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How does the solubility of most gases in liquids change with an increase in temperature?
It increases
It decreases
It remains constant
It becomes zero
It decreases
The solubility of most gases in liquids decreases as the temperature of the solvent increases. This occurs because the dissolution of gases in liquids is generally an exothermic process.
The solubility of most gases in liquids decreases as the temperature of the solvent increases. This occurs because the dissolution of gases in liquids is generally an exothermic process.
Think of a carbonated soda bottle: if you leave it out in the hot sun, the gas (carbon dioxide) escapes much faster than if the bottle is kept in a cold refrigerator, leading to a 'flat' drink.
HgasтАЛ+SolventтЗМSolution+Heat
According to Le Chatelier's Principle, if a process is exothermic (releases heat), increasing the temperature shifts the equilibrium to favor the reverse, endothermic direction (the gaseous state). Since the hydration of gas molecules releases energy (╬ФHsolnтАЛ<0), adding heat provides the kinetic energy necessary for gas molecules to overcome the intermolecular forces holding them in the liquid, causing them to escape back into the gas phase.
Gas dissolution is typically exothermic.
Higher kinetic energy allows gas molecules to break free from the liquid phase.
The solubility of gases is inversely proportional to temperature.
Thermal pollution in water bodies reduces dissolved oxygen levels, harming aquatic life.
Carbonated beverages lose fizz when warm.
Aquatic organisms suffer in warm water due to decreased dissolved oxygen.
This behavior is consistent with the Van't Hoff equation for temperature dependence of solubility.
Option A is incorrect because solubility increases with temperature only for most solids, not gases.
B is correct тАФ The solubility of most gases in liquids decreases as temperature increases due to the exothermic nature of the dissolution process.
Always remember that while solid solubility often increases with heat, gases act differently due to their high initial kinetic energy and the exothermic nature of their solvation.