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At 27°C, hydrogen is leaked through a tiny hole into a vessel for 20 min. Another unknown gas at the same temperature and pressure as that of hydrogen is leaked through same bole for 20 min. After the effusion of the gases the mixture exerts a pressure of 6 atm. The hydrogen content of the mixture is 0.7 mole. If the volume of the container is 3 L. What is the molecular weight of the unknown gas?
Correct answer is '1020'. Can you explain this answer?
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At 27°C, hydrogen is leaked through a tiny hole into a vessel for...
Number of moles of H, diffused = 0.7 in 20 min
Number of moles of gas diffused = n1 in 20 min for gaseous mixture (after diffusion)
Because, mixture contains = moles of H2 + moles of gas diffused = n
Because, mixture contains = moles of H2 + moles of gas diffused = n
Most Upvoted Answer
At 27°C, hydrogen is leaked through a tiny hole into a vessel for...
**Given information:**
- Temperature (T) = 27°C = 300 K
- Pressure (P) = 6 atm
- Time (t) = 20 min = 20/60 = 1/3 hr
- Hydrogen content (nH2) = 0.7 mole
- Volume of the container (V) = 3 L
**Step 1: Calculate the number of moles of the unknown gas**
We know that the ideal gas equation is given by PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature.
Since the pressure and temperature are the same for both gases, we can rewrite the equation as:
n1/V1 = n2/V2
Here, n1 and n2 are the number of moles of hydrogen and the unknown gas, respectively. V1 and V2 are the volumes of the container.
n2 = (n1 x V2) / V1
n2 = (0.7 x 3) / 3 = 0.7 mole
So, the number of moles of the unknown gas is also 0.7 mole.
**Step 2: Calculate the molecular weight of the unknown gas**
The molecular weight of a gas can be calculated using the formula:
Molecular weight = (mass of the gas) / (number of moles of the gas)
Since we don't know the mass of the unknown gas, we need to find it.
The mass of the unknown gas can be calculated using the equation:
Mass = (number of moles) x (molar mass)
We know that the molar mass of hydrogen is 2 g/mol.
Mass of hydrogen = 0.7 mole x 2 g/mol = 1.4 g
Since the mass of the unknown gas is the same as the mass of hydrogen, the molecular weight of the unknown gas is also the same.
Molecular weight = 1.4 g / 0.7 mole = 2 g/mol
However, the given correct answer is 1020. This suggests that there might be an error or missing information in the question or answer. The calculated molecular weight of 2 g/mol does not match the given answer of 1020. Therefore, further clarification or information is required to explain the given answer.
- Temperature (T) = 27°C = 300 K
- Pressure (P) = 6 atm
- Time (t) = 20 min = 20/60 = 1/3 hr
- Hydrogen content (nH2) = 0.7 mole
- Volume of the container (V) = 3 L
**Step 1: Calculate the number of moles of the unknown gas**
We know that the ideal gas equation is given by PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature.
Since the pressure and temperature are the same for both gases, we can rewrite the equation as:
n1/V1 = n2/V2
Here, n1 and n2 are the number of moles of hydrogen and the unknown gas, respectively. V1 and V2 are the volumes of the container.
n2 = (n1 x V2) / V1
n2 = (0.7 x 3) / 3 = 0.7 mole
So, the number of moles of the unknown gas is also 0.7 mole.
**Step 2: Calculate the molecular weight of the unknown gas**
The molecular weight of a gas can be calculated using the formula:
Molecular weight = (mass of the gas) / (number of moles of the gas)
Since we don't know the mass of the unknown gas, we need to find it.
The mass of the unknown gas can be calculated using the equation:
Mass = (number of moles) x (molar mass)
We know that the molar mass of hydrogen is 2 g/mol.
Mass of hydrogen = 0.7 mole x 2 g/mol = 1.4 g
Since the mass of the unknown gas is the same as the mass of hydrogen, the molecular weight of the unknown gas is also the same.
Molecular weight = 1.4 g / 0.7 mole = 2 g/mol
However, the given correct answer is 1020. This suggests that there might be an error or missing information in the question or answer. The calculated molecular weight of 2 g/mol does not match the given answer of 1020. Therefore, further clarification or information is required to explain the given answer.
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At 27°C, hydrogen is leaked through a tiny hole into a vessel for 20 min. Another unknown gas at the same temperature and pressure as that of hydrogen is leaked through same bole for 20 min. After the effusion of the gases the mixture exerts a pressure of 6 atm. The hydrogen content of the mixture is 0.7 mole. If the volume of the container is 3 L. What is the molecular weight of the unknown gas?Correct answer is '1020'. Can you explain this answer?
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At 27°C, hydrogen is leaked through a tiny hole into a vessel for 20 min. Another unknown gas at the same temperature and pressure as that of hydrogen is leaked through same bole for 20 min. After the effusion of the gases the mixture exerts a pressure of 6 atm. The hydrogen content of the mixture is 0.7 mole. If the volume of the container is 3 L. What is the molecular weight of the unknown gas?Correct answer is '1020'. Can you explain this answer? for Chemistry 2024 is part of Chemistry preparation. The Question and answers have been prepared according to the Chemistry exam syllabus. Information about At 27°C, hydrogen is leaked through a tiny hole into a vessel for 20 min. Another unknown gas at the same temperature and pressure as that of hydrogen is leaked through same bole for 20 min. After the effusion of the gases the mixture exerts a pressure of 6 atm. The hydrogen content of the mixture is 0.7 mole. If the volume of the container is 3 L. What is the molecular weight of the unknown gas?Correct answer is '1020'. Can you explain this answer? covers all topics & solutions for Chemistry 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for At 27°C, hydrogen is leaked through a tiny hole into a vessel for 20 min. Another unknown gas at the same temperature and pressure as that of hydrogen is leaked through same bole for 20 min. After the effusion of the gases the mixture exerts a pressure of 6 atm. The hydrogen content of the mixture is 0.7 mole. If the volume of the container is 3 L. What is the molecular weight of the unknown gas?Correct answer is '1020'. Can you explain this answer?.
At 27°C, hydrogen is leaked through a tiny hole into a vessel for 20 min. Another unknown gas at the same temperature and pressure as that of hydrogen is leaked through same bole for 20 min. After the effusion of the gases the mixture exerts a pressure of 6 atm. The hydrogen content of the mixture is 0.7 mole. If the volume of the container is 3 L. What is the molecular weight of the unknown gas?Correct answer is '1020'. Can you explain this answer? for Chemistry 2024 is part of Chemistry preparation. The Question and answers have been prepared according to the Chemistry exam syllabus. Information about At 27°C, hydrogen is leaked through a tiny hole into a vessel for 20 min. Another unknown gas at the same temperature and pressure as that of hydrogen is leaked through same bole for 20 min. After the effusion of the gases the mixture exerts a pressure of 6 atm. The hydrogen content of the mixture is 0.7 mole. If the volume of the container is 3 L. What is the molecular weight of the unknown gas?Correct answer is '1020'. Can you explain this answer? covers all topics & solutions for Chemistry 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for At 27°C, hydrogen is leaked through a tiny hole into a vessel for 20 min. Another unknown gas at the same temperature and pressure as that of hydrogen is leaked through same bole for 20 min. After the effusion of the gases the mixture exerts a pressure of 6 atm. The hydrogen content of the mixture is 0.7 mole. If the volume of the container is 3 L. What is the molecular weight of the unknown gas?Correct answer is '1020'. Can you explain this answer?.
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