Consider a reaction given by: 2A + BC + 2D
with a rate law of r = (1/2)d[A]/dt = k[A]^2 and k = 6.17 × 10^2 dm^3 mol^−1 s^−1. The reaction is run with initial concentrations of [A]₀ = 1.20 M, [B]₀ = 0.900 M, [C]₀ = 0.0, and [D]₀ = 0.
b) How long will it take for the A concentration to reach 0.050 M?
c) What are [A], [B], [C], and [D] after 10.0 seconds?