(adsbygoogle = window.adsbygoogle || []).push({}); 1. The problem statement, all variables and given/known data

A gas has a Henry's law constant of 0.150 M/atm. How much water would be needed to completely dissolve 1.49 L of the gas at a pressure of 720 torr and temp of 14 C.

2. Relevant equations

m = amount solute (in mol)/mass solvent(in kg)

M = amount solute (in mol)/volume solution (in L)

Henry's Law: [tex]S_{gas} = k_{H}*P_{gas}[/tex]

3. The attempt at a solution

Convert torr to atm:

[tex]S_{gas} = k_{H}*P_{gas}[/tex]

[tex]S_{gas} = .150 M/atm*(720/760) atm[/tex]

[tex]S_{gas} = .1421 M[/tex]

[tex].1420 \frac{mol}{L} = \frac{?}{1.49 L}[/tex]

1.49 L of this gas contains .2117 moles.

That's where I get stuck. Not sure about the dissolving portion of this problem. Any help would be appreciated.

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# Homework Help: Gen. Chem: Solubility

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