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Two identical cylinders contain Helium at 2.5 atm and Argon at 1 atm respectively . If both the cylinders are connected by a tube the pressure would be (i) 3.5 atm (ii) 1.75 atm (iii) 1.5 atm (iv)1 atm?
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Two identical cylinders contain Helium at 2.5 atm and Argon at 1 atm r...
Solution:
To determine the pressure of the system when the two cylinders are connected, we need to apply the ideal gas law.
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 cylinders are identical, they have the same volume, which we can assume to be V. The number of moles of gas in each cylinder can be calculated using the ideal gas law.
n = PV/RT
where P and V are the pressure and volume of the gas, R is the gas constant, and T is the temperature.
The temperature of both gases is assumed to be the same since they are in thermal equilibrium. Therefore, the number of moles of Helium and Argon can be calculated as:
n(He) = (2.5 atm)(V)/(R*T)
n(Ar) = (1 atm)(V)/(R*T)
When the two cylinders are connected by a tube, the total volume of the system remains constant, but the number of moles of gas increases. The total number of moles of gas can be calculated as:
n(total) = n(He) + n(Ar)
= (2.5 atm)(V)/(R*T) + (1 atm)(V)/(R*T)
= (3.5 atm)(V)/(R*T)
Therefore, the total pressure of the system can be calculated as:
P(total) = n(total)RT/V
= (3.5 atm)(R*T/V)
Therefore, the pressure of the system when the two cylinders are connected is 3.5 atm.
Answer: (i) 3.5 atm
To determine the pressure of the system when the two cylinders are connected, we need to apply the ideal gas law.
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 cylinders are identical, they have the same volume, which we can assume to be V. The number of moles of gas in each cylinder can be calculated using the ideal gas law.
n = PV/RT
where P and V are the pressure and volume of the gas, R is the gas constant, and T is the temperature.
The temperature of both gases is assumed to be the same since they are in thermal equilibrium. Therefore, the number of moles of Helium and Argon can be calculated as:
n(He) = (2.5 atm)(V)/(R*T)
n(Ar) = (1 atm)(V)/(R*T)
When the two cylinders are connected by a tube, the total volume of the system remains constant, but the number of moles of gas increases. The total number of moles of gas can be calculated as:
n(total) = n(He) + n(Ar)
= (2.5 atm)(V)/(R*T) + (1 atm)(V)/(R*T)
= (3.5 atm)(V)/(R*T)
Therefore, the total pressure of the system can be calculated as:
P(total) = n(total)RT/V
= (3.5 atm)(R*T/V)
Therefore, the pressure of the system when the two cylinders are connected is 3.5 atm.
Answer: (i) 3.5 atm
Community Answer
Two identical cylinders contain Helium at 2.5 atm and Argon at 1 atm r...
Ptotal = P1V1+P2V2/V1+V2. Ptotal = V ( 2.5+1)/ 2V= 1.75
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Two identical cylinders contain Helium at 2.5 atm and Argon at 1 atm respectively . If both the cylinders are connected by a tube the pressure would be (i) 3.5 atm (ii) 1.75 atm (iii) 1.5 atm (iv)1 atm?
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Two identical cylinders contain Helium at 2.5 atm and Argon at 1 atm respectively . If both the cylinders are connected by a tube the pressure would be (i) 3.5 atm (ii) 1.75 atm (iii) 1.5 atm (iv)1 atm? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about Two identical cylinders contain Helium at 2.5 atm and Argon at 1 atm respectively . If both the cylinders are connected by a tube the pressure would be (i) 3.5 atm (ii) 1.75 atm (iii) 1.5 atm (iv)1 atm? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Two identical cylinders contain Helium at 2.5 atm and Argon at 1 atm respectively . If both the cylinders are connected by a tube the pressure would be (i) 3.5 atm (ii) 1.75 atm (iii) 1.5 atm (iv)1 atm?.
Two identical cylinders contain Helium at 2.5 atm and Argon at 1 atm respectively . If both the cylinders are connected by a tube the pressure would be (i) 3.5 atm (ii) 1.75 atm (iii) 1.5 atm (iv)1 atm? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about Two identical cylinders contain Helium at 2.5 atm and Argon at 1 atm respectively . If both the cylinders are connected by a tube the pressure would be (i) 3.5 atm (ii) 1.75 atm (iii) 1.5 atm (iv)1 atm? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Two identical cylinders contain Helium at 2.5 atm and Argon at 1 atm respectively . If both the cylinders are connected by a tube the pressure would be (i) 3.5 atm (ii) 1.75 atm (iii) 1.5 atm (iv)1 atm?.
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