Question

3. A key step in the extraction of iron from its ore is FeO(s) + CO(g) ⇋ Fe(s) + CO2(g) Kp =0.403 at 1000°C. What are the equilibrium partial pressures off carbon monoxide and carbon dioxide when 1.00 atm of carbon monoxide and excess iron(II) oxide react in a sealed container at 1000°C.

Answer 1

Answer:

pCO = 0.713 atm

pCO2 = 0.287 atm

Explanation:

 

The partial equilibrium constant (Kp) characterizes the equilibrium in a function of the partial pressures of the gas substances. The partial pressure is the pressure that the gas would have if it was alone in the same container and at the same conditions. The equilibrium represents a moment in which the partials pressures and the concentrations of the substances remain constant.

Kp is the ratio of the multiplication of the partial pressure of the products by the reagents, each one elevated by the coefficient of the substance, thus, for the reaction given let's do an equilibrium chart to discover the equilibrium partial pressures:

FeO(s) + CO(g) ⇄ Fe(s) + CO₂(g)

           1.00 atm                 0        Initial

               -x                        +x       Reacts (stoichiometry is 1:1)

           1.00-x                      x        Equilibrium

$Kp = \frac{pCO_2}{pCO} \\\\0.403 = \frac{x}{1.00-x} \\\\x = 0.403 - 0.403x\\ \\1.403x = 0.403\\\\x = 0.287 atm$

Thus, at equilibrium

pCO = 1.00 - 0.287 = 0.713 atm

pCO2 = 0.287 atm