Unit 8 Kinetics and Rates of Reactions

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Presentation transcript:

Unit 8 Kinetics and Rates of Reactions

What can we do to increase or decrease the rate of a reaction?

Collision Theory

What is Collision Theory? Major idea of kinetic theory Reacting particles will hit each other and the walls of the container they are in millions and millions of times When they have enough energy, they stick to each other and will form a bond (products) If not enough energy they will bounce off and try again

Continue Particles will do this until they form a bond In addition to the energy level being correct, the particles also must be in the proper alignment to exchange/share electrons

What is a rate?

Rate Definition and notes Rate is the speed or pace of a reaction Measured in concentration and time We expect reactions to have a rate that produces products in an efficient way Faster is better for us

Activation Energy

Definition and Notes Minimum amount of energy that is required to start a reaction Think of it as a barrier to producing products If you cannot pass this point, you cannot produce products We search for ways to lower activation energy but NEVER TO INCREASE IT!!!!!!!!!!!!!!!!

Factors that effect the rate of a Reaction 1. Nature of Reactants 2. Concentration Covalent slow Ionic fast Increase concentration increase collisions and increase rate Decrease concentration decrease collisions and decrease rate

Factors 3. Surface Area 4. Pressure (Gases Only) Increase SA Increase Rate Increase Pressure Increase Collisions Increase Rate Decrease Pressure Decrease Collisions and Decrease Rate

Factors 5. Catalysts 6., Temperature Speed up reaction by lowering activation energy Provide an alternate pathway for the reaction to take place High temps increase rate Low temps decrease rate All about collisions