In the relationship defined by Henry's Law, what happens to the solubility of a gas as the pressure increases?

Henry's Law states that the amount of gas that dissolves in a liquid is directly proportional to the pressure of that gas above the liquid, assuming constant temperature. This means that as the pressure of the gas increases, more gas molecules are forced into the solution, leading to an increase in solubility. The rationale behind this is that higher pressure compresses gas molecules, which in turn increases their interactions with the solvent.

This principle is widely observed in nature and applications; for example, carbonated beverages are bottled under high pressure, allowing carbon dioxide to dissolve in the liquid. When the pressure is released (for instance, when the bottle is opened), the solubility decreases as the gas escapes, which aligns with the understanding of gas behavior under varying pressures.

Thus, the correct conclusion is that as the pressure of a gas increases, so does its solubility in a liquid, which is why the answer indicating an increase in solubility is correct.