According to Henry's Law, which factor affects the solubility of a gas?

Henry's Law states that the amount of gas that dissolves in a liquid at a given temperature is directly proportional to the partial pressure of that gas above the liquid. This means that as the partial pressure of the gas increases, more of that gas will dissolve in the solvent until a new equilibrium is reached. The relationship is typically described by the equation:

[ C = k_H \times P ]

where ( C ) is the concentration of the dissolved gas, ( k_H ) is Henry's law constant (which is specific to the gas and the solvent at a certain temperature), and ( P ) is the partial pressure of the gas.

This direct relationship indicates that manipulating the vapor partial pressure of the gas (such as increasing it by adding more gas to the system) will affect the solubility of that gas in the solvent. Therefore, the factor that directly influences gas solubility according to Henry's Law is indeed the vapor partial pressure of the gas.

The other factors, while they can affect the overall solubility in a broader perspective, do not directly influence the relationship defined by Henry's Law. For instance, while the temperature of the solvent can impact gas solubility, it is not a factor in Henry's