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A special type of error that you need to avoid that relates specifically to multitasking is deadlock, which occurs when two threads have a circular dependency on a pair of synchronized objects For example, suppose one thread enters the monitor on object X and another thread enters the monitor on object Y If the thread in X tries to call any synchronized method on Y, it will block as expected However, if the thread in Y, in turn, tries to call any synchronized method on X, the thread waits forever, because to access X, it would have to release its own lock on Y so that the first thread could complete Deadlock is a difficult error to debug for two reasons: In general, it occurs only rarely, when the two threads time-slice in just the right way It may involve more than two threads and two synchronized objects (That is, deadlock can occur through a more convoluted sequence of events than just described) To understand deadlock fully, it is useful to see it in action The next example creates two classes, A and B, with methods foo( ) and bar( ), respectively, which pause briefly before trying to call a method in the other class The main class, named Deadlock, creates an A and a B instance, and then starts a second thread to set up the deadlock condition The foo( ) and bar( ) methods use sleep( ) as a way to force the deadlock condition to occur

Part I:

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The transformation of raw materials into products of greater value by means of chemical reaction is a major industry, and a vast array of commercial products is obtained by chemical synthesis Sulfuric acid, ammonia, ethylene, propylene, phosphoric acid, chlorine, nitric acid, urea, benzene, methanol, ethanol, and ethylene glycol are examples of chemicals produced in the United States in billions of kilograms each year These in turn are used in the large-scale manufacture of fibers, paints, detergents, plastics, rubber, paper, fertilizers, insecticides, etc Clearly, the chemical engineer must be familiar with chemical-reactor design and operation Both the rate and the equilibrium conversion of a chemical reaction depend on the temperature, pressure, and composition of reactants Consider, for example, the oxidation of sulfur dioxide to sulfur trioxide A catalyst is required if a reasonable reaction rate is to be attained With a vanadium pentoxide catalyst the rate becomes appreciable at about 57315 K (300 C) and continues to increase at higher temperatures On the basis of rate alone, one would operate the reactor at the highest practical temperature However, the equilibrium conversion to sulfur trioxide falls as temperature rises, decreasing from about 90% at 79315 K (520 C) to 50% at about 95315 K (680 C) These values represent maximum possible conversions regardless of catalyst or reaction rate The evident conclusion is that both equilibrium and rate must be considered in the exploitation of chemical reactions for commercial purposes Although reaction rates are not susceptible to thermodynamic treatment, equilibrium conversions are Therefore, the purpose of this chapter is to determine the effect of temperature, pressure, and initial composition on the equilibrium conversions of chemical reactions Many industrial reactions are not carried to equilibrium; reactor design is then based primarily on reaction rate However, the choice of operating conditions may still be influenced by equilibrium considerations Moreover, the equilibrium conversion of a reaction provides a goal by which to measure improvements in a process Similarly, it may determine whether or not an experimentalinvestigationof a new process is worthwhileFor example, if thermodynamicanalysis indicates that a yield of only 20% is possible at equilibrium and if a 50% yield is necessary for the process to be economically attractive, there is no purpose to an experimental study On the other hand, if the equilibrium yield is 80%, an experimental program to determine the reaction rate for various conditions of operation (catalyst, temperature, pressure, etc) may be warranted Reaction stoichiometry is treated in Sec 131, and reaction equilibrium, in Sec 132 The equilibrium constant is introduced in Sec 133, and its temperature dependence and evaluation.

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