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I am wondering why we raise the concentration to the exponent of the stochiometric coefficient. I understand why we take the products of reactants or products.

For instance, let me give an example to show where I am getting mixed up.

Let's say 2A +3B = 8C as a reversible reaction.

Say the equilibrium concentration of A, B, and C are all 2 moles per liter.

then the equation is 2^8 / (2^2)(2^3) = 16

But the concentration of C is the same as the concentration of A and of B...so why is the equation saying the forward reaction is way more favored? If the forward reaction is so heavily favored, why is the concentration the same as for the reactants?