Chapter%2012_Rates%20and%20Equilibrium_part2_post

Chapter%2012_Rates%20and%20Equilibrium_part2_post - CHM...

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CHM 11200 Spring 10 Chapter 12 Reaction Rates and Equilibrium
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Multi-Step Reactions 2 Let’s look at how CFCs (chlorofluorocarbons) destroy the earth’s ozone layer. In the upper atmosphere the following reaction will take place: CF 2 Cl 2 CF 2 Cl + Cl UV light The resulting Cl atom is highly reactive and acts a a catalyst for the destruction of ozone in the upper atmosphere. Ozone in the upper atmosphere helps filter out harmful UV radiation that causes skin cancer.
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Multi-Step Reactions 3 The destruction of ozone by Cl is a two-step process: Step 1: O 3 (g) + Cl (g) ClO (g) + O 2 (g) Step 2: ClO (g) + O 3 (g) Cl (g) + 2 O 2 (g) Any intermediates or catalysts in a multi-step reaction are not seen in the overall reaction. overall: 2 O 3 (g) 3 O 2 (g)
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Example 1 (Back of Chapter #12.6) 4 What are two ways to increase the rate of the following reaction? 2 Ca (s) + O 2 (g) 2 CaO (s)
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Example 2 (Back of Chapter #12.11) 5 Consider the following reaction: 2 HI (g) H 2 (g) + I 2 (g) Determine if each of the following collisions has the proper orientation for an effective collision. A B C
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Example 3 (Back of Chapter #12.25) 6 The propane used in a gas grill does not usually react with air in a combustion reaction unless first initiation with a spark. Explain using collision theory.
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(Back of Chapter #12.41) 7 Consider the following two-step reaction: N 2 O 5 NO 3 + NO 2 NO 3 + NO 2 NO 2 (a) Identify any catalysts or intermediates. (b)
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Chapter%2012_Rates%20and%20Equilibrium_part2_post - CHM...

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