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Statement-1 : Due to adiabatic free expansion temperature of real gas may increase
Statement-2 : In adiabatic free expansion, temperature is always constant irrespective of real or ideal gas
- a)Statement-1 is True, Statement-2 is. True; Statement-2 is a correct explanation for Statement-1.
- b)Statement-1 is True, Statement-2 is True; Statement-2 is NOT a correct explanation for Statement-1.
- c)Statement-1 is True, Statement-2 is False.
- d)Statement-1 is False, Statement-2 is True.
Correct answer is option 'C'. Can you explain this answer?
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Verified Answer
Statement-1 : Due to adiabatic free expansion temperature of real gas ...
For ideal gas, change in internal energy=ΔU∝ΔT
During free adiabatic expansion,ΔQ=ΔW=0⇒ΔU=0⇒ΔT=0
However for real gases, ΔU=f(V,T)
In this case, for free adiabatic expansion ΔU=0⇒f(V,T)=0
Thus T may change in this case.
So, statement I is true while statement II is false.
During free adiabatic expansion,ΔQ=ΔW=0⇒ΔU=0⇒ΔT=0
However for real gases, ΔU=f(V,T)
In this case, for free adiabatic expansion ΔU=0⇒f(V,T)=0
Thus T may change in this case.
So, statement I is true while statement II is false.
Most Upvoted Answer
Statement-1 : Due to adiabatic free expansion temperature of real gas ...
As real gas depends on both temperature and pressure ..so its temperature can change due to pressure change when U remains constant
But in 2nd case ideal gas will only have a constant temperature as it only depends on temperature not pressure...so 1st statement is true and 2nd is false
But in 2nd case ideal gas will only have a constant temperature as it only depends on temperature not pressure...so 1st statement is true and 2nd is false
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Statement-1 : Due to adiabatic free expansion temperature of real gas ...
Statement-1: Due to adiabatic free expansion, temperature of real gas may increase.
Statement-2: In adiabatic free expansion, temperature is always constant irrespective of real or ideal gas.
Explanation:
Adiabatic Free Expansion:
Adiabatic free expansion is a process in which a gas expands into a vacuum without any heat exchange with the surroundings. During this process, the gas expands rapidly, and the pressure and temperature of the gas decrease.
Statement-1: Due to adiabatic free expansion, temperature of real gas may increase.
The statement is true. In adiabatic free expansion, the gas expands rapidly, leading to a decrease in pressure. For a real gas, the intermolecular forces between gas molecules cannot be ignored, and as the gas expands, the molecules move further apart. This decrease in intermolecular forces can lead to an increase in the kinetic energy of the gas molecules and, consequently, an increase in temperature.
Statement-2: In adiabatic free expansion, temperature is always constant irrespective of real or ideal gas.
The statement is false. In adiabatic free expansion, the temperature of the gas can change. The change in temperature depends on the specific conditions of the gas and the nature of the expansion. For an ideal gas, the temperature remains constant during adiabatic free expansion because there are no intermolecular forces to affect the kinetic energy of the gas molecules. However, for a real gas, the temperature can increase due to the decrease in intermolecular forces as explained in Statement-1.
Conclusion:
- Statement-1 is true as the temperature of a real gas can increase during adiabatic free expansion.
- Statement-2 is false as the temperature is not always constant during adiabatic free expansion, especially for real gases.
Statement-2: In adiabatic free expansion, temperature is always constant irrespective of real or ideal gas.
Explanation:
Adiabatic Free Expansion:
Adiabatic free expansion is a process in which a gas expands into a vacuum without any heat exchange with the surroundings. During this process, the gas expands rapidly, and the pressure and temperature of the gas decrease.
Statement-1: Due to adiabatic free expansion, temperature of real gas may increase.
The statement is true. In adiabatic free expansion, the gas expands rapidly, leading to a decrease in pressure. For a real gas, the intermolecular forces between gas molecules cannot be ignored, and as the gas expands, the molecules move further apart. This decrease in intermolecular forces can lead to an increase in the kinetic energy of the gas molecules and, consequently, an increase in temperature.
Statement-2: In adiabatic free expansion, temperature is always constant irrespective of real or ideal gas.
The statement is false. In adiabatic free expansion, the temperature of the gas can change. The change in temperature depends on the specific conditions of the gas and the nature of the expansion. For an ideal gas, the temperature remains constant during adiabatic free expansion because there are no intermolecular forces to affect the kinetic energy of the gas molecules. However, for a real gas, the temperature can increase due to the decrease in intermolecular forces as explained in Statement-1.
Conclusion:
- Statement-1 is true as the temperature of a real gas can increase during adiabatic free expansion.
- Statement-2 is false as the temperature is not always constant during adiabatic free expansion, especially for real gases.
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Statement-1 : Due to adiabatic free expansion temperature of real gas may increaseStatement-2 : In adiabatic free expansion, temperature is always constant irrespective of real or ideal gasa)Statement-1 is True, Statement-2 is. True; Statement-2 is a correct explanation for Statement-1.b)Statement-1 is True, Statement-2 is True; Statement-2 is NOT a correct explanation for Statement-1.c)Statement-1 is True, Statement-2 is False.d)Statement-1 is False, Statement-2 is True.Correct answer is option 'C'. Can you explain this answer?
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