What condition leads to more gas particles escaping into the vapor phase?

Increased temperature is a key factor that leads to more gas particles escaping into the vapor phase. When the temperature of a substance rises, the kinetic energy of its molecules also increases. This increased kinetic energy means that more molecules have sufficient energy to overcome intermolecular forces that may be holding them in the liquid phase. As a result, a greater number of molecules transition into the vapor phase, leading to an increase in vapor pressure.

At higher temperatures, the distribution of molecular speeds broadens, allowing a larger fraction of the molecules to possess enough energy to escape from the liquid into the gaseous state. This is a fundamental principle of phase changes in the context of gas laws, particularly relating to vaporization.

In contrast, options like increased pressure and decreased volume typically do not encourage gas particles to escape into the vapor phase; instead, they can compress the gas and keep more particles in the liquid state. Decreasing the number of molecules would likewise reduce the potential for evaporation, as there are fewer particles available to escape into the vapor phase.