# hw 13 - dziewa(jcd935 – Homework#14 – Holcombe...

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Unformatted text preview: dziewa (jcd935) – Homework #14 – Holcombe – (52460) 1 This print-out should have 15 questions. Multiple-choice questions may continue on the next column or page – find all choices before answering. 001 10.0 points The reaction 2 NO 2 (g) → 2 NO(g) + O 2 (g) is postulated to occur via the mechanism NO 2 (g) + NO 2 (g) → NO(g) + NO 3 (g) slow NO 3 (g) → NO(g) + O 2 (g) fast. What is an intermediate in this reaction? 1. O 2 (g) 2. NO(g) 3. ON- NO 3 (g) 4. NO 2 (g) 5. NO 3 (g) correct Explanation: 002 10.0 points Consider the mechanism NO 2 + F 2 → NO 2 F + F k 1 , slow F + NO 2 → NO 2 F k 2 , fast What is the rate law? 1. rate = k 1 [NO 2 F] [F] 2. rate = k 1 k 2 [NO 2 ] 2 3. rate = k 1 [NO 2 ] [F 2 ] correct 4. rate = k 2 [NO 2 ] 2 5. rate = k 2 [NO 2 ] [F] Explanation: 003 10.0 points Consider the reaction mechanism below: Step Reaction 1 CH 3 Br-→ CH 3 + + Br − 2 CH 3 + + HCl-→ CH 3 Cl + H + 3 H + + Br −-→ HBr overall CH 3 Br + HCl-→ CH 3 Cl + HBr If the rate law is experimentally determined to be rate = k · [CH 3 Br] · [HCl] · [Br − ] − 1 , what is the rate-limiting step? 1. step 1 2. step 3 3. not enough information 4. step 2 correct Explanation: The reactants that precede the slowest for- ward step will appear in the rate law for a reaction....
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hw 13 - dziewa(jcd935 – Homework#14 – Holcombe...

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