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Equal weights of CH4 and H2 are mixed in an empty container at 25oC. The fraction of the total pressure exerted by H2 is
- a)1/9
- b)1/2
- c)8/9
- d)16/17
Correct answer is option 'C'. Can you explain this answer?
Verified Answer
Equal weights of CH4 and H2 are mixed in an empty container at 25oC. T...
Let equal weights be w g.
Partial pressure = mole fraction × Total pressure
PH2 = 8/9 x Total pressure
Most Upvoted Answer
Equal weights of CH4 and H2 are mixed in an empty container at 25oC. T...
Given:
- Equal weights of CH4 and H2 are mixed in an empty container at 25°C.
To find:
- The fraction of the total pressure exerted by H2.
Solution:
1. Calculate the moles of each gas:
- Since the weights of CH4 and H2 are equal, we can assume that they have the same mass.
- The molar mass of CH4 (methane) is 16 g/mol, and the molar mass of H2 (hydrogen) is 2 g/mol.
- Therefore, the moles of CH4 and H2 will be the same when equal weights are taken.
2. Calculate the partial pressures of each gas:
- According to Dalton's law of partial pressures, the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of each gas.
- The partial pressure of a gas can be calculated using Dalton's law as the product of the mole fraction and the total pressure.
- Since the moles of CH4 and H2 are the same, their mole fractions will also be the same.
- Therefore, the mole fraction of H2 will be 1/2, and the mole fraction of CH4 will also be 1/2.
- Let the total pressure be P. The partial pressure of H2 will be (1/2)P, and the partial pressure of CH4 will also be (1/2)P.
3. Calculate the fraction of the total pressure exerted by H2:
- The fraction of the total pressure exerted by H2 can be calculated as the partial pressure of H2 divided by the total pressure.
- Therefore, the fraction of the total pressure exerted by H2 will be ((1/2)P)/P = 1/2.
Answer:
- The fraction of the total pressure exerted by H2 is 1/2 (option B).
- Equal weights of CH4 and H2 are mixed in an empty container at 25°C.
To find:
- The fraction of the total pressure exerted by H2.
Solution:
1. Calculate the moles of each gas:
- Since the weights of CH4 and H2 are equal, we can assume that they have the same mass.
- The molar mass of CH4 (methane) is 16 g/mol, and the molar mass of H2 (hydrogen) is 2 g/mol.
- Therefore, the moles of CH4 and H2 will be the same when equal weights are taken.
2. Calculate the partial pressures of each gas:
- According to Dalton's law of partial pressures, the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of each gas.
- The partial pressure of a gas can be calculated using Dalton's law as the product of the mole fraction and the total pressure.
- Since the moles of CH4 and H2 are the same, their mole fractions will also be the same.
- Therefore, the mole fraction of H2 will be 1/2, and the mole fraction of CH4 will also be 1/2.
- Let the total pressure be P. The partial pressure of H2 will be (1/2)P, and the partial pressure of CH4 will also be (1/2)P.
3. Calculate the fraction of the total pressure exerted by H2:
- The fraction of the total pressure exerted by H2 can be calculated as the partial pressure of H2 divided by the total pressure.
- Therefore, the fraction of the total pressure exerted by H2 will be ((1/2)P)/P = 1/2.
Answer:
- The fraction of the total pressure exerted by H2 is 1/2 (option B).
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Equal weights of CH4 and H2 are mixed in an empty container at 25oC. The fraction of the total pressure exerted by H2 isa)1/9b)1/2c)8/9d)16/17Correct answer is option 'C'. Can you explain this answer? for JEE 2025 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about Equal weights of CH4 and H2 are mixed in an empty container at 25oC. The fraction of the total pressure exerted by H2 isa)1/9b)1/2c)8/9d)16/17Correct answer is option 'C'. Can you explain this answer? covers all topics & solutions for JEE 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Equal weights of CH4 and H2 are mixed in an empty container at 25oC. The fraction of the total pressure exerted by H2 isa)1/9b)1/2c)8/9d)16/17Correct answer is option 'C'. Can you explain this answer?.
Equal weights of CH4 and H2 are mixed in an empty container at 25oC. The fraction of the total pressure exerted by H2 isa)1/9b)1/2c)8/9d)16/17Correct answer is option 'C'. Can you explain this answer? for JEE 2025 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about Equal weights of CH4 and H2 are mixed in an empty container at 25oC. The fraction of the total pressure exerted by H2 isa)1/9b)1/2c)8/9d)16/17Correct answer is option 'C'. Can you explain this answer? covers all topics & solutions for JEE 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Equal weights of CH4 and H2 are mixed in an empty container at 25oC. The fraction of the total pressure exerted by H2 isa)1/9b)1/2c)8/9d)16/17Correct answer is option 'C'. Can you explain this answer?.
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