Lesson 12.4 Collision Theory Suggested Reading Zumdahl Chapter 12 Sections 12.7 & 12.8 Essential Question What is collision theory? Learning Objectives: Describe the kinetic theory in terms of the movement of particles whose average energy is proportional to temperature in Kelvins. Describe the collision theory. Define the term activation energy. Describe transition state theory. Predict and explain, using collision theory, the qualitative effects of particle size, temperature, concentration and pressure on the rate of reaction. Sketch and explain qualitatively the Maxwell-Boltzmann energy distribution curve for a fixed amount of gas at different temperatures and its consequences for changes in reaction rate. Describe the effect of a catalyst on a chemical reaction. Sketch and explain Maxwell-Boltzmann curves for reactions with and without catalysts. Introduction You now know that the rate of a reaction depends on temperature. This shows up in the rate law through the rate constant, which varies with temperature. In most cases, the rate increases with temperature. How do you explain the dependence of reaction rate on temperature? To understand it, we need to look at a simple theoretical explanation of reaction rates. This is collision theory. There are many learning objectives in this area, lets take them one at a time. Describe the kinetic theory in terms of the movement of particles whose average energy is proportional to temperature in Kelvins. This objective was previously covered during our study of gases, but the IB also includes in as part of collision theory (IB 6.2.1), because it is relevant to both KMT and collision theory. Thornely's video on the topic should provide sufficent review. Watch the following YouTube Video: https://www.youtube.com/watch?v=WuElPE0Heaw Describe the collision theory. Define activation energy. Why the rate constant depends on temperature can be explained by collision theory. For a reaction to take place between two reactant particles, three conditions are necessary: 1. 2. 3. The particles (atoms, ions, or molecules) must come into physical contact (collide) with one another. They must collide in the correct orientation. The reactant molecules myst collide with sufficient kinetic energy to bring about the reaction. These three conditions are collectively know as collision theory. The minimum energy required for two molecules to react is called the activation energy, Ea. Activation energy depends on the particular reaction. Watch the following YouTube Video: https://www.youtube.com/watch?v=mBTSwJnZ6Sk Predict and explain, using collision theory, the qualitative effects of particle size, temperature, concentration and pressure on the rate of reaction. Describe the effect of a catalyst on a chemical reaction. Watch the following YouTube Video: https://www.youtube.com/watch?v=KQW1N-ERGBs Factors that increase the rate of a reaction: Concentration: Increasing concentration increases the frequency of the collisions, which results in a greater number of successful collisions and consequently, a faster rate. Pressure: In order to increase pressure we must reduce volume. This increases the frequency of the collisions and results in a faster rate as stated above. Temperature: The rate of a reaction depends on temperature because collision frequency depends on temperature. As the temperature rises, the molecules move faster and collide more frequently. Collision frequency is proportional to the root-mean-square (rms) speed, which is in turn proportional to temperature. Particle size: Reducing the particle size increases the rate of reaction, because it greatly increases the surface area. The greater surface area allows form more collisions, because there are more places in which a collision can occur. Catalysis: A catalyst is a substance that increases the rate of reaction without itself being consumed, or chemically changed during the reaction. Catalysts work by bringing the reactant particles into close contact with one another. The catalyst is said to provide an alternative pathway with a lower activation energy. More particles will possess this lower activation energy, and so the rate increases. Sketch and explain qualitatively the Maxwell-Boltzmann energy distribution curve for a fixed amount of gas at different temperatures and its consequences for changes in reaction rate. Watch the following YouTube Video: https://www.youtube.com/watch?v=YnHIfqUZi48 A Maxwell-Boltmann distribution shows the kinetic energy amongst particles for a fixed amount of gas. It has a characteristic shape and several features you should be aware of although you will not be tested on them directly. Features: 1. 2. 3. The area under the curve is directly related to number of particles, and so for a fixed amount of gas this area must remain constant. For a given T, most particles possess a KE close to the average. At the average value the area under the graph is equal on both sides, because the same number of particles will have a lower kinetic energy as have a higher kinetic energy. Why do we care? These curves can help us to understand activation energy as well as the effect of temperature on the rate of reaction. More generally, we can see that at higher temperatures, more molecules will posses the minimum threshold energy (activation energy) needed in order for a reaction to occur. Describe transition state theory. Collision theory explains some important features of a reaction, but it is limited in that it does not explain the role of activation energy. Transition state theory attempts to describe the role of activation energy by explaining the reaction resulting from the collision of two molecules in terms of an activated complex. An activated complex (transition state) is an unstable grouping of atoms that can break up to form products. Consider the reaction between hydroxide and bromomethane above. When the molecules come together with the proper orientation, a C-O bond begins to form. At the same time, the kinetic energy of the collision is absorbed by the activated complex as a vibrational motion of the atoms. This energy becomes concentrated in the bonds denoted by the dashed lines and can flow between them. If, at some moment, sufficient energy becomes concentrated in one of the bonds of the activated complex, that bond breaks and falls apart. Depending on whether the C-O or C-Br bond breaks, the activated complex either reverts back to reactants or yields the products. Potential-Energy Diagrams for Reactions A potential energy diagram can help you understand what is going on. The curve shows the change in potential energy that occurs during the progress of reaction. The potential energy curves starts at the left with the energy of the reactants, OH- and CH3Br. Moving along the curve toward the right, the potential energy increases to a maximum corresponding to the activated complex. Farther to the right the energy decreases to that of the products. Only if the reactant molecules have sufficient kinetic energy is it possible for the reaction to occur. This kinetic energy must be equal to or greater than the difference in potential energy between the reactants and the activated complex. The energy difference is the activation energy for the forward reaction. The difference in energy between the reactants and products equals the heat of reaction, ∆H. More generally, If the exothermic reaction above left was reversed, it would become an endothermic reaction. This is why we change the sign for enthalpy when we use Hess's law. Also, the activation energy would increase. It would equal ∆H + Ea. Similarly, the endothermic reaction on the right could be reversed. The reaction would then become exothermic and the activation energy would equal Ea - ∆H. Sketch and explain Maxwell-Boltzmann curves for reactions with and without catalysts. Watch the following YouTube Video: https://www.youtube.com/watch?v=RUNhM4AtMZ0 The distribution shows that the catalyzed reaction has a lower activation energy. More particles will now have the minimum energy required to react. The potential energy diagram also shows that the activation energy is lower for the catalyzed reaction. Not, however, that the change in energy for the reaction, ∆H (denoted by ∆E in the diagram), does not change for the catalyzed reaction. HOMEWORK: Make sure that you have all diagrams and drawing for these notes!!