How does temperature impact solubility of gasses?
The solubility of gases in a liquid generally decreases with increasing temperature. This relationship is known as Henry's law. According to Henry's law, at a constant pressure, the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid.
When the temperature is increased, the kinetic energy of the gas molecules also increases. As a result, the collisions between gas molecules become more energetic, causing them to escape from the liquid more frequently. This leads to a decrease in the solubility of gases as temperature increases.
Conversely, when the temperature is decreased, the kinetic energy of the gas molecules decreases, reducing their ability to escape from the liquid. This results in higher solubility of gases at lower temperatures.
It is important to note that the effect of temperature on gas solubility can vary depending on the specific gas and liquid involved.