By Lyle F. Albright
It is a vector PDF reproduction. Grayscale, 1930 pages. first-class caliber, with bookmarks and renumbered pages.
From basics to plant operations, Professor Albright’s guide is an intensive but succinct advisor to daily tools and calculations utilized in chemical engineering purposes. Leaders from a good range of specialties offer a transparent assessment of simple details, together with illustrative case examples and references to more information for extra complex examine. They talk about crucial rules, calculations, and key concerns corresponding to response engineering, method keep an eye on and layout, waste disposal, and electrochemical and biochemical engineering. the ultimate chapters disguise patents, highbrow estate, communications, and moral matters which are such a lot proper to engineers.
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Extra resources for Albright's Chemical Engineering Handbook
The book by Zaytsev and Aseyev  contains extensive tables based on smoothed experimental results; some caution is needed with such tables because smoothing procedures can introduce artifacts. The CRC Handbook of Chemistry and Physics  also contains density data for many electrolytes in water at 20°C. 3). 5 2 i i i zi is the charge on species i, coefficient A depends on various solute and solvent properties, and the coefficients Bi are specific to the individual ions. Parameters for the Jones-Dole equation at room temperature are tabulated by Marcus .
The most widely used method is that of Benson, for which software is available ; more limited calculations are available in the NIST Chemistry Webbook . For relatively small molecules, it is becoming routine to calculate thermochemical properties in the ideal-gas state with computational quantum mechanics. For organic species with fewer than about 10 nonhydrogen atoms, the methods are sufficiently well developed that they can rival or even surpass the accuracy that can be obtained from experiment.
The material exiting the apparatus is collected, and the amount of sample dissolved can be measured at the end of the experiment. Knowledge of the number of moles carried away, the number of moles of carrier gas used, and the pressure of equilibration allows calculation of the partial pressure of the sample at equilibrium, which is approximately its vapor pressure. Care must be taken to ensure that all of the carrier gas is equilibrated with the sample and to prevent premature condensation before the solute is collected.
Albright's Chemical Engineering Handbook by Lyle F. Albright