Excess Molar Volume Calculation and Viscosity Deviation and Excess Gibbs Energy for Binary Solution of 1- Propanol with Butyl Acetate at Temperatures (40,50,60) 0C

In this research, the solubility Process of the binary liquid solution(1-Propanol and butyl acetate) were studied at temperature(40,50.60)0C. Densities ρ by pycnometer method and viscosity ƞ by OSTWALD tube that calibrated with distilled water was measured. Then excess molar volume was calculated of pure component and its mixtures that was prepared over the entire mole fraction range. It has been observed that excess molar volumes values were negative at all temperatures. After that, the deviation in viscosity ∆ ƞ and Excess Gibbs free energy ∆GE was determined and it has been observed that it takes negative values at all temperatures. Excess molar volume, deviation in viscosity, excess Gibbs free energy were correlated with Redlich-Kister equation Type polynomial and the showed an accepted standard deviation between the experimental and calculated values it has been shown the effect of Hydrogen bonds formation and the spherical shape for the molecules and its size on the excess thermodynamic properties.

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Excess Gibbs free energy of butyl acetate with cyclohexane and aromatic hydrocarbons at 308.15K

Korean Journal of Chemical Engineering ◽

10.1007/s11814-008-0048-8 ◽

2008 ◽

Vol 25 (2) ◽

pp. 273-278 ◽

Cited By ~ 1

Author(s):

Sanjeev Maken ◽

Naveen Verma ◽

Ankur Gaur ◽

Ho-Jun Song ◽

Krishan Chander Singh ◽

...

Keyword(s):

Free Energy ◽

Gibbs Free Energy ◽

Aromatic Hydrocarbons ◽

Butyl Acetate ◽

Excess Gibbs Free Energy

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CALCULATION OF EXCESS MOLAR VOL-UMES OF SOME TERNARY LIQUID MIX-TURES AT 303.15 K

Baghdad Science Journal ◽

10.21123/bsj.1.2.274-279 ◽

2004 ◽

Vol 1 (2) ◽

pp. 274-279

Author(s):

Baghdad Science Journal

Keyword(s):

Statistical Theory ◽

Molar Volume ◽

Excess Molar Volume ◽

Entire Range ◽

Butyl Acetate ◽

Excess Molar Volumes ◽

Ternary Mixtures ◽

Positive Deviation ◽

Molar Volumes ◽

Wide Range

Excess molar volumes of five ternary mixtures of 2- methoxy ethanol(1) +butyl acetate(2)+benzene(3), +toluene(3), +chlorobenzene(3), +bromobenzene(3), and +nitrobenzene(3) have been measured at 303.15K. The excess molar volume exhibited positive deviation over the entire range of composition in the systems 2-methoxy ethanol(1)+ butyl acetate(2)+ benzene(3),+toluene(3) and sigmoid behavior in the case of the remaining systems. Flory's statistical theory have been extended to predict the excess molar volumes of the five ternary mixtures at 303.15 k over a wide range of composition . An excellent agreement has been found between the experimental and theoretical excess molar volumes , both in magnitude and sign .

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Thermodynamic Excess Functions of Binary Liquid Mixtures with Chain Association of One Component*. Part I: The Excess Gibbs Free Energy GE/RT

Zeitschrift für Naturforschung A ◽

10.1515/zna-1976-1229 ◽

1976 ◽

Vol 31 (12) ◽

pp. 1651-1660 ◽

Cited By ~ 6

Author(s):

F. Becker ◽

M. Kiefer ◽

P. Rhensius ◽

H. D. Schäfer

Keyword(s):

Free Energy ◽

Gibbs Free Energy ◽

Chain Length ◽

Liquid Mixtures ◽

Binary Liquid Mixtures ◽

Excess Gibbs Free Energy ◽

Component Part ◽

Excess Functions ◽

Binary Liquid ◽

Self Association

Abstract In this paper equilibrium models for the calculation of the excess Gibbs free energy of binary liquid mixtures are developed, the component A of which undergoes chain-forming self-association whilst the component B acts as an 'inert' solvent. It is shown that the extension of the well-known chain-association model of Mecke and Kempter, in which the probability of chain prolongation is assumed to be independent of chain length, is unable to establish satisfactory results because it does not exhibit sufficient unsymmetry. Reduction of the probability of chain growth with in-creasing chain length leads to an improved model with the geometric series replaced by the exponential series. This model, in which only two parameters are used, i. e. the equilibrium constants K for mutual solvation of A and B, and ρ for self-association of A, allows fitting of isothermal experimental GE /R T literature data on cycloalkanol-cycloalkane, alkanol-alkane, and NMF -CCl4 systems within the limits of experimental error. Compared with the two-parameter Wilson equation which gives equally small standard deviations, our equilibrium model has the advantage of allowing passage from GE to HE data and of being applicable to liquid-liquid equilibria.

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