Solubility of Gases: Why Decreases with Temp Increase?

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SUMMARY

The solubility of gases in liquids decreases with increasing temperature due to the increase in kinetic energy, which causes gas molecules to escape from the solution. This phenomenon is exemplified by the behavior of carbonated beverages, where heating leads to a loss of carbonation. While exceptions exist, such as helium in water, the general trend is consistent across most gases. For a deeper understanding, advanced thermodynamic texts are recommended for quantitative analysis.

PREREQUISITES
  • Basic understanding of thermodynamics
  • Familiarity with gas laws
  • Knowledge of kinetic molecular theory
  • Concept of vapor pressure and evaporation
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  • Research the impact of temperature on gas solubility using Henry's Law
  • Explore the kinetic molecular theory in detail
  • Study the principles of vapor pressure and its relation to temperature
  • Examine advanced thermodynamic texts for quantitative solubility data
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Chemistry students, environmental scientists, and professionals in the beverage industry seeking to understand the effects of temperature on gas solubility in liquids.

London Kngiths
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I was wondering if anyone could point me in the direction of some good information regarding why the solubility of gases decreases with the increase of temperature. The only description I have is a cheap example involving a pop can where as the temperature of the can is increased the kinetic energy increases and gas leaves the solution. This results in the flatness of the pop. I was wondering if anyone could point me in the direction of a more description explanation.
 
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--- excepting He in water, solubility increases with temperature, and maybe some others. How much thermo have you had? Or, how deeply did you feel like digging?
 
The evaporation occurs primarily through the top surface of the liquid. The concept should make perfect sense. If you want the quantitative details, you will need to peruse through some advanced books.
 

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