Question

according to le chateliers 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.

Explanation:

Le Chatelier’s principle states that if a stress is applied to a system at equilibrium, the system will shift to counteract that stress. Reducing the concentration of a product is a stress. To counteract this, the system will produce more products, which means the equilibrium will shift to the right (toward the products side) to favor product formation. The other options are incorrect: shifting left would further reduce products (opposite of what's needed), and the exothermic/endothermic directions relate to temperature changes, not concentration changes of products.

Answer:

A. The equilibrium shifts to the right to favor the formation of products.