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An amount of solid NH4 HS 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?
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Given:
- Initial pressure of ammonia gas (NH3) = 0.50 atm
- Total pressure at equilibrium = 0.84 atm
To determine the equilibrium constant (K) for the decomposition reaction of ammonium hydrogen sulphide (NH4HS), we can use the ideal gas law and the concept of partial pressures.
1. Write the balanced chemical equation for the decomposition of NH4HS:
NH4HS ⇌ NH3 + H2S
2. Let's assume that the initial number of moles of NH4HS is 'x'.
Therefore, the partial pressure of NH4HS at equilibrium is (0.50 - x) atm.
3. According to the balanced equation, 1 mole of NH4HS decomposes to yield 1 mole of NH3 and 1 mole of H2S.
So, at equilibrium, the number of moles of NH3 and H2S will also be 'x'.
4. The partial pressure of NH3 at equilibrium is x atm.
Similarly, the partial pressure of H2S at equilibrium is also x atm.
5. The total pressure at equilibrium is given as 0.84 atm.
Therefore, we can write the equation: (0.50 - x) + x + x = 0.84
6. Simplifying the equation, we get: 0.50 + x = 0.84
Solving for x, we find: x = 0.34
7. Now, substitute the value of x in the equation for partial pressures:
Partial pressure of NH4HS = 0.50 - x = 0.50 - 0.34 = 0.16 atm
Partial pressure of NH3 = x = 0.34 atm
Partial pressure of H2S = x = 0.34 atm
8. The equilibrium constant (K) is defined as the ratio of the product of partial pressures of the products to the product of partial pressures of the reactants, each raised to the power of their respective stoichiometric coefficients.
K = (P(NH3) * P(H2S)) / P(NH4HS)
= (0.34 * 0.34) / 0.16
= 0.1156 / 0.16
≈ 0.11
Therefore, the equilibrium constant (K) for the decomposition of NH4HS at this temperature is approximately 0.11, which corresponds to option 'A'.
- Initial pressure of ammonia gas (NH3) = 0.50 atm
- Total pressure at equilibrium = 0.84 atm
To determine the equilibrium constant (K) for the decomposition reaction of ammonium hydrogen sulphide (NH4HS), we can use the ideal gas law and the concept of partial pressures.
1. Write the balanced chemical equation for the decomposition of NH4HS:
NH4HS ⇌ NH3 + H2S
2. Let's assume that the initial number of moles of NH4HS is 'x'.
Therefore, the partial pressure of NH4HS at equilibrium is (0.50 - x) atm.
3. According to the balanced equation, 1 mole of NH4HS decomposes to yield 1 mole of NH3 and 1 mole of H2S.
So, at equilibrium, the number of moles of NH3 and H2S will also be 'x'.
4. The partial pressure of NH3 at equilibrium is x atm.
Similarly, the partial pressure of H2S at equilibrium is also x atm.
5. The total pressure at equilibrium is given as 0.84 atm.
Therefore, we can write the equation: (0.50 - x) + x + x = 0.84
6. Simplifying the equation, we get: 0.50 + x = 0.84
Solving for x, we find: x = 0.34
7. Now, substitute the value of x in the equation for partial pressures:
Partial pressure of NH4HS = 0.50 - x = 0.50 - 0.34 = 0.16 atm
Partial pressure of NH3 = x = 0.34 atm
Partial pressure of H2S = x = 0.34 atm
8. The equilibrium constant (K) is defined as the ratio of the product of partial pressures of the products to the product of partial pressures of the reactants, each raised to the power of their respective stoichiometric coefficients.
K = (P(NH3) * P(H2S)) / P(NH4HS)
= (0.34 * 0.34) / 0.16
= 0.1156 / 0.16
≈ 0.11
Therefore, the equilibrium constant (K) for the decomposition of NH4HS at this temperature is approximately 0.11, which corresponds to option 'A'.
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An amount of solid NH4 HS 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 isa)0.11b)0.17c)0.18d)0.30Correct answer is option 'A'. Can you explain this answer?
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An amount of solid NH4 HS 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 isa)0.11b)0.17c)0.18d)0.30Correct answer is option 'A'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about An amount of solid NH4 HS 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 isa)0.11b)0.17c)0.18d)0.30Correct answer is option 'A'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for An amount of solid NH4 HS 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 isa)0.11b)0.17c)0.18d)0.30Correct answer is option 'A'. Can you explain this answer?.
An amount of solid NH4 HS 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 isa)0.11b)0.17c)0.18d)0.30Correct answer is option 'A'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about An amount of solid NH4 HS 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 isa)0.11b)0.17c)0.18d)0.30Correct answer is option 'A'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for An amount of solid NH4 HS 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 isa)0.11b)0.17c)0.18d)0.30Correct answer is option 'A'. Can you explain this answer?.
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