Question

At 1200 K the partial pressures of an equilibrium mixture of H₂S, H₂, and S are 0.020, 0.045, and 0.030 atm, respectively. Calculate the value of the following equilibrium constant at 1200 K.

H₂S(g) ⥨ H₂(g) + S(g) Kp = ?

Answer 1

The equilibrium constant, Kp, for the given reaction at 1200 K is 0.0675.

Step-by-step explanation:

To calculate the equilibrium constant for the reaction:
H₂S(g) ⥨ H₂(g) + S(g)
at 1200 K, we can use the given partial pressures of the gases in the equilibrium mixture. The equilibrium constant, Kp, is calculated by dividing the product of the partial pressures of the products by the product of the partial pressures of the reactants.

Kp = (P(H₂) * P(S)) / P(H₂S)

Plugging in the given values:

Kp = (0.045 * 0.030) / 0.020 = 0.0675

Therefore, the value of the equilibrium constant, Kp, at 1200 K is 0.0675.