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Suppose we have a reversible reaction $$aA + bB <=> cC + dD$$ which is exothermic in the forward direction. If the temperature of the system decreases, the rate of the forward reaction will increase so that the quotient Q increases to the new (higher) value of K

Now consider reducing the concentration of C at a constant temperature. This will initially reduce the quotient, however the rate of forward reaction will then increase to restore the quotient to the original value of K

What am I missing here? Thanks :)

_{c}. This I think I am ok with (I am also taking Q to be a measure of the position of equilibrium).Now consider reducing the concentration of C at a constant temperature. This will initially reduce the quotient, however the rate of forward reaction will then increase to restore the quotient to the original value of K

_{c}. My question is that many sources would say that the position of equilibrium shifts to the right, when in fact it seems that the position of equilibrium has moved left then right again to its original position.What am I missing here? Thanks :)

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