CHEM 134 Lecture Notes - Lecture 9: Svante Arrhenius, Activation Energy, Viscosity
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5 Feb 2018
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Increasing the temperature of a system increases the average kinetic energy of its constituent particles. As the average kinetic energy increases, the particles move faster, so they collide more frequently per unit time and possess greater energy when they collide, causing increases in the rate of the reaction. Rate of all reactions increases with increasing temperature and decreases with decreasing temperature. (2) the activation energy (ea ), and. If the arrhenius equation is written for two temperatures, t2 and t1 with t2 >t1 . Consider the rate of a reaction for which ea=50 kj/mol, at 20oc (293 k) and at. For reactions that have an ea 50 kj/mol, the rate approximately doubles for a 100c rise in temperature, near room temperature. The rate-law expression is known to be r=k[icl][h2 ]. The nature of the solvent can affect the reaction rates of solute particles. Solvent viscosity is also important in determining reaction rates.
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