In general, how does the solubility of gases behave with temperature changes?

The solubility of gases in liquids typically decreases as the temperature increases. This behavior can be understood through the principles of gas solubility and kinetic molecular theory.

At higher temperatures, the kinetic energy of gas molecules increases, causing them to move more vigorously. As a result, the gas molecules are more likely to escape from the solvent into the atmosphere rather than remain dissolved. This phenomenon can be explained by Le Chatelier's principle, which states that if the conditions of a system at equilibrium are changed, the system will adjust to counteract that change. When the temperature increases, the system is essentially pushed to favor the formation of gas in the vapor phase over the dissolved state.

Additionally, this behavior is supported by experimental observations, such as the fact that warmer water can hold less oxygen, which is critical in aquatic environments. Understanding this inverse relationship between temperature and gas solubility is essential for various applications, including environmental science, biological systems, and chemical engineering.