Paper Summary:

This paper studies the theory that chemical reactions are the result of the collision between molecules. Also known as the collision model, the author explains how these collisions, when strong enough and with ambient environments, can cause kinetic energy. The paper also introduces the Arrhenius equation and explains how this equation measures the activation energy of a particular reaction and quantifies the collision model in a way that can be useful for scientists conducting experiments. Like any other equation, the paper describes the different experimental parameters that will have an impact on the product of the Arrhenius equation. The paper also demonstrates how the Arrhenius equation can be applied to other disciplines.

From the Paper:

"Not every collision between molecules will create new products. In fact, the vast majority of collisions do not because they are not strong enough to break the existing bonds, which are often quite strong between molecules. For the collision to be successful, the molecules have to be oriented in such a way that the activation energy is sufficient to generate a reaction in the substance in question. Temperature, the presence of catalysts, the concentration of the substance, and other factors affect activation energy. Also, the molecules within molecular bonds are also held together with different degrees of strength which affect the potential and kinetic energy released from collisions."

Sample of Sources Used:

• Akeson, Wayne H. "Application of the Arrhenius Equation to rat tail tendon collagen." Nature. 199, 185 - 186. 13 July 1963. 1 Oct 2008.http://www.nature.com/nature/journal/v199/n4889/abs/199185a0.html
• "The Arrhenius Equation." IUPAC Compendium of Chemical Terminology. 2nd Edition. 1997. 2 Oct 2008. http://www.iupac.org/goldbook/A00446.pdf
• "The Arrhenius Equation." Shordor Education Foundation. Department of Chemistry. University of North Carolina, Chapel Hill. Sept. 30, 2008. 1 Oct 2008. http://www.shodor.net/unchem/advanced/kin/arrhenius.htm
• Clark, Jim. "Rate constants." 2008. 1 Oct 2008. http://www.chemguide.co.uk/physical/basicrates/arrhenius.html
• "Chemical Kinetics: Chapter 12." AP Chemistry Notes. 1 Oct 2008.www.mpsomaha.org/mnhs/apchem/assignments/Notes/Html%20Notes/notes12.htm

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