Critical temperature can be defined as the
Temperature at which a gas is converted into its liquid state
Temperature at which there is no motion between the molecules
Temperature above which a gas cannot be liquefied no matter however high the pressure may be
Temperature at which volume of a gas becomes zero

Temperature at which there is no motion between the molecules

Temperature at which a gas is converted into its liquid state

Temperature above which a gas cannot be liquefied no matter however high the pressure may be

Temperature at which volume of a gas becomes zero

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Solution

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Critical temperature is that temperature at or below which a gas can be liquefied by pressure alone and above which a gas cannot be liquefied by pressure alone.

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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?

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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^{'}

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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}

(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}

and

T_{C}

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The temperature at which a gas must be cooled before it can be liquefied by compression is called:

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