Question

At T = 250 °C the reaction PCl5(g) PCl3(g) + Cl2(g) has an equilibrium constant in terms of pressures Kp = 2.15. (a) Suppose the initial partial pressure of PCl5 is 0.548 atm, and PPCl3 = PCl2 = 0.780 atm. Calculate the reaction quotient Qp and state whether the reaction proceeds to the right or to the left as equilibrium is approached

Answer 1

To the right

Step-by-step explanation:

Step 1: Given data

• Partial pressure of PCl₅ (pPCl₅) = 0.548 atm

• Partial pressure of PCl₃ (pCl₃) = 0.780 atm

• Partial pressure of Cl₂ (pCl₂) = 0.780 atm

Step 2: Write the balanced equation

PCl₅(g) ⇄ PCl₃(g) + Cl₂(g)

Step 3: Calculate the pressure reaction quotient

`Q_p = (pPCl_3 * pCl_2 )/(pPCl_5) = (0.780 * 0.780 )/(0.548) =1.11`

Step 4: Determine whether the reaction proceeds to the right or to the left as equilibrium is approached

Since Qp < Kp, the reaction will proceed to the right to attain the equilibrium.