activationenergy -...

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activation energy  (Ea) - minimum amount of energy needed for reaction to occur kinetic energy of colliding molecules used to break bonds activated complex (transition state) - atomic arrangement at the point of highest energy lower activation energy >> faster reaction rate f = e-Ea/RT o f = fraction of molecules w/ energy equal to or greater than Ea o R = gas constant o T = absolute temperature Arrhenius equation - takes into account 3 factors (activation energy, # of collisions, fraction of collisions w/ correct orientation) o k = Ae-Ea/RT o A = frequency factor constant ln (k1/k2) = Ea/R (1/T2 - 1/T1) o must knowk2 from T2 (another temperature) to calculate k1 and T1) reaction mechanisms  - process by which reaction occurs can describe the order in which bonds are broken/formed elementary steps (elementary processes) - single event/step o rate law based on molecularity for each elementary step molecularity - describes # of reactant molecules in an elementary step
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activationenergy -...

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