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In the video module, Lavelle says that when Q>K, the reaction hasn't reached equilibrium yet because there is too much product, so it goes from right to left (reverse reaction) to reach equilibrium. My question is: how is it possible to have more product than reactant without going against the idea of having a limiting reactant? Thank you in advance.
I think it is kind of like thinking of it in terms of the reverse reaction (so in this case the products are acting like reactants). But, I also don't think the limiting reactant concept really applies because you are trying to reach equilibrium (instead of trying to complete a reaction to completion, where all of one reactant is used up).
I think of it in terms of the reaction needing to accommodate the decrease in reactant concentration in relation to the concentration of the products, so it needs more reactants so that the equilibrium constant is retained.
Even if there is a limiting reactant, it is still possible to have more product than reactant. What happens is the majority of the reactant (limiting or not) is converted into product, meaning that more of the reacting molecules turned into product than has stayed as reactant.
Since the reaction goes both ways you can think of products being a reactant for the reverse reaction. This helps me think about it because you can just write the reaction with both
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