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As we learned, if at some time during a reaction, the reaction quotient, Q, is less than K then the forward reaction is favored. If Q is greater than K then the reverse reaction is favored. However, what happens if Q is equal to K? Does that just mean that the same amount of reactants and products are formed?
If Q is equal to K, that means that the concentrations at the time we are evaluating are equal to the concentrations found when the reaction is in equilibrium. This means that the reaction is in equilibrium, so neither reaction is favored because at equilibrium, the forward and reverse reactions occur at the same rate.
This would mean that the reaction is already at equilibrium and the concentrations of the products and the reactants are unchanging even though movement in each direction may still occur. At this point Q would not even exist and we would call it K. It's just a notation technicality but at a given temperature when Q equals K, Q ceases to exist and it is just K the equilibrium constant.
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