Explanation:
A + B + C → D
Given rate law of the reaction :
[tex]R=k[A]^2[B][/tex]
a) Rate of the reaction if [A] is doubled = R'
[tex]R'=k[2A]^2[B]=4k[A]^2[B][/tex]
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'
[tex]R'=k[A]^2[\frac{B}{4}]=0.25k[A]^2[B][/tex]
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 :
[tex]R'=k[A]^2[B][/tex]
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:
[tex]R=k[A]^2[B][/tex]
[tex]k=\frac{R}{[A]^2[B]}[/tex]
