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1aa3-2012-tut4-q

# 1aa3-2012-tut4-q - 6 The experimentally determined rate law...

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CHEMISTRY 1AA3 Week of JANUARY 30, 2012 TUTORIAL PROBLEM SET 4 QUESTIONS ______________________________________________________________________________ Page 1 of 1 1. The rate law for the reaction: F 2 (g) + 2 ClO 2 (g) 2 FClO 2 (g) is rate = k [F 2 ][ClO 2 ]. At 25 C, the rate constant for the reaction is 1.2 M 1 s 1 . Calculate the rate of the reaction at 25 C if [F 2 ] = 0.010 M and [ClO 2 ] = 0.020 M. 2. What is the main difference between a differential rate law and an integrated rate law? 3. Can you calculate the concentration of the transition state species in any meaningful way? 4. Draw reaction coordinates / kinetic schemes for the three cases of multi-step reactions discussed in class: a. Slow step followed by fast step b. Fast equilibrium followed by slow step c. No assumption about relative rates 5. Give four key properties of elementary reactions
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Unformatted text preview: 6. The experimentally determined rate law for the high temperature reduction reaction: 2 NO(g) + 2 H 2 (g) N 2 (g) + 2 H 2 O(g) was found to be Rate = k[NO] 2 [H 2 ]. A proposed reaction mechanism for this reaction is Elementary step 1 2 NO(g) + H 2 (g) N 2 O(g) + H 2 O(g) Elementary step 2 N 2 O(g) + H 2 (g) N 2 (g) + H 2 O(g) Is this mechanism consistent with the stoichiometry of the reaction and with the rate law? If so, what is the rate determining step? 7. A reaction that contributes to smog formation is the combination of oxygen with NO from automobile exhaust.: 2 NO (g) + O 2 (g) 2NO 2 (g) Show that the observed rate law: rate = k [NO] 2 [O 2 ] is consistent with the following proposed mechanism. NO (g) + O 2 (g) NO 3 (g) NO 3 (g) + NO (g) 2NO 2 (g) k 1 k-1 k 2 1 2 (fast) (slow)...
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