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Solubility of gas in liquid.

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Illustrate the relationship between a pressure of a gas above a liquid and the solubility of the gas in the liquid. Determine the concentration of CO2 in a carbonated beverage bottled under 4.0 atm of CO2. (a) If the mole fraction of CO2 in the air is 0.00355, how many times more concentrated is the CO2 in the unopened bottle than it is in a glass of the beverage that has gone completely flat? (b) Use the kinetic-molecular theory of gases to explain why the solubility of a gas is proportional to its pressure over the liquid.

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Please see the attached file.

You might want to check out the following sites:
http://scidiv.bcc.ctc.edu/wv/09/0009-006-henry.html
http://tutor.lscf.ucsb.edu/instdev/sears/biochemistry/tw-exp/henryslaw.htm
http://wine1.sb.fsu.edu/chm1045/notes/Gases/Mixtures/Gases06.htm
http://hyperphysics.phy-astr.gsu.edu/hbase/kinetic/henry.html

The solubility of a gas in a liquid depends on temperature, the partial pressure of the gas over the liquid, the nature of the solvent and the nature of the gas. The most common solvent is water.
Gas solubility is always limited by the equilibrium between the gas and a saturated solution of the gas. The dissolved gas will always follow Henry's law.
The concentration of dissolved gas depends on the partial pressure of the gas. The partial pressure controls the number of gas molecule collisions with the surface of the solution.

Henry's law states that the ratio of ...

Solution Summary

The solution demonstrates how to explain Henry's Law using the kinetic theory of gases.

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I don''t know where to start on this problem. I have tried many different attempts but now I think that not all of the information is necessary...it this the case? Could you assist me in setting up the problem?

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