For the reaction 2A(g) ⇌ B(g) + C(g), if the concentration of B is increased, wh

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Question: For the reaction 2A(g) ⇌ B(g) + C(g), if the concentration of B is increased, what will happen to the equilibrium?

Options:

Correct Answer: Shift to the left

Solution:

Increasing the concentration of a product shifts the equilibrium to the left to counteract the change.

For the reaction 2A(g) ⇌ B(g) + C(g), if the concentration of B is increased, what will happen to the equilibrium?

For the reaction 2A(g) ⇌ B(g) + C(g), if the concentration of B is increased, what will happen to the equilibrium?

Step 1: Identify the reaction: 2A(g) ⇌ B(g) + C(g).
Step 2: Recognize that B and C are products of the reaction.
Step 3: Understand that increasing the concentration of a product (B) disturbs the balance of the reaction.
Step 4: Apply Le Chatelier's Principle, which states that the system will adjust to counteract the change.
Step 5: Since B's concentration is increased, the equilibrium will shift to the left to reduce the amount of B.
Step 6: This means that more B will react to form A, thus decreasing the concentration of B.

Le Chatelier's Principle – This principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change.