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Based on le Châtelier’s Principle, when we make changes to a reaction at equilibrium, the equilibrium will respond by trying to undo the change. For example, if the concentration of products increases, then the reaction forming reactants is favored (reverse reaction). Additionally, if the forward reaction is exothermic and the temperature is increased, then the endothermic reverse reaction will be favored.
Just to clarify, the reverse reaction can only occur when there is some amount of products to turn back into reactants. So, the reverse reaction cannot begin until the forward reaction has produced some products. After that, the reverse reaction will continue to occur, even while the reaction is at equilibrium, and it will be favored when Q>K.
The reverse reaction will begin when Q is larger than K, because in order for Q to approach K, it needs to get smaller, and the only way to do that is to make the denominator of the Q expression, or the concentration of reactants, higher.
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