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

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

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

Step 1: Understand the equilibrium reaction: 2A(g) ⇌ B(g) + C(g). This means that A can turn into B and C, and B and C can turn back into A.
Step 2: Identify what happens when the concentration of B is increased. This means there is more B available in the reaction.
Step 3: 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 4: Since the concentration of B is increased, the system will try to reduce the amount of B by shifting the equilibrium to the left.
Step 5: Shifting the equilibrium to the left means that more B will turn back into A, which will decrease the concentration of A.

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.