According to Henry's law, the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid and inversely proportional to the temperature of the liquid. Therefore, as temperature is increased, the rate of dissolution of a gas in a liquid decreases.

This can be understood by considering the behaviour of gas molecules at different temperatures. At higher temperatures, gas molecules have more energy and move faster. This means that they are more likely to escape from the liquid and return to the gas phase, decreasing the concentration of dissolved gas in the liquid. Conversely, at lower temperatures, gas molecules have less energy and move slower, making them less likely to escape from the liquid and increasing the concentration of dissolved gas.

The effect of temperature on the rate of dissolution of a gas is particularly important in cases where the gas is sparingly soluble in the liquid. For example, the solubility of oxygen in water decreases by about 20% for every 10°C increase in temperature. This means that at higher temperatures, less oxygen is available for aquatic organisms to breathe, which can have negative impacts on their survival and growth.