Question

A + B + CD is:
a. How will the reaction rate change if [A] is doubled?

The reaction rate will increase.

Rate = k[A]2[B]
b. How will the reaction rate change if [B] is decreased to 1/4th of the initial concentration?

c. How will the reaction rate change if [C] is increased by 3times? What is the expected rate constant value for this experiment?

Answer 1

Step-by-step explanation:

A + B + C → D

Given rate law of the reaction :

`R=k[A]^2[B]`

a) Rate of the reaction if [A] is doubled = R'

`R'=k[2A]^2[B]=4k[A]^2[B]`

R' = 4 × R

The rate of the reaction will change by factor of 4.

b) Rate of the reaction if [B] is reduced to quarter = R'

`R'=k[A]^2[(B)/(4)]=0.25k[A]^2[B]`

R' = 0.25 × R

The rate of the reaction will change by factor of 0.25.

c) Rate of the reaction if [C] is increased by 3 times= R'

Rate law of the reaction :

`R'=k[A]^2[B]`

As we can see that [C] does not appears in rate law of the reaction, which means that rte of the reaction is independent of [C].

R' = R

The rate of the reaction will remain the same.

The expected rate constant value for this experiment:

`R=k[A]^2[B]`

`k=(R)/([A]^2[B])`