Heats of mixing. II. Acetonitrile and nitromethane systems

1956 ◽  
Vol 9 (2) ◽  
pp. 180 ◽  
Author(s):  
I Brown ◽  
W Fock
Keyword(s):  
Free Energy ◽  
Carbon Tetrachloride ◽  
Composition Range ◽  
Excess Entropy ◽  
Excess Free Energy ◽  
Energy Data ◽  
Entropy Of Mixing ◽  
Heats Of Mixing

The heats of mixing at 45.00 �C have been measured at intervals over the whole composition range for the systems : acetonitrile+carbon tetrachloride, acetonitrile+benzene, acetonitrile +nitromethane, nitromethane + carbon tetrachloride, and nitromethane+benzene. These data, together with the excess free energy data of Brown and Smith (1954, 1955a, 1955b), have been used to calculate the excess entropy of mixing for these systems.

Thermodynamic properties of alcohol solutions. II. Ethanol and isopropanol systems

1956 ◽  
Vol 9 (3) ◽  
pp. 364 ◽  
Author(s):  
I Brown ◽  
W Fock ◽  
F Smith
Keyword(s):  
Experimental Data ◽  
Free Energy ◽  
Thermodynamic Properties ◽  
Excess Entropy ◽  
Excess Free Energy ◽  
Published Data ◽  
Entropy Of Mixing ◽  
Heats Of Mixing ◽  
Equilibrium Data

New experimental data are given for the heats of mixing of the systems ethanol+toluene at 35 �C, ethanol+methylcyclohexane at 35 �C, and iso-propanol+benzene at 45 �C and for the liquid-vapour equilibrium data for the latter system at 45 �C. These data have been used together with previously published data to calculate the excess free energy, heat and excess entropy of mixing at even mole fractions for the above systems. These functions have also been calculated from published data for the systems ethanol+benzene at 45 �C and ethanol+2,2,4-trimethylpentane at 25 �C.

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.

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.

Molar excess Gibbs free energies of benzene – m-xylene mixtures

1969 ◽  
Vol 47 (4) ◽  
pp. 539-542 ◽  
Author(s):  
T. Boublík ◽  
G. C. Benson
Keyword(s):  
Free Energy ◽  
Excess Free Energy ◽  
Free Energies ◽  
Energy Data ◽  
Molar Excess ◽  
Polar Mixtures ◽  
Vapor Liquid Equilibria ◽  
Flory’S Theory ◽  
Vapor Liquid

Vapor–liquid equilibria for the system benzene – m-xylene were measured in a circulation still at 25, 37, and 50 °C. Excess free energy data were analyzed in terms of Flory's theory of non-polar mixtures.

Heats of mixing of Alcohol solutions

1955 ◽  
Vol 8 (3) ◽  
pp. 361
Author(s):  
I. Brown ◽  
W Fock
Keyword(s):  
Carbon Tetrachloride ◽  
Composition Range ◽  
Ethylene Dichloride ◽  
Binary Liquid ◽  
Heats Of Mixing ◽  
Liquid Systems

A calorimeter for the measurement of the heats of mixing of binary liquid systems at temperatures from 20 to 45 �C is described. Heats of mixing have been measured for approximately equimolar mixtures of benzene+carbon tetrachloride at 25 �C, benzene+ethylene dichloride at 25 �C, acetone+chloroform at 25 �C, and ethanol+-carbon tetrachloride at 45 �C. Measurements have been made at intervals over the whole composition range of the systems ethanol+2,2,4-trimethylpentane at 25 �C and ethanol+benzene at 45 �C.

Excess thermodynamic properties of the liquid system acetone + methyl iodide

1964 ◽  
Vol 281 (1386) ◽  
pp. 366-376 ◽  
Keyword(s):  
Free Energy ◽  
Thermodynamic Properties ◽  
Methyl Iodide ◽  
Excess Entropy ◽  
Heat Content ◽  
Liquid Mixtures ◽  
Liquid System ◽  
Excess Thermodynamic Properties ◽  
Temperature Range ◽  
Entropy Of Mixing

The increase in heat content attending the isobaric formation of liquid mixtures of acetone and methyl iodide in varying proportions has been determined calorimetrically in the temperature range 253 to 308 °K. The corresponding change in free energy has been measured from analyses of the mixed vapour at equilibrium with the mixed liquids. By difference, the change in entropy associated with the mixing has been found. Most of this derives, as is usual, from the randomness of the mixture, but there is a relatively small residuum (the so-called excess entropy of mixing) which is found to vary in an unusual way with respect to the composition.

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.

EXCESS VOLUMES, VAPOR PRESSURES, AND RELATED THERMODYNAMIC PROPERTIES OF THE SYSTEM ACETONE–CHLOROFORM–BENZENE, AND ITS COMPONENT BINARY SYSTEMS

1966 ◽  
Vol 44 (10) ◽  
pp. 1183-1189 ◽  
Author(s):  
A. N. Campbell ◽  
E. M. Kartzmark ◽  
R. M. Chatterjee
Keyword(s):  
Binary Systems ◽  
Excess Entropy ◽  
Excess Free Energy ◽  
Heat Of Mixing ◽  
Vapor Pressures ◽  
Free Energies ◽  
Volume Changes ◽  
Heats Of Mixing ◽  
Energy Of Mixing ◽  
Free Energy Of Mixing

The volume changes on mixing of the three binary mixtures, acetone–chloroform, benzene–chloroform, acetone–benzene, and the ternary mixture, acetone–chloroform–benzene, and their molar refractivities and viscosities, were determined.Determinations of total and partial vapor pressures were made. The systems acetone–chloroform and benzene–chloroform show negative deviations from Raoult's law. The system acetone–benzene shows positive deviations.The excess Gibbs free energies of mixing have been calculated for all systems. By combining these data with previously measured heats of mixing (1), the excess entropy has also been calculated. The curves representing zero excess volume, zero heat of mixing, zero excess free energy of mixing, and zero excess viscosity as functions of composition in the ternary system do not coincide. It, therefore, must be concluded that they result from compensating effects and do not represent ideality.

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.

THE ENERGY OF HYDROGEN BONDING IN THE SYSTEM: ACETONE–BROMOFORM

1966 ◽  
Vol 44 (8) ◽  
pp. 917-924 ◽  
Author(s):  
A. N. Campbell ◽  
E. M. Kartzmark
Keyword(s):  
Free Energy ◽  
Solid Phase ◽  
Freezing Point ◽  
Dipole Moments ◽  
Excess Entropy ◽  
Excess Free Energy ◽  
Eutectic Type ◽  
Vapor Pressures ◽  
Phase Compound ◽  
Volumes Of Mixing

A study of the equilibrium freezing-point diagram for the system acetone–bromoform shows that no solid-phase compound forms between acetone and bromoform. The diagram is of the simple eutectic type, the eutectic lying at −101° and 84 mole % acetone. The enthalpies of mixing have been determined for various compositions of mixture and the numerical value of ΔH (per mole of acetone or bromoform) extrapolated to infinite excess of bromoform or of acetone, to obtain the value for completely undissociated complex. This figure is −1.3 kcal per mole of complex (assumed mole to mole). The dipole moments, excess volumes of mixing, viscosities, and total and partial vapor pressures of the system have been measured. From these data, the excess free energy and excess entropy and other thermodynamic functions have been evaluated.

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