adipate). This prospective simulation has demonstrated a good potential of ionic liquids for the toluene removal. Nonetheless, the DCM removal efficiencies simulated were lower than 44%. It suggests that even more efficient ionic liquids can be tuned and synthesized in the future for this specific application. Highlights Toluene partition coefficients in 23 ILs were in the range 0.5-3.5 Pa m 3 mol -1  Dichloromethane partition coefficients in 23 ILs were in the range 5-17 Pa m 3 mol -1  VOC diffusion coefficients in the range 1-4×10 -11 m 2 s -1 were measured in 4 ILs  The computed toluene removal efficiency in a packed column was from 52 to 99.6%  The computed dichloromethane removal efficiency in a packed column was lower than 44% Graphical abstractVicious air containing VOC: Treated air Ionic liquid Loaded ionic liquid Metal Pall rings 3.0 m 1.0 m •Toluene •Dichloromethane Operating conditions Hydrodynamics Mass-transfer rate (K l a°) Pressure drop Removal efficiency Solvent assessment for VOC removal in a packed column Partition coefficient Diffusion coefficient Ionic liquid properties (m, r, s) Static headspace method Static thermogravimetric method Measurements Simulation •[bmim][NTf 2 ] •[AllylEt 2 S][NTf 2 ] Finally, the hydrodynamics and mass-transfer in a packed column fed with [Bmim][NTf 2 ] and [AllylEt 2 S][NTf 2 ] were simulated for DCM and toluene absorption. * AR is the affinity r...

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“…The partial molar volume describes the increase in volume of the sorbing medium when a mole of CO 2 is sorbed on it. The density ρ a = 264 kg/m 3 obtained for sorption on shale is very small with respect to equivalent densities when CO 2 dissolves in water or brine (Carrol and Mather, 1992;Enick and Klara, 2009;Parkinson and Nevers, 1969) or in ionic melts (Huang et al, 2005;Kumelan et al, 2009;Duncan and Agee, 2011;Jalili et al, 2010) or sorbs on polymers Kamiya et al, 1994). Therefore an explanation in terms of a sorbed phase density must be critically evaluated.…”

Section: Similar Observations Were Made Bymentioning

confidence: 99%

Sorption of CO2 in Shales Using the Manometric Set-up

et al. 2012

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In a transition period from a fossil fuel based society to a sustainable energy society it is expected that CO 2 capture and subsequent sequestration (CCS) in geological formations will play a major role in reducing greenhouse gas emissions. Possibilities of sequestration include storage in aquifers and depleted gas reservoir. The storage capacity of gas reservoirs for CO 2 depends also on the sorption in the omnipresent minerals and shales. It is important to investigate whether adsorption on shales gives an important contribution to the storage capacity. It is also important to relate the adsorption to the carbon content in the shale. Only a few measurements have been reported in the literature for high-pressure gas sorption on shales, and interest is largely focused on shales occurring outside Europe. We present results using a high pressure manometric setup on a dried black shale sample from Belgium. It consists of more than 57% of clay minerals and 6.58% organic matter. The excess sorption isotherm shows an initial increase to a maximum value of 0.19 mmol/gram and then starts to decrease until it becomes zero at 82 bar and subsequently the excess sorption becomes negative. Similar behavior was also observed for other shales and coal reported in the literature. We derive the equation for excess sorption in the manometric set-up allowing for a changing void volume. This equation is based on the finite density of the adsorbed phase. However, this is not the only mechanism causing a maximum in the sorption curve. Other reasons for void volume change are swelling of the shale and volume changes due to chemical reactions excluding sorption. Further research is necessary to investigate reasons for void volume changes in shales.

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Solubility and diffusion of CO2 and H2S in the ionic liquid 1-ethyl-3-methylimidazolium ethylsulfate

Cited by 179 publications

References 31 publications

Solubility of H₂S in Ionic Liquids 1-Ethyl-3-methylimidazolium Hexafluorophosphate ([emim][PF₆]) and 1-Ethyl-3-methylimidazolium Bis(trifluoromethyl)sulfonylimide ([emim][Tf₂N])

Solubility of H₂S in Ionic Liquids 1-Ethyl-3-methylimidazolium Hexafluorophosphate ([emim][PF₆]) and 1-Ethyl-3-methylimidazolium Bis(trifluoromethyl)sulfonylimide ([emim][Tf₂N])

Assessment of VOC absorption in hydrophobic ionic liquids: Measurement of partition and diffusion coefficients and simulation of a packed column

Sorption of CO2 in Shales Using the Manometric Set-up

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Solubility and diffusion of CO2 and H2S in the ionic liquid 1-ethyl-3-methylimidazolium ethylsulfate

Cited by 179 publications

References 31 publications

Solubility of H2S in Ionic Liquids 1-Ethyl-3-methylimidazolium Hexafluorophosphate ([emim][PF6]) and 1-Ethyl-3-methylimidazolium Bis(trifluoromethyl)sulfonylimide ([emim][Tf2N])

Solubility of H2S in Ionic Liquids 1-Ethyl-3-methylimidazolium Hexafluorophosphate ([emim][PF6]) and 1-Ethyl-3-methylimidazolium Bis(trifluoromethyl)sulfonylimide ([emim][Tf2N])

Assessment of VOC absorption in hydrophobic ionic liquids: Measurement of partition and diffusion coefficients and simulation of a packed column

Sorption of CO2 in Shales Using the Manometric Set-up

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Product

Resources

About

Solubility of H₂S in Ionic Liquids 1-Ethyl-3-methylimidazolium Hexafluorophosphate ([emim][PF₆]) and 1-Ethyl-3-methylimidazolium Bis(trifluoromethyl)sulfonylimide ([emim][Tf₂N])

Solubility of H₂S in Ionic Liquids 1-Ethyl-3-methylimidazolium Hexafluorophosphate ([emim][PF₆]) and 1-Ethyl-3-methylimidazolium Bis(trifluoromethyl)sulfonylimide ([emim][Tf₂N])