Final answer:
The principle that describes the equilibrium between gaseous and liquid phases is Henry's Law, distinguishing it from other gas laws such as Boyle's, Charles's, and Dalton's laws, and requiring temperatures to be in Kelvins.
So the correct answer is option (D).
Step-by-step explanation:
The principle stating that gases will reach equilibrium between gaseous and liquid environments is known as Henry's Law. This law indicates that the amount of dissolved gas in a liquid is proportional to its partial pressure above the liquid, provided the temperature is constant. This is different from other gas laws such as Boyle's Law, which relates the pressure and volume of a gas at constant temperature, Charles's Law, which relates gas volume and temperature at constant pressure, and Dalton's Law, which states that total pressure exerted by a mixture of non-reacting gases is equal to the sum of the partial pressures of individual gases. It's also important to note that in dealing with gas laws, temperatures must always be expressed in Kelvins.