As the temperature of a solution that contains a gas is decreased the solubility of that gas also increases.
This statement is generally incorrect. The solubility of most gases tends to decrease as the temperature of the solution decreases. This is based on the principle known as Henry's Law, which states that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid.
According to Henry's Law, at higher temperatures, the kinetic energy of gas molecules increases, leading to increased movement and escape of gas molecules from the liquid. This results in lower solubility of the gas in the liquid. Conversely, at lower temperatures, the kinetic energy of gas molecules decreases, reducing their ability to escape from the liquid and thus increasing the solubility.
However, it is important to note that there are some exceptions to this trend. For example, the solubility of some gases, such as carbon dioxide, may indeed increase with decreasing temperature due to the formation of certain types of intermolecular forces.