In a reversible reaction, if the concentration of products increases, what happe
Practice Questions
Q1
In a reversible reaction, if the concentration of products increases, what happens to the equilibrium position? (2021) 2021
It shifts to the left
It shifts to the right
It remains unchanged
It shifts to the center
Questions & Step-by-Step Solutions
In a reversible reaction, if the concentration of products increases, what happens to the equilibrium position? (2021) 2021
Step 1: Understand that a reversible reaction can go in two directions: from reactants to products and from products to reactants.
Step 2: Know that equilibrium is the point where the rate of the forward reaction equals the rate of the reverse reaction.
Step 3: Recognize that if the concentration of products increases, it means there are more products present in the reaction mixture.
Step 4: Apply 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 5: Since the concentration of products has increased, the system will try to reduce this concentration by shifting the equilibrium position.
Step 6: The equilibrium will shift to the left, meaning it will favor the formation of reactants to balance the increased concentration of products.
