Question

Analyzing a new reaction

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

3A→B+C

B+2D→C+F

1. What is the overall reaction?

2. What is the rate law for step one of this reaction?

3. What is the rate law for step two of this reaction?

Answer 1

1: Given that the reaction completes via the following two elementary steps.

3A----> B+C ----- (1)

B+2D -----> C+F ---- (2)

Now we can get the overall reaction by adding the abve two reactions. Hence the overall reaction is

3A + B + 2D ----- > B + C + C + F

Now 'B' will cancel out from both the sides. Hene the overall reaction is

3A + 2D ----- > 2C + F (answer)

(2): Rate law is proportional to the concentration of all the reactants raised to a power equals to the coffecient

Step-1 of the reaction is

3A ----> B+C

Hence rate law is

rate = k x [A]³ (answer)

(3): Step-2 of the reaction is

B + 2D ----> C + F

Hence rate law is

rate = k x [B]x[D]² ( answer)