IMG_0004_NEW_0032

IMG_0004_NEW_0032 - greater then Activation Energy(8" $dt r,ror"orr spccd(Kirtic EEB Higher T higher average molecule speed more reactive

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i I I I I I i I /7 TODAY'S LECTIJRE: ..REACTION KINETIGS" . Collision Model for Kinetics Reaction Profiles Transition States Catalysis Gollision Model for Kinetics Activation Energy NO + NrO -+ NO, +ry \ ,ffi In this reaction N-O bond must be broken N-O bond dissociation energy:201 kJ/mol Q: Where does this energy come from in order that the reaction can occur? A: Energy comes from the kinetic energy of the colliding molecules Average kinetic energy oc Temperature Minimum energy required: Activation Energy 4h -s Molecular Collisions and Reactions Collision Energy . Need collisions with enough kinetic energy for reaction o o s z Distribution of molecular speeds = Distribution ofkinetic energies Reaction only ifkinetic energy is
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Unformatted text preview: greater then Activation Energy (8") $dt r.,ror"orr. spccd (Kirtic EEB/) -{[[} . Higher T: higher average molecule speed + more reactive collisions + higher rate + large ft Orientation . Need correct orientation to form bonds e.g.2BrNO -+ Br2 + 2NO <(l{F -+ e (I)o <nq> For A Reaction To Occur: O The collision energy must be greater than the activation energy g The collision must have the correct orientation of the molecules k(r): Ae-E'lRr A :Frequency Factor T(K) : Collisions per second x fraction with correct orientation 4": n"ivatt"t.t"tgy (breaking and making bonds) li lt rl ,/ flrl .,t I ,-',...
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This note was uploaded on 12/27/2011 for the course CHEM 122 taught by Professor Williams during the Fall '10 term at Simon Fraser.

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