What is the relationship between the pressure of a gas and its solubility in a liquid, according to Henry's Law?

Henry's Law states that the solubility of a gas in a liquid is directly proportional to the partial pressure of that gas above the liquid. This implies that as the pressure of the gas increases, more gas molecules are pushed into the liquid, leading to greater solubility. Conversely, if the pressure decreases, the solubility of the gas in the liquid also diminishes because fewer gas molecules are present to dissolve.

This direct proportionality means that if you were to double the pressure of the gas, you would also expect the solubility to double, assuming temperature remains constant. Thus, the relationship outlined by Henry's Law provides a fundamental understanding of how gases behave in liquids, particularly in applications such as carbonated beverages and environmental science where gas solubility in water is critical.