Sulfur hexafluoride, which is used as a nonflammable insulator in high-voltage transformers, has a Henry’s law constant of 2.4 * 10⁻⁴ mol/L·atm at 25 °C. What is the solubility in mol/L of sulfur hexafluoride in water at 25 °C and a partial pressure of 2.00 atm?

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 relationship can be expressed mathematically as C = kH * P, where C is the concentration of the gas in the liquid, kH is the Henry's law constant, and P is the partial pressure of the gas.

Solubility refers to the maximum amount of a substance that can dissolve in a given volume of solvent at a specific temperature and pressure. In the context of gases, solubility is often expressed in terms of molarity (mol/L), indicating how many moles of gas can be dissolved in one liter of solvent.

Partial pressure is the pressure exerted by a single component of a mixture of gases. In the context of solubility, the partial pressure of a gas above a liquid influences how much of that gas can dissolve in the liquid, as described by Henry's Law. It is typically measured in atmospheres (atm) or other pressure units.