In a reaction at equilibrium, if the concentration of reactants is increased, wh
Practice Questions
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
Questions & Step-by-Step Solutions
In a reaction at equilibrium, if the concentration of reactants is increased, what will happen to the equilibrium?
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.
