For the equilibrium 2A(g) ⇌ B(g) + C(g), if the volume of the container is doubl

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Question: For the equilibrium 2A(g) ⇌ B(g) + C(g), if the volume of the container is doubled, what will happen to the equilibrium position?

Options:

Correct Answer: Shift to the right

Solution:

Doubling the volume decreases the pressure, which shifts the equilibrium towards the side with more moles of gas, in this case, the right side.

For the equilibrium 2A(g) ⇌ B(g) + C(g), if the volume of the container is doubled, what will happen to the equilibrium position?

For the equilibrium 2A(g) ⇌ B(g) + C(g), if the volume of the container is doubled, what will happen to the equilibrium position?

Step 1: Understand the equilibrium reaction: 2A(g) ⇌ B(g) + C(g).
Step 2: Identify the number of gas moles on each side of the equation. The left side has 2 moles (2A) and the right side has 2 moles (1B + 1C).
Step 3: Recognize that doubling the volume of the container decreases the pressure of the gases inside.
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 the pressure decreases, the equilibrium will shift towards the side with more moles of gas to increase the pressure.
Step 6: In this case, both sides have the same number of moles (2 moles), so the equilibrium position will not shift significantly.

Le Chatelier's Principle – This principle states that if an external change is applied to a system at equilibrium, the system will adjust to counteract that change and restore a new equilibrium.
Effect of Volume on Equilibrium – Changing the volume of a gas system affects the pressure; increasing the volume decreases the pressure, which can shift the equilibrium position depending on the number of moles of gas on each side.