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We know that at equilibrium the forwards reaction rate and the backwards reaction rate are equal to each other. When the reaction is favoring the reactants and going backwards, then we know that Q > K. Q is going to become less and less until it equals K and then the two will be at equilibrium. An example of this type of reaction is if we started with too much of the product and it reacts back into the reactants.
You can think of this in terms of how you calculate Q and K. You divide the products' concentration/pressure to their respective stoichiometric coefficients by the reactants' concentration/pressure to their respective stoichiometric coefficients. If Q>K, you know there is more products present than reactants relative to equilibrium concentrations since products are in the numerator. Therefore, in order to reach equilibrium, the system will shift "backwards" to produce more reactants.
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