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# 1aa3-2010-tut10-answerkey - CHEMISTRY 1AA3 March 22-26 2010...

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CHEMISTRY 1AA3 March 22-26, 2010 TUTORIAL PROBLEM SET 10 SOLUTIONS ________________________________________________________________________ Chemistry 1AA3 1. What are the overall orders of the reactions to which the following rate laws apply? (a) rate = k[H 2 ][I 2 ] (b) rate = k[NO 2 ] 2 [H 2 ] (c) rate = k[Cl 2 ] (3/2) [O 2 ] SOLUTION: The overall order of a reaction comes from the sum of the exponents in the rate law, i.e., for rate = k[A] x [B] y overall order = x + y (a) 1 + 1 = 2 (b) 2 + 1 = 3 (c) 1.5 + 1 = 2.5 2. Consider the reaction: 2 NO(g) + O 2 (g) 2 NO 2 (g) (a) Write expressions for the rate of the reaction in terms of the changes of concentrations of NO, O 2 , and NO 2 . (b) Suppose that at a particular moment the rate of reaction with respect to NO is 0.066 M s -1 . What is the rate at which O 2 is being consumed? SOLUTION: (a) rate = 1 Δ [NO] = −Δ [O 2 ] = +1 Δ [NO 2 ] 2 Δ t Δ t 2 Δ t (b) Δ [NO] = 0.066 M 1 s 1 Δ t 1 Δ [NO] = −Δ [O 2 ] 2 Δ t Δ t Δ [O 2 ] = (0.066 M s 1 ) = 0.033M s 1 Δ t 2

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CHEMISTRY 1AA3 March 22-26, 2010 TUTORIAL PROBLEM SET 10 SOLUTIONS ________________________________________________________________________ Chemistry 1AA3 3. The rate law for the reaction: F 2 (g) + 2 ClO 2 (g) 2 FClO 2 (g) is rate = k [F 2 ][ClO
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