Influence of hydrogen bond donor on zinc chloride in separation of binary mixtures: Activity coefficients at infinite dilution

Mgxadeni, Ncomeka; Mmelesi, Oarabile; Kabane, Bakusele; Bahadur, Indra

doi:10.1016/j.molliq.2022.118596

Cited by 23 publications

(20 citation statements)

References 46 publications

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“…For example, at T = 313.15 K, pentane produced γ 13 ∞ = 184.8, 1-pentene produced γ 13 ∞ = 93.02, and 1-pentyne produced γ 13 ∞ = 53.54. These effects were observed in the previous studies. , They are due to unlike forces, i.e., van der Waals and many other attractive forces, between the participating mixture components and favor solvent–solvent interactions and solute–solute interactions over solvent–solvent interactions in a mixture …”

Section: Data and Discussionsupporting

confidence: 51%

“…This is not true for water (Δ S 1 E,∞ = 14.57), as short chain alcohols like methanol produced Δ S 1 E,∞ = 16.40, cycloalkenes like cyclopentene produced Δ S 1 E,∞ = 59.54, ketones like acetone produced Δ S 1 E,∞ = 2.752, and alkynes like 1-hexyne produced Δ S 1 E,∞ = 18.57. If the entropy values are negative, it is conceivable that this solute molecule is organizing itself in ethaline. Positive values indicate the breaking of the hydrogen bonds, as is well-known …”

Section: Data and Discussionmentioning

confidence: 99%

“…The infinite dilution activity coefficient (IDAC) is a common attributor of all other excess thermodynamic properties, including partial molar excess functions such as enthalpy, entropy, and Gibbs free energy, as well as selectivity and capacity values . IDAC measurements can be determined by several techniques, including inert gas stripping, differential static cell, head space chromatography, and gas–liquid chromatography (GLC). , This study used GLC to determine the infinite dilution activity coefficient values of different organic solutes of different functional groups, including alkanes, alkenes, alkynes, cycloalkanes, cycloalkenes, aromatics, alcohols, ketones, and water in ethaline (1:2 molar ratio) at different temperatures and ambient pressures. In addition, the present study uses the method adopted from the previous studies, such as Manyoni, Kabane, and Redhi, Manyoni and Redhi, and Nkosi, Tumba, and Ramsuroop …”

Section: Introductionmentioning

confidence: 99%

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Separation Performance of Ethaline: Infinite Dilution Activity Coefficients and the Excess Thermodynamic Properties

Manyoni

Redhi

2023

J. Chem. Eng. Data

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This paper presents excess thermodynamic data of a mixture of choline chloride, a hydrogen bond acceptor (HBA), and ethylene glycol, a hydrogen bond donor (HBD), with a molar ratio of 1:2, correspondingly. This mixture is popularly known as ethaline. A gas−liquid chromatograph (GLC) fitted with a thermal conductivity detector (TCD) was used to determine infinite dilution activity coefficient (IDAC) values of different functional groups (e.g., alkanes, alkenes, alkynes, cycloalkanes, aromatics, alcohols, ketones, and water) for 32 different organic solutes at different temperatures (T = 313.15−343.15 K) and air pressures. The partial excess molar properties, including Gibbs free energy, enthalpy, and entropy, were computed from the infinite dilution activity coefficient measurements at T = 323.15 K. Furthermore, the separation performance of common separation problems, i.e., hexane/ benzene, cyclohexane/hexane, ethanol/toluene, and acetone/methanol, was evaluated through the selectivity and capacity values, and this was also computed from the infinite dilution activity coefficient values. It was found that ethaline could not be suitable for prospective separation issues, as a result of the poor thermodynamic data that were measured.

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Section: Data and Discussionsupporting

confidence: 51%

Section: Data and Discussionmentioning

confidence: 99%

Section: Introductionmentioning

confidence: 99%

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Separation Performance of Ethaline: Infinite Dilution Activity Coefficients and the Excess Thermodynamic Properties

Manyoni

Redhi

2023

J. Chem. Eng. Data

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“…28,29 They also have high thermal stability, low volatility, and convertible polarity, and can thus be used as suitable solvents in future alternative research and industry. 30 The HBD molecule interacts with the chloride ion of ChCl and induces the lower melting point of the blend caused by cationic molecular symmetry, etc.…”

Section: Preparation and Characterization Of Desmentioning

confidence: 99%

DES: their effect on lignin and recycling performance

Zhang

et al. 2023

RSC Adv.

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“…Currently, the theoretical model of

and temperature is derived from the relationship between the activity coefficient and the partial molar excess function, which is expressed as:

. Assuming infinite dilution molar entropy (

) and infinite dilution molar enthalpy (

) are constants within a certain temperature range, the above relationship expresses a two-parameter model [ 7 , 15 , 16 ]. The subsequent three-parameter model [ 17 ], four-parameter model [ 18 ], and five-parameter model with the introduction of molecular descriptors X i [ 19 ] were developed from this equation.…”

Section: Introductionmentioning

confidence: 99%

Research of a Thermodynamic Function (∂p∂x)T, x→0: Temperature Dependence and Relation to Properties at Infinite Dilution

Zheng

Chen

Wang

et al. 2022

IJMS

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In this work, we propose the idea of considering \({\left(\frac{\partial p}{\partial x}\right)_{T,x \rightarrow 0}}\) as an infinite dilution thermodynamic function. Our research shows that \({\left(\frac{\partial p}{\partial x}\right)_{T,x \rightarrow 0}}\) as a thermodynamic function is closely related to temperature, with the relation being simply expressed as: \({\ln \left(\frac{\partial p}{\partial x}\right)_{T,x \rightarrow 0}=\frac{A}{T}+B}\). Then, we use this equation to correlate the isothermal vapor–liquid equilibrium (VLE) data for 40 systems. The result shows that the total average relative deviation is 0.15%, and the total average absolute deviation is 3.12%. It indicates that the model correlates well with the experimental data. Moreover, we start from the total pressure expression, and use the Gibbs–Duhem equation to re-derive the relationship between \({\left(\frac{\partial p}{\partial x}\right)_{T,x \rightarrow 0}}\) and the infinite dilution activity coefficient (\({\gamma^{\infty}}\)) at low pressure. Based on the definition of partial molar volume, an equation for \({\left(\frac{\partial p}{\partial x}\right)_{T,x \rightarrow 0}}\) and gas solubility at high pressure is proposed in our work. Then, we use this equation to correlate the literature data on the solubility of nitrogen, hydrogen, methane, and carbon dioxide in water. These systems are reported at temperatures ranging from 273.15 K to 398.15 K and pressures up to 101.325 MPa. The total average relative deviation of the predicted values with respect to the experimental data is 0.08%, and the total average absolute deviation is 2.68%. Compared with the Krichevsky–Kasarnovsky equation, the developed model provides more reliable results.

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Influence of hydrogen bond donor on zinc chloride in separation of binary mixtures: Activity coefficients at infinite dilution

Cited by 23 publications

References 46 publications

Separation Performance of Ethaline: Infinite Dilution Activity Coefficients and the Excess Thermodynamic Properties

Separation Performance of Ethaline: Infinite Dilution Activity Coefficients and the Excess Thermodynamic Properties

DES: their effect on lignin and recycling performance

Research of a Thermodynamic Function (∂p∂x)T, x→0: Temperature Dependence and Relation to Properties at Infinite Dilution

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