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In a reaction at equilibrium, if the concentration of products is increased, wha

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Question: In a reaction at equilibrium, if the concentration of products is increased, what will happen? (2022)

Options:

  1. Equilibrium shifts to the left
  2. Equilibrium shifts to the right
  3. No change
  4. Reaction stops

Correct Answer: Equilibrium shifts to the left

Exam Year: 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.

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)
  1. Equilibrium shifts to the left
  2. Equilibrium shifts to the right
  3. No change
  4. 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.
  • Le Chatelier's Principle – This principle states that if a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the system will adjust to counteract that change and restore a new equilibrium.
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