# 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

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 )

Part A- The overall reaction is: 3X + M → 2 F + N.

Part B- The intermediate of this reaction is E.

Part C- Rate law for step 1 = k[X]³ = k*[X]^3.

Part D- Rate law for step 2 = k[E][M] = k*[E]*[M].

Explanation:

Part A: What is the overall reaction? Express your answer as a chemical equation.

We can get the overall reaction by summing the two steps of the reaction.

Step 1: 3X → E + F.

Step 2: E + M → F + N.

The E component in the products side in step 1 will cancel that in the reactants side of step 2.

∴ The overall reaction is: 3X + M → 2 F + N.

Part B: Which species is a reaction intermediate?

We should identify the intermediate firstly to determine the reaction intermediate.

The intermediate is the species that produced in a step of the reaction and consumed in next steps and do not appear in the overall reaction

So, the intermediate of this reaction is E.

Part C: What is the rate law for step 1 of this reaction?

The rate of the reaction is directly proportional to the concentration of the reactants.

Rate = k[reactants]ˣ.

where, k is the rate constant of the reaction,

x is the no. of moles of the reactants that involved in the reaction mechanism before the rate determining step.

So, The rate law for step 1 of this reaction (neglecting the mechanism) is:

Rate = k[X]³ = k*[X]^3.

Part D: What is the rate law for step 2 of this reaction?

Also, as in part C:

The rate law for step 2 of this reaction (neglecting the mechanism) is:

Rate = k[E][M] = k*[E]*[M].

rate = k*[A]^3

Explanation:

The following information is missing in the question:

Consider the following elementary steps that make up the mechanism of a certain reaction

1. 3A -> B+C

2. B+2D -> C+F

In elementary reactions, the order of each reactant in the rate law is equal to the coefficient in the balanced equation. Therefore, for the first step:

rate = k*[A]^3

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