In a reaction at equilibrium, if the concentration of products increases, what w
Practice Questions
Q1
In a reaction at equilibrium, if the concentration of products increases, what will happen to the equilibrium position?
Shift to the left
Shift to the right
No change
Depends on temperature
Questions & Step-by-Step Solutions
In a reaction at equilibrium, if the concentration of products increases, what will happen to the equilibrium position?
Step 1: Understand what equilibrium means. It is a state where the rate of the forward reaction equals the rate of the reverse reaction.
Step 2: Know that in a chemical reaction, there are reactants (starting materials) and products (end materials).
Step 3: Recognize 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: Identify that increasing the concentration of products means there are more products present in the reaction.
Step 5: According to Le Chatelier's principle, if the concentration of products increases, the system will try to reduce that concentration by shifting the equilibrium position.
Step 6: The equilibrium will shift to the left, which means it will favor the formation of reactants.
