Lecture Notes Week 02

Lecture Notes Week 02 - WEEK 2 CHEMICAL EQUILIBRIUM (Refer...

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WEEK 2 CHEMICAL EQUILIBRIUM (Refer to Chapter 15) Most chemical reactions NEVER go to completion! Usually “chemical equilibrium” is established, i.e., Rate of FORWARD reaction = Rate of REVERSE reaction This creates a dynamic system where there is constant movement in the forward and reverse direction but there is no overall change in the amount of reactants or products, i.e., A + B C + D DYNAMIC system Examples of Simple Equilibria: 1. CaCO 3 (s) CaO(s) + CO 2 (g) (enclosed sealed vessel) 2. H 2 O(l) H 2 O(g) (sealed bottle) 3. Ag + (aq) + Cl (aq) AgCl(s) In the case of: N 2 O 4 (g) 2NO 2 (g) Rate of DISSOCIATION = Rate of ASSOCIATION a DYNAMIC Equilibrium What is the NET effect? Over a wide range of conditions we find: - the ratio of [NO 2 ] 2 /[ N 2 O 4 ] = a constant at a given T OR - the ratio of {P(NO 2 )} 2 /P(N 2 O 4 ) = a constant at a given T The constant is called the Equilibrium Constant, K General Form for Equilibrium Constant For an equilibrium of the form: aA(aq or g) + bB(aq or g) cC(aq or g) + dD(aq or g) K C = K P = this is a specific value at a given temperature. This is known as the “
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This note was uploaded on 04/17/2011 for the course CHEM 1040 taught by Professor Prokiacpak during the Spring '08 term at University of Guelph.

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Lecture Notes Week 02 - WEEK 2 CHEMICAL EQUILIBRIUM (Refer...

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