The relation between structure of van der Waals molecular dimers and dielectric second virial coefficients

1977 ◽  
Vol 66 (6) ◽  
pp. 2753-2754 ◽  
Author(s):  
J. M. Deutch ◽  
William Klemperer
Keyword(s):  
Van Der Waals ◽  
Virial Coefficients ◽  
Second Virial Coefficients

scholarly journals Pressure dependence of the equilibrium constant of ammonia

1942 ◽  
Vol 179 (979) ◽  
pp. 433-438 ◽  
Keyword(s):  
Equilibrium Constant ◽  
High Temperatures ◽  
Pressure Dependence ◽  
Van Der Waals ◽  
Virial Coefficients ◽  
Numerical Results ◽  
Second Virial Coefficients ◽  
Imperfect Gas ◽  
Theory And Experiments ◽  
Good Agreement

The pressure dependence of the equilibrium constant of a slightly imperfect gas is calculated. At sufficiently high temperatures, the constants occurring in the formula for the equilibrium constant can be expressed in terms of the van der Waals constants. The latter can be obtained from the second virial coefficients. Numerical results for ammonia give good agreement between the theory and experiments.

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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