What happens to the equilibrium position of a reaction when the concentration of
Practice Questions
Q1
What happens to the equilibrium position of a reaction when the concentration of a reactant is increased?
The equilibrium shifts to the right
The equilibrium shifts to the left
The equilibrium remains unchanged
The reaction stops
Questions & Step-by-Step Solutions
What happens to the equilibrium position of a reaction when the concentration of a reactant is increased?
Step 1: Understand what equilibrium means. It is the point in a chemical reaction where the rate of the forward reaction equals the rate of the reverse reaction.
Step 2: Know that a reactant is a substance that is consumed in a chemical reaction.
Step 3: Learn about Le Chatelier's Principle. It states that if a change is made to a system at equilibrium, the system will adjust to counteract that change.
Step 4: When the concentration of a reactant is increased, it means there are more reactant molecules available for the reaction.
Step 5: According to Le Chatelier's Principle, the system will respond to this increase by shifting the equilibrium position to the right.
Step 6: Shifting to the right means that the reaction will produce more products to balance the increased concentration of the reactant.
