Significant fig help?

For the reaction below, Kc = 0.534 at 700 degrees Celsius. A mixture of 0.250 moles of CO and 0.450 moles of H20 are heated to 700 degrees Celsius in a 10.0 L container. Calculate the concentrations of all four species when equilibirium is reached.



H2 + CO2 ---%26gt; H20 + CO



I'm pretty sure everything is right im just not sure about a couple of significant digits, so if anyone can help it would be appreacited.



first I got the Molarity of CO - .250 moles/10L = .025M and

H20 .450 moles/10L = .045 M



next I did the ICE method to come up with the problem (.025-x)(.045-x)/x^2=0.534



I work this out to get it equal to 0 and it looks like:

.466x^2-.070x+.0011=0



should it be .001125?



I use the solve function on my calculator, And this gives me x=.0183 so, if everything is correct then the concentrations should be:



CO = .025-.018 = .007

H20 = .045-.018 = .027

H2 =.018

CO2 = .018



How does this look? Just want to know that im doing this right...Im not sure if x should be .018 or .0183 Thanks

Significant fig help?
.0183 because you need 3 significant figures