Final answer:
Solid CO₂(s) sublimes easily due to high vapor pressure and low intermolecular attractions, which enables its molecules to transition directly from solid to gaseous state without forming a liquid.
Step-by-step explanation:
The properties associated with a compound like CO₂(s) that readily sublimes at 25°C are high vapor pressure and low intermolecular attractions. Sublimation is the process where a solid changes directly to a gas without passing through the liquid state. This occurs when the molecules in the solid phase have enough energy to overcome their intermolecular forces and enter the gas phase. Since solid carbon dioxide, also known as dry ice, sublimes at a temperature of –78.5°C under atmospheric pressure, it suggests that the intermolecular forces in solid CO₂ are relatively weak and the solid has a high vapor pressure.