According to Henry's Law, what happens to gas solubility with increasing pressure?

Henry's Law states that the amount of gas that dissolves in a liquid at a given temperature is directly proportional to the partial pressure of that gas above the liquid. This means that as the pressure of the gas increases, more gas molecules are forced into the solution, resulting in an increase in solubility.

This principle is commonly observed in carbonated beverages, where the pressure of carbon dioxide gas in the can or bottle keeps the CO2 dissolved in the liquid. When you open the container, the pressure decreases, leading to a decrease in the gas solubility, and bubbles of CO2 escape from the solution. Thus, the direct relationship between pressure and gas solubility according to Henry's Law explains why the correct answer highlights that gas solubility increases with rising pressure.