Part A Consider the following multistep reaction: A + B --> AB (SLOW) A + B -->

Question

Part A Consider the following multistep reaction: A + B --> AB (SLOW) A + B --> A2B (FAST) ---------------------------------- 2A + B --> A2B (OVERALL) Based on this mechanism, determine the rate law for the overall reaction. Part B Consider the following multistep reaction: C + D <==> CD (FAST) CD + D --> CD2 (SLOW) CD2 + D --> CD3 (FAST) -------------------------------------- C + 3D --> CD3 (OVERALL) Based on this mechanism, determine the rate law for the overall reaction.

Explanation / Answer

For part A, the slow step determines the rate law. It depends on the reactants. rate = k*[A]*[B] As for the second part, the slow step determines the rate law: rate=k*[CD]*[D] However, CD is an intermediate and you cannot measure the intermediate, so if you write the equilibrium constant for the first equation: k'=[CD]/[C][D] which can be rearranged : [CD]=k'*[C][D] k' is a constant. When this is plugged into the rate equation: rate=k*k'*[C][D]*[D] a constant times a constant is a constant so it simplifies: rate=k'*[C][D]*[D]

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