CHE116_Lecture5_2011

CHE116_Lecture5_2011 - Chemistry Chemistry116 Lecture5...

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hemistry 116 Chemistry 116 Lecture 5 Topics: Chemical Equilibrium Equilibrium Constants Chapter 15.1 15.3
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The Concept of Equilibrium Chemical equilibrium occurs when a reaction and its reverse reaction proceed at the same rate. ey concept is N O ( 2 NO ( Key concept is that this action is 2 4 ( g ) 2 ( g ) reaction is reversible . clear brown
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The Concept of Equilibrium As a system approaches equilibrium, both the forward and reverse reactions are occurring. At equilibrium, the forward and reverse reactions are proceeding ( NO ( at the same rate . N 2 O 4 ( g ) 2 NO 2 ( g )
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epicting Equilibrium Depicting Equilibrium Since, in a system at equilibrium, both the forward and reverse reactions are being carried out, we write its equation with a double arrow . N 2 O 4 ( g ) 2 NO 2 ( g )
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he Equilibrium Constant The Equilibrium Constant N 2 O 4 ( g ) 2 NO 2 ( g ) Forward reaction: N 2 O 4 (g)  2 NO 2 (g) Rate Law: Rate = k f [N 2 O 4 ]
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he Equilibrium Constant The Equilibrium Constant N 2 O 4 ( g ) 2 NO 2 ( g ) Reverse reaction: 2 NO 2 (g)  N 2 O 4 (g) Rate Law: t O Rate = k r [NO 2 ] 2
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The Equilibrium Constant N 2 O 4 ( g ) 2 NO 2 ( g ) Therefore, at equilibrium: ate Rate Rate f = Rate r k [N O ] = k [NO ] 2 f [ 2 4 ] r [ 2 ] Rewriting this, it becomes: k f [NO 2 ] 2 = k r [N 2 O 4 ]
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he Equilibrium Constant The Equilibrium Constant e tio of the rate constants is a constant The ratio of the rate constants is a constant at that temperature, and the expression becomes: K q = k f [NO 2 ] 2 = eq k r [N 2 O 4 ] This is known as the equilibrium constant .
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The Equilibrium Constant Consider the generalized reaction: e equilibrium expression for this reaction aA + b Bc C + dD The equilibrium expression for this reaction (from the law of mass action ) would be: K c = [C] c [D] d ] a ] b [A] [B] The equilibrium constant depends only on the stoichiometry of the reaction, not the mechanism!
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CHE116_Lecture5_2011 - Chemistry Chemistry116 Lecture5...

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