For the system
CO(g) + H2O(g)<-->CO2(g) + H2(g)
Kp is 1.6 at 900 K. If 0.400 atm CO(g) and 0.400 atm H2O(g) are combined in a sealed flask, what is the equilibrium partial pressure of CO2(g)?
To find the equilibrium partial pressure of CO2(g), we can use the equilibrium expression and the given equilibrium constant (Kp) value.
The equilibrium expression for the given reaction is:
Kp = (P_CO2 * P_H2) / (P_CO * P_H2O)
where P_CO2, P_H2, P_CO, and P_H2O represent the partial pressures of CO2(g), H2(g), CO(g), and H2O(g) respectively.
We are given that Kp = 1.6 and P_CO = 0.400 atm, and P_H2O = 0.400 atm. We need to find P_CO2.
Let's substitute the given values into the equilibrium expression:
1.6 = (P_CO2 * P_H2) / (0.400 * 0.400)
To find P_CO2, we can rearrange the equation:
P_CO2 = (1.6 * 0.400 * 0.400) / P_H2
Since the value of P_H2 is not given, we cannot directly calculate the exact value of P_CO2 using this equation alone. However, we can calculate P_CO2 in terms of P_H2 using this equation.
Please provide the value of P_H2 (partial pressure of H2) to proceed with the calculation and obtain the equilibrium partial pressure of CO2(g).