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

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

For the reaction A(g) ⇌ B(g), if the concentration of A is increased, what will happen to the concentration of B 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 increasing the concentration of A means there are more A molecules available.
Step 3: According to Le Chatelier's principle, if you change the concentration of a reactant (A), the system will adjust to counteract that change.
Step 4: The system will shift the equilibrium to the right to use up some of the added A.
Step 5: As the equilibrium shifts to the right, more A will be converted into B.
Step 6: This conversion will result in an increase in 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.