Increasing the temperature of a solution where the solute is a gas typically results in the decrease of solubility of the gas in the solution. This phenomenon is known as the effect of temperature on gas solubility.
When a gas dissolves in a liquid, the process is governed by various factors including temperature. According to Henry's law, which describes the relationship between the solubility of a gas in a liquid and the pressure of the gas, the solubility of a gas is directly proportional to its partial pressure. However, Henry's law assumes that the temperature remains constant.
When the temperature of the solution is increased, the solubility of the gas generally decreases. This is because an increase in temperature typically leads to an increase in the kinetic energy of the gas molecules. As the kinetic energy increases, the gas molecules gain more energy and move more rapidly. Consequently, the gas molecules are more likely to escape from the liquid phase and return to the gas phase, resulting in decreased solubility.
It is important to note that the effect of temperature on gas solubility is not universal for all gases. Some gases may exhibit an increase in solubility with increasing temperature, but these cases are less common. The specific behavior of a gas in response to temperature changes depends on factors such as the nature of the gas, the nature of the solvent, and the overall conditions of the system.