Chem1202PReviewCh15

Chem1202PReviewCh15 - Chemistry 1202 Review/Preview Chapter...

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Chapter Fifteen Review Guide Dr. Saundra McGuire Spring 2007 Director, Center for Academic Success Adj. Prof., Dept. of Chemistry I. The Concept of Equilibrium A reaction at equilibrium indicates that the rates of the forward and reverse reactions are equal. It does NOT indicate that the amounts of reactants and products are equal. For the reaction A B the rates of the forward reaction and reverse reactions are : rate f = k f [A] and rate r = k r [B] When the two rates are equal: k f [A] = k r [B] Dividing both sides of the equation above by k r [A], we obtain k f = [B] = a constant k r [A] II. The Equilibrium Constant A. The Equilibrium Constant, Kc, represents the quantitative relationship between the concentrations of reactants and products in a chemical reaction. The equilibrium constant expression for a general reaction is shown below. aA + bB cC + dD Kc = [C]c [D]d [A]a [B]b Note that the brackets indicate moles/liter concentrations. B. The Equilibrium Constant, Kp The quantitative relationship between the partial pressures (in atmospheres) of the reactants and products in a chemical reaction at equilibrium is described by the form of the equilibrium equation shown below: Kp = (P C ) c (P D ) d (P A ) a (P B ) b Note that P A represents the partial pressure of A. The relationship between Kp and Kc is given by the following relationship: Kp = Kc(RT) n where n is the number of moles of gaseous products minus the number of moles of gaseous reactants. T is in kelvins; R is the gas constant, 0.0821 L-atm/mol-K.
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Chem1202PReviewCh15 - Chemistry 1202 Review/Preview Chapter...

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