Which gas will be adsorbed on a solid to greater extent? (a)...

Which gas will be adsorbed on a solid to greater extent?
(a) Having non-polar molecule
(b) Having highest critical temperature
(c) Having lowest critical temperature
(d) Having lowest critical pressure

Key Concepts

Intermolecular Forces

Intermolecular forces, including van der Waals (dispersion) forces, dipole-dipole interactions, and hydrogen bonding, dictate the strength of interactions between gas molecules and the adsorbent surface. Stronger intermolecular forces lead to higher polarizability and a greater tendency for molecules to interact with the surface, thereby increasing the extent of adsorption. These forces are crucial in understanding why gases with certain thermodynamic properties, such as a high critical temperature, exhibit enhanced adsorption.

Adsorption

Adsorption is the process in which atoms, ions, or molecules from a substance (gas, liquid, or dissolved solid) adhere to the surface of an adsorbent. This process is highly dependent on the nature of the interactions between the adsorbate and the adsorbent, primarily through intermolecular forces such as van der Waals forces. The extent and strength of adsorption are influenced by the physical properties of the gas and the characteristics of the solid surface.

Critical Temperature

The critical temperature of a gas is the highest temperature at which it can be liquefied by pressure alone. A gas with a higher critical temperature tends to have stronger intermolecular attractions and is generally more easily condensed. This greater propensity to liquefy is directly related to an increased likelihood of adsorbing onto a solid surface, as the interactions that favor condensation also enhance adsorption.

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