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CHM 130 GCC Chapter 16. 16.1 Collision Theory Molecules must hit/collide in order to react and make products A successful collision results in reactant.

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Presentation on theme: "CHM 130 GCC Chapter 16. 16.1 Collision Theory Molecules must hit/collide in order to react and make products A successful collision results in reactant."— Presentation transcript:

1 CHM 130 GCC Chapter 16

2 16.1 Collision Theory Molecules must hit/collide in order to react and make products A successful collision results in reactant bonds breaking and/or product bonds forming To increase the # of successful collisions: you need more collisions. you need enough energy, E a, activation energy. the molecules must be oriented correctly. wf

3 To Increase the Rate of Reaction Increase [reactant], more reactants = more collisions Increase temperature, molecules move faster = more collisions AND more energy Add a catalyst which provides an alternate reaction pathway with lower E a Activation Energy, E a, is the minimum energy needed to react (turn reactants to products)

4 16.2 Energy Profiles Transition state = in between reactants and products, the reactant bonds are ½ broken and product bonds ½ formed, so this is a very high energy and unstable species, exists less than a millisecond  H = change in heat energy = product’s heat – reactant’s heat Endothermic = reactants gain or absorb heat, heat is a reactant, heat enters the rxn Reactants + Heat  Products Exothermic = reactants lose or release heat, heat is a product, heat exits the rxn Reactants  Products + Heat

5 Exothermic, is  H + or -? -

6 Draw the energy profile for an endothermic reaction Label the TS  H Reactants Products E A

7 Endothermic, is  H + or -? +

8 With Catalyst

9 Self Test Page 477 Try 1-2, 10 Answers in Appendix J


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