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Unformatted text preview: itch places, and thus the terms in the numerator move to the denominator and vice versa. Consequently, the equilibrium constant of the reverse reaction becomes 1/KP. For example, from Table A28,
% mol H 0.00 0.16 14.63 76.80 97.70 99.63 KP KP 0.1147 8.718 10 11 10
11 for for H2 1 2 O2 H 2O H2
1 2 O2 at 1000 K at 1000 K H 2O FIGURE 169 The larger the KP, the more complete the reaction. Initial composition Equilibrium composition at 3000 K, 1 atm 0.921 mol H2 0.158 mol H KP = 0.0251 (a) 1 mol H2 (b) 1 mol H2 1 mol N2 0.380 mol H2 1.240 mol H 1 mol N2 KP = 0.0251 FIGURE 1610 The presence of inert gases does not affect the equilibrium constant, but it does affect the equilibrium composition. 3. The larger the KP, the more complete the reaction. This is also apparent from Fig. 169 and Eq. 1613. If the equilibrium composition consists largely of product gases, the partial pressures of the products (PC and PD) are considerably larger than the partial pressures of the reactants (PA and PB), which results in a large value of KP. In the limiting case of a complete reaction (no leftover reactants in the equilibrium mixture), KP approaches infinity. Conversely, very small values of KP indicate that a reaction does not pro...
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This note was uploaded on 06/15/2009 for the course MAE 3311 taught by Professor Hajisheik during the Summer '08 term at UT Arlington.
- Summer '08