In a reversible reaction at equilibrium, what happens if the concentration of a
Practice Questions
Q1
In a reversible reaction at equilibrium, what happens if the concentration of a reactant is increased? (2023)
The equilibrium shifts to the right
The equilibrium shifts to the left
The equilibrium remains unchanged
The reaction stops
Questions & Step-by-Step Solutions
In a reversible reaction at equilibrium, what happens if the concentration of a reactant is increased? (2023)
Step 1: Understand that a reversible reaction can go in both directions: from reactants to products and from products back to reactants.
Step 2: Know that equilibrium is the point where the rate of the forward reaction equals the rate of the reverse reaction.
Step 3: Recognize 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, the system will try to reduce that concentration.
Step 5: To reduce the concentration of the added reactant, the equilibrium will shift to the right, favoring the formation of more products.
