Chem 211 1st Edition Lecture 13 Outline of Last Lecture I. Determine the kinetic parameters of a reactionII. Integrated Rate LawsIII. Reaction Half-lifeIV. Half-life EquationsOutline of Current Lecture I. Collision Theory and ConcentrationII. Temperature and the Rate ConstantIII. Activation EnergyIV. Temperature and Collision EnergyV. Calculating Activation EnergyVI. Molecular Structure and Reaction RateVII. Transition State TheoryCurrent LectureI. Collision Theory and ConcentrationA. The basic principle of collision theory is that particles must collide in order to react.B. An increase in the concentration of a reactant leads to a larger number of collisions, hence increasing reaction rate.C. The number of collisions depends on the product of the numbers of reactant particles, not their sum.D. Concentrations are multiplied in the rate law, not added.II. Temperature and the Rate ConstantA. Temperature has a dramatic effect on reaction rate.B. For many reactions, an increase of 10°C will double or triple the rate.C. Experimental data shows that k increases exponentially as Tincreases. This is expressed in the Arrhenius equation:III. Activation EnergyA. In order to be effective,collisions betweenparticles must exceed a certain energy threshold.B. When particles collide effectively, they reach an activated state. The energy difference between the reactants and the activated state is the activation energy (Ea) for the reaction.These notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.C. The lower the activation energy, the faster the reaction.IV. Temperature and Collision EnergyA. An increase in temperature causes an increase in the kinetic energy ofthe particles. This leads to more frequent collisions and reaction rateincreases.B. At a higher temperature, the fraction of collisions with sufficient energy equalto or greater than Ea increases. Reaction rate therefore increases.V. Calculating Activation EnergyA. Ea can be calculated from the Arrhenius equationB. If data is available at two different temperaturesVI. Molecular Structure and Reaction RateA. For a collision between particles to be effective, it must have bothsufficient energy and the appropriate relative orientationbetween the reacting particles.B. The term A in the Arrhenius equation is the frequency factor forthe reaction.a) p = orientation probability factorb) Z = collision frequencyC. The term p is specific for each reaction and is related to the structuralcomplexity of the reactants.VII. Transition State TheoryA. An effective collision between particles leads to the formation of a transition state or activated complex.B. The transition state is an unstable species that contains partial bonds. It is a transitional species partway between reactants and products.C. Transition states cannot be isolated.D. The transition state exists at the point of maximum potential energy. E. The energy required to form the transition state is the activation