In a reversible reaction, if the concentration of products increases, what happe

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Question: In a reversible reaction, if the concentration of products increases, what happens to the equilibrium position? (2021)

Options:

Correct Answer: It shifts to the left

Exam Year: 2021

Solution:

According to Le Chatelier\'s principle, if the concentration of products increases, the equilibrium will shift to the left to counteract the change.

In a reversible reaction, if the concentration of products increases, what happens to the equilibrium position? (2021)

In a reversible reaction, if the concentration of products increases, what happens to the equilibrium position? (2021)

Step 1: Understand that a reversible reaction can go in both 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 increase in products.

Le Chatelier's Principle – This principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change.