In a reaction at equilibrium, if the concentration of reactants is increased, wh

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Question: In a reaction at equilibrium, if the concentration of reactants is increased, what will happen to the equilibrium?

Options:

Correct Answer: Shift to the right

Solution:

According to Le Chatelier\'s principle, increasing the concentration of reactants will shift the equilibrium to the right to form more products.

In a reaction at equilibrium, if the concentration of reactants is increased, what will happen to the equilibrium?

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.

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.