The solubility of a gas is more affected by which factor?

The solubility of a gas is significantly influenced by pressure due to Henry's Law, which states that the amount of gas that can be dissolved in a liquid is directly proportional to the partial pressure of that gas above the liquid. When the pressure increases, more gas molecules are forced into solution, thereby increasing the gas's solubility. This is particularly observable in carbonated beverages, where the high pressure inside the bottle keeps more carbon dioxide dissolved until the cap is removed, allowing the pressure to drop and the gas to escape.

Other factors, such as temperature, certainly do affect gas solubility as well, typically showing that gases are less soluble at higher temperatures; however, the effect of pressure remains more pronounced in many scenarios. Volume and viscosity are not primary factors impacting gas solubility in the same direct manner as pressure, making pressure the most critical factor to consider in this context.