Lecture20, 2-29-08 temp effects and mechansims

Lecture20, 2-29-08 temp effects and mechansims - Scores,...

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Scores, Mid-Term Exam 2, 2-27-08 0 10 20 30 40 50 60 12 20 28 36 44 52 60 68 76 84 92 100 More Exam Score Number of Scores A 72-100 B 64-68 C 40 - 60 D 32-36 F 0 - 28
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Temperature and Rate • Generally, as temperature increases, so does reaction rate. • This is because k is temperature dependent.
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Temperature and Rate Collision theory • In a chemical reaction, bonds are broken and new bonds are formed. In order for molecules to react, they must collide. • Collisions are either effective or ineffective due to orientation of molecules. • Collisions must have enough energy to overcome the barrier to reaction, the activation energy. • Temperature affects the number of collisions.
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Molecular Collisions Orientation of reactants when they collide influences whether or not reaction occurs
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Activation Energy, E a • Energy barrier (hump) that must be overcome for a chemical reaction to proceed • Activated complex or transition state – arrangement of atoms at the top of the barrier
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The Arrhenius Equation Collision Theory: A bimolecular reaction occurs when two correctly oriented molecules collide with sufficient energy. Activation Energy ( E a ): The potential energy barrier that must be surmounted before reactants can be converted to products.
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Energy Profile Diagram
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• At higher temperatures, more molecules will have adequate energy to react. • This increases
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This note was uploaded on 08/06/2008 for the course CHEM 1B taught by Professor Watts during the Winter '08 term at UCSB.

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Lecture20, 2-29-08 temp effects and mechansims - Scores,...

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