Once the equilibrium constant is available it can be

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Unformatted text preview: n of reacting ideal-gas mixtures. This is accomplished by expressing the partial pressures of the components in terms of their mole fractions: Pi yi P Ni P N total (1) In terms of partial pressures KP = PCC P D D P AA PB B n n n n where P is the total pressure and Ntotal is the total number of moles present in the reaction chamber, including any inert gases. Replacing the partial pressures in Eq. 1613 by the above relation and rearranging, we obtain (Fig. 167) KP N nCN nD P n C D a b N nAN nB N total A B (1615) (2) In terms of G*(T ) K = e G*(T )/RuT P (3) In terms of the equilibrium composition KP = N CC N D D n NA A n NB B n n ( ( P Ntotal n where n nC nD nA nB Equation 1615 is written for a reaction involving two reactants and two products, but it can be extended to reactions involving any number of reactants and products. FIGURE 167 Three equivalent KP relations for reacting ideal-gas mixtures. 798 | Thermodynamics EXAMPLE 161 Equilibrium Constant of a Dissociation Process Using Eq. 1614 and the Gibb...
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