Solubility in Relation to Partial Pressure vs. System Pressure

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SUMMARY

The solubility of a gas is primarily governed by Henry's Law, which states that the solubility of a gas in a liquid is directly proportional to its partial pressure. An increase in total system pressure does not inherently increase the solubility of a specific gas unless its partial pressure also rises. In scenarios where non-soluble gases are added, the overall pressure increases, but this does not affect the solubility of the gas in question unless its own partial pressure is altered.

PREREQUISITES
  • Understanding of Henry's Law
  • Knowledge of gas solubility principles
  • Familiarity with concepts of partial pressure
  • Basic principles of thermodynamics
NEXT STEPS
  • Research the implications of Henry's Law on gas solubility in various liquids
  • Explore the relationship between partial pressure and solubility in real-world applications
  • Investigate the effects of temperature on gas solubility
  • Study the impact of non-soluble gases on system pressure and solubility dynamics
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Students and professionals in chemistry and physics, particularly those studying gas behavior in liquids, as well as researchers focusing on environmental science and engineering applications involving gas solubility.

ejnovek
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Hi Physics Forums,

The solubility of a gas according to Henry's Law depends on partial pressure. Would an increase in pressure in a system increase the solubility of a specific gas, even if the partial pressure of that particular gas doesn't change?

The system described above increases in pressure due to additional non-soluble gases.

Thank You,

EJ
 
Last edited:
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Thanks for the post! Sorry you aren't generating responses at the moment. Do you have any further information, come to any new conclusions or is it possible to reword the post?
 

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