Lecture_34_120111

# Lecture_34_120111 - Lecture 34 Le Chtelier's Principle...

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Lecture 34: Le Châtelier’s Principle Goals: Use Le Chatelier’s principle to describe the changes made in equilibrium when reaction conditions change. Write the solubility product expression for a slightly soluble salt and calculate its K sp . Use the K sp to determine the solubility of a slightly soluble salt. Outline (Timberlake 9.5-9.6): ± Changing Equilibrium Conditions: Le Châtelier’s Principle (9.5) ± Equilibrium in Saturated Solutions (9.6) Problems for Extra Practice: 9.27, 9.29, 9.31, 9.33, 9.35, 9.37, 9.39

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Le Châtelier’s Principle Le Châtelier’s principle states that • any change in equilibrium conditions upsets the equilibrium of the system • a system at equilibrium under stress will shift to relieve the stress • there will be a change in the rate of the forward or reverse reaction to return the system to equilibrium
Effect of Adding Reactant Consider the following reaction at equilibrium. H 2 ( g ) + F 2 ( g ) 2HF( g ) • If more reactant (H 2 or F 2 ) is added, there is an increase in the number of collisions. • The rate of the forward reaction increases and forms more HF product until new equilibrium concentrations equal K c again. • The effect of adding a reactant shifts the equilibrium toward the products.

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Consider the following reaction at equilibrium. H 2 ( g ) + F 2 ( g ) 2HF( g ) • When more HF is added, there is an increase in collisions of HF molecules. • The rate of the reverse reaction increases and forms more H 2 and F 2 reactants. • The effect of adding a product shifts the
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## This note was uploaded on 01/18/2012 for the course CHEM 120A taught by Professor Leahmiller during the Fall '11 term at University of Washington.

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Lecture_34_120111 - Lecture 34 Le Chtelier's Principle...

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