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In lecture, Dr. Lavelle had on the slides that if Q<K, then [R]>[P] and the forward reaction is favored. I understand that when Q is less than K that means the ratio of products over reactants is less, signifying that there are more reactants (and less products) at that time than there would be at equilibrium. Thus, the reaction will form more product. However, even if Q<K, I'm not sure if that always means that [R]>[P], right? For example, you could have a Q greater than 1 which means that there are more products than reactant. However, if K is greater than that Q, it will still favor the forward reaction. Even though there are already more products than reactants, there needs to be even more product to reach equilibrium.
Yes, just because Q<K doesn't necessarily mean that [R]>[P]. It just means that more product is favored. For instance, Q can be 10^2 and K can be 10^5. There's a lot more product than reactant, but the K requires even more product.
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