It is easier to liquefy a gas with higher critical temperature-explain.

The gas with the highest critical temperature is

The higher the critical temperature of the gas

The higher the critical temperature of the gas

The higher the critical temperature of the gas

The essential conditions for liquefaction of gases were discovered by Andrews in 1869 as a result of his study of pressure-volume-temperature relationship for CO_(2) . If was found that above a certain temperature, it was impossible to liquefy a gas whatever the pressure was applied. The temperature below which the gas can be liquefied by the application of pressure alone is called critical temperature (T_(c)) . The pressure required to liquefy a gas at this temperature is called the critical pressure (P_(c)) . The volume occupied by one mole of the substance at the critical temperature and pressure is called critcal volume. Critical constants are related with van der Waals' constant as follows: V_(c) = 3b, P_(c) = (a)/(27b^(2)), T_(c) = (8a)/(27 Rb) The pressure required to liquefy a gas at the critical temperature is called :

Assertion: A gas with higher critical temperature gets adsorbed to more extent than a gas with lower critical temperature. Reason: The easily liquefiable gases get adsorbed to more extent which have higher critical temperature.

Assertion: A gas with higher critical temperature gets adsorbed to more extent than a gas with lower critical temperature. Reason: The easily liquefiable gases get adsorbed to more extent which have higher critical temperature.

Is it possible to liquefy a gas at any temperature?