Consider the sublimation of iodine at 25.0 °C : I₂(s) → I₂(g) c. Explain why iodine spontaneously sublimes in open air at 25.0 °C

Key Concepts

Sublimation

Sublimation is the phase transition in which a substance changes directly from a solid to a gas without passing through the liquid phase. This process occurs when the molecules in the solid gain enough energy to overcome intermolecular forces and escape into the gas phase. For iodine, sublimation is favored at certain temperatures and pressures, particularly when the solid is exposed to open air.

Vapor Pressure

Vapor pressure is the pressure exerted by a vapor in equilibrium with its solid or liquid phase at a given temperature. For iodine, at 25.0 °C, the vapor pressure is significant enough to allow iodine molecules to escape from the solid phase into the gas phase. When the vapor pressure exceeds the atmospheric pressure, sublimation occurs spontaneously, leading to the transition of solid iodine to gaseous iodine.

Thermodynamics and Spontaneity

Thermodynamics helps determine whether a process is spontaneous based on changes in enthalpy and entropy. For iodine subliming at 25.0 °C, the process is driven by an increase in entropy, as gas molecules have greater disorder than solid molecules. The Gibbs free energy change (ΔG) for sublimation is negative under these conditions, indicating that the process occurs spontaneously in open air.