In a reaction at equilibrium, if the concentration of a reactant is increased, w

₹0.0

Question: In a reaction at equilibrium, if the concentration of a reactant is increased, what will happen to the equilibrium position? (2019)

Options:

Correct Answer: Shift to the right

Exam Year: 2019

Solution:

Increasing the concentration of a reactant will shift the equilibrium position to the right, favoring the formation of products.

In a reaction at equilibrium, if the concentration of a reactant is increased, what will happen to the equilibrium position? (2019)

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.

Le Chatelier's Principle – This principle states that if a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the system will adjust to counteract that change and restore a new equilibrium.