Question

according to le chatelier’s principle, what happens when the concentration of reactants is doubled 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 is unaffected by the increase in concentration.
○ the equilibrium is lost because the concentrations have been disturbed.

Explanation:

Le Chatelier's principle states that if a stress (like changing concentration) is applied to a system at equilibrium, the system will shift to counteract the stress. When reactant concentration is doubled, the system tries to reduce the excess reactants by converting them to products, so the equilibrium shifts right (towards product formation). The equilibrium isn't lost (it adjusts), isn't unaffected (concentration change is a stress), and doesn't shift left (left would make more reactants, worsening the excess).

Answer:

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