CHEM 1AA3 Study Guide - Midterm Guide: Kinetic Theory Of Gases, Collision Theory, Kinetic Energy
14 Jul 2018
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Based on the kinetic molecular theory, the central idea of the collision model is that molecules must collide to react. The greater the number of collisions per second, the greater the reaction rate. As discussed previously, concentration, surface area, and temperature will all increase the rate of a reaction. If a collision is necessary for a reaction to occur, then it makes sense that the rate of the reaction will increase if there are more collisions per unit time. More reactant particles in a given volume will increase the number of collisions between the particles per second. Not every collision between reactants results in a reaction. In order for a collision between reactants to result in a reaction, the collision must be effective. An effective collision must satisfy the following 2 criteria: correct orientation of reactants, sufficient collision energy. The relative orientations of the molecules during their collisions determine whether the atoms are suitably positioned to form new bonds.
