Final answer:
The solubility of gases in liquids decreases as temperature increases because higher thermal energy allows gas molecules to overcome the attraction to solvent molecules and escape back into the gas phase. Pressure can also influence gas solubility; higher pressure usually increases solubility.
Step-by-step explanation:
Effect of Temperature on the Solubility of Gases
Temperature is a crucial factor affecting the solubility of gases in liquids. The solubility of gases tends to decrease with increasing temperature. This occurs because higher temperatures provide thermal energy that overcomes the attractive forces between the gas molecules and solvent, leading to a decrease in solubility. This phenomenon is similar to that which causes an increase in vapor pressure of liquids with temperature. For instance, substances like HCl, NH3, and SO2 demonstrate reduced solubility as temperature rises, which is a common observation for many gases.
Pressure also influences the solubility of gases, as described by Henry's law. An increase in pressure typically leads to an increase in gas solubility. However, when temperatures rise, any dissolved gas is more likely to escape into the gas phase due to increased kinetic energy, thus decreasing its solubility in the solvent.