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Ammonium bisulfide, NH4HS, forms ammonia, NH3, and hydrogen sulfide, H2S, through the reaction NH4HS(s) ⇌ NH3(g) + H2S(g) This reaction has a Kp value of 0.120 at 25 degrees C. In addition to the H2S already present in the flask, solid NH4HS is added until there is excess unreacted solid remaining. What is the minimum mass of NH4HS that must be added to the 5.00-L flask when charged with the 0.450 g of pure H2S(g), at 25 °C to achieve equilibrium? Express your answer numerically in grams.