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?

Explanation:

A + B + C → D

Given rate law of the reaction :

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

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' = 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 :

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:

i'll just take the points xd

answer; negative punishment;