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

To the right

Explanation:

Step 1: Given data

Step 2: Write the balanced equation

PCl₅(g) ⇄ PCl₃(g) + Cl₂(g)

Step 3: Calculate the pressure reaction quotient

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.

a  solution  is always transparent, light passes through with no scattering from solute particles which are molecule in size. the  solution  is homogeneous and does not settle out. a colloid is intermediate between asolution  and a  suspension. while asuspension  will separate out a colloid will not.

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