14. Consider the reaction 3A + B + C D + E where the rate law is defined as –(∆[A]/∆t) = k[A]2 [B][C]. An experiment is carried out where [B]0 = [C]0 = 1.00 M and [A]0 = 1.00 × 10-4 M. We also know that after 3.00 min of the reaction, [A]is 3.26 × 10-5 M. What will be the concentration of A after 10.0 min? (A) 1.27 × 10-5 M (B)2.5 × 10-6 M (C) 1.00 M (D) 2.50 × 10-5 M (E)7.90 × 10-5