Corrigendum to “Vapour pressure and excess Gibbs free energy of binary mixtures of hydrogen sulphide with ethane, propane, and n-butane at temperature of 182.33 K” [J. Chem. Thermodyn. 38 (2006) 1651–1654]

2007 ◽  
Vol 39 (6) ◽  
pp. 990 ◽  
Author(s):  
L.Q. Lobo ◽  
A.G.M. Ferreira ◽  
I.M.A. Fonseca ◽  
A.M.P. Senra
Keyword(s):  
Free Energy ◽  
Gibbs Free Energy ◽  
Binary Mixtures ◽  
Hydrogen Sulphide ◽  
Vapour Pressure ◽  
Excess Gibbs Free Energy

Activity coefficients and excess Gibbs’ free energy of some binary mixtures formed by p-cresol at 95.23kPa

2007 ◽  
Vol 39 (7) ◽  
pp. 1022-1026 ◽  
Author(s):  
T.E. Vittal Prasad ◽  
N. Venkanna ◽  
Y. Naveen Kumar ◽  
K. Ashok ◽  
N.M. Sirisha ◽  
...  
Keyword(s):  
Free Energy ◽  
Gibbs Free Energy ◽  
Binary Mixtures ◽  
Activity Coefficients ◽  
Excess Gibbs Free Energy

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

1976 ◽  
Vol 31 (12) ◽  
pp. 1651-1660 ◽  
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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