Consider the Reaction 3A + B + C $\to$ D + E Where the Rate Law Is Defined as

Multiple Choice

Consider the reaction 3A + B + C $\to$ D + E where the rate law is defined as .
An experiment is carried out where [B]₀ = [C]₀ = 1.00 M and [A]₀ = 1.00 $\times$ 10^-4 M.
-After 3.00 minutes,[A] = 3.26 $\times$ 10^-5 M.The value of k is

A) 6.23 $\times$ 10^-3 L³/mol³·s
B) 3.26 $\times$ 10^-5 L³/mol³·s
C) 1.15 $\times$ 10² L³/mol³·s
D) 1.00 $\times$ 10⁸ L³/mol³·s
E) none of these