Editing Activated complex (section)

=== Transition state theory ===
Transition state theory explains the dynamics of reactions. The theory is based on the idea that there is an equilibrium between the activated complex and reactant molecules. The theory incorporates concepts from [[collision theory]], which states that for a reaction to occur, reacting molecules must collide with a minimum energy and correct orientation. The reactants are first transformed into the activated complex before breaking into the products.<ref name=":0" /> From the properties of the activated complex and reactants, the reaction rate constant is

<math display="block">k = K \frac{k_\text{B} T}{h}</math>

where ''K'' is the [[equilibrium constant]], <math display="inline">k_\text{B}</math> is the [[Boltzmann constant]], T is the [[thermodynamic temperature]], and ''h'' is the [[Planck constant]].<ref name=":2">{{Cite journal |last=Eyring |first=Henry. |date=1935 |title=The Activated Complex and the Absolute Rate of Chemical Reactions. |url=https://pubs.acs.org/doi/abs/10.1021/cr60056a006 |journal=Chemical Reviews |language=en |volume=17 |issue=1 |pages=65–77 |doi=10.1021/cr60056a006 |issn=0009-2665|url-access=subscription }}</ref> Transition state theory is based on [[classical mechanics]], as it assumes that as the reaction proceeds, the molecules will never return to the transition state.<ref>{{Cite journal |last=Pechukas |first=P |date=1981 |title=Transition State Theory |journal=[[Annual Review of Physical Chemistry]] |language=en |volume=32 |issue=1 |pages=159–177 |doi=10.1146/annurev.pc.32.100181.001111 |issn=0066-426X}}</ref>