When gas is free, it has more entropy than when it is in a solution. The molecules become more active and tend to be in a situation of greater freedom as the temperature rises. Therefore, solubility would decrease.
As the kinetic energy of the molecules increases, more molecules will transition into vapors, increasing the vapor pressure.
<h3>Why does the solubility of gas decrease with increasing temperature?</h3>
In contrast to a solution, a gas has more entropy when it is free. As the temperature rises, the molecules become more energetic and tend to be in a condition of greater freedom. Solubility would consequently decline.
Just like liquid molecules, gas molecules dissolved in liquids are always moving. Because they are drawn to the liquid molecules, the gas molecules remain in the solution. Lower solubility results from the fact that as temperature rises, all molecules, including gas molecules, gain more kinetic energy, move more quickly, and can escape from solutions more readily when they strike the surface. As a result, fewer molecules remain inside the solution.
<h3>Why does vapor pressure increase with increasing temperature?</h3>
The pressure that a pure component applies at equilibrium when both the liquid and vapor phases are present, regardless of temperature, is known as the vapor pressure.
The kinetic energy of the molecules in a liquid increase with their temperature. The number of molecules that transition into a vapor also rises as a function of the molecules' kinetic energy, which raises the vapor pressure.
Learn more about the variation of solubility with the temperature here:
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