Chem 113 1st Edition Lecture 16Outline of Last Lecture I. Chemical EquilibriumII. The synthesis of AmmoniaIII. The Equilibrium Constant (K)IV. K and the extent of reactionOutline of Current Lecture I. The Equilibrium ConstantII. Equilibrium with gas phase reactionsIII. K for Heterogeneous EquilibriumCurrent LectureI. The Equilibrium Constanta. For the general reaction aA+bBcC+dDi. The equilibrium constant (K)= [C]c[D]d/[A]a[B]bb. Equilibrium constants have no unitsi. The concentrations/pressures used in the eq. expressions arte ratios of the standard concentration/ pressure values (1M) or 1 atmII. Equilibrium with gas phase reactionsa. Equilibrium constant in term of concentrationi.Kc=[C ]c[D ]d[ A ]a[ B ]bb. Equilibrium constant in terms of pressurei.KP=PCcPDdPAaPBbc. To convert between the two, manipulate the ideal gas law (PV=nRT)These notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.i. P/RT=n/V=concentrationIII. K for Heterogeneous Equilibriuma. A heterogeneous equilibrium involves reactants and/or products in different phasesb. A pure solid or liquid always has the same “concentration” (the same moles per liter of solid or liquid)c. The expressions for K include only species whose concentrations change as the reaction approaches equilibriumi. Pure solids and liquids are omitted from the expression for
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