Isothermal Vapor−Liquid Equilibria of 2-Methoxy-2-methylbutane (TAME) + n-Alcohol (C1−C4) Mixtures at 323.15 and 333.15 K

Isothermal vapor-liquid equilibrium (VLE) data at 333.15 K are measured for the binary systems {di-isopropyl ether (DIPE) + ethanol} and {DIPE + 2,2,4-trimethylpentane} and for the ternary system {DIPE + ethanol + 2,2,4-trimethylpentane} by using headspace gas chromatography. The experimental VLE data were correlated with the G E model: Margules, van Laar, Wilson, nonrandom two-liquid, and UNIQUAC equations. The excess molar volume and deviations in molar refractivity data are reported for the binary systems {DIPE + ethanol}, {DIPE + 2,2,4-trimethylpentane}, and {ethanol + 2,2,4-trimethylpentane} at 303.15 K. In addition, excess molar enthalpies for two binaries, {DIPE + ethanol} and {DIPE + 2,2,4-trimethylpentane}, at 303.15 K are also reported. These data were correlated with the Redlich-Kister equation. The excess molar volume and deviations in molar refractivity data are also reported for the ternary system {DIPE + ethanol + 2,2,4-trimethylpentane} at 303.15 K. The ternary data were correlated with the Cibulka equation. Also, the isocline of excess molar enthalpies for the same ternary system at 303.15 K was calculated using the Radojkovič equation.

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“…1/2 (10) where N is the number of experimental data points and n is the number of fitted parameters.…”

Section: Resultsmentioning

confidence: 99%

“…The procedure of measurement has been described in detail elsewhere. 10,11 Densities were measured by a digital vibrating glass tube density meter (Anton Paar, model DMA 5000, Graz, Austria).…”

Section: Methodsmentioning

confidence: 99%

Isothermal Vapor−Liquid Equilibrium at 333.15 K and Excess Molar Volumes, Refractive Indices, and Excess Molar Enthalpies at 303.15 K for the Binary and Ternary Mixtures of Di-isopropyl Ether, Ethanol, and 2,2,4-Trimethylpentane

2009

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“…In our VLE measuring method, the equilibrium pressure and liquid phase mole fractions are not directly measured, but they are calculated from the experimental vapor phase composition and thermodynamic equations [13]. The experimental VLE compositions and calculated pressures for the binary system ethanol (1) + 2,2,4-trimethylpentane (2) at 333.15 K are listed in Table 2 and plotted in Fig.…”

Section: Resultsmentioning

confidence: 99%

“…The HSGC consists of a gas chromatograph (HP 6890N) and a headspace sampler (HP19395A), which has an electro-pneumatic sampling system and a precision thermostat, having an accuracy of ±0.1 K. A HP-5 (30 m × 0.32 mm × 0.25 m) capillary column and a thermal conductivity detector were used for the analysis. The experimental procedure is described in detail elsewhere [3,13]. Densities were measured by a digital vibrating glass tube density meter (Anton Paar, model DMA 5000, Graz, Austria).…”

Section: Apparatus and Proceduresmentioning

confidence: 99%

Isothermal vapor–liquid equilibrium at 333.15K and excess molar volumes and refractive indices at 298.15K for the mixtures of di-methyl carbonate, ethanol and 2,2,4-trimethylpentane

Hwang

Park

2009

Fluid Phase Equilibria

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“…3 Unfortunately, environmental studies 4 and thermophysical key properties of TAME as co-oxygenate (specifically vapor liquid equilibrium and interfacial tension data) are scarce when compared to other more traditional ether oxygenates. 2 Previous works reporting vaporÀliquid equilibrium (VLE) data of ethanol þ TAME cover atmospheric conditions 5 and isothermal conditions ranging from (323.15 to 333.15) K. 6,8 In addition, azeotropic coordinates have also been characterized. 5À8 According to these works, ethanol þ TAME exhibits a positive deviation from ideal behavior, and its azeotrope impoverishes in ethanol as pressure (or temperature) increases.…”

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confidence: 99%

Vapor–Liquid Equilibria and Interfacial Tensions of the System Ethanol + 2-Methoxy-2-methylbutane

