The hypothetical reaction A + 2B Products has the rate law Rate = k[A]2[B]3. If the

Question:

The hypothetical reaction A + 2B → Products has the rate law Rate = k[A]2[B]3. If the reaction is run two separate times, holding the concentration of A constant while doubling the concentration of B from one run to the next, how would the rate of the second run compare to the rate of the first run?