Questions3 - time (x 10 3 s) Name: 2 Part II: Calculating...

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Name: Chemistry 008, Spring 2008 Cornell University Dr. Pontrello Due 2/17/08 Learning Strategy Questions 3 Any time you write down a number, please include correct units when applicable. Clearly write any equation(s) that you are using to answer each question, and also clearly indicate the steps used to answer the questions, if appropriate. Part I: Calculating a Rate Constant. I.1 (14 points) The following table of data was collected for the N 2 O 5 reaction at 30.0 o C. N 2 O 5 (g) 2 NO 2 (g) + ½ O 2 (g) time (s) [N 2 O 5 ] (M) 7200 0.80 8600 0.72 9400 0.68 10800 0.58 Using the graph, plot the data in such a way as to verify that the reaction is first order. Using your plotted data, calculate the value of the rate constant, k.
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Unformatted text preview: time (x 10 3 s) Name: 2 Part II: Calculating the Activation Energy. II.1 (18 points) The same reaction from Part I was monitored at different temperatures, and rate constants were determined as done in Part I. These data are presented in the following table. N 2 O 5 (g) → 2 NO 2 (g) + ½ O 2 (g) T (K) k (s-1 ) 318 5.0 x 10-4 308 1.4 x 10-4 298 3.5 x 10-5 Using the data from the table above, the value of k you calculated in Part I, and the graph below, calculate the activation energy (E a ) of the reaction. II.2 (10 points) What is the half-life of the reaction at 298 K? Show derivation of the equation starting with the integrated rate law....
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This note was uploaded on 07/09/2008 for the course CHEM 342132 taught by Professor Davis during the Spring '08 term at Cornell.

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Questions3 - time (x 10 3 s) Name: 2 Part II: Calculating...

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