Problem 5I 25 ICE Table Help

[Lilly Catarozoli 1B]

In this problem, the initial concentrations are given for both of the reactants (SO2 and NO2) and one of the products (SO3 but NOT NO). How would you set up an ICE table for this reaction? For the reactants, would it still be -x, -x, and for the products +x, and +x? Or would this change because the product has an inital concentration? Thanks!

[Lilly Catarozoli 1B]

The question is: "A reaction mixture is prepared by mixing 0.100 mol SO2, 0.200 mol NO2, 0.100 mol NO, and 0.150 mol SO3 in
a 5.00-L reaction vessel. The reaction SO2(g) NO2(g) --> NO(g) SO3(g) is allowed to reach equilibrium at 460 C, when Kc 85.0. What is the equilibrium concentration of each substance?"

[RDove_3G]

The ice box process is still the same but you will have initial concentration values. I suggest using the moles given to find the current/initial concentrations and using that to calculate Q and compare to K. Then you will be able to see which direction the reaction is shifted so you know which initial values will have -x or +x. Once you know that you just have to set up the equilibrium expression and you will have to use a quadratic to solve for x.

[arisawaters2D]

So to clarify, when the question doesn't explicitly state what is being produced, we have to find the direction of the reaction first by calculating Q? I was confused at first by the problem wording because it just says everything is mixed in a vessel.