CHM152Chapter 12 Cont

Chemistry (MasteringChemistry Series)

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1/28/2009 1 12.8 Reaction Mechanisms ` Mechanisms outline the steps in a reaction that will convert the reactant(s) into product(s) ` May be one or many steps involved ` Chemical equation may or may not describe the mechanism 12.8 Reaction Mechanisms ` NO 2 (g) + CO (g) NO (g) + CO 2 (g) ` Rate = k [NO 2 ] 2 ` Does the rate match the equation? ` Divide reaction into elementary steps: ` NO + NO 2 NO 3 + NO Slow NO 2 NO NO ` NO 3 + CO NO 2 + CO 2 Fast 12.9 Rate Laws for Elementary Steps ` Elementary steps are defined by their molecularity - the number of molecules that have to collide to give the defined products. ` Uni molecular - 1 reactant = Rate = k[A] ` B molecular 2 reactants = Rate = k[A 2 Bi - 2 reactants Rate = k[A] or Rate = k[A][B] ` Ter molecular - 3 reactants = Rate = k[A] 3 or Rate = k[A] 2 [B] or Rate = k[A][B][C] ` See Table 12.5, p. 466
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1/28/2009 2 12.8 Reaction Mechanisms ` NO 2 + NO 2 NO 3 + NO Slow ` NO 3 + CO NO 2 + CO 2 Fast ` NO 3 is an intermediate (produced in 1st step, consumed in last) ` NO is a catalyst (consumed in 1st step produced in last NO 2 is a catalyst (consumed in 1st step, produced in last) ` Elementary steps sum to give overall equation (Hess’s Law) 12.8 Reaction Mechanisms ` Identify the intermediate(s) and catalyst(s) in the following steps: C 4 H 9
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CHM152Chapter 12 Cont - 1/28/2009 12.8 Reaction Mechanisms...

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