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Question

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 CO2. It 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 (Tc). The pressure required to liquefy a gas at this temperature is called the critical pressure (Pc). The volume occupied by one mole of the substance at the critical temperature and pressure is called critical volume. Critical constants are related with van der Waals' constant as follows:
Vc=3b,Pc=a27b2,Tc=8a27Rb.

Which of the following parameters is three times the van der Waals' constant ′b′?

A
Critical volume
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B
Critical temperature
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C
Vapour density
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D
Critical pressure
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Solution

The correct option is A Critical volume
Critical volume is three times the van der Waals' constant ′b′.

Note:
Vc=3b,Pc=a27b2,Tc=8a27Rb

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