## Abstract

We consider a one-phase system (so that the assumptions of invertibility discussed in the preceding chapter are justified) in which a single chemical reaction is taking place, say, e.g.,
Equation (3.1.1) does not, of course, imply addition in the ordinary algebraic sense of the quantities CO and O

$$\mathrm{CO+\frac{1}{2}O_{2}}\;=\;\mathrm{CO_{2}}$$

(3.1.1)

_{2}. The meaning of equation (3.1.1) is to recall the experimentally observed fact that, when a given number of moles of CO is consumed by the reaction, the same number of moles of CO_{2}is produced, and half as many moles of O_{2}are consumed. Let the components appearing in the reaction be numbered consecutively, say CO is*B*_{1}, O_{2}is*B*_{2}, and CO_{2}is*B*_{3}, and let σ_{ j }be the corresponding stoichiometric coefficients, say σ_{1}= −1, σ_{2}= −1/2, and σ_{3}= 1. We note that the stoichiometric coefficients of the species appearing on the left-hand side (the “reactants”) are assigned negative stoichiometric coefficients. Equation (3.1.1) can now be written as follows:$$\underset{j}\sum\sigma_{j}B_{j}\;=\;0$$

(3.1.2)

## Keywords

Free Enthalpy Extensive Property Homogeneous Reaction Stoichiometric Coefficient Functional Derivative
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## Literature

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