For a reaction at equilibrium, what happens if the concentration of a reactant is increased?
Practice Questions
1 question
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
According to Le Chatelier's principle, increasing the concentration of a reactant will shift the equilibrium position to the right, favoring the formation of products.
Questions & Step-by-step Solutions
1 item
Q
Q: For a reaction at equilibrium, what happens if the concentration of a reactant is increased?
Solution: According to Le Chatelier's principle, increasing the concentration of a reactant will shift the equilibrium position to the right, favoring the formation of products.
Steps: 6
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.
