In the equilibrium reaction 2A(g) ⇌ B(g) + C(g), if the concentration of B is in

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

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

Step 1: Understand that the reaction is at equilibrium, meaning the concentrations of A, B, and C are balanced.
Step 2: Recognize that the reaction can shift left or right based on changes in concentration.
Step 3: Note that increasing the concentration of B adds more of that product to the system.
Step 4: According to Le Chatelier's principle, the system will try to counteract this change by shifting the equilibrium to the left.
Step 5: Shifting to the left means that the reaction will produce more A and consume B and C.
Step 6: As a result, the concentration of A will increase while the concentration of B will decrease.

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