How does an increase in pressure affect the solubility of a gas in a liquid?

An increase in pressure significantly affects the solubility of a gas in a liquid by increasing it. This relationship is described by Henry's Law, which states that at a constant temperature, the amount of gas that will dissolve in a liquid is directly proportional to the partial pressure of that gas above the liquid. When pressure increases, it compresses the gas molecules, pushing more of them into the liquid phase, thereby enhancing solubility.

This principle is often observed in practical scenarios like carbonated beverages, where the gas (carbon dioxide) is dissolved in the liquid under high pressure. When the bottle is opened, the pressure is released, and the solubility of carbon dioxide decreases, causing it to escape as bubbles.

Thus, an increase in pressure leads to greater solubility of gases in liquids, illustrating a fundamental concept in physical chemistry regarding the behavior of gases under varying pressure conditions.