the initial pressure of phosgene gas (COCl2), was 1.31 atm. it was heated, and at equilibrium the pressure of CO was found to be .547 atm. what are the equilibrium pressures of Cl2 and COCl2? CO +Cl2=COCl2
i've done it twice and keep getting the wrong answer
If you show your work perhaps we can find the error.
ОКлЭ
To find the equilibrium pressures of Cl2 and COCl2, we can use the concept of the equilibrium constant (Kp) and the stoichiometry of the balanced chemical equation.
The given balanced chemical equation is:
CO + Cl2 ⇌ COCl2
From the equation, we can see that:
- The coefficient of CO is 1.
- The coefficient of Cl2 is 1.
- The coefficient of COCl2 is 1.
We are given the initial pressure of phosgene gas (COCl2), which is 1.31 atm, and the pressure of CO at equilibrium, which is 0.547 atm.
Let's assume the equilibrium pressure of Cl2 is x atm, and the equilibrium pressure of COCl2 is also x atm.
Using the ideal gas law, the equation relating pressure, volume, and moles of gas is:
PV = nRT
Since the number of moles (n), temperature (T), and volume (V) remain constant, we can write:
P1/P2 = (n1/n2)
We can set up an expression for the equilibrium constant (Kp) using the partial pressures of the gases:
Kp = (P(COCl2)/P(CO))^1 * (P(COCl2)/P(Cl2))^1
At equilibrium, the pressure of COCl2 is x atm, and the pressure of CO is 0.547 atm. Substituting these values, we get:
Kp = (x/0.547)^1 * (x/x)^1 = (x/0.547)^1
The equilibrium constant (Kp) for this reaction can be provided in the question or you can calculate it using the given data or other known values.
Now, the expression for Kp for this reaction is:
Kp = (P(Cl2))^1 * (P(COCl2))^1 = (x)^1 * (x)^1 = x^2
Since we know the equilibrium pressure of CO is 0.547 atm, and the initial pressure of COCl2 is 1.31 atm (which will be the equilibrium pressure of COCl2), we can rewrite the expression for Kp as:
Kp = (0.547)^1 * (1.31)^1 = 0.547 * 1.31
Now, we can solve for x by setting up the equation:
Kp = x^2 = (0.547)(1.31)
To solve for x, take the square root of both sides of the equation:
√(x^2) = √((0.547)(1.31))
Simplifying the equation, we get:
x = √(0.547)(1.31)
Calculating this expression will give you the equilibrium pressure (x) for both Cl2 and COCl2.
Make sure that you substitute the obtained equilibrium pressure for x in the corresponding equation to check if it satisfies the given condition of the initial pressure. If it does, then you have the correct answer for the equilibrium pressures of Cl2 and COCl2.