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A gas can be liquified:
1. At critical temperature
2. Above critical temperature
3. Below critical temperature
4. At any temperature

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Correct Answer - Option 3 : Below critical temperature

Explanation:

Critical temperature:

  • The critical temperature of a gas is defined as the temperature above which it cannot be liquified, howsoever high pressure is applied.
  • For example, the critical temperature of carbon dioxide is 304.2 K, which means that it is impossible to liquefy carbon dioxide above 304.2 K by any means.
  • The critical temperature of gas gives an indication of the strength of the intermolecular attractive forces of that gas.
  • We can change the phase of gas from vapour to liquid by applying pressure.
  • When we increase the pressure, the gas molecules come closer and liquefaction happens.
  • Substances with high intermolecular forces are easier to liquefy and can be liquified over a wide range of temperature, even high temperatures by applying sufficient pressure and thus have high critical temperatures.
  • Whereas, a substance with weak attractive forces would have a low critical temperature and vice versa.
  • Above the critical point, the gas will not exist in liquid form.
  • Thus gases with low critical temperature exist in gaseous form at room temperature.
  • At the critical point, all the phases exist together.


Hence, a gas can be liquified only below the critical temperature.

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