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When you increase the concentrations of products, is the equilibrium reaction affected? I know that the value of K does not change, so can I say that the position of the reaction rate Q changes relative to K? Would that make the statement true?
Increasing the concentration of the products affects the equilibrium reaction in that it causes the reaction to shift left in favor of the reactants. Q represents the reaction quotient at a certain point and by comparing it to K, you can predict how the reaction will proceed.
What you said about the "position" of Q being changed relative to K due to the greater concentration of products is true, but it might be better to say that Q would end up being more than K since the reaction is now going in the reverse direction (or favoring the reactants to the left).
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