Which of the following statements about gases dissolving in liquids is correct?

The statement that pressure increases gas solubility is correct and is based on Henry's Law, which states that the amount of gas that dissolves in a liquid at a given temperature is directly proportional to the pressure of that gas in equilibrium with the liquid. This means that as the pressure exerted by the gas above a liquid increases, more of that gas will dissolve into the liquid. This principle is particularly crucial in scuba diving, where increased pressure underwater allows greater amounts of gases, such as oxygen and nitrogen, to be dissolved in a diver's bloodstream.

Other statements do not hold true in the same way. For instance, while gases can dissolve in liquids under various conditions, saying they will always dissolve regardless of conditions is misleading, as solubility can be affected by temperature and pressure, among other factors. Additionally, warm temperatures typically decrease the solubility of gases in liquids because warmer liquids have increased kinetic energy, leading to more gas molecules escaping back into the air rather than remaining dissolved. Lastly, while inert gases can dissolve in liquids, they are not the only gases that can do so; many reactive gases, like oxygen and carbon dioxide, also dissolve in liquids effectively.