At 850 C, the equilibrium constant Kp for the reaction:
C(s)+CO2(g) >< 2CO(g)
has a value of 10.7. If the total pressure in the system at equilibrium is 1.000 atm, what is the partial pressure of carbon monoxide.
.937
To find the partial pressure of carbon monoxide (CO) at equilibrium, we can use the equilibrium constant expression:
Kp = (Pco)² / (Pco2 * Pc)
Where:
Pco = partial pressure of carbon monoxide
Pco2 = partial pressure of carbon dioxide
Pc = partial pressure of carbon
Given:
Kp = 10.7
Total pressure (Ptotal) = 1.000 atm
Since the reaction is C(s) + CO2(g) <--> 2CO(g), the partial pressure of carbon dioxide (Pco2) can be assumed to be negligible compared to the other pressures because it is a solid. Therefore, we can disregard Pco2 in our calculations.
Now let's solve for the partial pressure of carbon monoxide (Pco):
Kp = (Pco)² / (Pco2 * Pc)
10.7 = (Pco)² / (Pco2 * Pc)
10.7 = (Pco)² / (0 * Pc) // Pco2 is negligible
10.7 = (Pco)² / 0
Since division by zero is undefined, this means that the partial pressure of carbon monoxide (Pco) is zero.
Therefore, the partial pressure of carbon monoxide at equilibrium is zero.
To find the partial pressure of carbon monoxide (CO) at equilibrium, we can use the equilibrium constant expression and the given total pressure of the system.
The equilibrium constant expression for the reaction is:
Kp = (PCO)^2 / (PCO2 * PC)
Where PCO represents the partial pressure of carbon monoxide, PCO2 represents the partial pressure of carbon dioxide, and PC represents the partial pressure of carbon (in this case, solid carbon is considered to have a partial pressure of 1).
We are given:
Kp = 10.7 (equilibrium constant)
Ptotal = 1.000 atm (total pressure of the system)
To find the partial pressure of CO, we can rearrange the equilibrium constant expression as follows:
(PCO)^2 = Kp * (PCO2 * PC)
Since PC = 1 (given), we can simplify the equation further:
(PCO)^2 = Kp * PCO2
Taking the square root of both sides, we get:
PCO = √(Kp * PCO2)
Now we can substitute the values into the equation:
PCO = √(10.7 * PCO2)
To get the partial pressure of CO, we need to know the partial pressure of CO2 (PCO2). Unfortunately, the partial pressure of CO2 is not given in the question. So, without that information, we cannot determine the partial pressure of carbon monoxide.