Posted by Erka on Sunday, July 22, 2012 at 7:14pm.
One thing that you should note quickly is that the equilibrium constant expression depends on how we write the chemical reaction.
For example, consider the following reaction
N2O5(g) < - > 2NO2(g) + 1/2O2(g) K = [NO2]2[O2]1/2/[N2O5]
However, we can just as easily multiply the whole reaction by 2- perhaps we don't like the stoichiometric coefficient of 1/2 in front of the oxygen. This gives
2N2O5(g) < - > 4NO2(g) + O2(g) K' = [NO2]4[O2]/[N2O5]2
K depends on how you write the chemical reaction! If you multiply the chemical equation by a given number (such as 2), it is the same as raising the equilibrium constant expression to that power. (K' = K2 in the above example.)
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