when CO2 (.15mol) and H2 (.302g) in a 500L vessel at 576'C are allowed to come to equilibrium the mixture contains .000183 mol/L of H20. what is the equilibrium concentration of CO?

CO2 + H2 --> <-- CO +H2O

The equilibrium concentration of H2O = the equilibrium concentration of CO, does it not? Starting from scratch, with zero mol CO and zero mol H2O, 1 mol CO is formed for each 1 mol H2O formed. Check my thinking.

Based on the given reaction equation, CO2 + H2 ⇌ CO + H2O, it is clear that the equilibrium concentration of H2O would be equal to the equilibrium concentration of CO, assuming the reaction has reached equilibrium.

To determine the equilibrium concentration of CO (COeq), we can use the information provided regarding the initial amount of CO2, H2, and the equilibrium concentration of H2O.

First, we need to calculate the number of moles of H2O formed:

Given:
Equilibrium concentration of H2O (H2Oeq) = 0.000183 mol/L
Volume of the vessel (V) = 500 L

Number of moles of H2O (nH2O) = H2Oeq * V
= 0.000183 mol/L * 500 L
= 0.0915 mol

Since the reaction equation shows that 1 mol of CO is formed for each 1 mol of H2O, the equilibrium concentration of CO (COeq) would also be equal to 0.0915 mol/L.

Therefore, the equilibrium concentration of CO is 0.0915 mol/L.