Equilibrium Textbook Q!

[Andiio]

Hey guys, just wondering for Q28(b) in the Heinemann textbook;

The answer states that The value of K will increase as the temp decreases, so carbon dioxide will be more soluble at low temps.

The equilibrium part makes complete sense, I just don't quite understand why, with a higher K value, and higher concentration of carbon dioxide, why does that make it more soluble? I'd have assumed it would be less soluble :\

Or is it something to do with the relationship of the eq constant and the extent of the reaction? I.e. Higher K value = more spontaneous reaction etc?

Thanks guys!

(the q is:
Sealed bottles of fizzy drinks, such as lemonade and sparkling wines, contain carbon dioxide gas in equilibrium with dissolved carbon dioxide:
CO2(g) <-> CO2(aq)
b) Why are drinks usually cooled before they are carbonated?)

[jane1234]

If the K value is higher this means that the reaction will moved forward more (remember K = products/reactants). So more products means more CO2 (aq) thus making it more soluble at lower temperatures.