Lecture notes for Nov 30 Chem135 Johnson

Lecture notes for Nov 30 Chem135 Johnson - Lecture notes...

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Lecture notes for Monday, Nov 26 for Exam V Dr. Johnson CHEM135 Acid-Base Equilibrium Chemical Kinetics B&H Chapter 10. Quiz 10 given and lecture evaluation forms completed by class Please remember to also complete the electronic evaluation forms at: www.courseEvalUM.umd.edu Overall reaction: A products Rate expression: Rate = - ∆[A]/∆t Rate Law: (instantaneous rate initially; based on initial [A] where x is the order of reaction with respect to A and the overall order of reaction. Rate = k[A] x Zero order reaction x=0 Rate = k[A] o = k First order reaction x=1; rate is directly proportional to the [A] Rate = k[A] Integrated Rate Law: relates time and the change in [A] For first order reaction: Set the rate expression and the rate law equal to each other; rearrange and integrate. You are not responsible to know this process; just the end result which is: ln [A] t – ln [A] o = - k t this can be rearranged into the equation for a straight line: y = mx + b ln [A] t = (- k )t – ln [A] o A plot of ln [A] t vs t(s) gives a straight line with a slope of –k
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kt A A o t - = ] [ ] [ ln This is the integrated rate law for a first order reaction. You will be only required to know the integrated rate law for a first order reaction for this course ; the integrated rate laws for other reaction orders are different: KINETICS OF FIRST ORDER AND SECOND ORDER REACTIONS TYPE: A products or 2A → products Order Rate Law Concentration- Time Equation
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