Which of the following is correct for critical temperature?

It is the highest temperature at which liquid and vapour can coexit

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

Beyond this temperature, there is no distinction between the two phases and a gas cannot be liquefied by compression

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

At this temperature, the gas and the liquid phases have different critical densities

No worries! We‘ve got your back. Try BYJU‘S free classes today!

All are correct

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct options are
A It is the highest temperature at which liquid and vapour can coexit
B Beyond this temperature, there is no distinction between the two phases and a gas cannot be liquefied by compression
Critical temperature: The highest temperature at which a substance can exist as a liquid. Above the critical temperature, the molecules have too much kinetic energy for the intermolecular attractive forces to hold them together in a separate liquid phase.
At a temperature below $T_{c}$ , the molecules are close enough for the attractive forces to act, and condensation occurs and no condensation takes place above $T_{c}$ .

Suggest Corrections

Similar questions

Consider the following statements.

I. Gaseous substances whose critical temperatures are above room temperatures can be liquefied by applying sufficient pressure to the gas.

II. Gaseous substances whose critical temperatures are below room temperature can be liquefied by the application of pressure and lowering of temperature below $T_{c}$ .

Select the correct alternate.

Q. The critical temperature of a gas is the temperature above which a gas cannot be liquefied, if pressure is less than critical pressure.If this is true enter 1, if false enter 0.

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}

and

T_{C}

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}

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

^{'} b^{'}

Q. Assertion: At critical point the densities of substance in gaseous and liquid states are same.
Reason: Critical temperature is the temperature at which the real gas exhibit ideal behaviour for considerable range of pressure.

Join BYJU'S Learning Program