[defang01]

Here is the question:

The equilibrium constant for the reaction 2BrCl (g) = Br2 (g) + Cl2 (g) is 32 at 500 K. A mixture of BrCl, Br2 and Cl2 each at 0.050 M, was introduced into a container at 500 K. Which of following is true?

The answer is B) the system is at equilibrium and therefore no net change occurs.  

But I think D) The reaction proceeds to the right, forming more products   is correct.

Shouldn't the reaction proceed until (Br2)x(Cl2) / (BrCl)^2 equals to 32, which means the reaction will proceed to the right?  

Can anyone tell me which choice is correct?

THANKS

[Demotivator]

You're right. D.