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As always… Lon-Capa assignments Lecture videos Textbook Read Do text homework

Exam III Thursday, December 7, 7:00-9:00 pm; rooms are on the website. Conflict: (12/7) 4:30-6:30 pm in 101 Transportation; sign up in 1026 Chem Annex Conflict with conflict? Email me right away. Review sessions: Monday, December 4: 7-9 pm 165 Noyes Lab Tuesday, December 5: 7-9 pm 165 Noyes Lab

Pseudo-Order Question Determine the rate law and value of k given the following data. 2H2(g) + 2NO(g)  N2(g) + 2H2O(g) EXPERIMENT #1 EXPERIMENT #2 TIME (sec) [NO] [NO] ________ 0 1.00 x 10-2 M 1.00 x 10-2 M 10.0 6.67 x 10-3M 5.00 x 10-3 M 20.0 5.00 x 10-3 M 3.33 x 10-3 M 30.0 4.00 x 10-3 M 2.50 x 10-3 M 40.0 3.33 x 10-3 M 2.00 x 10-3 M   In experiment #1, [H2]0 = 10.0 M In experiment #2, [H2]0 = 20.0 M

Pseudo-Order Question (con’t) A H2 + NO  H2O + N (slow) N + NO  N2 + O (fast) O + H2  H2O (fast) ------------------------------------------------------------------------------------------------------------------------- B H2 + 2NO  N2O + H2O (slow) N2O + H2  N2 + H2O (fast) -------------------------------------------------------------------------------------------------------------------------- C 2NO N2O2 (fast equil.) N2O2 + H2  N2O + H2O (slow) D Two of the above are equally good.  

Clicker Question Consider the reaction 2A  C which has the following proposed mechanism: 1. A B 2. A + B  C Defining rate = d[C]/dt , use the steady-state approximation to determine the rate law for the mechanism and choose the correct statement below. (Note: nothing is implied about the order in B in the responses below). a) The rate law appears first order in A at very low [A], and second order in A at very high [A]. b) The rate law appears first order in A at very high [A], and second order in A at very low [A]. c) The reaction appears first order in A at very high and very low [A]. d) The rate law appears second order in A at very high and very low [A]. e) The rate law is zero order in A.

Clicker Question Consider the activated complex demonstration. Suppose we run two trials, one at 55C and one at 65C. The times for the reaction are 85 seconds and 41 seconds, respectively. Determine the activation energy for this reaction. Assume the frequency factor, A, to be constant. a) 261 J/mol b) 663 J/mol c) 48.5 kJ/mol d) 67.2 kJ/mol e) 98.3 kJ/mol