Gases tend to escape when they are trapped inside small containers more readily than in large open spaces due to the principles of diffusion and pressure.
Diffusion: Gases naturally exhibit a property called diffusion, which is the spontaneous mixing of gas molecules in a space. Gas molecules are in constant motion and tend to move from areas of higher concentration to areas of lower concentration. In small containers, the confined space limits the distance gas molecules have to travel to escape, resulting in a faster rate of diffusion and escape of the gas.
Pressure: Gas molecules exert pressure on the walls of their container due to their constant collisions. This is known as gas pressure. In a small container, the concentration of gas molecules is higher, which leads to a higher pressure compared to a larger open space where the gas is more spread out. Higher pressure increases the likelihood of gas molecules finding an opening or weak spot to escape, leading to a greater tendency for gases to escape from small containers.
Additionally, factors such as temperature and the nature of the gas molecules themselves can also influence the rate of gas escape. Higher temperatures generally increase the kinetic energy of gas molecules, making them move more rapidly and escape more easily. Furthermore, the size and mass of gas molecules can affect their diffusion rate, with smaller and lighter molecules tending to diffuse faster than larger and heavier ones.
In contrast, in large open spaces, gases have more room to disperse and diffuse, resulting in lower concentrations and pressures. The escape of gas molecules becomes less noticeable as they mix and spread throughout the larger space, reducing the overall rate of escape compared to the confinement of a small container.