Question

NH4HS+s)=NH3(g)+H2S(s) The equilibrium pressure at 25°C is 0.66 atm.What is the Kp for the reaction?

Answer 1

Given,

NH₄HS (s) ⇔ NH₃ (g) + H₂S (g)

In the equilibrium mixture, the partial pressure (P) of the solid reactant, (NH₄HS) = 0

∴ Equilibrium constant at partial pressure, Kp = P(NH₃) × P(H₂S)................(i)

As per question, total pressure = 0.66 atm

                     ⇒ P(NH₃) + P(H₂S) = 0.66 atm

                     ⇒ P(NH₃) = P(H₂S) = 0.33 atm , (∵ Molar ratio NH₃:H₂S = 1:1 )

From equation (i),

Kp = 0.33 atm × 0.33 atm

    = 0.11 atm²

Answer 2

Answer:

Given,

NH₄HS (s) ⇔ NH₃ (g) + H₂S (g)

In the equilibrium mixture, the partial pressure (P) of the solid reactant, (NH₄HS) = 0

∴ Equilibrium constant at partial pressure, Kp = P(NH₃) × P(H₂S)................(i)

As per question, total pressure = 0.66 atm

                    ⇒ P(NH₃) + P(H₂S) = 0.66 atm

                    ⇒ P(NH₃) = P(H₂S) = 0.33 atm , (∵ Molar ratio NH₃:H₂S = 1:1 )

From equation (i),

Kp = 0.33 atm × 0.33 atm

   = 0.11 atm²

Explanation: