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 concentrations?

Options:

Correct Answer: Concentrations of B and C will increase

Solution:

Doubling the volume decreases the pressure, which shifts the equilibrium towards the side with more moles of gas (B and C).

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

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

Step 1: Identify the equilibrium reaction: 2A(g) ⇌ B(g) + C(g).
Step 2: Count the number of moles of gas on each side of the equilibrium.
Step 3: On the left side (reactants), there are 2 moles of A.
Step 4: On the right side (products), there are 1 mole of B and 1 mole of C, totaling 2 moles.
Step 5: Note that both sides have the same number of moles (2 moles).
Step 6: Understand that when the volume of the container is doubled, the pressure decreases.
Step 7: According to Le Chatelier's principle, the equilibrium will shift to counteract the change in pressure.
Step 8: Since both sides have the same number of moles, the equilibrium position will not shift towards either side.
Step 9: Therefore, the concentrations of A, B, and C will all decrease due to the increased volume.

Le Chatelier's Principle – This principle states that if a system at equilibrium is subjected to a change in conditions (such as pressure or volume), the equilibrium will shift in a direction that counteracts the change.
Gas Laws – Understanding how changes in volume affect pressure and concentration in gaseous systems.