For the reaction A(g) ⇌ B(g), if the concentration of B is increased, what will

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

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

Step 1: Understand that A and B are in a reversible reaction, meaning they can change back and forth.
Step 2: Recognize that A is a reactant and B is a product in the reaction A(g) ⇌ B(g).
Step 3: Know that equilibrium is the point where the concentrations of A and B remain constant.
Step 4: Learn about 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: When the concentration of B (the product) is increased, the system will try to reduce this increase.
Step 6: To counteract the increase in B, the equilibrium will shift to the left, which means it will favor the formation of A.
Step 7: As a result, the concentration of A will increase while the concentration of B will decrease until a new equilibrium is reached.

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.