Chapter 17-Equilibrium

Chapter 17-Equilibrium - Review of Equilibria Chapter 17...

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Review of Equilibria – Chapter 17 What does it mean when a system is in equilibrium? If a system at equilibrium is perturbed, what happens to the system? At equilibrium, the ratio of the product concentration(s) to the reactant concentration(s), each raised to the power of their stoichiometric coefficients, is equal to a constant, the equilibrium constant, K. aA + bB cC + dD K = c d a b [C] [D] [A] [B] and for 2aA + 2bB 2cC + 2dD K’ = K 2 cC + dD aA + bB K’ = 1/K = K -1 1. The value of K a. is unique for each reaction. b. is determined experimentally based on the concentration of all players at equilibrium. c. is temperature dependent. d. includes all constant terms; therefore in heterogeneous equilibria, solids and liquids won’t appear in the expression. e. gives insight to the extent of reaction. f. can be used to determine equilibrium amounts. 2. Since the ratio of the product and reactant concentrations is constant, if the one concentration changes then the concentration of the other(s) must change. 3. Equilibrium constants specify the type of equilibrium involved: K c : the equilibrium constant in terms of concentration K p : the equilibrium constant in terms of pressure and K p = K c (RT) n K a : the equilibrium constant for weak acid equilibria K b : the equilibrium constant for weak base equilibria
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This note was uploaded on 04/01/2008 for the course CHEM 1131 taught by Professor Redin,kend during the Summer '08 term at Colorado.

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Chapter 17-Equilibrium - Review of Equilibria Chapter 17...

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