At 25° C the reaction has Kp = 0.120. A 5.00-L flask is charged with 0.300 g of...

At 25° C the reaction

has K_p = 0.120. A 5.00-L flask is charged with 0.300 g of pure H₂S(g) at 25 °C. Solid NH4HS is then added until there is excess unreacted solid remaining. (a) What is the initial pressure of H₂S(g) in the flask? (b) Why does no re-action occur until NH₄H_S is added? (c) What are the partial pressures of NH₃ and H₂S at equilibrium? (d) What is the mole fraction of H₂S in the gas mixture at equilibrium? (e) What is the minimum mass, in grams, of NH₄HS that must be added to the flask to achieve equilibrium?