LECTURE12

# LECTURE12 - Last Time aA + bB cC + dD [C] c [A] 1mol/L d PC...

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1 aA + bB cC + dD Last Time K c = [A] a [B] b [C] c [D] d 1mol/L 1mol/L 1mol/L 1mol/L K P = K c ( RT ) Δ n gas K p = P A a P B b P C c P D d 1bar 1bar 1bar 1bar Q c = [A] t a [B] t b [C] t c [D] t d At equilibrium Q c = K c Le Châtelier’s Principle : When a system at equilibrium is subjected to a change in temperature, pressure, or concentration of a reacting species, the system responds to reestablish equilibrium by partially offsetting the change. Pressure / Volume Changes • Adding a gaseous reactant or product changes P gas or [gas] disturbs equilibrium • Adding an inert gas changes the total pressure. – Partial pressures of reacting species are unchanged. • Changing the volume of the system changes partial pressures of all components disturbs equilibrium. Q c = [SO 2 ] 2 t [O 2 ] t [SO 3 ] 2 t V n SO 3 2 V n SO 2 V n O 2 = = V n SO 3 2 2 n SO 2 n O 2 e.g. At equilibrium, Q=K. Then increase V by factor of 10 ? 2 2 SO 2 (g) + O 2 (g) 2 SO 3 (g)

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2 Changing Temperature Raising the temperature of an equilibrium mixture shifts the equilibrium condition in the direction of the endothermic reaction . Lowering the temperature causes a shift in the direction of the exothermic reaction.
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## This note was uploaded on 07/09/2011 for the course CHE 2B 2B taught by Professor Tobyallen during the Spring '11 term at UC Davis.

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LECTURE12 - Last Time aA + bB cC + dD [C] c [A] 1mol/L d PC...

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