In a reaction at equilibrium, if the concentration of products is increased, what will happen? (2022)
Practice Questions
1 question
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
According to Le Chatelier's principle, increasing the concentration of products will shift the equilibrium to the left, favoring the formation of reactants.
Questions & Step-by-step Solutions
1 item
Q
Q: In a reaction at equilibrium, if the concentration of products is increased, what will happen? (2022)
Solution: According to Le Chatelier's principle, increasing the concentration of products will shift the equilibrium to the left, favoring the formation of reactants.
Steps: 5
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.
