The following equilibrium partial pressures were measured at 750 deg C. PH2=0.387atm,PCO2=0.152atm,PCO= 0.180 atm,and PH2O=0.252atm. What is the value of the equilibrium constant Kp for the reaction?
H2+CO2 ====CO+H2O
See your other post below on solving for Kc. This is just a substitution problem. Substitute partial pressures and solve for Kp.
To find the value of the equilibrium constant, Kp, for the reaction, you can use the equation that relates the partial pressures of the reactants and products at equilibrium.
The general equation is:
Kp = (P_CO * P_H2O) / (P_H2 * P_CO2)
You are given the equilibrium partial pressures:
PH2 = 0.387 atm
PCO2 = 0.152 atm
PCO = 0.180 atm
PH2O = 0.252 atm
Substitute these values into the equation to find the value of Kp:
Kp = (0.180 * 0.252) / (0.387 * 0.152)
Kp = 0.04536 / 0.058824
Kp ≈ 0.771
Therefore, the value of the equilibrium constant, Kp, for the given reaction at 750°C is approximately 0.771.