Final answer:
An increase in pressure raises the solubility of gases in liquid by compressing the gas and increasing its concentration, while a decrease in pressure has the opposite effect, exemplified by the release of carbon dioxide when opening a soda can.
Step-by-step explanation:
Understanding how pressure affects the solubility of gases in a solution is an important aspect of chemistry. According to Henry's Law, the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the solution. When you increase the pressure, more gas molecules enter the solution as the concentration of molecules in the gas phase above the solution increases, resulting in a higher concentration of dissolved gases. Conversely, decreasing the pressure causes gas molecules to escape from the solution, decreasing their solubility.
An increase in pressure decreases the volume of gas, leading to a higher concentration of gas molecules, and consequently, more gas dissolves in the liquid. This is evident when opening a soda can; as the pressure above the liquid drops, carbon dioxide bubbles out since its solubility decreases. Understanding these principles helps explain everyday phenomena and informs practices in various industries involving the dissolution or release of gases.