Final answer:
Removing a product from an exothermic reaction at equilibrium causes the reaction to shift in the forward direction to produce more product, as per Le Chatelier's Principle, until a new equilibrium is established.
Step-by-step explanation:
When a product is removed from an exothermic reaction at equilibrium, the system shifts to compensate for the loss. This phenomenon is explained by Le Chatelier's Principle, which states that if an external change is applied to a reaction at equilibrium, the reaction adjusts to minimize that change.
In response to the removal of a product, the reaction shifts in the forward direction, or rightward, to replenish the product that was removed. This means that the concentrations of the reactants will decrease as more reactants are converted into products to restore equilibrium. The overall concentration of products will initially decrease due to the removal, but as the reaction shifts to the right, it will start to increase again until equilibrium is re-established.
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