Consider the aqueous reaction:
Overall reaction: 2A(aq) + B(aq) → products
Mechanistic evidence suggests the following two-step pathway at 25 °C:
Step 1 (slow): A(aq) + B(aq) → C(aq)
Step 2 (fast): C(aq) + A(aq) → products
In one experiment the initial concentrations are [A]₀ = 0.10 M and [B]₀ = 0.20 M, producing an initial rate r₀.
(a) Determine the rate law predicted by the mechanism.
(b) Calculate the factor by which the initial rate changes when [A]₀ is doubled.
(c) Calculate the factor by which the initial rate changes when [B]₀ is tripled.
(d) Explain the difference between the factors obtained in parts (b) and (c).