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In the reaction: 2A(g) ⇌ B(g) + C(g), if the volume of the container is decrease

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Question: In the reaction: 2A(g) ⇌ B(g) + C(g), if the volume of the container is decreased, what will happen?

Options:

  1. Shift to the left
  2. Shift to the right
  3. No change
  4. Depends on the temperature

Correct Answer: Shift to the left

Solution: 

Decreasing the volume increases the pressure, and the equilibrium will shift towards the side with fewer moles of gas, which is the left side in this case.

In the reaction: 2A(g) ⇌ B(g) + C(g), if the volume of the container is decrease

Practice Questions

Q1
In the reaction: 2A(g) ⇌ B(g) + C(g), if the volume of the container is decreased, what will happen?
  1. Shift to the left
  2. Shift to the right
  3. No change
  4. Depends on the temperature

Questions & Step-by-Step Solutions

In the reaction: 2A(g) ⇌ B(g) + C(g), if the volume of the container is decreased, what will happen?
  • Step 1: Understand the reaction: 2A(g) ⇌ B(g) + C(g). This means that 2 moles of gas A can turn into 1 mole of gas B and 1 mole of gas C.
  • Step 2: Identify the number of gas moles on each side of the reaction. The left side (reactants) has 2 moles of A, and the right side (products) has 1 mole of B + 1 mole of C, which totals 2 moles.
  • Step 3: Recognize that decreasing the volume of the container increases the pressure inside the container.
  • Step 4: Apply Le Chatelier's principle, which states that if a system at equilibrium is disturbed, it will shift to counteract the disturbance.
  • Step 5: Since both sides of the reaction have the same total number of moles (2 moles), the equilibrium will not shift to either side based on the number of moles alone.
  • Le Chatelier's Principle – When a system at equilibrium is subjected to a change in pressure, temperature, or concentration, the equilibrium will shift to counteract that change.
  • Gas Laws – Understanding how changes in volume affect pressure and the behavior of gases in a closed system.
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