For the Equilibrium 2 NOBr(g) ⇄ 2 NO(g) + Br₂ $\lt$

For the equilibrium 2 NOBr(g) ⇄ 2 NO(g) + Br₂ (g) , K_c = 1.56 * 10^-3 at 300 K.Suppose 0.400 M NOBr is placed in a reaction vessel at 300 K.At a given point, the concentration of Br₂ is 0.0134 M.Which statement below is true?

A) Q $\lt$ K, so the reaction will continue to make more products.
B) Q $\gt$ K, so the reaction will consume products to make more reactants.
C) Q = K, so the system is at equilibrium.
D) The value of K will decrease until it is equal to Q.
E) The value of K will increase until it is equal to Q.