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 change in concentration) is applied to a system at equilibrium, the system will shift to counteract the stress. Doubling reactant concentration is a stress; the system will shift to consume reactants (favoring product formation), so equilibrium shifts right. The other options are incorrect: shifting left would increase reactants (opposite of countering), equilibrium is affected by concentration change, and equilibrium isn't lost but re - established after shift.

Answer:

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