Part A Consider the following multistep reaction: A+BAB(slow) A+ABA2B(fast) 2A+B

Question

Part A Consider the following multistep reaction:

A+BAB(slow)

A+ABA2B(fast)

2A+BA2B(overall)

Based on this mechanism, determine the rate law for the overall reaction. Express your answer in standard MasteringChemistry format. For example, if the rate law is k[A]3[B]2 type k*[A]^3*[B]^2.

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Part B Consider the following multistep reaction:

C+DCD(fast)

CD+DCD2(slow)

CD2+DCD3(fast)

C+3DCD3(overall)

Based on this mechanism, determine the rate law for the overall reaction. Express your answer in standard MasteringChemistry format. For example, if the rate law is k[C]3[D]2 type k*[C]^3*[D]^2.

Explanation / Answer

Based on this: A + B = AB(slow)

the rate law for the overall reactionis :

Rate = k [A] [B]

he overall reaction is based on the slowest step CD + D = CD2.

So, k*[CD]*[D]
But you don't want to include the intermediate [CD] in the overall reaction rate, so substitute based on the reaction rate of the first step k*[C]*[D] = k*[CD]

k*[C]*[D]*[D]

Simplify:
k*[C]*[D]^2

Hope this helps

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