JEE Exam > JEE Questions > An amount of solid NH4 HS is placed in a flas...
Start Learning for Free
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?
| FREE This question is part of | Download PDF Attempt this Test |
Most Upvoted Answer
An amount of solid NH4 HS is placed in a flask already containing ammo...
Free Test
FREE
| Start Free Test |
Community Answer
An amount of solid NH4 HS is placed in a flask already containing ammo...
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'.
Attention JEE Students!
To make sure you are not studying endlessly, EduRev has designed JEE study material, with Structured Courses, Videos, & Test Series. Plus get personalized analysis, doubt solving and improvement plans to achieve a great score in JEE.
|
Explore Courses for JEE exam
|
|
Top Courses for JEEView all
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?
Question Description
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?.
Solutions 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? in English & in Hindi are available as part of our courses for JEE.
Download more important topics, notes, lectures and mock test series for JEE Exam by signing up for free.
Here you can find the meaning of 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? defined & explained in the simplest way possible. Besides giving the explanation of
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?, a detailed solution 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? has been provided alongside types of 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? theory, EduRev gives you an
ample number of questions to practice 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? tests, examples and also practice JEE tests.
|
|
Explore Courses for JEE exam
|
|
Suggested Free Tests
Signup for Free!
Signup to see your scores go up within 7 days! Learn & Practice with 1000+ FREE Notes, Videos & Tests.
|
© EduRev
|
Education Revolution
|
Follow Us
|
Signup to see your scores
go up within 7 days!
Access 1000+ FREE Docs, Videos and Tests
Takes less than 10 seconds to signup