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enthalpies of all elements are arbitrarily set equal to zero as the basis of calculation, then the standard-state enthalpy of each compound is its heat of formation In this event, H: = A Hyi and Eq (414) becomes:

where the summation is over all products and reactants This formalizes the procedure described in the preceding section for calculation of standard heats of other reactions from standard heats of formation Applied to the reaction,

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Eq (415) is written:

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As long as the argument signatures or return values differ, you can add as many overloads of an operator as you want. You don t need to use the Overloads keyword either.

With data from Table C4 for 29815 K, this becomes:

in agreement with the result of Ex 45 For standard reactions, products and reactants are always at the standard-state pressure of 1 bar Standard-state enthalpies are therefore functions of temperature only, and by Eq (221),

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where subscript i identifies a particular product or reactant Multiplying by vi and summing over all products and reactants gives:

Since vi is a constant, it may be placed inside the differential:

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The term vi H: is the standard heat of reaction, defined by Eq (414) as A H O The standard heat-capacity change of reaction is defined similarly:

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As a result of these definitions, the preceding equation becomes:

This is the fundamental equation relating heats of reaction to temperature Integration gives:

|

FIGURE 14-4

where A H O and A H i are heats of reaction at temperature T and at reference temperature To respectively If the temperature dependence of the heat capacity of each product and reactant

is given by Eq (44), then the integral is given by the analog of Eq (47) ( t r T / To):

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