chapter 14 notes - A. General Equilibrium Overview B....

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A. General Equilibrium Overview B. Reaction Quotient C. Le Chatelier’s Principle A. General Equilibrium Overview In equilibrium, the forward and reverse reaction proceeds at equal rates, and the concentration of reactants and products remain constant. Equilibrium reactions are denoted by double arrows and have equilibrium constant and expression associated with it. The Law of Mass and Action provides the equilibrium expression. If a reaction is a A + b B --> c C + d D , then the law of mass action states the equilibrium expression is products over reactants or, [ C] c [D] d ---------- = K eq [A] a [B] b 1. [A], [B], [C], [D], are molar concentrations OR partial pressures at equilibrium 2. Products are in the numerator, reactants in the denominator 3. Coefficients in the balanced equation become exponents in the expression 4. Solids and pure liquids are ignored because their concentrations don’t change. 5. No units 6. Keq= Ka (for acids), Kb(for bases) Kp (partial pressures), Ksp (solubility product) 7. For all equilibrium expressions, the constant Keq, is different at different
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This note was uploaded on 04/05/2008 for the course CHEM 161, 101 taught by Professor Hansell during the Spring '08 term at Rutgers.

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chapter 14 notes - A. General Equilibrium Overview B....

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