In a reaction at equilibrium, if the concentration of products increases, what w

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Question: In a reaction at equilibrium, if the concentration of products increases, what will happen to the equilibrium position?

Options:

Correct Answer: Shift to the left

Solution:

According to Le Chatelier\'s principle, if the concentration of products increases, the equilibrium will shift to the left.

In a reaction at equilibrium, if the concentration of products increases, what will happen to the equilibrium position?

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.

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.