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.

> b takes place in the gas phase in an isothermal tubular reactor. the feed is one mole of a per one mole of c, an inert. the entering temperature and pressure are 427°c and 10 atm, respectively. the gas constant r = 0.08206 atm · l/mol · k.