In a reversible reaction, if the concentration of products is increased, what wi

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Question: In a reversible reaction, if the concentration of products is increased, what will happen to the equilibrium? (2021)

Options:

Correct Answer: Shift to the left

Exam Year: 2021

Solution:

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

In a reversible reaction, if the concentration of products is increased, what will happen to the equilibrium? (2021)

In a reversible reaction, if the concentration of products is increased, what will happen to the equilibrium? (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: 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: Recognize that increasing the concentration of products means there are more products present in the reaction.
Step 5: According to Le Chatelier's principle, the system will try to reduce the effect of this increase by shifting the equilibrium to the left, which means favoring the formation of reactants.

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.