posted by andy on .
I was having trouble with this problem. initial pressure for the compounds involved in the reaction displayed were determined to be P(CO(g)) = 0.5794 atm, P(H2O(g)) = 0.5662 atm, P(CO2(g)) = 0.7950 atm, P(H2(g)) = 0.2754 atm. Calculate the value of the equilibrium constant (Kp) at 1650 °C if the equilibrium pressure of CO2(g) was 0.6830 atm.
CO(g)+H2O(g) = CO2(g)+H2(g)
This looks straight forward to me. What is you trouble? What values do you have for the equilibrium concns?