What is the effect of temperature on the solubility of gases in liquids?

The solubility of gases in liquids generally decreases as temperature increases. This is a consequence of the kinetic energy of the gas molecules. When the temperature rises, the increased kinetic energy allows gas molecules to escape from the liquid more easily, leading to a decrease in the amount of gas that remains dissolved in the liquid.

This relationship is often explained using Henry's Law, which states that at a constant temperature, the solubility of a gas in a liquid is directly proportional to the partial pressure of that gas above the liquid. However, as temperature increases, the ability of the gas to be "held" in solution is diminished because the gas molecules gain enough energy to overcome the attractive forces binding them to the liquid, thus escaping into the atmosphere.

In contrast, the other options describe incorrect scenarios. The idea that solubility increases with temperature is more applicable to solids in liquids than to gases. Saying that solubility remains constant implies that no temperature effects are present, which does not reflect the behavior of gases. Lastly, the notion that solubility varies unpredictably with temperature contradicts the established trend that predicts a specific decrease in solubility with rising temperature for gases.