Consider the following elementary steps that make up the mechanism of a certain reaction: 3A→B+C B+2D→C+F Part A What is the overall reaction? Express your answer as a chemical equation. View Available Hint(s) nothing Part B Which species is a reaction intermediate? View Available Hint(s) Which species is a reaction intermediate? A B C D F Part C What is the rate law for step 1 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. View Available Hint(s) Rate = Part D 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. View Available Hint(s) Rate = Provide Feedback

A.    3A + 2D → 2C + F

B.    B is an intermediate

C.   rate = k[A]³

 D.  rate = k`[D]²

Explanation:

Part A

The overall reaction is the sum of all the elementary steps:

       3A→B+C

+

       B+2D→C+F

         3A + 2D → 2C + F

Part B

A reaction intermediate is one that participates in the elementary steps, but it is not a product. Notice B is produced in the first step and consumed in the second, therefore it is an intermediate species.

Part C

The rate law is  the product of the reaction constant, k, times the concentration of the reactants raised to the power of their coefficients in the balanced reaction assuming that it is the slow step in the reaction mechanism.

rate = k[A]³

Part D

Again as in part C:

rate = k [D]²  ( B is not included since as we saw it is an intermediate )