2011

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Isobaric vaporÀliquid equilibrium (VLE) data have been measured for the binary system ethanol þ 2-methoxy-2-methylbutane at (50, 75, and 94 kPa) and over the temperature range (334 to 356) K. Equilibrium determinations were performed in a VLE still with circulation of both phases. The dependence of interfacial tensions of this mixture on concentration was also determined at atmospheric pressure and 303.15 K, using the maximum differential bubble pressure technique. According to experimental results, the mixture exhibits a positive deviation and a minimum boiling point azeotrope for which the mole fraction impoverishes in ethanol as pressure (or temperature) increases. In addition, the determined interfacial tensions exhibit a negative deviation from the linear behavior. The VLE data of the binary mixture satisfy the Fredenlund's consistency test and were wellcorrelated by the Wohl, nonrandom two-liquid (NRTL), Wilson, and universal quasichemical (UNIQUAC) equations for all of the measured isobars. Interfacial tensions, in turn, were satisfactorily correlated using the RedlichÀKister equation. ' INTRODUCTIONOxygenated gasolines have been incorporated in commercial fuels from the past decade, to reduce carbon monoxide emissions, and for reducing ozone depletion in zones where air pollution levels exceed the allowed limits. 1 Oxygenated gasoline approximately contains 2.7 wt % of oxygen and emit 15 % less unburned hydrocarbons than traditional gasoline mixtures. The purpose of oxygenate blending it to add oxygen-bearing solvents to fuels, and alcohols (e.g., methanol, ethanol, butanol) as well as ether oxygenates (such as 2-methoxy-2-methylpropane or MTBE, 2-ethoxy-2-methyl-propane or ETBE, 2,2 0 -oxybis- [propane] or DIPE, and 2-methoxy-2-methylbutane or TAME) have been demonstrated to be reliable and economical alternatives for the purpose. MTBE and ethanol were first introduced as oxygenates showing an adequate performance as motor fuels with high octane number. However, due to high solubility of MTBE in water it presents significant hazard in case of accidental release to environment, thus forcing to evaluate its substitution by other less harmful ethers. Some well-known alternatives for replacing MTBE are ETBE, DIPE, or TAME. Particularly, TAME shows an attractive potential over DIPE and ETBE since, compared to MTBE, it exhibits comparable thermophysical properties however showing clear benefits as: (a) a lower environmental impact, 2 (b) effective gasoline antiknocking, and (c) it may be produced from commercially available feedstocks. 3 Unfortunately, environmental studies 4 and thermophysical key properties of TAME as co-oxygenate (specifically vapor liquid equilibrium and interfacial tension data) are scarce when compared to other more traditional ether oxygenates. 2 Previous works reporting vaporÀliquid equilibrium (VLE) data of ethanol þ TAME cover atmospheric conditions 5 and isothermal conditions ranging from (323.15 to 333.15) K. 6,8 In addition, azeotropic coordinates have also been characterized. ...

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Isothermal Vapor−Liquid Equilibria of 2-Methoxy-2-methylbutane (TAME) + n-Alcohol (C₁−C₄) Mixtures at 323.15 and 333.15 K

Cited by 42 publications

References 11 publications

Isothermal Vapor−Liquid Equilibrium at 333.15 K and Excess Molar Volumes, Refractive Indices, and Excess Molar Enthalpies at 303.15 K for the Binary and Ternary Mixtures of Di-isopropyl Ether, Ethanol, and 2,2,4-Trimethylpentane

Isothermal Vapor−Liquid Equilibrium at 333.15 K and Excess Molar Volumes, Refractive Indices, and Excess Molar Enthalpies at 303.15 K for the Binary and Ternary Mixtures of Di-isopropyl Ether, Ethanol, and 2,2,4-Trimethylpentane

Isothermal vapor–liquid equilibrium at 333.15K and excess molar volumes and refractive indices at 298.15K for the mixtures of di-methyl carbonate, ethanol and 2,2,4-trimethylpentane

Vapor–Liquid Equilibria and Interfacial Tensions of the System Ethanol + 2-Methoxy-2-methylbutane

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