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For the reaction A + B → products, it is observed that: (i) On doubling the initial concentration of A only, the rate of reaction is also doubled (ii) On doubling the initial concentrations of both A and B, there is a change by a factor of 8 in the rate of the reaction. The rate of this reaction is given by:

1. rate = k[A]²[B]²
2. rate = k[A]²[B]
3. rate = k[A][B]²
4. rate = k[A]²[B]

Correct answer: rate = k[A][B]²

Solution

From (i), the reaction is first order with respect to A. From (ii), doubling both A and B increases the rate by 8, implying the reaction is second order with respect to B. Thus, the rate law is rate = k[A][B]².

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