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Heat transfer is one of the most common operations in the chemical industry Consider, for example, the manufacture of ethylene glycol (an antifreeze agent) by the oxidation of ethylene to ethylene oxide and its subsequent hydration to glycol The catalytic oxidation reaction is most effective when carried out at temperatures near 52315 K (250 C) The reactants, ethylene and air, are therefore heated to this temperature before they enter the reactor To design the preheater one must know how much heat is transferred The combustion reactions of ethylene with oxygen in the catalyst bed tend to raise the temperature However, heat is removed from the reactor, and the temperature does not rise much above 52315 K (250 C) Higher temperatures promote the production of C02,an unwanted product Design of the reactor requires knowledge of the rate of heat transfer, and this depends on the heat effects associated with the chemical reactions The ethylene oxide product is hydrated to glycol by absorption in water Heat is evolved not only because of the phase change and dissolution process but also because of the hydration reaction between the dissolved ethylene oxide and water Finally, the glycol is recovered from water by distillation, a process of vaporization and condensation, which results in the separation of a solution into its components All of the important heat effects are illustrated by this relatively simple chemical-manufacturing process In contrast to sensible heat effects, which are characterized by temperature changes, the heat effects of chemical reaction, phase transition, and the formation and separation of solutions are determined from experimental measurements made at constant temperature In this chapter we apply thermodynamics to the evaluation of most of the heat effects that accompany physical and chemical operations However, the heat effects of mixing processes, which depend on the thermodynamic properties of mixtures, are treated in Chap 12.

Heat transfer to a system in which there are no phase transitions, no chemical reactions, and no changes in composition causes the temperature of the system to change Our purpose here is to develop relations between the quantity of heat transferred and the resulting temperature change When the system is a homogeneous substance of constant composition, the phase rule indicates that fixing the values of two intensive properties establishes its state The molar or specific internal energy of a substance may therefore be expressed as a function of two

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(The SecurityProfile array has items that range from 0 to MaxLibrarySecurity, but the loop at the end of this code starts from element 1. Because the Activity table starts its counting at 1, I decided to just skip element 0.) The InitializeSystem method is called from the MyApplication_Startup event in the ApplicationEvents.vb file, just before establishing a connection to the database. Let s add that code now.

other state variables These may be arbitrarily selected as temperature and molar or specific volume: U = U ( T ,V )

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Whence, As a result of Eq (216) this becomes:

The final term may be set equal to zero in two circumstances: For any constant-volume process, regardless of substance Whenever the internal energy is independent of volume, regardless of the process This is exactly true for ideal gases and incompressible fluids and approximately true for lowpressure gases In either case, and

' ----- Perform general initialization. InitializeSystem( )

For a mechanically reversible constant-volume process, Q = A U , and Eq (219) may be rewritten:

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Similarly, the molar or specific enthalpy may be expressed as a function of temperature and pressure: H = H(T, P) Whence, As a result of Eq (220) this becomes:

Each time an administrator tries to use the system, and each time the administrator logs off and returns the program to patron mode, all of the security-related global variables must be reset. This is done in the ReprocessSecuritySet method, added to the General module.

Again, two circumstances allow the final term to be set equal to zero: For any constant-pressure process, regardless of the substance Whenever the enthalpy of the substance is independent of pressure, regardless of the process This is exactly true for ideal gases and approximately true for low-pressure gases

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