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What happens to the equilibrium position when the concentration of a reactant is

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Question: What happens to the equilibrium position when the concentration of a reactant is increased in a reversible reaction?

Options:

  1. The equilibrium shifts to the right
  2. The equilibrium shifts to the left
  3. The equilibrium remains unchanged
  4. The reaction stops

Correct Answer: The equilibrium shifts to the right

Solution: 

According to Le Chatelier\'s Principle, increasing the concentration of a reactant will shift the equilibrium position to the right to favor the formation of products.

What happens to the equilibrium position when the concentration of a reactant is

Practice Questions

Q1
What happens to the equilibrium position when the concentration of a reactant is increased in a reversible reaction?
  1. The equilibrium shifts to the right
  2. The equilibrium shifts to the left
  3. The equilibrium remains unchanged
  4. The reaction stops

Questions & Step-by-Step Solutions

What happens to the equilibrium position when the concentration of a reactant is increased in a reversible reaction?
  • Step 1: Understand that a reversible reaction can go in two directions: from reactants to products and from products back 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 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 4: When the concentration of a reactant is increased, the system will try to reduce that concentration.
  • Step 5: To reduce the concentration of the added reactant, the equilibrium will shift to the right, favoring the formation of more products.
  • Step 6: As a result, more products are formed until a new equilibrium is established.
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