Liquefaction of Gases

Edited By Shivani Poonia | Updated on Sep 30, 2024 11:56 AM IST

Introduction

Liquefaction of gases is a process of transforming gas into its liquid form. Herein, a gas is cooled and/or its pressure is increased to an extent that it condenses into a liquid state. It is one of the basic concepts in thermodynamics, and it has innumerable practical applications in everyday life. For example, liquefied natural gas, or LNG, is used as fuel for heating and cooking. Liquefied natural gas is used to store and transport natural gas due to its minimal volume use compared to gas. Liquefied oxygen and nitrogen are other important gases in this form in the medical and industrial fields. Oxygen is required for many medical procedures and thus is stored in a liquid state in hospitals to reduce the volume of space consumed and guarantee its continuous availability. Nitrogen is also applied in food processing, where it can fast-freeze foods to preserve them. Other applications for the principles of liquefaction of gases are in air conditioning and refrigeration to make our homes and offices comfortable. In a nutshell, the liquefaction of gases makes possible and efficient storage, transportation, and application of gases in various practical applications which bring convenience and comfort in daily living.

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Introduction
Liquefaction of GasesLiquefaction of gases is done under the following two conditions: (i) Low temperature (i) High pressure
Some Solved Examples
Summary

Liquefaction of Gases

Liquefaction of Gases
Liquefaction of gases is done under the following two conditions: (i) Low temperature (i) High pressure

Low Temperature: As the temperature of the gas is lowered, the kinetic energy of the molecules decreases. The volume occupied by the gas also decreases. At very low-temperature molecules come very close to each other, later on coming more closer they ultimately change into the liquid state.
High Pressure: Increase in pressure brings the gaseous molecules closer and closer to one another. So, this factor also helps in converting the gas into the liquid.

For each gas there is a certain temperature above which the gas cannot be liquefied however high pressure is applied. Therefore we can say that the effect of temperature is more important than that of the pressure.

Critical Temperature T_c
Critical temperature of a gas may be defined as that temperature above which the gas cannot be liquefied however high the pressure is applied on the gas.

The critical temperature of a real gas is given by $\mathrm{T}_{\mathrm{c}}=\frac{8 \mathrm{a}}{27 \mathrm{Rb}}$

Critical Pressure P_c
The minimum pressure that must be applied on a gas at its critical temperature to just liquefy it.

The critical pressure of a real gas is given by $P_c=\frac{a}{27 b^2}$

Critical Volume V_c
The volume occupied by one mole of a gas at its critical temperature and critical pressure is known as the critical volume.

The critical volume of a real gas is given by $V_c=3 b$

At critical point,$\mathrm{Z}=\frac{\mathrm{P}_{\mathrm{c}} \mathrm{V}_{\mathrm{c}}}{\mathrm{RT}_{\mathrm{c}}}=\frac{3}{8}$

Significance of a and b

It gives the magnitude of attraction forces present between gas molecules.
Liquefication of gases ∝ a
Hence more the value of 'a' or force of attraction between the molecules of a gas, more will be its liquefaction:

Example
$
\begin{aligned}
& \text { Values of 'a' } \\
& \mathrm{He}<\mathrm{H}_2<\mathrm{O}_2<\mathrm{N}_2<\mathrm{CO}_2<\mathrm{HCl}<\mathrm{NH}_3<\mathrm{SO}_2 \\
& \mathrm{a} \rightarrow(0.034)(0.244)(1.36)(1.39)(3.59)(3.8)(4.17)(6.71)
\end{aligned}
$
Increasing order of liquefication of some gases
Its constancy in value shows that gas molecules are incompressible. $\mathrm{b}=4 \mathrm{~N}\left(\frac{4}{3} \pi \mathrm{r}^2\right)$
At low pressure 'a' dominates but at high pressure 'b' dominates.

For a better understanding of the topic and to learn more about the Liquefaction of Gases with video lesson we provide the link to the

YouTube video:

Some Solved Examples

Example 1: For a real gas the P-V curve was experimentally plotted and it had the following appearance. With respect to liquefaction. Choose the correct statement.

1)at T = 500 K, P = 40 atm, the state will be liquid.

2)at T = 300 K, P = 50 atm, the state will be gas.

3)at T < 300 K, P > 20 atm, the state will be gas.

4) at 300 K < T < 500 K, P > 50 atm, the state will be liquid.

Solution

Liquefaction of gases -

At high pressure, molecules of gas come close to each other. As a result, intermolecular attraction forces increase. When it is allowed to escape through a nozzle into a region of low pressure, the molecules move apart.

In doing so, energy is needed to overcome intermolecular attraction forces. This energy is taken from the molecules themselves. Therefore the gas is cooled.
This process is repeated many times until the gas is completely changed into the liquid state.

(a) at T = 500 K, P = 40 atm corresponds to 'a' substance - gas

(b) at T = 300 K, P = 50 atm corresponds to 'b' substance - liquid

(d) at T < 500 K, P > 50 atm corresponds to 'd' substance - liquid

Example 2: Critical temperatures of ammonia and carbon dioxide are 405.5 K and 304.10 K, respectively. Which of these gases will liquify first when you start cooling from 500 K to their critical temperature?

1) Ammonia

2)Carbon dioxide

3)Both will liquify at same time

4)Nothing can be predicted

Solution

Since the critical temperature of ammonia is higher than that of carbon dioxide, ammonia will liquify first as its critical temperature will be reached first. The liquefaction of carbon dioxide will require cooling to a lower temperature.

Hence, the answer is the option (1).

Example 3: Critical temperature for carbon dioxide and methane are $31.1^{\circ}$ and $-81.9^{\circ} \mathrm{C}$ respectively. Which of these has stronger intermolecular forces?

1) Carbon dioxide

2)Methane

3)Both have same intermolecular forces
4)Nothing can be predicted

Solution

We have1:
$T_c$ for $\mathrm{CH}_4=-81.9^{\circ} \mathrm{C}$ and $T_c$ for $\mathrm{CO}_2=31.1^{\circ} \mathrm{C}$

Clearly, $\mathrm{CO}_2$ has more vital intermolecular forces of attraction as it has a higher value of critical temperature.

Hence, the answer is the option (1).

Example 4: The critical temperature of $\mathrm{O}_2$ is less than $\mathrm{H}_2 \mathrm{O}$ because the $\mathrm{H}_2 \mathrm{O}$ molecules have:

1)Two covalent bonds

2) Dipole moment

3)Fewer electrons than $\mathrm{O}_2$

4)V-shaped structure

Solution

We know that the dipole moment in a molecule results in strong intermolecular forces and since

$T_c=\frac{8 a}{27 R b}$
Thus, the critical temperature of $\mathrm{H}_2 \mathrm{O}$ is more for $\mathrm{O}_2$ .
Hence, the answer is the option (2).

Summary

Liquefaction of gases is the process whereby gases are converted to liquids either by cooling and/or under increased pressure. This is very important in storage and transportation because it takes less space than the gas. For example, natural gas is liquefied primarily, hence the term LNG, for storage and transportation, especially to homes for heating and cooking. Liquid oxygen becomes an important element in medical operations, so it is stored as a liquid to supply patients continuously. Liquid nitrogen is used industrially for fast freezing during food processing to ensure it remains wholesome and safe for consumption. The concepts of gas liquefaction are also applied in air conditioning and refrigeration to cool our surrounding environments for a better life with more comfort. Everything would generally make a vast difference in the application of the liquefaction of gases in diverse industries, especially in contributing mainly to health, food preservation, the convenience of delivery, and efficiency in human life.