An amount of solid NH_(4)HSis placed in a flask already containing ammonia gas at a certain temperature and 1.0 atm pressure. Ammonium hydrogen sulphide decomposes to yield NH_(3)and H_(2)Sgases in the flask. When the decomposition reaction reaches equilibrium, the total pressure in the flask rises to 2 atm. What will be the equilibrium constant for NH_4HS decomposition at this temperature?

An amount of solid NH_(4)HSis placed in a flask already containing amm

1.	An amount of solid NH_(4)HSis placed in a flask already containing ammonia gas at a certain temperature and 1.0 atm pressure. Ammonium hydrogen sulphide decomposes to yield NH_(3)and H_(2)Sgases in the flask. When the decomposition reaction reaches equilibrium, the total pressure in the flask rises to 2 atm. What will be the equilibrium constant for NH_4HS decomposition at this temperature?
Answer» <P> SOLUTION :`underset("initial At. EQN")(NH_(4)HS(s)) X atm)(H_(2)S)(g)` Then, `1.0 + x + x=2x+1.0=2.0` (given) `rArr x=0.5` atm `P_(NH-(3)) =1.0 + 1.5 1.5 atm, p-(H_(2)S) = 0.5 atm^(2)` `0.75 atm^(2)`