According to Henry's law, how is gas solubility in a liquid related to pressure?

According to Henry's law, the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid. This means that as the pressure of the gas increases, more gas molecules are forced into the liquid, resulting in higher solubility. Mathematically, this relationship can be expressed as ( S = k_H \cdot P ), where ( S ) is the solubility of the gas, ( P ) is the partial pressure of the gas, and ( k_H ) is Henry's law constant, which is specific to the gas-liquid combination.

This relationship highlights that if the pressure is doubled, the solubility of the gas in the liquid will also double, demonstrating a linear increase in solubility with increasing pressure. Understanding this principle is essential in various applications, such as scuba diving, carbonated beverages, and environmental science, where gas solubility impacts biological and chemical processes.