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Liquefaction of Gases and Critical Constants

Critical temp...

Question

Critical temperature and critical pressure values of four gases are given

$\begin{matrix} Gas & C. Temp (K) & C. Pressure (atm) P & 5.1 & 2.2 Q & 33 & 13 R & 126 & 34 S & 135 & 40 \end{matrix}$

Which of the gas/gases cannot be liquefied at a temperature of 100 K and a pressure of 50 atmospheres?

A

S only

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B

P only

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C

R and S

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D

P and Q

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Solution

The correct option is D P and Q
Gases cannot be liquefied above the critical temperature however high the pressure may be applied.
As P and Q gases have critical temperature less than $100 K$ whereas, R and S have critical temprature higher than $100 K$ , therefore P and Q gases cannot be liquified at a temperature $100 K$ and $50 a t m$ .

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Similar questions

Critical temperature and critical pressure values of four gases are given

Gas	C. Temp(K)	C.pressure(atm)
P	5.1	2.2
Q	33	13
R	126	34
S	135	40

Which of the gas/gases cannot be liquefied at a temperature of 100 K and a pressure of 50 atmospheres?

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. 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.

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Liquefaction of Gases and Critical Constants

Standard XI Chemistry

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