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Select correct statements:
- a)A real gas can be liquefied at critical temperature
- b)Critical pressure is the maximum pressure at which substance present in its liquid state at TC
- c)Ideal gas can be liquefied below TC
- d)Critical volume is the molar volume or substance in gaseous state at TC and PC
Correct answer is option 'A'. Can you explain this answer?
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Select correct statements:a)A real gas can be liquefied at critical te...
Understanding Real Gases and Liquefaction
A real gas can indeed be liquefied at its critical temperature (TC). This statement is correct for several reasons:
What is Critical Temperature?
- The critical temperature is the highest temperature at which a substance can exist as a liquid, regardless of the pressure applied.
- Above this temperature, no amount of pressure can force the gas into a liquid state.
Real Gases vs. Ideal Gases
- Real gases deviate from ideal behavior due to intermolecular forces and the volume occupied by gas molecules.
- At temperatures below TC, real gases can be liquefied when subjected to sufficient pressure because attractive forces between molecules become significant.
Why Other Statements are Incorrect
- Statement B: Critical pressure is not the maximum pressure for a substance to remain in a liquid state at TC. Instead, it is the pressure required to liquefy a gas at its critical temperature.
- Statement C: Ideal gases cannot be liquefied below TC; they follow the ideal gas law without interactions, and therefore, they do not exhibit liquefaction behavior like real gases.
- Statement D: Critical volume refers to the volume occupied by one mole of the substance at its TC and critical pressure (PC), not just in the gaseous state.
Conclusion
In summary, option 'A' is correct because real gases can be liquefied at their critical temperature when sufficient pressure is applied, allowing them to overcome intermolecular forces. Understanding these concepts is essential for studying phase transitions in chemistry.
A real gas can indeed be liquefied at its critical temperature (TC). This statement is correct for several reasons:
What is Critical Temperature?
- The critical temperature is the highest temperature at which a substance can exist as a liquid, regardless of the pressure applied.
- Above this temperature, no amount of pressure can force the gas into a liquid state.
Real Gases vs. Ideal Gases
- Real gases deviate from ideal behavior due to intermolecular forces and the volume occupied by gas molecules.
- At temperatures below TC, real gases can be liquefied when subjected to sufficient pressure because attractive forces between molecules become significant.
Why Other Statements are Incorrect
- Statement B: Critical pressure is not the maximum pressure for a substance to remain in a liquid state at TC. Instead, it is the pressure required to liquefy a gas at its critical temperature.
- Statement C: Ideal gases cannot be liquefied below TC; they follow the ideal gas law without interactions, and therefore, they do not exhibit liquefaction behavior like real gases.
- Statement D: Critical volume refers to the volume occupied by one mole of the substance at its TC and critical pressure (PC), not just in the gaseous state.
Conclusion
In summary, option 'A' is correct because real gases can be liquefied at their critical temperature when sufficient pressure is applied, allowing them to overcome intermolecular forces. Understanding these concepts is essential for studying phase transitions in chemistry.
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Select correct statements:a)A real gas can be liquefied at critical te...
Option (A)and option (D) are correct
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Select correct statements:a)A real gas can be liquefied at critical temperatureb)Critical pressure is the maximum pressure at which substance present in its liquid state at TCc)Ideal gas can be liquefied below TCd)Critical volume is the molar volume or substance in gaseous state at TC and PCCorrect answer is option 'A'. Can you explain this answer?
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