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Chemistry 23 Wednesday, October 25, 2006

Chemistry 23 Wednesday, October 25, 2006 - Wednesday...

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Wednesday, October 25, 2006 Chemistry EQUILIBRIUM – PART II Why do you have to “light” a combustion reaction? What dictates reaction rates? How are rates & equilibrium related to energetics? Text: Sections 9.8-9.10 ACTIVATION ENERGY (E a ) 1. Our model reaction CH 3 I + OH 1- ↔ CH 3 OH + I 1- 2. Reaction energy diagram (Figure 9.5) Transition state Pot E E a (f) E a (r) ∆ E Products Reaction Coord 3. Activation E a. Needed to get to top (to transition state) o initially add E to get reaction started REACTION RATES 1. Rate: How many events per unity time Ex. 65 mph 5 x 10 -3 moles of compound reacting per sec. 2. Depends on frequency of collisions a. Related to concentration of reactants b. Related to temperature For our one-step reaction Rate f α [CH 3 I] [OH -1 ] 3. Depends on fraction of “successful” collisions a. Related to orientation
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Wednesday, October 25, 2006 b. Related to temperature (collision E) Rate f = k f [CH I] [OH -1 ] Rate constant This is called rate law Cannot determine from balanced equation Note: k = A exp [-E a /RT] 4.
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