Which of the following increases solubility according to exceptions of Le Chatelier's Principle?

The correct choice is based on Le Chatelier's Principle, which states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract that change.

In the case of solubility, heating an exothermic dissolution reaction leads to an increase in solubility. For exothermic reactions, energy is released when the solute dissolves; therefore, if the temperature is increased, the system will shift equilibrium to absorb that added energy, favoring the dissolution of more solute and resulting in increased solubility.

This principle applies specifically to solvation reactions that are exothermic, where heat can be thought of as a product. By increasing the temperature, the system effectively drives the equilibrium towards producing more dissolved solute, increasing solubility.

Other options do not typically lead to an increase in solubility according to the principles of chemical equilibria. For example, increasing pressure generally affects gases more than solids and liquids, while adding a nonreactive gas to a solution does not impact the solubility of a solute. Reducing the quantity of solvent typically concentrates the solute rather than increasing solubility.