Question

1. Given the equilibrium: SO2Cl2(g)  SO2(g) + Cl2(g) Kp = 3.60 at 125 °C Is this reaction at equilibrium under the following conditions. If the reaction is not at equilibrium state which direction it will go to reach equilibrium. a) PSO2CL2 = 0.568 atm, PSO2 = 0.125 atm, and PCl2 = 0.500 atm b) PSO2CL2 = 0.125 atm, PSO2 = 0.250 atm, and PCl2 = 1.200 atm c) PSO2CL2 = 0.108 atm, PSO2 = 0.500 atm, and PCl2 = 3.000 atm d) PSO2 = 0.500 atm and PCl2 = 0.500 atm

Answer 1

Given equilibrium reaction can be written as follows:

      Kp = 3.60

Expression for equilibrium constant Q for above reaction can be written as follows:

Where, P_SO2 = partial pressure of SO2

P_Cl2=partial pressure of Cl2

P_SO2Cl2= partial pressure of SO2Cl2

If Q = Kp then, reaction can be said to be at equilibrium.

If Q > Kp then, concentration of product is very high and reaction moves from right (products) to left(reactants) in order to reach equilibrium.

If Q < Kp then, concentration of reactants is very high and reaction moves from left (reactant) to right(products) in order to reach equilibrium.

Ans a)

Q = (0.125 atm x 0.500atm) / 0.568 atm

Q = 0.11

Thus, Q < Kp. Therefore, reaction is not at equilibrium and it will move from left (reactant) to right(products) in order to reach equilibrium.

Ans b)

Q = (0.250atm x 1.200 atm) / 0.125 atm

Q = 2.40

Thus, Q < Kp. Therefore, reaction is not at equilibrium and it will move from left (reactant) to right (products) in order to reach equilibrium.

Ans c)

Q = (0.500atm x 3.000atm) / 0.108 atm

Q = 13.9

Thus, Q > Kp. Therefore, reaction is not at equilibrium and it will move right (products) to left(reactants) in order to reach equilibrium.

Ans d)

Q = (0.500atm x 0.500atm) /Pso2cl2

Q = 0.25 atm / Pso2Cl2

In order to find the state of reaction, value of PSO2Cl2 is required.