An increase in temperature generally decreases the solubility of gases in water. This relationship is described by 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.
When temperature increases, the kinetic energy of the gas molecules also increases. This leads to more energetic and rapid motion of gas molecules, which makes it easier for them to escape from the liquid phase into the gas phase. As a result, the equilibrium between the gas phase and the dissolved gas in the liquid is disturbed, leading to a decrease in solubility.
This relationship can be observed in everyday examples. For instance, carbonated beverages (such as soda) contain dissolved carbon dioxide (CO₂) under high pressure. When the bottle is opened and the pressure is released, the solubility of CO₂ decreases as the gas comes out of solution and forms bubbles. Additionally, you might have noticed that cold water can hold more dissolved oxygen than warm water, which is why colder water generally supports aquatic life better.
It's important to note that the effect of temperature on gas solubility is not the same for all gases. Some gases, such as ammonia (NH₃), actually exhibit an increase in solubility with increasing temperature due to specific molecular interactions. However, for most gases, including common atmospheric gases like oxygen (O₂) and carbon dioxide (CO₂), the solubility decreases with increasing temperature.