chapter_15 - Chemistry, The Central Science, 10th edition...

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Equilibrium Chapter 15 Chemical Equilibrium Chemistry, The Central Science , 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Andrzej A. Jarzecki Fall 2007 Brooklyn College
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Equilibrium The Concept of Equilibrium Chemical equilibrium occurs when a reaction and its reverse reaction proceed at the same rate.
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Equilibrium 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 at the same rate.
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Equilibrium A System at Equilibrium Once equilibrium is achieved, the amount of each reactant and product remains constant.
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Equilibrium Depicting Equilibrium In a system at equilibrium, both the forward and reverse reactions are being carried out ; as a result, we write its equation with a double arrow N O 2 NO
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Equilibrium The Equilibrium Constant
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Equilibrium The Equilibrium Constant Forward reaction: N 2 O 4 ( g ) → 2 NO 2 ( g ) Rate law: Rate = k f [N 2 O 4 ]
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Equilibrium The Equilibrium Constant Reverse reaction: 2 NO 2 ( g ) → N 2 O 4 ( g ) Rate law: Rate = k r [NO 2 ] 2
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Equilibrium The Equilibrium Constant Therefore, at equilibrium Rate f = Rate r k f [N 2 O 4 ] = k r [NO 2 ] 2 Rewriting this, it becomes k [NO ] =
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Equilibrium The Equilibrium Constant The ratio of the rate constants is a constant at that temperature, and the expression becomes k [NO ] =
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Equilibrium The Equilibrium Constant To generalize this expression, consider the reaction The equilibrium expression for this reaction would be a A + b B c C + d D
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chapter_15 - Chemistry, The Central Science, 10th edition...

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