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"If one starts with higher concentrations of reactants, the equilibrium concentrations of the products will be larger." Why is this statement true? Can there be a case where the equilibrium concentration of the product is smaller than the initial concentration of the reactants?
I think it just means that if you have more reactant initially then compared to how much product would be formed if you had less reactant there would be more. Like if you had 2 moles of reactant and it made 3 moles of product, if you had 4 moles of reactant then it would make 6 moles of product.
I'm guessing that the question is kind of talking about how relative to the equilibrium concentration, when there is more initial concentration, then the reaction tends to favor the products in order to reach the equilibrium concentrations. So there probably is a case where the product is smaller than the initial concentration of reactants.
Although adding a reactant increases the concentration of products at equilibrium, the increase in product concentration won't necessarily mean that the equilibrium product concentration becomes higher than that for the reactants. If K is bigger than one, the equilibrium concentration of the products will be greater than that for the reactants. If K is less than one, the equilibrium concentration of the reactants is bigger.
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