Morgan Textbook

Morgan, J.P. Designer Drugs. In Substance Abuse—A Comprehensive Textbook (Lowinson JH, Ruiz P, Millman RB, Langrod JG, eds). 3rd ed. Baltimore Williams Wilkins, 1997, 264-269. 

Stumm, W., and J. J. Morgan, Aquatic Chemistry, Wiley, New York, 1981. Chapter 5 of this standard textbook gives many examples of the concepts discussed in the present chapter. A broad conceptual picture of mineral dissolution kinetics and mechanisms is developed in the celebrated three-part paper The Coordination Chemistry of Weathering ... 

Many literature sources document closed-form algebraic expressions for view factors. Particularly comprehensive references include the compendia by Modest (op. cit., App. D) and Siegel and Howell (op. cit., App. C). The appendices for both of these textbooks also provide a wealth of resource information for radiative transfer. Appendix F of Modest, e.g., references an extensive listing of Fortan computer codes for a variety of radiation calculations which include view factors. These codes are archived in the dedicated Internet web site maintained by the ublisher. The textbook by Siegel and Howell also includes an extensive atabase of view factors archived on a CD-ROM and includes a reference to an author-maintained Internet web site. Other historical sources for view factors include Hottel and Sarofim (op. cit., Chap. 2) and Hamilton and Morgan (NACA-TN 2836, December 1952). 

There appears to be a disparity in terminology of isotherms between the hydrogeology and chemistry literature. While chemistry textbooks describe adsorption isotherms (e.g., Drever, 1988, p. 362 Stumm and Morgan, 1996, p. 521), the hydrogeology literature uses the term sorption isotherms (e.g., Domenico and Schwartz, 1998, p.299 Fetter, 1999, p. 122 Freeze and Cherry, 1979, p.403). Manuals for popular transport codes also describe sorption isotherms (Zheng, 1990, pp.2-9). According to Sposito (1984), the term adsorption includes all reactions on the two-dimensional solid-water interface physical and chemical adsorption and ion-exchange the term sorption refers to all processes that transfer an ion from aqueous to solid phase. 

R. N. Andersen (1986). No book on Aquatic Chemistry can hardly be better than the one written by W. Stumm and J.J. Morgan (1996). There is furthermore the textbook written by K. Grasshofif,... 

Riley, D. M. (2011). Engineering thermodynamics and 21st century energy problems A textbook companion for student engagement. San Rafael Morgan and Claypool. 

The progress of the field can be traced with the aid of a series of five review articles published at two-year intervals in Analytical Chemistry. These articles cover noteworthy advances within each two-year interval Kowalski, Frank and Kowalski, Delaney, Ramos et al., and Brown et al. Detailed descriptions of the methods used in multivariate analysis in analytical chemistry can be obtained from a series of recently published textbooks Sharaf et al., Massart et al., Deming and Morgan, Massart and Kaufman, and Strouf. ... 

The International Abstracts of the World s Corrosion Control Literature COR AB, issued by NACE covering the years since 1980, is one of the widest literature databases in the world (approx. 72 (KX) abstracts), and includes approximately 3000 papers concerning CP and over 100 papers on AP. The first textbooks devoted to CP were published in the U.K. and the U.S.A. and written by Morgan (1959) and Apple-gate (1960). In Poland in the same year a textbook was published devoted to the anodic, cathodic, and sacrificial protection of metals in technology (Juchniewicz, 1960). In the U.S.A. Peabody (1967) produced an... 

Burch, P.R.J. 1967. Radiation physics. In Principles of Radiation Protection—A Textbook of Health Physics, K.Z. Morgan and J.E. Turner, eds., pp. 366-397. New York John Wiley and Sons. 

Values of Henry s law constants are tabulated in a variety of sources, such as Lyman et al. (1990), Howard (1989-1991), Mackay and Shiu (1981), and Hine and Mookerjee (1975). Table 1.3 lists Hemy s law constants for some common chemicals. Occasionally a Henry s law constant is expressed in an inverse fashion, as the ratio of a chemical s concentration in water to its partial pressure in air see, e.g., Stumm and Morgan (1996, p. 213). In that reference, Kh is equivalent to 1/H as H is defined in this textbook. When H is not tabulated, it can be estimated by dividing the vapor pressure of a chemical at a particular temperature by its aqueous solubility at that temperature. Henry s law constants generally increase with increased temperature, primarily due to the significant temperature dependency of chemical vapor pressures as previously mentioned, solubility is less sensitive to the range of temperatures normally found in the environment. Note that even if a chemical has a low vapor pressure, it may still have a high Henry s law constant, if its solubility is very low. 

---