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An amount of solid NH4HS is placed in a flask already containing ammonia gas at a certain temperature and 0.50 atm pressure. Ammonium hydrogen sulphide decomposes to yield NH3 and H2S gases in the flask. When the decomposition reaction reaches equilibrium, the total pressure in the flask rises to 0.84 atm? The equilibrium constant for NH4HS decomposition at this temperature is
- 0.11
- 0.17
- 0.18
- 0.30
Correct answer: 0.11
Solution
The equilibrium constant is calculated using the partial pressures of the gases at equilibrium. Given that the total pressure increased to 0.84 atm and the initial pressure of NH3 was 0.50 atm, the change in pressure due to the decomposition of NH4HS allows us to derive the equilibrium constant, which is found to be 0.11.
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