Question

12) Given the mechanism shown, which of the following statements would be false?

A + B  C slow

C + D  E + F fast

A) The rate law would be rate = k[A][B]

B) Increasing the concentration of [D] would not accelerate the reaction

C) is an intermediate

D) is a catalyst

E) The overall balanced reaction would be A + B + D  E + F

Answer 1

a)

The rate law is based on the SLOW step, since it is determining the reaction

so

Rate law for "slow" step is --> Rate = k[A][B]

this must be true

b)

Increase of [D] is not likely to accelerate the reaction, since A and B are limiting

c)

C is an intermediate, since it is produced and consumed

d)

D is NOT a catalyst, since it is consumed

A + B = C

C + D = E + F

A+B+D = E+ F

from the overall reaction, D is a reactant

e)

overal balance, as stated before, is

A+B+D = E+ F