What does Henry's Law explain about gas solubility?

Henry's Law describes the relationship between the solubility of a gas in a liquid and the pressure of that gas above the liquid. Specifically, it states that the concentration of a gas in a liquid is directly proportional to the partial pressure of that gas in equilibrium with the liquid. This means that as the pressure exerted by the gas increases, more gas molecules are forced into the liquid, increasing the solubility of the gas. This principle is crucial in various environmental applications, such as understanding the behavior of gases in natural water bodies, the design of gas absorption systems, and evaluating the impact of atmospheric pressure changes.

In this context, the other options do not accurately describe Henry's Law. The solubility of a gas is not solely governed by its molecular size, nor is it directly proportional to temperature, especially at varying pressures. Additionally, the assertion that solubility is independent of pressure contradicts the fundamental principle of Henry's Law, which emphasizes the importance of pressure in determining gas solubility in liquids.