Question

The reaction of iron(III) oxide with carbon monoxide is important in making steel. At 1000 K,...

The reaction of iron(III) oxide with carbon monoxide is important in making steel. At 1000 K, Kp=19.9 for the reaction Fe2O3(s) + 3CO(g) <-----> 2Fe(s) + 3CO2(g). What are the equilibrium partial pressures of CO and CO2 if CO is the only gas present initially, at a partial pressure of 0.978 atm?

Homework Answers

Answer #1

Solution :-

Balanced reaction equation

Fe2O3(s) + 3CO(g) <-----> 2Fe(s) + 3CO2(g).

In the Kp equation only gases state species are involved

Initial pressure of CO = 0.978 atm

Equilibrium pressured of CO and CO2 = ?

Kp=19.9

Lets make the ICE table

Fe2O3(s) + 3CO(g) <-----> 2Fe(s) + 3CO2(g).

0.978                                  0

-3x                                      +3x

0.978-3x                              3x

Kp = [CO2]^3 / [CO]^3

19.9 = [3x]^3/[0.978-3x]^3

19.9 = 27x^3 / [0.978-3x]^3

19.9* [0.978-3x]^3 = 27x^3

Solving this equation for the x

We get

X = 0.238

Therefore equilibrium pressure are as follows

[CO]eq = 0.978 atm – 3x = 0.978 atm – (3*0.238) = 0.264 atm

And

[CO2]eq = 3x = 3*0.238 atm = 0.714 atm

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