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Liquefaction of Gases and Critical Constants

The change in...

Question

The change in volume $V$ with respect to an increase in pressure $P$ is shown in the diagram. For a fixed amount of a non ideal gas at a temperature $T$ of the gas must be:

A

less than the critical temperature

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B

equal to the critical temperautre

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C

greater than the critical temperature

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D

nothing can be definitely said

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Solution

The correct option is C less than the critical temperature
According to the graph, there exists a horizontal line (between 1 and 2) which represents there is liquid-vapor phase equilibrium and after the point 2 it decreases sharply. Now according to the $P V$ diagram shown to the left, $T$ is less than the critical temperature.

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Q. The change in volume V with respect to an increase in pressure P has been shown in the adjoining figure for a non-ideal gas at four different temperatures

T_{1}, T_{2}, T_{3}

T_{4}

. The critical temperature of the gas is :

Q. Assertion (A): Real gases tend to behave as ideal gas at low pressure and high Temperature.
Reason (R): At temperature more than critical temperature, a gas can’t be liquefied just by increasing the pressure. Which of the followings is correct?

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^{'}

?

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. Critical temperature and pressure of a real gas is

27^{o} C

& 150 atm respectively. The critical volume of 1 mole of real gas is :

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