Vapor–liquid equilibrium in the production of the ionic liquid, 1-hexyl-3-methylimidazolium bromide ([HMIm][Br]), in acetone

Minnick, David L.; Scurto, Aaron M.

doi:10.1016/j.fluid.2013.11.030

Cited by 7 publications

(3 citation statements)

References 35 publications

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“…Moreover at ambient pressure without CO 2 , the solubility of 1-haloalkanes in the IL is relatively low while 1-methylimidazole is miscible with the IL. The mole fraction solubility of 1-bromohexane in [HMIm][Br] at 25 • C is 0.022 mole fraction [48] which is similar to other systems [49]. However, the presence of CO 2 in the IL phase makes the solubility of even polar solutes decrease significantly in the IL phase; this has been described as using CO 2 pressure as a "separation switch" for IL mixtures [31].…”

Section: Reaction System Phase Behavior and Equilibriasupporting

confidence: 52%

Kinetics and polarity effects in the synthesis of the ionic liquid, 1-hexyl-3-methyl-imidazolium bromide, using compressed CO2

Nwosu

Schleicher

Scurto

2015

The Journal of Supercritical Fluids

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Section: Reaction System Phase Behavior and Equilibriasupporting

confidence: 52%

Kinetics and polarity effects in the synthesis of the ionic liquid, 1-hexyl-3-methyl-imidazolium bromide, using compressed CO2

Nwosu

Schleicher

Scurto

2015

The Journal of Supercritical Fluids

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“…Table shows the quantitative results obtained when the test is applied to a group of 70 published nv‐VLE data series . The results show a rejection ratio (rejected/analyzed systems) of 40% for a κ ψ = 3, see Equation , although this value decreases to 12% when κ ψ = 5.…”

Section: Application Of the Proposed Consistency Test To Real Series mentioning

confidence: 97%

Extension of the validation method for vapor–liquid equilibrium data to systems with nonvolatile components

2019

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In this work, a method is proposed to validate the experimental data of solutions of n-components in vapor-liquid equilibria (VLE) with some nonvolatile component (nv-VLE). The methodology is based on the resolution of the differential Gibbs-Duhem equation using two forms (differential and integral) described in a previous work. The combination of both forms evaluates as many relationships between the variables that define each data series in equilibrium (p, T, x 1, … , n-1 , y 1, … , n-1 ) as degrees of freedom the problem has, although in this work it is only necessary to use the integral form. The proposed method is applied to 70 experimental data series published in the literature, considering the numerical limits previously assigned to parameters established for the integral-form, according to the following. (a) A parameter ψ is identified as p or T according to if the data are iso-T or iso-p; (b) verification of the data is assessed by the difference ε M ψ, i − ψ i,exp −ψ i, cal =ψ, witĥ

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“…Relatively few works are available devoted to the imidazolium-based RTILs in ACET and some other RTILs sporadically. [25][26][27][28][29][30][31][32][33][34][35][36][37] Based on its molecular and physical chemical properties, ACET excellently mixes with most ILs thanks to the carbonyl group. Furthermore, ACET exhibits a low viscosity, 0.307 cP, 38 which correlates with its low normal-pressure boiling point.…”

Section: Introductionmentioning

confidence: 99%

Acetone as a polar cosolvent for pyridinium-based ionic liquids

Chaban

2016

RSC Adv.

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The work reports transport and structure properties of the three pyridinium-based ionic liquids (RTILs) -N-butylpyridinium hexafluorophosphate [BPY][PF 6 ], N-butylpyridinium trifluorosulfonate [BPY][TF] and N-butylpyridinium bis(trifluoromethanesulfonyl)imide [BPY][TFSI] -in their mixtures with acetone (ACET). The ionic conductivity maximum occurs at 10 mol% RTIL, irrespective of the anion. The absolute ionic conductivity value of [BPY][TF] is higher than those of other RTILs. This is explained by a weaker cation-anion binding than that in [BPY][PF 6 ] and smaller anion size than that of [BPY][TFSI]. All the investigated RTILs are infinitely miscible with ACET, which boosts their diffusivity and conductivity. A small viscosity of ACET favors a drastic viscosity decay in the RTIL-ACET mixtures. Structure analysis (radial distribution functions, ionic clusters) of the mixtures are in line with their transport properties providing a reliable microscopic interpretation of the observed macroscopic properties. As a molecular co-solvent, ACET constitutes an interesting alternative and competitor to more intensively investigated liquids.

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Vapor–liquid equilibrium in the production of the ionic liquid, 1-hexyl-3-methylimidazolium bromide ([HMIm][Br]), in acetone

Cited by 7 publications

References 35 publications

Kinetics and polarity effects in the synthesis of the ionic liquid, 1-hexyl-3-methyl-imidazolium bromide, using compressed CO2

Kinetics and polarity effects in the synthesis of the ionic liquid, 1-hexyl-3-methyl-imidazolium bromide, using compressed CO2

Extension of the validation method for vapor–liquid equilibrium data to systems with nonvolatile components

Acetone as a polar cosolvent for pyridinium-based ionic liquids

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