Solubility of gas using Henry's law

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SUMMARY

The solubility of an unknown gas in water at 1.0 atm can be calculated using Henry's Law, represented by the equation Sg = k * Pg. Given that the solubility at 3.0 atm is 1.02M, the solubility at 1.0 atm is determined to be 0.34M. The calculation involves dividing the solubility at 3.0 atm by the corresponding pressure and multiplying by the new pressure. It is crucial to ensure that units are correctly managed throughout the calculation.

PREREQUISITES
  • Understanding of Henry's Law and its application in gas solubility
  • Knowledge of molarity (M) and atmospheric pressure (atm)
  • Ability to perform unit conversions and dimensional analysis
  • Familiarity with basic chemistry concepts related to gas behavior
NEXT STEPS
  • Study the implications of varying pressures on gas solubility using Henry's Law
  • Explore the relationship between temperature and gas solubility
  • Learn about different gases and their solubility coefficients in various solvents
  • Investigate applications of Henry's Law in real-world scenarios, such as carbonated beverages
USEFUL FOR

Chemistry students, researchers in physical chemistry, and professionals involved in environmental science or chemical engineering will benefit from this discussion.

protractor
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Homework Statement


What is the solubility of an unknown gas in water at 1.0 atm if its solubility at 3.0 atm is 1.02M?

Homework Equations


Henry's law Sg = k*Pg

The Attempt at a Solution


Sg = 1.02M/3.0atm * 1.0 atm = .34 atm

I'm not sure if Pg, the partial pressure of the gas, is 1.0 atm or 3.0 atm.
 
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protractor said:
Sg = 1.02M/3.0atm * 1.0 atm = .34 atm
Are the units correct?
 
mjc123 said:
Are the units correct?
.34 is in M instead of atm (I forgot to cancel out the atm).
 

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