Answer:
rate = l[A][B]
Explanation:
We are given the information that step 1: A + B → 2C + D is the the rate determinng steps, while the other 2 are fast in the reaction mechanism.
The rate law which is what we need to determine in this question is dependent on the the slowest step,
Therefore, the rate law will be a second order overall and dependent on the concentrations of A and B:
rate = k [A][B]
The rate law based on this reaction mechanism is , rate = k[A][B]
Given:
Step 1: A + B → 2C + D (slow)
Step 2: C → E (fast)
Step 3: D → 2F (fast)
The rate of reaction can be determined by the slowest step of a reaction. So out of three steps; Only step 1 is slow thus it will be the rate determining step else both steps are fast.
And, the rate law will be a second order overall and dependent on the concentrations of A and B:
Hence, Rate = k [A][B]
Find more information about Rate of reaction here:
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