Solubility of gas using Henry's law

AI Thread Summary
To find the solubility of an unknown gas in water at 1.0 atm using Henry's law, the equation Sg = k*Pg is applied. Given that the solubility at 3.0 atm is 1.02M, the calculation shows Sg = 1.02M/3.0atm * 1.0 atm, resulting in a value of 0.34M. There is confusion regarding whether Pg should be 1.0 atm or 3.0 atm, but the calculation assumes 1.0 atm. Additionally, there is a note that the units were incorrectly interpreted, as the final value should be in molarity (M) rather than atm. The correct solubility of the gas at 1.0 atm is 0.34M.
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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