Rate Law From a Reaction Mechanism

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A reaction is proposed to occur via the following mechanism:
Step 1: $A + A \rightarrow X$ (fast)
Step 2: $X + B \rightarrow Y$ (slow)
Step 3: $Y + B \rightarrow C$ (fast)
Given that the second step is the rate-determining step and assuming the first step establishes a rapid equilibrium, what is the rate law for the formation of product C?

$k[A]^2[B]^2$

$k[A][B]^2$

$k[A][B]$

$k[A]^2[B]$

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