K p at a certain temperature for PCl₅ PCl 3 (g) + Cl₂ (g), is 4.0 10 - 2 . PCl₅ is placed into a 1.0 L flask. At equilibrium the partial pressure of PCl 3 = 0.15 atm. What is the partial pressure of PCl₅ ?

Question

Quizplus · Accepted Answer

Using the equilibrium constant expression for the given reaction:

Kp = (PCl3) / (PCl2) * (Cl2)

where (PCl3) is the partial pressure of PCl3 and (PCl2) and (Cl2) are the partial pressures of PCl2 and Cl2, respectively.

Since the partial pressure of PCl3 at equilibrium is 0.15 atm, we can substitute this value into the equilibrium constant expression:

4.0 x 10^-2 = 0.15 / (PCl2) * (Cl2)

Assuming x is the partial pressure of PCl2 and Cl2 at equilibrium, we can set up the following equation:

4.0 x 10^-2 = 0.15 / x^2

Rearranging and solving for x, we get:

x = 0.56 atm

Therefore, the partial pressure of PCl2 is 0.56 atm and the answer is choice B.

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