lecture 070904

lecture 070904 - Chemical Kinetics Chapter 13 Reaction...

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1 Chemical Kinetics Chapter 13 Reaction Mechanisms Is there a theoretical basis for the rate laws that we observe? There is a connection to the reaction mechanism (the sequence of simple reactions that make-up the overall reaction at the molecular level) Reaction Mechanisms 2 NO 2 + F 2 2NO 2 F Experimentally determined rate law is: rate = k[NO 2 ][F 2 ] First order in NO 2 and first order in F 2 Look at the elementary steps
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2 Reaction Mechanisms 1 st step: NO 2 + F 2 NO 2 F + F 2 nd step: NO 2 + F NO 2 F Overall: 2 NO 2 + F 2 2 NO 2 F Each elementary step is bimolecular (involves the collision of 2 molecules) F is an intermediate (also a free radical) Reaction Mechanisms The rate law is governed by the rate- determining step (the slowest elementary step) This reaction’s rate-determining step is the 1 st step 1 st step: NO 2 + F 2 NO 2 F + F Because this step has NO 2 and F 2 as reactants, the rate law will be rate =k[NO 2 ][F 2 ] Elementary Steps The rate law can be predicted from the rate- determining elementary step A products rate = k[A] A + A products rate = k[A] 2 A + A + B products rate = k[A] 2 [B] Termolecular (3 species) steps are rare
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lecture 070904 - Chemical Kinetics Chapter 13 Reaction...

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