Consider the following multistep reaction: A + B rightarrow AB (slow) A + AB rig

Question

Consider the following multistep reaction: A + B rightarrow AB (slow) A + AB rightarrow A_2B (fast)/2A + B rightarrow A_2B (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. Consider the following multistep reaction: C + D CD (fast) CD + D rightarrow CD_2 (slow) CD_2 + D rightarrow CD_3 (fast)/C + 3D rightarrow CD_3 (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

part A )

rate law depends on only slow step

so   rate = k [A][B] --------------------------> answer

part B)

slow step rate determining step

rate = k [CD] [D] -------------------> 1

in equation 1 CD is not reactant so we cannot take it in rate law

so from first fast step

Kc = [CD] / [C] [D]

[CD] = Kc [C] [D] ---------------------->2

from 1 and 2

rate = k [CD] [D]

rate = k Kc [C] [D] [D]

rate = k [C] [D]^2 --------------------------> answer

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