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

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

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

Correct Answer: The equilibrium will shift to the right side (B and C).

Step 1: Understand that the reaction is at equilibrium, meaning both the forward and reverse reactions are happening at the same rate.
Step 2: Identify the reaction: 2A(g) ⇌ B(g) + C(g).
Step 3: Count the number of gas molecules on each side of the equation. The left side (reactants) has 2 moles of gas (2A), and the right side (products) has 2 moles of gas (1B + 1C).
Step 4: Recognize that decreasing the volume of the container increases the pressure inside the container.
Step 5: Apply Le Chatelier's principle, which states that if a system at equilibrium is disturbed, it will shift to counteract the disturbance.
Step 6: Since both sides of the reaction have the same number of moles of gas (2 moles), the equilibrium will not shift to either side based on the change in volume.

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.
Gas Laws – Understanding how changes in volume affect pressure and the behavior of gases in equilibrium reactions.