For a reaction at equilibrium, what happens if the concentration of a reactant i
Practice Questions
Q1
For a reaction at equilibrium, what happens if 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
For a reaction at equilibrium, what happens if the concentration of a reactant is increased?
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, there are reactants (starting materials) and products (end materials).
Step 3: Know 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 4: If 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, meaning more products will be formed.
Step 6: As a result, the formation of products is favored when the concentration of a reactant is increased.
Le Chatelier's Principle – This principle states that if a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the system will adjust to counteract that change and restore a new equilibrium.
