6csp06kineticshandout

6csp06kineticshandout - PLEASE REVIEW THE BASIC CONCEPTS OF...

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PLEASE REVIEW THE BASIC CONCEPTS OF REACTION RATES IN SECTIONS 13.1 AND 13.2IN ADDITION TO THE FOLLOWING. 13.3 Rate Laws and Reaction Order The general form of a rate law is Rate = k[A] n the “k” is the rate constant for the reaction and depends only upon the temperature the [A] is the concentration of substance A at the beginning of the reaction the “n” is the order of the rate with respect to substance A Several species taking place in a reaction (including reactants and products) may appear in the rate law. The order may be positive, negative, a whole number, or a fraction. The key thing to remember about rate laws is that the order are determined experimentally and never by the chemical equation or the stoichiometry. The overall order of a reaction is the sum of the orders of the individual species. This can be found by simply adding up all of the exponents that appear in the rate law. Comprehensive Example: 2 A + B C + 3 D Experimental Data: # [A] [B] [C] [D] Rate 1 10 5 20 5 30 2 10 10 20 5 120 3 10 5 20 20 120 4 10 10 40 5 60 5 20 5 20 20 120 What is the rate law for this reaction? Remember, it cannot be obtained from the reaction equation, so
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This note was uploaded on 12/26/2009 for the course CHEM CHEM 6C taught by Professor Hoeger during the Spring '08 term at UCSD.

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6csp06kineticshandout - PLEASE REVIEW THE BASIC CONCEPTS OF...

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