How do I solve this AP Chemistry problem on the reaction A+2B==>C.

Question

Consider the reaction A+2B==>C. The rate law for this reaction is second order in A and second order in B. If the rate constant  at 25°C 1.25×10^-2 s^-1, find the rate  of reaction when the concentration  of A is 0.27M and the concentration of B is 0.32M.

Answer 1

Since it is 2nd or in A and B, you can write the rate law as rate = k[A]²[B]²

You are given k (rate constant) and [A] and [B], so you should be able to plug the numbers in and solve for rate. Right?

Rate = (1.25x10^-2)(0.27)²(0.32)²

NOTE: The units given for k cannot be correct as s-1 because those are the units for a first order reaction.  This is oveall a fourth order reaction so units will be M^-3s^-1.