Excess molar volumes of ternary mixtures {n-butylacetae+1-butanol+1, 2-butanediol} and {n-butylacetate+1-butanol+1, 3-butanediol} at T=303.15K

Rezaei–Sameti, M.; Iloukhani, H.; Rakhshi, M.

doi:10.1016/j.molliq.2009.08.010

Cited by 9 publications

(10 citation statements)

References 19 publications

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“…Hence, the average absolute deviations (AADs) are 0.05 and 0.02%, respectively. But these experimental data did not agree with the report of Sameti et al 23 However, both data have a similar trend, which indicates that there is a good agreement with the reference data at an average absolute deviation (AAD) of 1.7%. Literature comparison for the rest of the binary mixtures was not done due to lack of published data, even using free online tool ThermoLit.…”

Section: Water Content Water Contents In Ils [Emim]-[hso 4 ] [Emim][e...contrasting

confidence: 60%

Liquid Densities and Excess Quantities for the Green Esterification Process

Christabel¹,

Ramalingam²,

Reji³

et al. 2019

J. Chem. Eng. Data

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Liquid densities of deep eutectic solvents (DESs) such as choline chloride + glycerol {[ChCl][Gly]}, choline chloride + acetic acid {[ChCl][AA]}; ionic liquids (ILs), such as 1-ethyl-3-methylimidazolium hydrogen sulfate {[EMIM][HSO4]}, 1-ethyl-3-methylimidazolium ethyl sulfate {[EMIM][EtSO4]}, and 1-butyl-3-methylimidazolium acetate {[BMIM][Ac]}; and mixture of DESs + ILs as well as organic mixtures, such as n-butyl acetate + butanol and n-butyl acetate + acetic acid were measured at different temperatures from 293.15 to 343.15 K with an increase of 5 K. From this measured density, isobaric expansivity, excess molar volume, partial molar volume, excess partial molar volume, and apparent molar volume were calculated to understand and characterize the solution behavior as well as solvent–solvent interactions for the entire mole fraction at different temperatures. The excess molar properties showing positive deviation for DESs + ILs system, which indicates a creation of volume in the binary mixtures and disruption of H-bonds in the solution environment. Further, the sign and magnitude of all of the studied binary systems gave a good estimate of the attractive and disruptive interactions, chemical aggregation, H-bond formation, salt (choline chloride)–H (imidazolium) interaction, and salt (choline chloride)–O (acetate anion) interaction between those two components in the binary mixtures. The Redlich–Kister equation was used to fit the excess molar volume data and their corresponding regression coefficients (R 2) were also found. The σ-profile and σ-potential for the compounds in the present study have been generated and analyzed by means of specific molecular interactions between all of the studied compounds using the conductor like screening model for real solvents model.

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Section: Water Content Water Contents In Ils [Emim]-[hso 4 ] [Emim][e...contrasting

confidence: 60%

Liquid Densities and Excess Quantities for the Green Esterification Process

Christabel¹,

Ramalingam²,

Reji³

et al. 2019

J. Chem. Eng. Data

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“…We have compared our experimental densities of butan-1-ol + butane-1,2-diol with those of Zorębski et al Our measurements agree with their values within an average absolute percentage deviation of 0.04, 0.05, and 0.05% at 298.15, 303.15, 308.15 K, respectively. Sameti et al reported densities of binary mixture of butan-1-ol + butane-1,2-diol at 303.15 K. Our values agree with their measurements within an absolute percentage deviation of 0.09%. Experimental viscosities of butan-1-ol + butane-1,2-diol at 303.15 K have been compared with those of Rezaei-Sameti et al Our measurements agree with their values within an average absolute percentage deviation of 4.6% from x 1 = 0.2–0.9.…”

Section: Resultssupporting

confidence: 90%

“…The estimated standard uncertainty in V E is 0.001 cm 3 ·mol –1 . Figure shows a comparison of our V E values with data reported by Zorębski et al and Sameti et al at 303.15 K for butan-1-ol + butane-1,2-diol. As shown in Figure , the values of the excess molar volumes disagree with more than 0.1 cm 3 ·mol.…”

Section: Resultssupporting

confidence: 64%

“…Excess molar volumes, V E , for the butan-1-ol (1) + butane-1,2-diol (2) mixture as a function of mole fraction x 1 at T = 303.15 K: ●, this work; ■, Zorębski et al; ◆, Sameti et al; and , corresponds to eq .…”

Section: Resultsmentioning

confidence: 96%

“…Percent relative deviations Δρ = ρ(exp) – ρ(lit) (a), and Δη = η(exp) – η(lit) (b), of experimental densities ρ(exp) and viscosities η(exp) of butan-1-ol (1) + butane-1,2-diol (2) mixture from values ρ(lit) and η(lit) of literature measurements as a function of mole fraction x 1 : ◆, Zorębski et al; ■, Sameti et al; ▲, Rezaei-Sameti et al …”

Section: Resultsmentioning

confidence: 99%

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Densities and Viscosities for Binary Liquid Mixtures of Butan-1-ol + Propane-1,2-diol, + Butane-1,2-diol and 2-Methylpropan-1-ol + Propane-1,2-diol, + Butane-1,2-diol from 298.15 to 333.15 K at 0.1 MPa

et al. 2017

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This paper presents densities and viscosities of binary mixtures of butan-1-ol (or 2-methylpropan-1-ol) with propane-1,2-diol, and butane-1,2-diol from 298.15 to 333.15 K at 0.1 MPa over the entire concentration range. A vibrating tube densimeter provides the densities while a glass capillary viscometer provides the efflux time which is related with the kinematic viscosity. Experimental densities and viscosities of the pure components agree with data reported in the literature within an average absolute percentage deviation of 0.03% and 1.16%, respectively. The excess molar volumes and viscosity deviation calculated from experimental data present negative deviations from ideality in the entire temperature range. The Redlich−Kister equation is used to represent the composition behavior of excess molar volumes and the viscosity deviations. The Nava-Rios equation correlates our kinematic viscosity data within an overall average absolute percentage deviation of 1.085% while the McAllister equation correlates the kinematic viscosity within 1.541%.

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