110302 - 1 CHM3400 - Lecture 23 Mar 2 Reaction rate...

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Unformatted text preview: 1 CHM3400 - Lecture 23 Mar 2 Reaction rate theories, reactions in solution (Chapter 9 336-342, 346-349) Collision theory (hard sphere, temperature) Transition state theory Reactions in solution 2 Potential energy In these plots, where is activation energy Ea? What where is G of reaction? = RT E A k a exp Arrhenius equation: 3 Collision rate for A+A For the bimolecular reaction: A + A products c d V N Z AA 2 2 2 2 = Collisions m-3 s-1 : See lecture 090828 No. of molecules Volume (set to 1 m 3 ) Collision area Mean velocity Why , why 2 1/2 ? Mean velocity: A B m T k c = 8 A B AA m T k d N Z 2 2 2 = This becomes: Mass per molecule (kg) 4 A + B products For the bimolecular reaction: T k d N N Z B AB B A AB 8 2 = This time no term B A B A m m m m + = Reduced mass = Collision rate for A+B 5 Reaction rates If every collision gave rise to a reaction product, the reaction rate would be: 10 31 dm-3 s-1 for 1 atm at 298 K This means that the reaction would be done in nanoseconds (10-9 s) = RT E Z rate a AB exp Actual rate: Activation energy = RT E T k d N N a B AB B A exp 8 2...
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This note was uploaded on 05/29/2011 for the course CHM 3400 taught by Professor Seabra during the Spring '08 term at University of Florida.

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110302 - 1 CHM3400 - Lecture 23 Mar 2 Reaction rate...

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