hw 13 - dziewa (jcd935) Homework #14 Holcombe (52460) 1...

Info iconThis preview shows pages 1–2. Sign up to view the full content.

View Full Document Right Arrow Icon

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
This is the end of the preview. Sign up to access the rest of the document.

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....
View Full Document

Page1 / 4

hw 13 - dziewa (jcd935) Homework #14 Holcombe (52460) 1...

This preview shows document pages 1 - 2. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online