How does increasing temperature affect gas solubility in liquids?

Increasing temperature typically decreases gas solubility in liquids due to the increased kinetic energy of the gas molecules. As the temperature rises, gas molecules move more rapidly, which makes it more likely for them to escape from the liquid into the atmosphere rather than remain dissolved. This behavior is explained by Henry's Law, which states that the amount of gas that dissolves in a liquid is directly proportional to the partial pressure of the gas above the liquid and inversely related to temperature. Therefore, as temperature increases, it becomes more difficult for the gas to remain in solution, resulting in decreased solubility.

In contrast, lower temperatures tend to favor solubility, allowing gases to dissolve better as their kinetic energy decreases, and they are more likely to stay in solution. The options suggesting an increase in solubility or no effect ignore the fundamental thermodynamic principles governing gas behavior in liquids. Additionally, stating that increased temperature leads to complete solubility does not reflect the behavior of gases, which may become less soluble as they escape more readily into the air.