missrogers2018
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Consider the following three-step representation of a reaction mechanism.

Step 1: A + B --> AB (fast) and the rate = k[A][B]
Step 2: AB + B --> AB2 (slow) and the rate = k[AB][B]
Step 3: AB2 + B --> AB3 (fast) and the rate = k[AB2][B]
Overall: A + 3B --> AB3 and the rate = k[A][B]2

Which explains why the rate law for the overall equation is not the same as the rate equation for the rate-determining step?
A; The fastest step determines the overall rate law.
B: The overall rate law is determined from the balanced equation.
C: AB is an intermediate; therefore the rate law is determined from the reactants in the previous step.
D: B is an intermediate; therefore the rate law is determined from the reactants in the previous step.

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Answer:

The answer is C. AB is an intermediate; therefore the rate law is determined from the reactants in the previous step.

I just took the test and C. was correct. Please mark me as brainliest!

Answer:  C: AB is an intermediate; therefore the rate law is determined from the reactants in the previous step.

Explanation:  :  Rate law is usually determined from the slowest step of the reaction mechanism.

Thus as we can see that the reaction which is slow has AB as its intermediate, rate law can be determined from the same.

Moreover , we can see that the overall rate law is very different from the rat law determined from the slowest step.

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