Table XXIV-l.—Van der Waals Constants for Imperfect Gases |

Since Mayer s theory originated in a theory for imperfect gases, it naturally tends to calculate the nearest analogue of gas pressure that an ionic solution exhibits—osmotic pressure. [Pg.317]

Orcutt RH, Cole RH (1967) Dielectric constants of imperfect gases. III. Atomic gases, hydrogen, and nitrogen. J Chem Phys 46 697-702 [Pg.149]

Ursell, H. D., The evaluation of Gibbs phase integral for imperfect gases. Proc. Cambridge Philos. Soc. 23, 685 (1927). [Pg.227]

K2. Kennard, E. H., Kinetic Theory of Gases. McGraw-Hill, New York, 1938. K3. Kihara, T., Imperfect Gases. Asakusa Bookstore, Tokyo, 1949 (in Japanese). Translated into English by the U. S. Office of Air Research, Wright-Patterson Air Force Base. [Pg.237]

Thus real gases are those whose behaviour no longer fits the Ideal Gas Equation (31.1) and in this sense they are defined as non-ideal (imperfect) gases. The Ideal Gas Law is thus a limiting law in the sense that it serves to provide the demarcation between ideal gas and non-ideal (real) gas behaviour. [Pg.93]

The relations between the and the 6 are the same as those in the case of imperfect gases and can be obtained either by using an iteration method or by constructing a recurrence formula. We shall, however, omit the discussion and rewrite Eq. (2.24) in terms of the weight concentration c instead of the density Cg = The use of the weight concentration [Pg.240]

Recalling the calculations of gas equilibria carried out earlier, we have for imperfect gases [Pg.128]

STATISTICAL MECHANICS Principles and Applications, Terrell L. Hill. Standard text covers fundamentals of statistical mechanics, applications to fluctuation theory, imperfect gases, distribution functions, more. 448pp. 5X 8X. [Pg.122]

We conclude with the matter of adsorbate-adsorbate interactions these give rise to deviations from Henry s law behavior. These may be expressed in the form of a virial equation, much as is done for imperfect gases. Following Steele [8], one can write [Pg.638]

A number of different empirical equations have been proposed to allow for the deviations of physisorption isotherms from Henry s law. An approach which is analogous to that used in the treatment of imperfect gases and non-ideal solutions is to adopt a virial treatment. Kiselev and his co-workers (Avgul et al. 1973) favoured the form [Pg.95]

In Eq. (2), contributions to the energy from electronic states have been neglected, since they are not signiflcant at room temperature for most molecules. Also, any small intermo-lecular energies that occur for imperfect gases are not considered. [Pg.108]

There is another reservation that should be mentioned for those who see Monte Carlo and MD techniques as all-conquering they use classical mechanics. This is all very well for some movements, e.g., translation in imperfect gases. But what of the quantized vibration Or what of quantal aspects in rate calculations or the tunneling of protons in the conduction of aqueous acid solutions (see Section 4.11.5), for example [Pg.323]

In following the most direct path from the principles of thermodynamics to the understanding of equilibrium in chemical systems, we have bypassed many useful thermodynamic relations that involve the properties of perfect and imperfect gases. These are summarized in this chapter. [Pg.120]

Explain in about 250 words the essential approach of the Mayer theory of ionic solutions and how it differs from the ionic-atmosphere view. The parent of Mayer s theory was the McMillan-Mayer theory of 1950. With what classical equation for imperfect gases might it be likened [Pg.352]

Flere N is the number of segments in the polymer chain, n is the number segment density, and v and w account for the pair and triplet interactions, respectively, between segments. In fact, v and w are counterparts of the second and third virial coefficients in the theory of imperfect gases " v and w can be calculated if information about the polymer chain and the solvent is available [Pg.207]

Again, therefore, all thermodynamic properties of a system in quantum statistics can be derived from a knowledge of the partition function, and since this is the trace of an operator, we can choose any convenient representation in which to compute it. The most fruitful application of this method is probably to the theory of imperfect gases, and is well covered in the standard reference works.23 [Pg.472]

Here the quantity PV/nRT is often called the virial and the quantities 1, B(T), C(7T), etc., the coefficients of its expansion in inverse powers of the volume per mole, F/n, are called the virial coefficients, so that B(T) is called the second virial coefficient, C(T) the third, etc. The experimental results for equations of state of imperfect gases are usually stated by giving B(T), C(T), etc., as tables of values or as power series in the temperature. It now proves possible to derive the second virial coefficient B T) fairly simply from statistical mechanics. [Pg.190]

It should be noted that it is assumed that the intermolecular forces do not affect the internal degrees of freedom so that is independent of whether these forces are present or not. When they are absent (Zf = 0), the integral Z collapses to and equation (2.2.31) becomes the same as equation (2.2.23). The important task of the statistical thermodynamics of imperfect gases and liquids is to evaluate Z. This subject is discussed in detail later in this chapter. However, the nature of the intermolecular forces which give rise to the potential energy U is considered next. [Pg.52]

See also in sourсe #XX -- [ Pg.41 ]

See also in sourсe #XX -- [ Pg.119 ]

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