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  • Consider a complex reaction with the following hypothetical mechanism: <img alt="\\\mathrm{Step 1: \(\mathrm{A}+\mathrm{B} \rightarrow \mathrm{AB}\) (slow)}\\\\\mathrm{ Step 2: \(A B+C \r

Consider a complex reaction with the following hypothetical mechanism:

\\\mathrm{Step 1: \(\mathrm{A}+\mathrm{B} \rightarrow \mathrm{AB}\) (slow)}\\\\\mathrm{ Step 2: \(A B+C \rightarrow A B C\) (fast)}\\\\\mathrm{ Step 3: \(\mathrm{ABC} \rightarrow \mathrm{D}+\mathrm{E}\) (slow)}

If the rate of formation of product D is given by the equation: Rate = k[A][B][C], where k is the rate constant, the overall order of the reaction is:

Option: 1

First order


Option: 2

Second order


Option: 3

Third order


Option: 4

Zero order


Answers (1)

best_answer

The overall order of a reaction is the sum of the individual orders with respect to each of the reactants. In the given mechanism, Step 1 and Step 3 are both slow steps, and the rate-determining step is the slowest step in the mechanism.

From Step 1, we can see that the rate of formation of intermediate AB is dependent on the concentrations of A and B, and the reaction is first order with respect to both A and B

From Step 2, we can see that the rate of formation of intermediate ABC is dependent on the concentration of AB and C, and the reaction is second order with respect to AB and first order with respect to C.

From Step 3, we can see that the rate of formation of product D is dependent on the concentration of ABC, and the reaction is second order with respect to ABC.

Combining all the orders, the overall order of the reaction is (1 + 1 + 2) = 4, which makes it a fourth-order reaction. However, since reactions with orders higher than 2 are rare, it is most likely an incorrect answer choice.

Therefore, the correct option is 3) Third order

Posted by

Devendra Khairwa

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