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NH(3) can be liquefied at ordinary tempe...

`NH_(3)` can be liquefied at ordinary temperature without the application of pressure. But `O_(2)` cannot be because :

A

its critical temperature is very high

B

its critical temperature is low

C

its critical temperature is moderate

D

its critical temperature is higher than that of ammonia

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The correct Answer is:
B
The critical temperature of `O_(2)` is lower than that of `NH_(3)`
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CO_(2) gas can be liquefied under pressure between

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) Gas A and can be liquefied at room temperature by applying pressure but gas B cannot. This reflects:

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