What happens to the equilibrium position when the concentration of a reactant is
Practice Questions
Q1
What happens to the equilibrium position when the concentration of a reactant is increased in a system at equilibrium?
The equilibrium shifts to the right
The equilibrium shifts to the left
No change occurs
The reaction rate increases
Questions & Step-by-Step Solutions
What happens to the equilibrium position when the concentration of a reactant is increased in a system at equilibrium?
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 in a reaction at equilibrium, there are reactants (starting materials) and products (end materials).
Step 3: 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 4: When the concentration of a reactant is increased, it means there are more starting materials available for the reaction.
Step 5: According to Le Chatelier's Principle, the system will respond by shifting the equilibrium position to the right, which means it will produce more products.
Step 6: As a result, the amount of products will increase until a new equilibrium is established.
