Calculate the time required for each of the following second-order reactions to take place:

(a) 2 A → B + C, for the concentration of A to decrease from 0.10 mol · L^–1 to 0.080 mol · L^–1, given that k_r = 0.015 L · mol^–1 · min^–1 for the rate law expressed in terms of the loss of A;

(b) A → 2 B + C, when [A]₀ = 0.15 mol · L^–1, for the concentration of B to increase to 0.19 mol · L^–1, given that k_r = 0.0035 L · mol^–1 · min^–1 in the rate law for the loss of A.