Lecture_Notes_092109b

Lecture_Notes_092109b - Lecture Note 9/21/2009

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Chem 105 B Exam 1 Review 9/21/09
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Chapter 12 #31 z The decomposition of hydrogen peroxide was studied, and the following data were obtained at a particular temperature. Determine the rate law, the integrated rate law, and the value of the rate constant. Calculate [H 2 O 2 ] at 4000. s after the start of the reaction. 0.050 3600 0.082 3000 0.13 2400 0.22 1800 0.37 1200 0.59 600 0.78 300 0.91 120 1.00 0 [H 2 O 2 ] (mol/L) Time (s) first order y = -0.0008x - 0.0049 R 2 = 0.9998 -3.5 -3 -2.5 -2 -1.5 -1 -0.5 0 0 1000 2000 3000 4000
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Chapter 12 #43 z A first-order reaction is 75.0% complete in 320. s. { What are the first and second half-lives for this reaction? { How long does it take for 90.0% completion?
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Chapter 12 #48 z Consider the hypothetical reaction: A + B + 2C 2D + 3E, where the rate law is: rate = k[A][B] 2 . An experiment is carried out where [A] o = 1.0 x 10 -2 M, [B] o = 3.0 M, and [C] o = 2.0 M. The reaction is started, and after 8.0 seconds, the concentration of A is 3.8 x 10 -3 M. { Calculate k for this reaction { Calculate the half-life for this experiment
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Chapter 12 #48 continued z Calculate the concentration of A after 13.0 seconds.
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Lecture_Notes_092109b - Lecture Note 9/21/2009

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