For the Following Reaction

For the following reaction:
2 NOCl(g) 2 NO(g) + Cl₂(g)     K_c = 5.6 x 10^-6 (at 400 K)

If (NOCl) = 0.0222 M, (Cl₂) = 0.0222 M, and (NO) = 0.989
M at some moment in time, we can conclude that

A) the reaction is at equilibrium.
B) some of the NOCl must be converted to NO and Cl₂ to reach equilibrium.
C) some of the NO and Cl₂ must be converted to NOCl to reach equilibrium.
D) it is impossible to determine which way the reaction must go to reach equilibrium.
E) the reaction can never reach equilibrium.