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For values of K which are less than 10-3, the reaction favors the reactants and for K larger than 103 a reaction favors the product. But could someone help me clarify what "not strongly favored" means for intermediate values?
When K>103 products are favored, meaning there is largely more product than reactant at equilibrium. The opposite is true for when K<10-3. For the intermediate values, neither reactants nor products are "strongly favored", meaning there is a relatively equal amount of reactant and product at equilibrium.
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