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Unformatted text preview: EXAM 3 REVIEW- PRACTICE QUESTIONS LBS 172 REACTION MECHANISMS RATES 1.) Given the equation: 2NO(g) + 2H 2 (g) Æ N 2 (g) + 2H 2 O(g) And the assumed mechanism: 1. 2NO(g) Æ N 2 O 2 (g) 2. N 2 O 2 (g) + H 2 (g) Æ N 2 O(g) + H 2 O(g) 3. N 2 O(g) + H 2 (g) Æ N 2 (g) + H 2 O(g) List any intermediate species. Note the molecularity of each step. Write a rate equation for the third step. Do the elementary steps add up to the overall reaction? 2.) Given the equation: 2NO 2 (g) Æ 2NO(g) + O 2 (g) And two proposed mechanisms: A 1. NO 2 (g) Æ NO(g) + O(g) slow step 2. O(g) + NO 2 (g) Æ NO(g) B 1. NO 2 (g) + NO 2 (g) Æ OONO(g) + NO(g) slow step 2. OONO(g) Æ NO(g) + O 2 (g) Write an overall rate equation for each mechanism. How could one disprove one or both of the two proposed mechanisms in a laboratory? 3.) Given the equation: 2NO 2 Cl(g) Æ 2NO 2 (g) + Cl 2 (g) And the assumed mechanism 1. NO 2 Cl(g) ↔ NO 2 (g) + Cl(g) fast, equilibrium, where k 1 is constant for forward rxn and k-1 is constant for reverse reaction...
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This note was uploaded on 07/25/2008 for the course LBS 172 taught by Professor Laduca during the Spring '08 term at Michigan State University.
- Spring '08