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

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

Options:

Correct Answer: Shift to the right

Solution:

According to Le Chatelier\'s principle, increasing the concentration of a reactant will shift the equilibrium to the right.

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

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

Step 1: Identify the reaction: A(g) ⇌ B(g) + C(g).
Step 2: Understand that A is a reactant in this reaction.
Step 3: Recognize that increasing the concentration of A means there is more of it available.
Step 4: Apply Le Chatelier's principle, which states that if a change is made to a system at equilibrium, the system will adjust to counteract that change.
Step 5: Since we increased the concentration of A, the system will try to reduce the amount of A by producing more products (B and C).
Step 6: Therefore, the equilibrium position will shift to the right, favoring the formation of B and C.

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.