Final answer:
Gases dissolve in liquids in proportion to their partial pressure, solubility, and temperature. Henry's law outlines that solubility is directly proportional to pressure. Temperature increases lead to decreased gas solubility, while pressure increases lead to increased solubility.
Step-by-step explanation:
Yes, gases dissolve in liquids in proportion to their partial pressure (Pg), solubility (Cg), and temperature according to Henry's law. This law states that the solubility of a gas in a liquid is directly proportional to the pressure of the gas above the solution. The formula that represents this relationship is Cg = kPg, where k is the proportionality constant, which varies depending on the nature of the gas, the solvent, and the temperature of the solution.
The effect of temperature on the solubility of gases is that an increase in temperature generally leads to a decrease in gas solubility. This is because higher temperatures provide more thermal energy to overcome the attractive forces between the gas molecules and the solvent, resulting in lower solubility. In contrast, the solubility of most solid or liquid solutes typically increases with an increase in temperature.
Pressure and Gas Solubility
Pressure also significantly affects the solubility of gases. When the partial pressure of the gas above the liquid increases, the solubility of the gas also increases. More gas molecules come in contact with the liquid and dissolve into it when the pressure is increased, leading to a higher concentration of dissolved gas.