Answer to Question #263497 in General Chemistry for Jjjj

Question

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

This step occurs in the 700°C to 1200°C zone within a blast fur-

nace. What are the equilibrium partial pressures of CO(g) and

CO2(g) when 1.00 atm of CO(g) and excess FeO(s) react in a

sealed container at 1000°C?

Answer 1

Equilibrium pressure is follows as:

$K_p = \frac{P(CO_2)}{P(CO)} \\ K_p = 0.403$

As the reaction proceeds, it attains equilibrium and hence the equilibrium pressure can be determined using ICE table.

Equilibrium partial pressures of CO(g) and CO₂ (g) can be determined substituting values from the ICE table in the equation for K_p

$K_p = \frac{x}{2.05-x}=0.403 \\ x = 0.589$

Equilibrium partial pressure of CO = (2.05 -x) = (2.05 -0.589) = 1.46 atm

Equilibrium partial pressure of CO₂ = x = 0.589 atm