![]() ![]() This increased partial pressure means that more gas particles will enter the liquid (there is therefore less gas above the liquid, so the partial pressure decreases) in order to alleviate the stress created by the increase in pressure, resulting in greater solubility. An increase in pressure would result in greater partial pressure (because the gas is being further compressed). Extending the implications from Henry's law, the usefulness of Le Chatelier's principle is enhanced in predicting the effects of pressure on the solubility of gases.Ĭonsider a system consisting of a gas that is partially dissolved in liquid. Conversely, when the partial pressure increases in such a situation, the concentration of gas in the liquid will increase as well the solubility also increases. This formula indicates that (at a constant temperature) when the partial pressure decreases, the concentration of gas in the liquid decreases as well, and consequently the solubility also decreases. \(c\) is the concentrate of the gas in the liquid. ![]() \(p\) is the partial pressure of the gas above the liquid,.Consider the following formula of Henry's law: Henry's law dictates that when temperature is constant, the solubility of the gas corresponds to it's partial pressure. Gases: The effects of pressure on the solubility of gases in liquids can best be described through a combination of Henry's law and Le Chatelier principle.Solids & Liquids: The effects of pressure changes on the solubility of solids and liquids are negligible.The effects of pressure are only significant in affecting the solubility of gases in liquids. Consequently, the equilibrium concentration of the gas particles in gaseous phase would decrease, resulting in greater solubility. In turn, Le Chatelier's principle predicts that the system shifts toward the product side in order to compensate for this new stress. Consequently, the equilibrium concentration of the gas particles in gaseous phase increases, resulting in lowered solubility.Ĭonversely, decreasing temperatures result in stress on the reactant side (because heat is on the product side). In turn, Le Chatelier's principle predicts that the system shifts towards the reactant side in order to alleviate this new stress. As such, increasing temperatures result in stress on the product side (because heat is on the product side). First, note that the process of dissolving gas in liquid is usually exothermic. Le Chatelier's principle allows better conceptualization of these trends. ![]() The trend is thus as follows: increased temperatures mean lesser solubility and decreased temperatures mean higher solubility. As a result, the gas particles dissolved in the liquid are more likely to escape to the gas phase and the existing gas particles are less likely to be dissolved. The greater kinetic energy results in greater molecular motion of the gas particles. As temperature increases, kinetic energy increases. In understanding the effects of temperature on the solubility of gases, it is first important to remember that temperature is a measure of the average kinetic energy. By shifting towards the reactant's side, less of the solid is dissociated when equilibrium is again established, resulting in decreased solubility. Le Chatelier's principle predicts that the system shifts toward the reactant side in order to alleviate this stress. <0\)): Increasing the temperature results in a stress on the products side from the additional heat. ![]()
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