According to Henry's law, the concentration of a dissolved gas is directly proportional to which factor?

Henry's law states that the concentration of a dissolved gas in a liquid is directly proportional to the partial pressure of that gas above the liquid. This fundamental principle helps to understand how gases behave when they are in contact with liquids. When the partial pressure of the gas increases, more gas molecules enter the solution, increasing the gas's concentration in that solution. Conversely, if the partial pressure decreases, the concentration of the gas in the solution also decreases as gas molecules leave the solution.

The other options do not reflect the correct relationship described by Henry's law. For instance, while temperature can affect the solubility of gases (typically, higher temperatures lead to lower solubility), it is not a variable accounted for by Henry's law in its fundamental form. Additionally, the concentration of the solvent and the volume of the solution are not directly related to the gas concentration as defined by this law. Overall, understanding the relationship between gas concentration and partial pressure is critical to grasping the implications of Henry's law in various scientific and practical applications.