Verified answer

Kp=0.0611 at 2000 K

This was provided in the question.

CO(g) + H2O(g) ⇌ CO2(g ) + H2(g)

Kp = (P(products))/(P(reactants)) = ((P(CO2))*(P(H2)))/((P(CO))*(P(H2O)))

Set up an ICE table:

Cmpd...Initial...Change...Equil...

CO.......1326......-x........(1326-x) ...

H2O.......1772....-x........(1772-x)....

CO2.......0..........+x...........x

H2..........0...........+x..........x

Substitute these Equil values into the Kp expression.

Kp = ((x)*(x))/((1326-x)*(1772-x)) = 0.0611

Multiply this out to obtain a quadratic equation

((x)*(x))/((1326-x)*(1772-x)) = 0.0611

x^2 = 0.0611*((1326-x)*(1772-x)) = 0.0611*(2349672 - 3098x + x^2)

x^2 = 143564.96 - 189.2878x + 0.0611x^2

0.9389x^2 + 189.2878x - 143564.96 = 0

Using the quadratic formula, we solve this for x: The negative root is a negative number which is not realistic and is discarded. The positive root gives

x = 303 Torr (to three sig figs)

From the ICE table, we see that this is the partial pressure for CO2 at equilibrium:

P(CO2) = x = 303 Torr

"J", I'd really like to help you, but you need the Equilibrium constant to solve this problem. If you ask it again and include Keq and I see it, I'll be glad to run through it with you.