scholarly journals Thermodynamic evidence for complex formation between carbon tetrachloride and triethylamine

1973 ◽  
Vol 26 (5) ◽  
pp. 1143 ◽  
Author(s):  
DV Fenby
Keyword(s):  
Carbon Tetrachloride ◽  
Complex Formation ◽  
Electron Acceptor ◽  
Excess Enthalpy ◽  
Molar Excess ◽  
Molar Excess Enthalpy

The molar excess enthalpy of the system carbon tetrachloride+ triethylamine has been measured at 298.15 K. The results are consistent with complex formation between the unlike molecules and provide further evidence for the electron acceptor ability of carbon tetrachloride.

AN ADIABATIC SOLUTION CALORIMETER USED FOR MEASURING THE MOLAR EXCESS ENTHALPY OF THE SYSTEM CARBON TETRACHLORIDE – BENZENE AT 25 °C

1965 ◽  
Vol 43 (7) ◽  
pp. 1912-1917 ◽  
Author(s):  
J. E. Bennett ◽  
G. C. Benson
Keyword(s):  
Carbon Tetrachloride ◽  
Excess Enthalpy ◽  
Adiabatic Calorimeter ◽  
Molar Excess ◽  
Heats Of Mixing ◽  
Maximum Value ◽  
Molar Excess Enthalpy ◽  
Continuous Record ◽  
Flexible Diaphragm ◽  
Solution Calorimeter

A new adiabatic calorimeter for measuring heats of mixing is described. The design of the mixing cell avoids the presence of a vapor space, and accommodates changes in volume by means of a flexible diaphragm. The apparatus is equipped with automatic adiabatic control and produces a continuous record of the temperature of the mixing cell. An extensive series of measurements was carried out for the system carbon tetrachloride – benzene at 25 °C. The maximum value of the molar excess enthalpy, 113.4 ± 0.5 J mole−1, occurred at a mole fraction of carbon tetrachloride equal to 0.4907. For most of the concentration range, the results are from 1 to 2 J mole−1 lower than data reported recently by other investigators.

COMPLEXES OF STANNIC IODIDE WITH AROMATIC HYDROCARBONS

1965 ◽  
Vol 43 (5) ◽  
pp. 1272-1278 ◽  
Author(s):  
J. F. Murphy ◽  
D. E. Baker
Keyword(s):  
Carbon Tetrachloride ◽  
Complex Formation ◽  
Aromatic Hydrocarbon ◽  
Aromatic Hydrocarbons ◽  
Extinction Coefficient ◽  
Regular Solutions ◽  
Benzene Toluene ◽  
Yield Values ◽  
Complex Stabilities ◽  
Iodide Complex

Spectrophotometric measurements on solutions of stannic iodide were found to provide evidence for complex formation with aromatic hydrocarbons. Calculations, based on spectra for mixed solutions of benzene and stannic iodide in carbon tetrachloride, yield values of 0.26 for the equilibrium constant (mole fraction), 28 400 1/mole cm for the molar extinction coefficient of the benzene – stannic iodide complex. Kinetic evidence indicates that the order of decreasing complex stabilities is from xylene to toluene to benzene. The formation of stannic iodide – aromatic hydrocarbon complexes provides an explanation for the discrepancy between measured solubilities of stannic iodide in benzene, toluene, and xylene, and the solubilities predicted by the Hildebrand theory of regular solutions.

Aromatic fluorocarbon mixtures. VI. Vapour pressures of carbon tetrachloride + hexafluorobenzene

1974 ◽  
Vol 27 (10) ◽  
pp. 2159 ◽  
Author(s):  
NF Pasco ◽  
DV Fenby
Keyword(s):  
Carbon Tetrachloride ◽  
Thermodynamic Properties ◽  
Equations Of State ◽  
Liquid Mixture ◽  
Excess Enthalpies ◽  
Molar Excess ◽  
Mixture Theories

Measurements are reported of the vapour pressures of the system carbon tetrachloride + hexafluorobenzene at 278.68 K. The molar excess Gibbs functions GE/M, obtained from these measurements have been combined with previously reported molar excess enthalpies to give GE/M at 298 K. Thermodynamic properties of CCl4+C6F6 at 298 K are compared with the predictions of liquid mixture theories based on analytic equations of state.

scholarly journals Verdampfungsgleichgewicht und thermodynamisehe Funktionen des flüssigen Systems Wasser + Essigsäure / Vapour-Liquid. Equilibrium and Thermodynamic Functions of the Liquid System Water + Acetic Acid

1973 ◽  
Vol 28 (10) ◽  
pp. 1740-1742 ◽  
Author(s):  
R. Haase ◽  
M. Pehlke ◽  
K.-H. Dücker
Keyword(s):  
Acetic Acid ◽  
Composition Dependence ◽  
Excess Enthalpy ◽  
Excess Entropy ◽  
Liquid System ◽  
Gibbs Function ◽  
Liquid Equilibrium ◽  
Molar Excess ◽  
C 30 ◽  
System Water

Vapour pressures and vapour compositions of the liquid system water + acetic acid have been measured at 25 °C, 30 °C, 35 °C, 40 °C, and 45 °C in the whole range of compositions. The dimerization of acetic acid in the vapour being taken into account, the molar excess Gibbs function ḠE is derived from the measurements. Earlier measurements of the molar excess enthalpy HE are combined with the -GE values to give the molar excess entropy SE. The “symmetry rule” (Haase, 1951) concerning the composition dependence of ḠE, -HE, and S̄E has been confirmed.

Sign in / Sign up

Export Citation Format

Share Document