For a reaction at equilibrium, if the concentration of products is increased, wh
Practice Questions
Q1
For a reaction at equilibrium, if the concentration of products is increased, what will happen to the position of equilibrium according to Le Chatelier's principle?
Shift to the right
Shift to the left
No change
Depends on temperature
Questions & Step-by-Step Solutions
For a reaction at equilibrium, if the concentration of products is increased, what will happen to the position of equilibrium according to Le Chatelier's principle?
Step 1: Understand that a chemical reaction can reach a state called equilibrium, where the rate of the forward reaction equals the rate of the reverse reaction.
Step 2: Recognize that Le Chatelier's principle states that if a change is made to a system at equilibrium, the system will adjust to counteract that change.
Step 3: Identify that increasing the concentration of products means there are more products present in the reaction mixture.
Step 4: Apply Le Chatelier's principle: to counteract the increase in products, the equilibrium will shift in the direction that reduces the concentration of products.
Step 5: Conclude that this shift will move the equilibrium position to the left, favoring the formation of reactants.
Le Chatelier's Principle – This principle states that if a system at equilibrium is subjected to a change in concentration, pressure, or temperature, the system will adjust to counteract that change and restore a new equilibrium.
