In a reaction at equilibrium, if the concentration of reactants is increased, what will happen to the equilibrium?
Practice Questions
1 question
Q1
In a reaction at equilibrium, if the concentration of reactants is increased, what will happen to the equilibrium?
Shift to the right
Shift to the left
No change
Equilibrium constant increases
According to Le Chatelier's principle, increasing the concentration of reactants will shift the equilibrium to the right to form more products.
Questions & Step-by-step Solutions
1 item
Q
Q: In a reaction at equilibrium, if the concentration of reactants is increased, what will happen to the equilibrium?
Solution: According to Le Chatelier's principle, increasing the concentration of reactants will shift the equilibrium to the right to form more products.
Steps: 6
Step 1: Understand that a reaction at equilibrium means the rates of the forward and reverse reactions are equal.
Step 2: Recognize that reactants are the starting materials in a chemical reaction.
Step 3: Know that increasing the concentration of reactants means there are more reactant molecules available.
Step 4: Apply 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 5: Since we increased the concentration of reactants, the system will try to reduce this change by using some of the reactants to form more products.
Step 6: Therefore, the equilibrium will shift to the right, resulting in the formation of more products.
