Liquid-Vapour equilibria. V. The system Carbon Tetrachloride + Acetonitrile at 45°C

1954 ◽  
Vol 7 (3) ◽  
pp. 269 ◽  
Author(s):  
I Brown ◽  
F Smith
Keyword(s):  
Free Energy ◽  
Carbon Tetrachloride ◽  
Excess Free Energy ◽  
Energy Of Mixing ◽  
Equilibrium Data ◽  
Free Energy Of Mixing

Liquid-vapour equilibrium data are given for the system carbon tetrachloride + acetonitrile at 45.00 �C. These data are used to calculate the excess free energy of mixing for this system.

Liquid-vapour equilibria. VII. The systems nitromethane + benzene and nitromethane + carbon tetrachloride at 45°C

1955 ◽  
Vol 8 (4) ◽  
pp. 501
Author(s):  
I Brown ◽  
F Smith
Keyword(s):  
Free Energy ◽  
Carbon Tetrachloride ◽  
Excess Free Energy ◽  
Energy Of Mixing ◽  
Equilibrium Data ◽  
Free Energy Of Mixing

The liquid-vapour equilibrium data are given for the systems nitromethane+benzene and nitromethane+carbon tetrachloride at 45.00 �C. These data are used to calculate the excess free energy of mixing for these systems.

Liquid-vapour equilibria viii. The systems acetoke +benzene and acetone +carbon tetrachloride at 45°C

1957 ◽  
Vol 10 (4) ◽  
pp. 423 ◽  
Author(s):  
I Brown ◽  
F Smith
Keyword(s):  
Free Energy ◽  
Carbon Tetrachloride ◽  
Excess Free Energy ◽  
Energy Of Mixing ◽  
Equilibrium Data ◽  
Free Energy Of Mixing

The liquid-vapour equilibrium data are given for the systems acetone+benzene and acetone+carbon tetrachloride at 45.00� C . These data are used to calculate the excess free energy of mixing for these systems.

Liquid-Vapour Equilibria. VI. The systems Acetonitrile + Benzene at 45°C. and Acetonitrile + Nitromethane at 60°C

1955 ◽  
Vol 8 (1) ◽  
pp. 62 ◽  
Author(s):  
I Brown ◽  
F Smith
Keyword(s):  
Free Energy ◽  
Excess Free Energy ◽  
Energy Of Mixing ◽  
Equilibrium Data ◽  
Free Energy Of Mixing

Liquid-vapour equilibrium data are given for the systems acetonitrile + benzene at 45.00 �C and acetonitrile + nitromethane at 60.00 �C. These data are used to calculate the excess free energy of mixing for these systems.

Liquid-Vapour equilibria. IV. The system ethanol + benzene at 45°C

1954 ◽  
Vol 7 (3) ◽  
pp. 264 ◽  
Author(s):  
I Brown ◽  
F Smith
Keyword(s):  
Free Energy ◽  
Excess Free Energy ◽  
Energy Of Mixing ◽  
Equilibrium Data ◽  
Free Energy Of Mixing

New liquid-vapour equilibrium data are given for the system ethanol + benzene at 45.00 �C. These data are used to calculate the excess free energy of mixing for this system.

Liquid-Vapour Equilibria. IX. The Systems n-Propanol + Benzene and n-Butanol + Benzene at 45°C

1959 ◽  
Vol 12 (3) ◽  
pp. 407 ◽  
Author(s):  
I Brown ◽  
F Smith
Keyword(s):  
Free Energy ◽  
Excess Free Energy ◽  
Energy Of Mixing ◽  
Equilibrium Data ◽  
Free Energy Of Mixing

Liquid-vapour equilibrium data are given for the systems n-propanol+benzene and n-butanol+benzene at 45.00 OC. The data are used to calculate the excess free energy of mixing for these systems.

Liquid-Vapour Equilibria. X. The Systems Acetone+Nitromethane and Acetone+Acetonitrile at 45°C

1960 ◽  
Vol 13 (1) ◽  
pp. 30 ◽  
Author(s):  
I Brown ◽  
F Smith
Keyword(s):  
Free Energy ◽  
Experimental Error ◽  
Binary Systems ◽  
Virial Coefficient ◽  
Excess Free Energy ◽  
Specific Interaction ◽  
A Value ◽  
Energy Of Mixing ◽  
Equilibrium Data ◽  
Free Energy Of Mixing

Liquid-vapour equilibrium data are given for the systems acetone+nitromethane and acetone+acetonitrile at 45.00 �C. The data are used to calculate the excess free energy of mixing for these systems. The former system has a negative value of the excess free energy of mixing and shows a change in sign of the deviation of the activity of nitromethane from the Raoults law value at a mole fraction of acetone of 0.36. A value of the virial coefficient β12 in the equation of state of the mixed vapours was estimated from the equilibrium data for this system. The excess free energy of mixing for the system acetone+acetonitrile is zero within the experimental error over the whole concentration range. The Stockmayer potential was used to calculate values of β12, for the binary systems formed from acetone, nitromethane, and acetonitrile. For the system acetone+nitromethane the value estimated from our data is more negative than the value calculated using the Stockmayer potential, indicating a specific interaction, possibly hydrogen bonding, between the acetone and nitromethane molecules.

