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In reaction, A + B → Product, rate is doubled when the concentration of B is doubled, and rate increases by a factor of 8 when the concentrations of both the reactants (A and B) are doubled. Rate law for the reaction can be written as :

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

Correct answer: Rate = k[A]²[B]

Solution

When [B] is doubled, the rate doubles, indicating the reaction is first order with respect to B. When both [A] and [B] are doubled, the rate increases by a factor of 8, implying the reaction is second order with respect to A. Thus, the rate law is Rate = k[A]²[B].

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