What is the rate law for step 2 of this reaction? Express your answer in standard MasteringChemistry notation. For example, if the rate law is k[A][C]3 type k*[A]*[C]^3.

Rate=k*[A]^m[B]^n For the reaction A+B→ products m and n: orders of reaction of A and B respectively   Explanation:  Rate law is the equation that describes the initial rate of the reaction and its relation with the reactants concentration:  For the reaction A+B→ products Rate=k*[A]^m[B]^n k: Rate constant. It is constant only at the same temperature. The units of the constant depends on the overall reaction order. [A] and [B]: concentration of each reactant m and n: order of reaction of each reactant. This numbers indicate how the rate is affected by the concentration of each reactant : -When the order of reaction is 0, means that the concentration of that reactant does not affect the rate of the reaction. -When the order is 1, it means that doubling the concentration of the reactant will double the rate of the reaction (mantaining constante the other reactants concentrations). - When the order is 2, it means that doubling the concentration of the reactant will quadruple the rate (mantaining constante the other reactants concentrations).  The overall order reaction is the sum of the orders of reation of all the reactants. In this case m+n

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