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.
i forgot to enter the formula:
CO(g)+H2O(g) = CO2(g)+H2(g)
If you still have trouble with this, please re-post at th top of the board and someone will help.
To calculate the value of the equilibrium constant (Kp), we can use the equation:
Kp = (P(CO2))^n / [(P(CO))^m * (P(H2O))^p * (P(H2))^q]
Where n, m, p, and q are the stoichiometric coefficients of CO2, CO, H2O, and H2 respectively in the balanced chemical equation.
Given the initial pressures:
P(CO(g)) = 0.5794 atm
P(H2O(g)) = 0.5662 atm
P(CO2(g)) = 0.7950 atm
P(H2(g)) = 0.2754 atm
And the equilibrium pressure of CO2:
P(CO2(g)) = 0.6830 atm
We need to determine the stoichiometric coefficients n, m, p, and q for the balanced chemical equation. Unfortunately, you haven't provided the chemical equation for the reaction involving CO2, CO, H2O, and H2.
Please provide the balanced chemical equation, and then I can help you calculate the equilibrium constant (Kp).