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Week 3 Chem 120B: Kinetics

by: Sarahjallen

Week 3 Chem 120B: Kinetics Chem 120B

Cal State Fullerton

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About this Document

Equilibrium and activation energy
General Chemistry 120B
Dr. Richard Deming
Class Notes
Chemistry, kinetics, CSUF, cal state fullerton, Equilibrium, Activiation Energy
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This 2 page Class Notes was uploaded by Sarahjallen on Friday February 5, 2016. The Class Notes belongs to Chem 120B at California State University - Fullerton taught by Dr. Richard Deming in Spring 2016. Since its upload, it has received 18 views. For similar materials see General Chemistry 120B in Chemistry and Biochemistry at California State University - Fullerton.

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Date Created: 02/05/16
Week 3 Notes: Kinetics Activation energy is the energy needed for a reaction to take place. It’s the energy needed to turn the reactants into products. We can recognize activation energy as the bump on top of the graph used to display the reaction.  Activation Energy! A reaction with a smaller amount of activation energy has a much higher reaction rate and happens faster. This is because the reaction doesn’t need as much energy in order to move the reactants to products. On a graph we can calculate the (–activation energy/R) by finding the slope when it is graphed Ln (k) vs. (1/t) * on Kelvin scale* If the activation energy peak has bumps on it then that signifies there is an intermediate within the reaction. Forward reaction  Exothermic Backward Reaction  Endothermic Some ways to calculate the Activation Energy, E a : −Ea Ea 1 1 Ea 1 K=Ae Rt ln(k= R T 2 − T 1) lnk=lnA− R (t) High activation energies mean they are sensitive to temperature. ↑Temp = ↓ Activation Energy = faster reaction A catalyst is a substance that lowers the amount of activation energy required and because of this speeds up the reaction. A reaction rate is determined by the slowest elementary step. - Termolecular: happens fast however rare! - Bimolecular: happens very often. Equilibrium is when the forward rate of the reaction equals the reverse rate! Only include gases and aqueous solutions when calculating K!


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