Consider the reaction

                        3A + B + C -> D + E

            where the rate law is defined as

                        Rate = k[A]²[B][C]

            An experiment is carried out where [B]₀ = [C]₀ = 1.00 M and [A]₀ = 1.00 x 10^–4 M.

After 3.00 minutes, [A] = 3.26 x 10^–5 M. The value of k is

The first-order reaction of A molecules (gray spheres) occurs in three vessels, 1, 2, and 3, of equal volume.

If the volume of each vessel is increased by a factor of 2, what will happen to the rates and half-lives of the reaction?

A first-order reaction is 45% complete at the end of 35 minutes.  What is the length of the half-life of this reaction?