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

For the reaction A(g) + B(g) ⇌ C(g), if the concentration of C is increased, what will be the effect on the equilibrium? (2020)

For the reaction A(g) + B(g) ⇌ C(g), if the concentration of C is increased, what will be the effect on the equilibrium? (2020)

Step 1: Understand that the reaction A(g) + B(g) ⇌ C(g) is in equilibrium, meaning the forward and reverse reactions are happening at the same rate.
Step 2: Recognize that C is a product of the reaction.
Step 3: When the concentration of C is increased, it means there is more of the product in the system.
Step 4: According to Le Chatelier's principle, if a change is made to a system at equilibrium, the system will adjust to counteract that change.
Step 5: Since the concentration of C has increased, the system will try to reduce the concentration of C by shifting the equilibrium to the left.
Step 6: Shifting the equilibrium to the left means that more of C will be converted back into A and 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.