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When K is between 10^-3 and 10^3, it means that neither the reactants nor the products are favored when the reaction is in equilibrium. You can't necessarily tell which side of the equilibrium has more in concentrations.
When 10^-3<K<10^3, neither the products nor the reactants are significantly favored. However, if K< 1, the reactants are slightly favored and the reaction lies to the left. Also, if K> 1, the products are slightly favored and the reaction lies to the right.
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