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Liquefaction of Gases and Critical Constants

Which of the ...

Question

Which of the following conditions are not suitable for liquefaction of gases?

A

Lowering the Temperature

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B

Compressing the gas at any temperature

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C

Compressing the gas as well as cooling

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D

Compressing the gas below critical temperature

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Solution

The correct option is B
Compressing the gas at any temperature

Gases cannot be liquefied above critical temperature

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Similar questions

The critical temperature of ammonia and hydrogen are 405.5K and 33.2K respectively. Ammonia can be liquefied at room temperature just by compression of the gas at high pressure. Liquifaction of hydrogen , on the other hand, requires cooling as well as compression. (True/False)

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

C O_{2}

. 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

(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 critical volume. Critical constants are related with van der Waals' constant as follows:

V_{c} = 3 b, P_{c} = \frac{a}{27 b^{2}}, T_{c} = \frac{8 a}{27 R b}

.

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

^{'} b^{'}

?

Q. The temperature below which a gas must be cooled before it can be liquefied by compression is called as .

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

C O_{2}

. 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

(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 critical volume. Critical constants are related with van der Waals' constant as follows:

V_{c} = 3 b, P_{c} = \frac{a}{27 b^{2}}, T_{c} = \frac{8 a}{27 R b}

.

The relationship between

P_{C}, V_{C}

T_{C}

Q. The greater the critical temperature of a gas, the easier is the liquefaction of the gas.

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Liquefaction of Gases and Critical Constants

Standard XII Chemistry

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