In a reaction at equilibrium, if the concentration of products is increased, wha
Practice Questions
Q1
In a reaction at equilibrium, if the concentration of products is increased, what will happen? (2022)
Equilibrium shifts to the left
Equilibrium shifts to the right
No change
Reaction stops
Questions & Step-by-Step Solutions
In a reaction at equilibrium, if the concentration of products is increased, what will happen? (2022)
Step 1: Understand that a reaction at equilibrium means the rates of the forward and reverse reactions are equal.
Step 2: Know that Le Chatelier's principle states that if a change is made to a system at equilibrium, the system will adjust to counteract that change.
Step 3: Recognize that increasing the concentration of products means there are more products present in the reaction mixture.
Step 4: According to Le Chatelier's principle, the system will respond by trying to reduce the concentration of products.
Step 5: To reduce the concentration of products, the equilibrium will shift to the left, which means more reactants will be formed.
