[Marcus Soutlo]

If 1.00 mol each of carbon dioxide and hydrogen is initially injected into a 10.0-L reaction chamber at 986 degrees Celsius, what would be the concentrations of each entity at equilibrium?

CO2(g) + H2(g) „²„³ CO(g) + H2O(g) k = 1.60 for 986 degrees Celsius
Heres my work:

C = n/v
= 0.1 mol/L
CO2(g) + H2(g) „²„³ CO(g) + H2O(g)
I 0.1 0.1 0 0
C -x -x +x +x
E 0.1-x 0.1-x x x

Keq = [CO][H2O]/[CO2][H2]

1.60 = x(x)/(0.1 -x)(0.1 ¡V x)

This is the part I am stuck with please help thanks a lotƒº 

[Rabn]

Do any of the species present exist in their standard state? i.e. H2O liquid is not included in the equilibrium equation. (HUGE CLUE) How do you treat gases in equilibrium equations? i.e. a weak acid has units of moles/liter in equilibrium equations and is a concentration.