What does Henry's Law state about gas dissolution in liquids?

Henry's Law states that the amount of gas dissolved in a liquid at a constant temperature is directly proportional to the partial pressure of that gas above the liquid. This means that if the partial pressure of the gas increases, more of that gas will dissolve in the liquid until a new equilibrium is reached. This principle is particularly important in various fields such as chemistry, environmental science, and medicine, where understanding gas solubility under different pressure conditions is necessary.

In practical terms, this law explains phenomena such as why carbonated beverages contain dissolved carbon dioxide under pressure; when the pressure is released (for example, by opening a bottle), the gas escapes, leading to the formation of bubbles. This law does not consider the temperature's role in gas solubility or suggest that the amount of gas dissolved is independent of pressure, which is why options referencing temperature or independence from pressure do not accurately reflect Henry's Law.