Question

State whether the following statements are true or false. The greater the critical temperature of a gas, the easier is the liquefaction of the gas.

Short answer

Answer: True

Step-by-step solution

Understand Critical Temperature

The critical temperature of a gas is the temperature above which it cannot be liquefied, no matter the applied pressure. In other words, if the temperature of a gas is above its critical temperature, it is impossible to convert that gas into its liquid state.

Relation of Critical Temperature to Liquefaction

Gases with higher critical temperatures are typically easier to liquefy because their molecules are more strongly attracted to each other due to stronger intermolecular forces. To liquefy a gas, we need to bring its particles close enough together for the intermolecular forces to take effect, and high critical temperature means that these forces are considerable even at relatively high temperatures.

Determine the Truth of the Statement

Given the information from the previous steps, we can conclude that the statement "The greater the critical temperature of a gas, the easier is the liquefaction of the gas" is indeed true. Gases with a high critical temperature have strong intermolecular forces, making it easier to bring particles close together and facilitate the process of liquefaction.

Key concepts

Liquefaction of Gases

Understanding the liquefaction process of gases is pivotal for various industrial applications, from refrigeration to the petrochemical industry. Liquefaction is the transformation of a gas into a liquid state, usually achieved by compressing the gas and reducing its temperature. During this process, we rely on the reduction of kinetic energy within gas molecules, which allows intermolecular forces to dominate, resulting in a condensed liquid state.

Liquefaction can occur naturally, as seen in the formation of dew, or be technologically induced for transportation and storage of gases like natural gas or oxygen. The efficiency of this process is inherently linked to the gas's critical temperature, a concept further expanded in the subsequent sections of this article.

Intermolecular Forces

Intermolecular forces are the forces that mediate interaction between molecules, affecting the physical properties of substances, such as boiling points, melting points, and their ability to liquefy. These forces include London dispersion forces, dipole-dipole interactions, and hydrogen bonds. The strength and type of these forces vary depending on molecule polarity, size, and shape.

For example, hydrogen bonding is a strong type of intermolecular force present in water molecules, leading to water’s unusually high boiling point. In the context of gases, those with stronger intermolecular forces tend to liquefy more easily, as the intrinsic attraction between particles facilitates their transition into a liquid state when temperature and pressure are conducive.

Critical Temperature

The critical temperature of a gas is a distinctive point that marks the highest temperature at which a substance can exist as a liquid. Above this threshold, no matter how much pressure is applied, the gas will not condense into a liquid. Thus, gases with higher critical temperatures can be liquefied more readily under less stringent conditions.

One can infer, therefore, that the nature of intermolecular forces within a gas greatly influences its critical temperature. Gases with substantial intermolecular forces will boast higher critical temperatures. This is foundational knowledge for industries that harness the liquefaction process, as it impacts design considerations for pressure vessels and cooling systems. Recognizing the relationship between critical temperature and ease of liquefaction, as proven by the initial exercise, arms us with the foresight to predict the behavior of gases under varying conditions.