10-21-08[lecture14]ll

10-21-08[lecture14]ll - Chem 116 Lecture 14 Notes(LL...

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Chem 116 Lecture 14 Notes 10/21/08 (LL) iClicker Question Answer C Rate = k[CO 2 ] 2 [O 2 ] Key points about kinetics so far Collision Theory= For chemicals to react they must collide. The collisions also have to occur at correct orientation Depends on: Temperature, activation energy, and fraction of collisions that occur at the right orientations of the molecules Reaction Pathway Transition state (Activated complex)- Intermediate state between reactants and products where the energy is the highest Relating energy profiles, activation energies, and speeds of reactions Activation energy determines the speed of reactions - if the activation energy is higher, the speed is slower Fastest reaction- Lowest E a Slowest reaction- Highest E a Ranking the reactions in order from fastest to slowest, if the reactions occur at the same temperature and have the same value for A (related to the fraction of collisions at the right orientation) 1, E a = 15 kJ/mol (fastest) 3, E a = 20 kJ/mol 2 E a = 24 kJ/mol (slowest)
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This note was uploaded on 12/02/2011 for the course PHYSICS 235 taught by Professor Staff during the Fall '08 term at Rutgers.

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10-21-08[lecture14]ll - Chem 116 Lecture 14 Notes(LL...

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