1. The Collision Theory and Activation Energy Explaining how and why factors affect reaction rates

2. The Maxwell-Boltzmann apparatus Maxwell and Boltzmann performed an experiment to determine the kinetic energy distribution of atoms Because all atoms of an element have roughly the same mass, the kinetic energy of identical atoms is determined by velocity (KE= ½mv 2 )

3. The Maxwell-Boltzmann apparatus Maxwell and Boltzmann performed an experiment to determine the kinetic energy distribution of atoms Because all atoms of an element have roughly the same mass, the kinetic energy of identical atoms is determined by velocity (KE= ½mv 2 )

4. The Maxwell-Boltzmann apparatus Maxwell and Boltzmann performed an experiment to determine the kinetic energy distribution of atoms Because all atoms of an element have roughly the same mass, the kinetic energy of identical atoms is determined by velocity (KE= ½mv 2 )

5. The Maxwell-Boltzmann distribution The resulting disk looks like this: Basically, if we plot the intensity of the dots on a graph we get a graph of fraction of atoms/molecules vs. kinetic energy: Fraction of molecules Kinetic energy  Molecules hit disk first Molecules hit disk last

6. Why is the graph skewed? This curve is characteristic of all molecules The curve is elongated due to how atoms collide, and to the units of the graph Recall all particles are in motion. An average speed will be reached. The graph is skewed because 0 is the lower limit, but theoretically there is no upper limit Same data, different axes. E.g. v=1, KE=1 v=2, KE=4 v=3, KE=9 velocity KE More than that the graph is skewed because the x-axis has units of energy not velocity

7. Temperature and reaction rate By understanding the Maxwell-Boltzmann distribution, we can begin to understand the two reasons why an increase in temperature causes an increase in reaction rate Q- Look back at the five factors that affect reaction rates. Three of these factors can be (at least in part) explained by the collision theory. Identify the 3 factors and explain how the affect of each can be explained with reference to the collision theory

8. Temperature and reaction rate A- Ability to meet (molecules that are well mixed will have a greater chance of colliding) Concentration of reactants (more molecules means more collisions) Temperature (faster moving molecules means more collisions per unit of time).

9. Temperature and reaction rate By increasing the temperature, a small number of molecules reach Ea. The reaction is exothermic, further increasing temperature and causing more molecules to reach Ea, etc. Ea Fraction of molecules Kinetic energy  Shift due to higher temperature

10. © 2009, Prentice-Hall, Inc. Maxwell–Boltzmann Distributions This fraction of molecules can be found through the expression where R is the gas constant and T is the Kelvin temperature. f = e - E a RT

11. © 2009, Prentice-Hall, Inc. Reaction Coordinate Diagrams It is helpful to visualize energy changes throughout a process on a reaction coordinate diagram like this one for the rearrangement of methyl isonitrile.

12. © 2009, Prentice-Hall, Inc. Reaction Coordinate Diagrams The diagram shows the energy of the reactants and products (and, therefore,  E). The high point on the diagram is the transition state. The species present at the transition state is called the activated complex. The energy gap between the reactants and the activated complex is the activation energy barrier.

13. Endothermic Reactions

14. Exothermic Reactions

15. The Arrhenius Equation k = rate constant at temperature T  k = rate constant at temperature T  A = frequency factor  E a = activation energy  R = Gas constant, 8.31451 J/K·mol

16. The Arrhenius Equation, Rearranged  Simplifies solving for E a  -E a / R is the slope when (1/T) is plotted against ln(k)  ln(A) is the y-intercept  Linear regression analysis of a table of (1/T) vs. ln(k) can quickly yield a slope  E a = -R(slope)

17. © 2009, Prentice-Hall, Inc. Arrhenius Equation Taking the natural logarithm of both sides, the equation becomes ln k = - ( ) + ln A 1T1T y = m x + b Therefore, if k is determined experimentally at several temperatures, E a can be calculated from the slope of a plot of ln k vs.. EaREaR 1T1T

18. Catalysis : A substance that speeds up a reaction without being consumedCatalyst: A substance that speeds up a reaction without being consumed : A large molecule (usually a protein) that catalyzes biological reactions.Enzyme: A large molecule (usually a protein) that catalyzes biological reactions. : Present in the same phase as the reacting molecules.Homogeneous catalyst: Present in the same phase as the reacting molecules. : Present in a different phase than the reacting molecules.Heterogeneous catalyst: Present in a different phase than the reacting molecules.

19. Lowering of Activation Energy by a Catalyst

20. Catalysts Increase the Number of Effective Collisions

21. Heterogeneous Catalysis Step #1: Adsorption and activation of the reactants. Carbon monoxide and nitrogen monoxide adsorbed on a platinum surface

22. Heterogeneous Catalysis Step #2: Migration of the adsorbed reactants on the surface. Carbon monoxide and nitrogen monoxide arranged prior to reacting

23. Heterogeneous Catalysis Step #3: Reaction of the adsorbed substances. Carbon dioxide and nitrogen form from previous molecules

24. Heterogeneous Catalysis Step #4: Escape, or desorption, of the products. Carbon dioxide and nitrogen gases escape (desorb) from the platinum surface