Final answer:
Henry's law states the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid, expressing the relationship with the formula С = kHP. The law is crucial for predicting gas solubility changes with pressure in various scientific and industrial applications.
Step-by-step explanation:
Understanding Henry's Law
Henry's law pertains to the relationship between the pressure and the solubility of a gas. Specifically, it states that the concentration of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid. This can be formulated as: С = kHP, where C represents the concentration of the dissolved gas, P is the partial pressure. For any given system of a particular gas and solvent at a constant temperature, this law enables us to predict how the gas's solubility will change with changes in pressure.
Henry's Law provides insight into various practical applications such as carbonated beverages, where the solubility of CO2 is maintained by keeping the drinks under high pressure. In the natural world, it affects how gases dissolve in our oceans and other bodies of water, having implications on aquatic life and ecosystem dynamics. This principle is also important in industries that involve gases dissolving in liquids, such as in chemical manufacturing and the use of anesthetics.