In a reversible reaction at equilibrium, if the concentration of reactants is increased, what will happen to the equilibrium position? (2023)
Practice Questions
1 question
Q1
In a reversible reaction at equilibrium, if the concentration of reactants is increased, what will happen to the equilibrium position? (2023)
Shift to the right
Shift to the left
No change
Depends on temperature
According to Le Chatelier's principle, increasing the concentration of reactants will shift the equilibrium position to the right, favoring the formation of products.
Questions & Step-by-step Solutions
1 item
Q
Q: In a reversible reaction at equilibrium, if the concentration of reactants is increased, what will happen to the equilibrium position? (2023)
Solution: According to Le Chatelier's principle, increasing the concentration of reactants will shift the equilibrium position to the right, favoring the formation of products.
Steps: 6
Step 1: Understand that a reversible reaction can go in two directions: from reactants to products and from products 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: 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: Recognize that increasing the concentration of reactants means there are more reactant molecules available.
Step 5: According to Le Chatelier's principle, the system will respond by trying to reduce the concentration of reactants.
Step 6: The system will shift the equilibrium position to the right, which means it will favor the formation of more products.
