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:

the economic difference between the three colonial regions. shipbuilding, whaling, fishing, and trapping where also main factors to the economy. the southern regional colonies economy was based on sugarcane, rice, cotton, tobacco, and indigo.

answer; beware of exaggerated claims without supporting evidence;