Answer:
The solubility of the gas in a liquid increases as the temperature drops and the pressure of the gas on the liquid increases.
Step-by-step explanation:
As the temperature rises, the energy of movement (that is, the kinetic energy) of the solute and solvent particles increases, thereby weakening the intermolecular forces. In this way, interactions between its particles and those of solvent are established, favoring the mixing.
In the case of gases, the decrease in intermolecular forces "releases" the gas molecules from the forces that keep them in solution and will escape from the container, so it will be observed that as the temperature increases, the solubility of a gas decreases in a solvent like water.
On the other hand, the solubility of a gas in a liquid increases with the pressure exerted by the gas on the solvent. If the pressure decreases, the solubility also decreases. Then it is said that the solubility of the gases is directly proportional to the pressure. This influence of the pressure on the solubility of a gas is expressed by Henry's law. This establishes that in a solution, at a constant temperature, the concentration of the dissolved gas is proportional to the partial pressure of the gas that is on the solution, once equilibrium is reached. If Cg is the molar concentration of the gas dissolved in the liquid and Pg its pressure, then:
Cg = kH*Pg
where kH is Henry's constant