Excess second virial coefficients and critical temperatures of methyl acetate and diethyl sulfide

1990 ◽  
Vol 35 (1) ◽  
pp. 38-40 ◽  
Author(s):  
Peter J. McElroy ◽  
A. T. Gellen ◽  
S. S. Kolahi
Keyword(s):  
Methyl Acetate ◽  
Virial Coefficients ◽  
Critical Temperatures ◽  
Diethyl Sulfide ◽  
Second Virial Coefficients

Excess second virial coefficients and critical temperatures: Acetone+ methyl acetate

AIChE Journal ◽  
1983 ◽  
Vol 29 (6) ◽  
pp. 1007-1010 ◽  
Author(s):  
P. J. McElroy ◽  
H. Hashim ◽  
Wong Loke Tatt
Keyword(s):  
Methyl Acetate ◽  
Virial Coefficients ◽  
Critical Temperatures ◽  
Second Virial Coefficients

The second virial coefficients of mixed polar vapours

1959 ◽  
Vol 249 (1258) ◽  
pp. 414-426 ◽  
Keyword(s):  
Methyl Acetate ◽  
Virial Coefficient ◽  
Methyl Formate ◽  
Second Virial Coefficient ◽  
Virial Coefficients ◽  
Ethyl Formate ◽  
Carbonyl Oxygen ◽  
Second Virial Coefficients ◽  
Theoretical Significance ◽  
Boyle’S Law

The second virial coefficients of binary mixtures of chloroform with methyl formate, n -propyl formate, methyl acetate, ethyl acetate and diethylamine have been measured in a ‘Boyle’s law apparatus’ at temperatures between 50 and 95 °C. The measured values are consistently higher than predicted by the theory of corresponding states, and a quantitative interpretation is proposed, based on the hypothesis that the esters and amine are partially dimerized and are involved in association with the chloroform by hydrogen bonding. A linear relation is shown to exist between the heats and entropies of association for the various mixtures, and the theoretical significance of this is discussed. There is some evidence that hydrogen bonds are formed through the alkoxyl oxygen by formate esters and through the carbonyl oxygen by acetate esters. The paper includes data on the second virial coefficient for the pure esters and for ethyl formate and methyl propionate.

Upper critical solution temperatures of hydrocarbon + fluorocarbon mixtures

1978 ◽  
Vol 31 (1) ◽  
pp. 19 ◽  
Author(s):  
CP Hicks ◽  
RL Hurle ◽  
LS Toczylkin ◽  
CL Young
Keyword(s):  
Reasonable Agreement ◽  
Fluid Model ◽  
Virial Coefficients ◽  
Temperature Data ◽  
Solution Temperature ◽  
Critical Temperatures ◽  
Critical Solution Temperature ◽  
Second Virial Coefficients ◽  
Upper Critical Solution Temperature ◽  
Critical Solution Temperatures

Values of the interaction parameter ξ have been calculated from upper critical solution temperature data by use of the van der Waals one- fluid model for a range of hydrocarbon+fluorocarbon mixtures. The values obtained are compared with values calculated from gas-liquid critical temperatures and mixed second virial coefficients where experimental data on these properties are available. The overall agreement between calculated from these properties is only fair but there is reasonable agreement between ξ calculated from gas-liquid critical temperatures and upper critical solution temperatures for mixtures of quasi-spherical molecules. ��� Experimental upper critical solution temperatures are reported for 26 systems which have not been studied previously. Gas-liquid critical temperatures of four systems are reported.

The Bender Equation of State and Virial Coefficients

2000 ◽  
Vol 65 (9) ◽  
pp. 1464-1470 ◽  
Author(s):  
Anatol Malijevský ◽  
Tomáš Hujo
Keyword(s):  
Equation Of State ◽  
Virial Coefficient ◽  
Virial Coefficients ◽  
Low Density ◽  
Second Virial Coefficients ◽  
The Third ◽  
Temperature Dependences ◽  
Experimental Values

The second and third virial coefficients calculated from the Bender equation of state (BEOS) are tested against experimental virial coefficient data. It is shown that the temperature dependences of the second and third virial coefficients as predicted by the BEOS are sufficiently accurate. We conclude that experimental second virial coefficients should be used to determine independently five of twenty constants of the Bender equation. This would improve the performance of the equation in a region of low-density gas, and also suppress correlations among the BEOS constants, which is even more important. The third virial coefficients cannot be used for the same purpose because of large uncertainties in their experimental values.

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