Consider the reaction:

2A₃ 3A₂

The reaction rate was studied experimentally. It was observed that if the initial concentration of A₃ was doubled, the reaction rate was 4 times higher and that when the A₂ concentration is halved, the velocity of the reaction doubles.

The following mechanism was proposed for this reaction:

A₃ A₂+A (Quick step)

A₃ + A A₂+A₂ (Slow Step)

The reverse reaction of the second step is very slow.

(a) Write the experimental rate law, indicating the order of reaction for each species and the total order of reaction. Show the reasoning

(b) What will be the effect on the reaction rate if the initial concentration of A₃ is multiplied by 1.5 and the initial concentration of A₂ by 3?

(c) The proposed mechanism is in according to the observed experimental rate law? make the deduction of speed law from the proposed mechanism to justify the answer.

(d) What is the unit of the rate constant?