The greater kinetic energy results in greater molecular motion of the gas particles. 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 converse is true as well. The trend is thus as follows: increased temperatures mean lesser solubility and decreased temperatures mean higher solubility. Le Chatelier's principle allows better conceptualization of these trends.
First, note that the process of dissolving gas in liquid is usually exothermic. As such, increasing temperatures result in stress on the product 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. Consequently, the equilibrium concentration of the gas particles in gaseous phase increases, resulting in lowered solubility.
Conversely, 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 toward the product side in order to compensate for this new stress. Consequently, the equilibrium concentration of the gas particles in gaseous phase would decrease, resulting in greater solubility. 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.
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. 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.
Consider a system consisting of a gas that is partially dissolved in liquid. An increase in pressure would result in greater partial pressure because the gas is being further compressed. 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.
The converse case in such a system is also true, as a decrease in pressure equates to more gas particles escaping the liquid to compensate. Bob is in the business of purifying silver compounds to extract the actual silver. He is extremely frugal. One day, he finds a barrel containing a saturated solution of silver chloride. Which of the three should Bob add to the solution to maximize the amount of solid silver chloride minimizing the solubility of the silver chloride?
Bob should add table salt to the solution. According to the common-ion effect, the additional Cl - ions would reduce the solubility of the silver chloride, which maximizes the amount of solid silver chloride. Allison has always wanted to start her own carbonated drink company. Recently, she opened a factory to produce her drinks. She wants her drink to "out-fizz" all the competitors. That is, she wants to maximize the solubility of the gas in her drink. Butters is trying to increase the solubility of a solid in some water.
He begins to frantically stir the mixture. Should he continue stirring? Why or why not? He stop stop stirring. Stirring only affects how fast the system will reach equilibrium and does not affect the solubility of the solid at all.
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