According to le chatelier’s principle, what happens when the concentration of a product is reduced in a chemical reaction that was in equilibrium? the equilibrium shifts to the right to favor the formation of products. the equilibrium shifts to the left to favor the formation of reactants. the equilibrium shifts in the exothermic direction. the equilibrium shifts in the endothermic direction.

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According to Le Chatelier’s principle, when the concentration of a product is reduced in a chemical reaction that was in equilibrium The equilibrium shifts to the right to favor the formation of products.

Le Chatelier's principle states that in a chemical reaction that is in equilibrium, a disturbance in the reaction conditions will make the equilibrium to shift in the opposing direction of the change to restore the steady state. If the concentration of a product is reduced, the equilibrium will shift to the left to try to restore the initial amount of product and achieve the steady state again.

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Answer:

a. energy is absorbed in the reaction.

explanation:

if in a given reaction the energy of products is greater than the energy of reactants it means that reaction is endothermic and during the reaction, the energy is absorbed by reactants. in an endothermic reaction, the products have more stored chemical energy than the reactants. and in this reaction the reactants are more stable than products before the compounds with less energy are always more stable.