The equilibrium constant for the reaction
PCl3(g) + Cl2(g) ⇀↽ PCl5(g)
is 35000 at 760 ◦C. At equilibrium, the partial
pressure of PCl5 was 160 bar and that of
PCl3 was 9.85 bar. Calculate the equilibrium
partial pressure of Cl2.
Answer in units of bar.
To calculate the equilibrium partial pressure of Cl2, we can use the equilibrium constant expression and the given partial pressures of PCl5 and PCl3.
The equilibrium constant expression for the given reaction is:
Kp = ([PCl5] / [PCl3][Cl2])
Where [PCl5], [PCl3], and [Cl2] are the partial pressures of PCl5, PCl3, and Cl2, respectively.
We also know that the equilibrium constant (Kp) is given as 35000.
Given partial pressures:
[PCl5] = 160 bar
[PCl3] = 9.85 bar
Let's assume the equilibrium partial pressure of Cl2 is 'p' bar.
Now, we can substitute the given values and 'p' into the equilibrium constant expression and solve for 'p':
35000 = (160 / (9.85 * p))
To solve for 'p', we can rearrange the equation:
35000 * 9.85 * p = 160
p = 160 / (35000 * 9.85)
p ≈ 0.000459 bar
Therefore, the equilibrium partial pressure of Cl2 is approximately 0.000459 bar.