In a reversible reaction, if the concentration of products is increased, what will happen to the equilibrium position? (2021)
Practice Questions
1 question
Q1
In a reversible reaction, if the concentration of products is increased, what will happen to the equilibrium position? (2021)
Shift to the left
Shift to the right
No change
Depends on temperature
According to Le Chatelier's principle, increasing the concentration of products will shift the equilibrium position to the left to counteract the change.
Questions & Step-by-step Solutions
1 item
Q
Q: In a reversible reaction, if the concentration of products is increased, what will happen to the equilibrium position? (2021)
Solution: According to Le Chatelier's principle, increasing the concentration of products will shift the equilibrium position to the left to counteract the change.
Steps: 6
Step 1: Understand that a reversible reaction can go in both 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 products means there are more products present in the reaction.
Step 5: According to Le Chatelier's principle, the system will try to reduce the effect of this change by shifting the equilibrium position.
Step 6: Since we increased the products, the equilibrium will shift to the left, which means it will favor the formation of reactants.
