What generally happens to the solubility of gas solutes as temperature increases?

As the temperature increases, the solubility of gas solutes typically decreases. This phenomenon is primarily due to the increased kinetic energy of the gas molecules, which allows them to escape from the solvent more easily. As the gas molecules gain energy, they move more rapidly and are less likely to be captured by the solvent molecules, leading to a reduction in the overall amount of gas that can remain dissolved in the liquid.

Additionally, the principles governing gas solubility can be understood through Henry's Law, which states that at a constant temperature, the amount of gas that dissolves in a liquid is proportional to the partial pressure of the gas above the liquid. When the temperature rises, if the pressure remains constant, the solubility decreases because the gas molecules will tend to leave the solution, further supporting the observation that higher temperatures diminish the solubility of gases.

In contrast, the solubility behavior of solids typically increases with temperature, but this does not apply to gases, reinforcing why the correct choice reflects a decrease in gas solubility with rising temperatures.