By Arthur Adamson (Auth.)
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Additional resources for A Textbook of Physical Chemistry
Liquid phase vapor phase (P - p) dx, (1-65) where Ρ is the general, isotropic pressure, ρ is the local pressure component parallel to the surface, and χ is distance normal to the surface. If we can, by some analysis, calculate how the density or molar volume varies across a liquid-vapor interface, then use of an equation of state such as the van der Waals equation allows a calculation of ρ as a function of x, and hence of the surface tension (see Tolman, 1949). A final brief consideration concerns the determination of the critical point of a substance.
In addition, a collection of worked-out examination questions is available: ADAMSON, A. W. (1969). "Understanding Physical Chemistry," 2nd ed. Benjamin, New York. CITED REFERENCES BENSON, S. , AND GOLDING, R. A. (1951). J. Chem. Phys. 1 9 , 1413. GLASSTONE, S. (1946). " Van Nostrand-Reinhold, Princeton, New Jersey. HIRSCHFELDER, J. , CURTISS, C. , AND BIRD, R. B . (1964). "Molecular Theory of Gases and Liquids," corrected ed. Wiley, New York. MACDOUGALL, F. H . (1936). / . Amer. Chem. Soc. 5 8 , 2585.
Molecular velocity distribution in one dimension for N . 2 of a molecule having components u and ν is 1 N — 7/2 _|_ (2-26) JJ2 and the Boltzmann equation is 2 dN(u, v) = A^exp^- 2 m(u + v ) •j 2kf j du dv, (2-27) where dN(u, v)/N0 is now the fraction of molecules having velocity components between u and u + du and ν and t; + ifo. Equation (2-27) factors into two integrals, each analogous to that of Eq. P P 2 m(u + v ) ' 2kf . du dv. (2-28) The distribution function of Eq. (2-28) now requires a three-dimensional plot for its display, as illustrated in Fig.