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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:
  • a)
    0.11
  • b)
    0.17
  • c)
    0.18
  • d)
    0.30
Correct answer is option 'A'. Can you explain this answer?
Most Upvoted Answer
An amount of solid NH4HS is placed in a flask already containing ammo...

Equilibrium Constant Calculation:
- The equilibrium constant (Kp) can be calculated using the formula: Kp = (P(NH3) * P(H2S)) / P(NH4HS)
- Initially, only NH3 is present in the flask, so P(NH3) = 0.50 atm and P(H2S) = 0 atm
- When equilibrium is reached, the total pressure is 0.84 atm, so P(NH4HS) = 0.84 - 0.50 = 0.34 atm
- Substituting these values into the formula gives: Kp = (0.50 * 0) / 0.34 = 0

Equilibrium Constant for NH4HS Decomposition:
- The equilibrium constant for the decomposition of NH4HS can be represented as: NH4HS ⇌ NH3 + H2S
- The expression for the equilibrium constant is given by: Kp = (P(NH3) * P(H2S)) / P(NH4HS)
- At equilibrium, the total pressure in the flask is 0.84 atm, which means NH3 and H2S are both present
- Since the initial pressure of NH3 is 0.50 atm, the pressure of H2S can be calculated as: 0.84 - 0.50 = 0.34 atm
- Substituting these values into the equilibrium constant expression gives: Kp = (0.50 * 0.34) / 0.34 = 0.50

Therefore, the equilibrium constant for NH4HS decomposition at this temperature is 0.50, which corresponds to option 'A'.
Free Test
Community Answer
An amount of solid NH4HS is placed in a flask already containing ammo...
Total pressure at equilibrium
= 0.5 + x + x = 0.84
∴ x = 0.17 atm
= 0.67 × 0.17 = 0.114 atm.
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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:a)0.11b)0.17c)0.18d)0.30Correct answer is option 'A'. Can you explain this answer?
Question Description
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:a)0.11b)0.17c)0.18d)0.30Correct answer is option 'A'. Can you explain this answer? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about 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:a)0.11b)0.17c)0.18d)0.30Correct answer is option 'A'. Can you explain this answer? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 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:a)0.11b)0.17c)0.18d)0.30Correct answer is option 'A'. Can you explain this answer?.
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