Explain the relationship between critical temperature and the ease of adsorption of gases on a solid surface, and rank the given gases by their ease of adsorption.

The ease of adsorption of a gas on a solid surface is directly related to its critical temperature ($T_c$). Gases with higher critical temperatures are more easily liquefied because they possess stronger intermolecular forces. These stronger forces allow for greater interaction between the gas molecules and the adsorbent surface, leading to easier adsorption.

• Carbon dioxide ($CO_2$): $T_c = 31.04 \text{ }^\circ C$
• Nitrogen ($N_2$): $T_c = -146.9 \text{ }^\circ C$
• Oxygen ($O_2$): $T_c = -181.6 \text{ }^\circ C$
• Neon ($Ne$): $T_c = -228.75 \text{ }^\circ C$

1. Carbon dioxide ($CO_2$): $31.04 \text{ }^\circ C$
2. Nitrogen ($N_2$): $-146.9 \text{ }^\circ C$
3. Oxygen ($O_2$): $-181.6 \text{ }^\circ C$
4. Neon ($Ne$): $-228.75 \text{ }^\circ C$

Based on the principle that higher critical temperature leads to easier adsorption, the gases can be rated as follows:

• Most easily adsorbed: Carbon dioxide ($CO_2$)
• Nitrogen ($N_2$)
• Oxygen ($O_2$)
• Least easily adsorbed: Neon ($Ne$)

The final order of ease of adsorption (from most to least) is:
$\boxed{\text{Carbon dioxide} > \text{Nitrogen} > \text{Oxygen} > \text{Neon}}$