Higher Order Conditional Probabilities and Thermodynamics of Binary Molten Alloys

1997 ◽  
Vol 11 (02n03) ◽  
pp. 93-106 ◽  
Author(s):  
O. Akinlade
Keyword(s):  
Free Energy ◽  
Experimental Evidence ◽  
Cluster Model ◽  
Excess Free Energy ◽  
Higher Order ◽  
Thermodynamic Quantities ◽  
Equiatomic Composition ◽  
Conditional Probabilities ◽  
Energy Of Mixing ◽  
Free Energy Of Mixing

The recently introduced four atom cluster model is used to obtain higher order conditional probabilities that describe the atomic correlations in some molten binary alloys. Although the excess free energy of mixing for all the systems studied are almost symmetrical about the equiatomic composition, most other thermodynamic quantities are not and thus, the study enables us to explain the subtle differences in their physical characteristics required to describe the mechanism of the observed strong heterocoordination in Au–Zn or homocoordination in Cu–Ni within the same framework. More importantly, we obtain all calculated quantities for the whole concentration range thus complimenting experimental evidence.

scholarly journals Theoretical investigations on temperature dependence of thermodynamic properties and concentration fluctuations of In-Tl binary liquid alloys by optimization method

BIBECHANA ◽  
2017 ◽  
Vol 15 ◽  
pp. 11-23
Author(s):  
G K Shrestha ◽  
I S Jha ◽  
B K Singh
Keyword(s):  
Free Energy ◽  
Liquid Alloy ◽  
Entire Range ◽  
Excess Free Energy ◽  
Concentration Fluctuations ◽  
Binary Liquid ◽  
Energy Of Mixing ◽  
Different Temperatures ◽  
Free Energy Of Mixing ◽  
Best Fit

The thermodynamic properties, i.e. free energy of mixing (GM), heat of mixing (HM), entropy of mixing (SM) and activity (ai) of the component i (i , and structural property i.e. concentration fluctuations in long wave-length limit [Scc(0)] of In-Tl binary liquid alloy at a specified temperature have been investigated in the framework of quasi-lattice model on assuming the coupled effect of size ratio and entropic (or energetic) as well as enthalpic effect. These properties of In-Tl liquid alloy at 723 K have been computed theoretically by estimating the best fit value of order energy parameter (W) and size ratio () over the entire range of concentration in order to match their experimental values. The best fit value of  W at 723 K has been used to determine the values of W at different temperatures with the help of temperature derivative of W which are then used for the optimization procedure in order to calculate the corresponding values of excess free energy of mixing, partial excess free energy of mixing and activity of the components involved in the alloy at different temperatures. These parameters have been used to investigate the concentration fluctuations in long wavelength limit {Scc(0)} of In-Tl binary liquid alloy at different temperatures over the entire range of concentration which have been used to predict the various other structural properties like excess stability function (EXS), diffusion coefficient ratio (Dm/Did), short range order parameter (α1) at different temperatures.BIBECHANA 15 (2018) 11-23

The rubidium chloride – sodium chloride phase diagram

1970 ◽  
Vol 48 (22) ◽  
pp. 3483-3486 ◽  
Author(s):  
A. D. Pelton ◽  
S. N. Flengas
Keyword(s):  
Phase Diagram ◽  
Free Energy ◽  
Sodium Chloride ◽  
Excess Entropy ◽  
Excess Free Energy ◽  
Thermochemical Data ◽  
Cooling Curves ◽  
Molar Excess ◽  
Energy Of Mixing ◽  
Free Energy Of Mixing

The phase diagram of the RbCl–NaCl system has been measured by the method of cooling curves. By combining these data with available thermochemical data for the system, the integral molar excess free energy of mixing at 800 °C has been calculated as ΔGE = −632XRbClXNaCl cal/mole; and the integral molar excess entropy of mixing has been calculated as ΔSE = −0.208XRbClXNaCl cal/°K mole. Estimated precisions are ±50 cal for ΔGE and ±0.05 cal/°K mole for ΔSE at XRbCl = XNaCl = 0.5.

Theory of Immiscibility in Mineral Systems

1964 ◽  
Vol 33 (266) ◽  
pp. 1015-1023 ◽  
Author(s):  
Robert F. Mueller
Keyword(s):  
Free Energy ◽  
Excess Free Energy ◽  
Standard Free Energy ◽  
Regular Solutions ◽  
Qualitative Interpretation ◽  
Energy Of Mixing ◽  
Mineral Assemblages ◽  
Free Energy Of Mixing ◽  
The Stability ◽  
End Members

SummaryThe theoretical basis for the stability of binary and quasi-binary solutions is discussed with special emphasis on miscibility relations. Solutions of the distribution equations are presented for the case of two and three coexisting regular solutions and this model is used to illustrate the energetics of miscibility relations. The same principles are then extended to give a qualitative interpretation to sequences of mineral assemblages consisting of pyroxenes, amphiboles, micas, and feldspars. A formulation is presented for the intrinsic stability of a solution, which depends on the presence or absence of an excess free energy of mixing, and the extrinsic stability of a solution, which depends on the standard free energy of the component end members.

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