In a reaction at equilibrium, if the concentration of a reactant is increased, w
Practice Questions
Q1
In a reaction at equilibrium, if the concentration of a reactant is increased, what will happen to the equilibrium position? (2019)
Shift to the right
Shift to the left
No change
Depends on temperature
Questions & Step-by-Step Solutions
In a reaction at equilibrium, if the concentration of a reactant is increased, what will happen to the equilibrium position? (2019)
Step 1: Understand what equilibrium means. In a chemical reaction, equilibrium is when the rate of the forward reaction equals the rate of the reverse reaction.
Step 2: Identify the reactants and products in the reaction. Reactants are the starting materials, and products are what is formed.
Step 3: Recognize that increasing the concentration of a reactant means there are more of that reactant available for the reaction.
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 a reactant, the system will try to reduce that concentration by producing more products.
Step 6: Conclude that the equilibrium position will shift to the right, favoring the formation of products.
