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For the reaction A(g) ⇌ B(g), if the concentration of B is increased, what will

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Question: For the reaction A(g) ⇌ B(g), if the concentration of B is increased, what will happen to the concentration of A at equilibrium?

Options:

  1. Increase
  2. Decrease
  3. Remain the same
  4. Cannot be determined

Correct Answer: Decrease

Solution: 

According to Le Chatelier\'s principle, increasing the concentration of a product will shift the equilibrium to the left, decreasing the concentration of A.

For the reaction A(g) ⇌ B(g), if the concentration of B is increased, what will

Practice Questions

Q1
For the reaction A(g) ⇌ B(g), if the concentration of B is increased, what will happen to the concentration of A at equilibrium?
  1. Increase
  2. Decrease
  3. Remain the same
  4. Cannot be determined

Questions & Step-by-Step Solutions

For the reaction A(g) ⇌ B(g), if the concentration of B is increased, what will happen to the concentration of A at equilibrium?
  • Step 1: Understand that A and B are in a reversible reaction, meaning they can change back and forth.
  • Step 2: Recognize that A is a reactant and B is a product in the reaction A(g) ⇌ B(g).
  • Step 3: Know that equilibrium is the point where the concentrations of A and B remain constant.
  • Step 4: 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 5: When the concentration of B (the product) is increased, the system will try to reduce this increase.
  • Step 6: To counteract the increase in B, the equilibrium will shift to the left, which means it will favor the formation of A.
  • Step 7: As a result, the concentration of A will increase while the concentration of B will decrease until a new equilibrium is reached.
  • 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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