Lecture Notes Nov 20 Equilibrium LeChatelier CHEM135 Dr. Johnson

Lecture Notes Nov 20 Equilibrium LeChatelier CHEM135 Dr. Johnson

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Lecture Notes Monday, November 20, 2007 CHEM135 Dr. Johnson EQUILIBRIUM Writing Equilibrium Constants Do not include solids and liquids when writing the equilibrium constant expression When a chemical reaction is reversed then the K for the reversed reaction is the reciprocal of the K for the unreversed reaction 3 H 2 (g) + N 2 (g)  2 NH 3 (g) K c 2 NH 3 (g)  3 H 2 (g) + N 2 (g) K c ’’ = 1/ K c K’s for multistep reactions: When equilibrium reactions add up to an overall total reaction, the K’s are multiplied. This is quite applicable to di- and tri- protic acids. PO 4 3+ (aq) + H + (aq)  HPO 4 2- (aq) K 1 HPO 4 (aq) + H + (aq)  H 2 PO 4 - (aq) K 2 Total equilibrium reaction: PO 4 3- (aq) + 2 H + (aq)  H 2 PO 4 - K 3 = K 1 . K 2 Magnitude of K A lage K value indicates that the equilibrium favors the products. A small K value indicates that the equilibrium favors the reactants. Which ion, CN - or Br - , will be more likely to precipitate with Ag + The one which has the larger K value
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The following data were collected for a system at equilibrium at 140 o C. Calculate the equilibrium constant at this temperature for the reaction, 3 H 2 (g) + N 2 (g)  2 NH 3 (g) at this temperature. [H 2 ]=0.10 mol L -1 , [N 2 ]=1.1 mol L -1
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Lecture Notes Nov 20 Equilibrium LeChatelier CHEM135 Dr. Johnson

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