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Can someone explain why this is true? "If one starts with higher concentrations of reactants, the equilibrium concentrations of the products will be larger." I don't really understand what they mean by "the equilibrium concentrations of the products will be larger." Larger than the equilibrium concentrations of the reactants? I feel like you can't figure out whether the equilibrium concentrations of the products will be larger than the equilibrium concentrations of the reactants without knowing the equilibrium constant.
I think this implies that increasing the concentration of the reactants would push the formation of more product, hence increasing the concentration of the product. But this still makes sure that the ratio of the concentration of products/ concentration of reactants remains the same, therefore the value of K does not change.
To elaborate, increasing the amount of reactant increases the number of moles. This increase in moles then increases the moles per liter of the reactant, also known as the concentration. Because K will only change if the temperature changes, the ratio must be adjusted proportionately, and the product will therefore increase in concentration.
Because the only thing changed in the problem is concentration and k is constant regardless of initial concentrations, more product must be formed in order to make the ratio of concentration of products to concentration of reactants (k) the same.
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