activationenergy

activationenergy -...

Info iconThis preview shows pages 1–2. Sign up to view the full content.

View Full Document Right Arrow Icon
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
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Image of page 2
This is the end of the preview. Sign up to access the rest of the document.

Page1 / 2

activationenergy -...

This preview shows document pages 1 - 2. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online