A + B + CD 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?
Answers
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:
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