The critical temperature T C and critical pressure -P c of CO 2 are 30-98- C and 73 atm respectively-Can CO 2 g be liquefied at 32- C and 80 atm pressure-

The given critical temperature and pressure of CO_2 gas are 30.98^∘C and 73 atm respectively. This suggests that CO_2 gas cannot be liquefied above 30.98^∘C ...

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Standard XII

Chemistry

Liquefaction of Gases and Critical Constants

The critical ...

Question

The critical temperature $(T_{c})$ and critical pressure $p_{c})$ of $C O_{2}$ are ${30.98}^{\circ} C$ and 73 atm respectively.Can $C O_{2}$ (g) be liquefied at $32^{\circ} C$ and 80 atm pressure?

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Solution

The given critical temperature and pressure of $C O_{2}$ gas are ${30.98}^{\circ} C$ and 73 atm respectively. This suggests that $C O_{2}$ gas cannot be liquefied above ${30.98}^{\circ} C$ and 73 atm. Howsoever high temperature and pressure may be applied on $C O_{2}$ gas. Hence, $C O_{2}$ gas cannot be liquefied at ${32.}^{\circ} C$ and 80 atm.

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Similar questions

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. If

\frac{P}{P_{c}} = P_{r}, \frac{T}{T_{c}} = T_{r}, a n d \frac{V_{m}}{V_{m, c}} = V_{r}

where

P_{r}

is reduced pressure,

P_{c}

is critical pressure

T_{r}

is reduced temperature,

T_{c}

is critical temperature

V_{r}

is reduced volume,

V_{c}

is critical volume
then the equation of state (or van der Waals equation), only in terms of

P_{r}, T_{r}

and

V_{r}

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. 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?

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The critical temperature (Tc) and critical pressure pc) of CO2 are 30.98∘C and 73 atm respectively.Can CO2 (g) be liquefied at 32∘C and 80 atm pressure?

The given critical temperature and pressure of CO2 gas are 30.98∘C and 73 atm respectively. This suggests that CO2 gas cannot be liquefied above 30.98∘C and 73 atm. Howsoever high temperature and pressure may be applied on CO2 gas. Hence, CO2 gas cannot be liquefied at 32.∘C and 80 atm.

The critical temperature $(T_{c})$ and critical pressure $p_{c})$ of $C O_{2}$ are ${30.98}^{\circ} C$ and 73 atm respectively.Can $C O_{2}$ (g) be liquefied at $32^{\circ} C$ and 80 atm pressure?