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Thread: Henry's law of solubility

  1. #1 Henry's law of solubility 
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    I am told by reviewers that diffusion in gasses and liquids occurs only as a result of concentration gradients or concentration difference, not some other variable like temperature.
    How then does one explain these effects?:
    1. CO2 is kept in solution in a carbonated beverage by exchange with CO2 gas trapped in the can. If you open a can from the fridge the fizz is gradually lost (and so eventually is the acrid tast of carbonate, but that is another argument I have with the reviewers).
    Then if you open a can that has been at room temperature the fizz is lost much more quickly. Same concentration difference as before.
    2. If you pour the contents of the can from the fridge over fresh ice cubes they froth like crazy. Flow goes against the concentration gradient and the fizz is lost in seconds.


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  3. #2  
    Him
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    I’m quite sure I have the solution to your problem.
    Your observations are correct and yes the reviewers are also right. The thing that happens is that the solubility of CO2 in water is lower in cold water.
    Water is releasing gas because there’s more CO2 in the water then it can hold. When poring over ice the water can hold even less CO2 creating a high concentration of gas right above his surface, which expands in a concentration gradient manner (independently from temperature).

    I hope this helped you?


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