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A flask is filled with 13 gm of an ideal gas at 27°C and its temperature is raised to 52°C. The mass of the gas that has to be released to maintains the temperature of the gas in the flask at 52°C and the pressure remaining the same is (in gm).
Correct answer is '1'. Can you explain this answer?
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Verified Answer
A flask is filled with 13 gm of an ideal gas at 27°C and its tempe...
pV ∝ Mass of gas x Temperature
In this problem, pressure and volume remains constant so M1 T1 = M2 T2 = constant
i.e., mass of the gas released from the flask = 13 – 12 = 1gm.
The correct answer is: 1
In this problem, pressure and volume remains constant so M1 T1 = M2 T2 = constant
i.e., mass of the gas released from the flask = 13 – 12 = 1gm.
The correct answer is: 1
Most Upvoted Answer
A flask is filled with 13 gm of an ideal gas at 27°C and its tempe...
To calculate the pressure of the gas, we need to use the ideal gas law equation: PV = nRT.
Where:
P = pressure of the gas (unknown)
V = volume of the gas (unknown)
n = number of moles of the gas (unknown)
R = ideal gas constant (0.0821 L·atm/mol·K)
T = temperature of the gas (27°C = 300 K)
First, we need to find the number of moles of the gas. To do this, we can use the equation:
n = mass / molar mass
The molar mass of the gas will depend on the specific gas used. Let's assume the gas is nitrogen (N2). The molar mass of nitrogen is approximately 28.0134 g/mol.
n = 13 g / 28.0134 g/mol ≈ 0.464 mol
Now we can rearrange the ideal gas law equation to solve for pressure:
P = nRT / V
Given that the volume of the flask is not provided, we cannot solve for pressure without this information.
Where:
P = pressure of the gas (unknown)
V = volume of the gas (unknown)
n = number of moles of the gas (unknown)
R = ideal gas constant (0.0821 L·atm/mol·K)
T = temperature of the gas (27°C = 300 K)
First, we need to find the number of moles of the gas. To do this, we can use the equation:
n = mass / molar mass
The molar mass of the gas will depend on the specific gas used. Let's assume the gas is nitrogen (N2). The molar mass of nitrogen is approximately 28.0134 g/mol.
n = 13 g / 28.0134 g/mol ≈ 0.464 mol
Now we can rearrange the ideal gas law equation to solve for pressure:
P = nRT / V
Given that the volume of the flask is not provided, we cannot solve for pressure without this information.
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A flask is filled with 13 gm of an ideal gas at 27°C and its temperature is raised to 52°C. The mass of the gas that has to be released to maintains the temperature of the gas in the flask at 52°C and the pressure remaining the same is (in gm).Correct answer is '1'. Can you explain this answer?
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A flask is filled with 13 gm of an ideal gas at 27°C and its temperature is raised to 52°C. The mass of the gas that has to be released to maintains the temperature of the gas in the flask at 52°C and the pressure remaining the same is (in gm).Correct answer is '1'. Can you explain this answer? for Physics 2024 is part of Physics preparation. The Question and answers have been prepared according to the Physics exam syllabus. Information about A flask is filled with 13 gm of an ideal gas at 27°C and its temperature is raised to 52°C. The mass of the gas that has to be released to maintains the temperature of the gas in the flask at 52°C and the pressure remaining the same is (in gm).Correct answer is '1'. Can you explain this answer? covers all topics & solutions for Physics 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A flask is filled with 13 gm of an ideal gas at 27°C and its temperature is raised to 52°C. The mass of the gas that has to be released to maintains the temperature of the gas in the flask at 52°C and the pressure remaining the same is (in gm).Correct answer is '1'. Can you explain this answer?.
A flask is filled with 13 gm of an ideal gas at 27°C and its temperature is raised to 52°C. The mass of the gas that has to be released to maintains the temperature of the gas in the flask at 52°C and the pressure remaining the same is (in gm).Correct answer is '1'. Can you explain this answer? for Physics 2024 is part of Physics preparation. The Question and answers have been prepared according to the Physics exam syllabus. Information about A flask is filled with 13 gm of an ideal gas at 27°C and its temperature is raised to 52°C. The mass of the gas that has to be released to maintains the temperature of the gas in the flask at 52°C and the pressure remaining the same is (in gm).Correct answer is '1'. Can you explain this answer? covers all topics & solutions for Physics 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A flask is filled with 13 gm of an ideal gas at 27°C and its temperature is raised to 52°C. The mass of the gas that has to be released to maintains the temperature of the gas in the flask at 52°C and the pressure remaining the same is (in gm).Correct answer is '1'. Can you explain this answer?.
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A flask is filled with 13 gm of an ideal gas at 27°C and its temperature is raised to 52°C. The mass of the gas that has to be released to maintains the temperature of the gas in the flask at 52°C and the pressure remaining the same is (in gm).Correct answer is '1'. Can you explain this answer?, a detailed solution for A flask is filled with 13 gm of an ideal gas at 27°C and its temperature is raised to 52°C. The mass of the gas that has to be released to maintains the temperature of the gas in the flask at 52°C and the pressure remaining the same is (in gm).Correct answer is '1'. Can you explain this answer? has been provided alongside types of A flask is filled with 13 gm of an ideal gas at 27°C and its temperature is raised to 52°C. The mass of the gas that has to be released to maintains the temperature of the gas in the flask at 52°C and the pressure remaining the same is (in gm).Correct answer is '1'. Can you explain this answer? theory, EduRev gives you an
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