For a reaction at equilibrium, if the concentration of products increases, what

For a reaction at equilibrium, if the concentration of products increases, what will happen to the equilibrium position?

For a reaction at equilibrium, if the concentration of products increases, what will happen to the equilibrium position?

Step 1: Understand that a chemical reaction can reach a state called equilibrium, where the rate of the forward reaction equals the rate of the reverse reaction.
Step 2: Recognize that at equilibrium, the concentrations of reactants and products remain constant.
Step 3: Learn about Le Chatelier's principle, which states that if a change is made to a system at equilibrium, the system will adjust to counteract that change.
Step 4: Identify that increasing the concentration of products is a change to the system.
Step 5: According to Le Chatelier's principle, when the concentration of products increases, the equilibrium will shift to reduce that concentration.
Step 6: Conclude that the equilibrium will shift to the left, meaning it will favor the formation of reactants.

Le Chatelier's Principle – This principle states that if a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the system will adjust to counteract that change and restore a new equilibrium.