Am I setting up my ICE table and equation properly?

Hey guys. I posted this in the homework forum, and I am sort of in desperate need of a response. I understand if this post is deleted. So we just learned how to do ICE charts for equilibrium, and with this problem in particular I am having some difficulty..I don't know if I set the equation up properly. Thanks a bunch

A mixture of 0.546 mole of carbon monoxide and 0.407 mole of bromine was placed into a rigid 1.21-L container (i.e. these are initial amounts) and the system was allowed to come to equilibrium. The equilibrium concentration of COBr2 was 0.246 M. What is the value of Kc for this reaction? Use an ICE table to help you. Round your answer to three significant figures.

CO+Br2<----->COBr2

I .45124 .336364 0

C -X -X +X

E .45124-X .336364-X .246

(.246)/ (.45124-x)(.33636-x)=x

Solving for x I got: .9153 as Kc

Merged post follows:

Scratch that, found my mistake!