Lec 04 Jan 12 Rate Laws Summary

Lec 04 Jan 12 Rate Laws Summary - Chem 102 (Klobukowski)...

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Chem 102 (Klobukowski) Handout 1 Winter 2009 Summary of Rate Laws (14-7) Summary of kinetic equations for the reaction: A products ORDER ZERO FIRST SECOND Rate Law Rate = k Rate = k [A] Rate = k [A] 2 Units of k (for rate in M/s) Ms -1 s -1 M -1 s -1 Integrated Rate Law [A] t = [A] o - kt ln[A] t = ln[A] o - kt 1 [A] = 1 [A] O + kt Plot needed to give a straight line [A] versus t ln[A] versus t 1/[A] versus t Relationship between rate constant and slope slope = - k slope = - k slope = k Half-life t 1/2 = [A] O 2k t 1/2 = 1n2 k t 1/2 = 1 k[A] O Problem: The decomposition of N 2 O 5 was studied at 298 K, and the following data was collected. A possible overall decomposition of N 2 O 5 is: 2 N 2 O 5 (g) 2 NO 2 (g) + N 2 O 4 (g) + O 2 (g) (1) How would you determine the order if you were given only [N 2 O 5 ] as a function of time? t (min) [N 2 O 5 ] (M) ln[N 2 O 5 ] 1/[N 2 O 5 ] 0 0.0165 -4.104 60.6 600 0.0124 -4.390 80.65 1200 0.0093 -4.678 107.53 1800 0.0071 -4.948 140.85 2400 0.0053
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This note was uploaded on 03/25/2009 for the course CHEM 102 taught by Professor Drk during the Spring '09 term at University of Alberta.

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Lec 04 Jan 12 Rate Laws Summary - Chem 102 (Klobukowski)...

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