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For the reaction A(g) + B(g) ⇌ C(g), if the concentration of C is increased, wha

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Question: For the reaction A(g) + B(g) ⇌ C(g), if the concentration of C is increased, what will be the effect on the equilibrium? (2020)

Options:

  1. Shift to the left
  2. Shift to the right
  3. No effect
  4. Increase the rate of reaction

Correct Answer: Shift to the left

Exam Year: 2020

Solution: 

Increasing the concentration of a product (C) will shift the equilibrium to the left to counteract the change, according to Le Chatelier\'s principle.

For the reaction A(g) + B(g) ⇌ C(g), if the concentration of C is increased, wha

Practice Questions

Q1
For the reaction A(g) + B(g) ⇌ C(g), if the concentration of C is increased, what will be the effect on the equilibrium? (2020)
  1. Shift to the left
  2. Shift to the right
  3. No effect
  4. Increase the rate of reaction

Questions & Step-by-Step Solutions

For the reaction A(g) + B(g) ⇌ C(g), if the concentration of C is increased, what will be the effect on the equilibrium? (2020)
  • Step 1: Understand that the reaction A(g) + B(g) ⇌ C(g) is in equilibrium, meaning the forward and reverse reactions are happening at the same rate.
  • Step 2: Recognize that C is a product of the reaction.
  • Step 3: When the concentration of C is increased, it means there is more of the product in the system.
  • Step 4: According to Le Chatelier's principle, if a change is made to a system at equilibrium, the system will adjust to counteract that change.
  • Step 5: Since the concentration of C has increased, the system will try to reduce the concentration of C by shifting the equilibrium to the left.
  • Step 6: Shifting the equilibrium to the left means that more of C will be converted back into A and B.
  • 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.
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