Editing Chemical kinetics (section)

== History ==
The pioneering work of chemical kinetics was done by German chemist [[Ludwig Wilhelmy]] in 1850.<ref>L. Wilhelmy, "Ann. Phys. Chem. (Poggendorf)" Vol 81, (1850) 413</ref> He experimentally studied the rate of [[inversion of sucrose]] and he used [[Rate_equation#Integral_method|integrated rate law]] for the determination of the reaction kinetics of this reaction. His work was noticed 34 years later by [[Wilhelm Ostwald]]. In 1864, [[Peter Waage]] and [[Cato Guldberg]] published the [[law of mass action]], which states that the speed of a chemical reaction is proportional to the quantity of the reacting substances.<ref name="GW1">C.M. Guldberg and P. Waage,"Studies Concerning Affinity" ''Forhandlinger i Videnskabs-Selskabet i Christiania'' (1864), 35</ref><ref name="GW2">P. Waage, "Experiments for Determining the Affinity Law" ,''Forhandlinger i Videnskabs-Selskabet i Christiania'', (1864) 92.</ref><ref name="GW3">C.M. Guldberg, "Concerning the Laws of Chemical Affinity", ''Forhandlinger i Videnskabs-Selskabet i Christiania'' (1864) 111</ref>

[[Jacobus Henricus van 't Hoff|Van 't Hoff]] studied chemical dynamics and in 1884 published his famous "Études de dynamique chimique".<ref>{{Cite book|url=https://archive.org/details/studiesinchemica00hoffrich|title=Studies in chemical dynamics|last=Hoff|first=J. H. van't (Jacobus Henricus van't)|last2=Cohen|first2=Ernst|last3=Ewan|first3=Thomas|date=1896-01-01|publisher=Amsterdam : F. Muller; London : Williams & Norgate}}</ref> In 1901 he was awarded the first Nobel Prize in Chemistry "in recognition of the extraordinary services he has rendered by the discovery of the laws of chemical dynamics and osmotic pressure in solutions".<ref>[https://www.nobelprize.org/nobel_prizes/chemistry/laureates/1901/ The Nobel Prize in Chemistry 1901], Nobel Prizes and Laureates, official website.</ref> After van 't Hoff, chemical kinetics dealt with the experimental determination of [[reaction rate]]s from which [[rate law]]s and [[reaction rate constant|rate constants]] are derived. Relatively simple [[rate law]]s exist for [[Rate law#Zero-order reactions|zero order reactions]] (for which reaction rates are independent of concentration), [[Rate equation#First-order reactions|first order reaction]]s, and [[second-order reaction|second order reaction]]s, and can be derived for others. [[Elementary reaction]]s follow the [[law of mass action]], but the rate law of [[stepwise reaction]]s has to be derived by combining the rate laws of the various elementary steps, and can become rather complex. In consecutive reactions, the [[rate-determining step]] often determines the kinetics. In consecutive first order reactions, a [[steady state (chemistry)|steady state]] approximation can simplify the [[rate law]]. The [[activation energy]] for a reaction is experimentally determined through the [[Arrhenius equation]] and the [[Eyring equation]]. The main factors that influence the [[reaction rate]] include: the [[physical state]] of the reactants, the [[concentrations]] of the reactants, the [[temperature]] at which the reaction occurs, and whether or not any [[catalysts]] are present in the reaction.

[[Alexander Nikolaevich Gorban|Gorban]] and Yablonsky have suggested that the history of chemical dynamics can be divided into three eras.<ref>A.N. Gorban, G.S. Yablonsky [https://www.researchgate.net/publication/281411623_Three_Waves_of_Chemical_Dynamics Three Waves of Chemical Dynamics], ''Mathematical Modelling of Natural Phenomena'' 10(5) (2015), p. 1–5.</ref> The first is the van 't Hoff wave searching for the general laws of chemical reactions and relating kinetics to thermodynamics. The second may be called the [[Nikolay Semyonov|Semenov]]-[[Cyril Norman Hinshelwood|Hinshelwood]] wave with emphasis on reaction mechanisms, especially for [[Chain reaction#chemical chain reactions|chain reactions]]. The third is associated with [[Rutherford Aris|Aris]] and the detailed mathematical description of chemical reaction networks.