In the reaction A(g) + B(g) ⇌ C(g) + D(g), if the volume is increased, what will

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Question: In the reaction A(g) + B(g) ⇌ C(g) + D(g), if the volume is increased, what will happen to the equilibrium?

Options:

Correct Answer: Shifts to the right

Solution:

Increasing the volume decreases the pressure, and the equilibrium will shift to the side with more moles of gas to counteract the change.

In the reaction A(g) + B(g) ⇌ C(g) + D(g), if the volume is increased, what will happen to the equilibrium?

In the reaction A(g) + B(g) ⇌ C(g) + D(g), if the volume is increased, what will happen to the equilibrium?

Step 1: Understand that the reaction involves gases A, B, C, and D.
Step 2: Recognize that increasing the volume of the container means there is more space for the gases.
Step 3: Know that when the volume increases, the pressure inside the container decreases.
Step 4: Remember Le Chatelier's principle, which states that if a system at equilibrium is disturbed, it will shift to counteract the disturbance.
Step 5: Identify the number of moles of gas on each side of the reaction: A + B (2 moles) and C + D (2 moles).
Step 6: Since both sides have the same number of moles of gas (2 moles), the equilibrium will not shift to either side.

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