In a reaction at equilibrium, what happens if the concentration of a reactant is

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Question: In a reaction at equilibrium, what happens if the concentration of a reactant is increased?

Options:

Correct Answer: The equilibrium shifts to the right

Solution:

According to Le Chatelier\'s principle, increasing the concentration of a reactant shifts the equilibrium to the right, favoring product formation.

In a reaction at equilibrium, what happens if the concentration of a reactant is increased?

In a reaction at equilibrium, what happens if the concentration of a reactant is increased?

Step 1: Understand that a chemical reaction can reach a state called equilibrium, where the rate of the forward reaction equals the rate of the reverse reaction.
Step 2: Recognize that in this equilibrium state, the concentrations of reactants and products remain constant.
Step 3: Know that if you increase the concentration of a reactant, you are adding more of that substance to the reaction.
Step 4: According to Le Chatelier's principle, the system will respond to this change by trying to reduce the effect of the added reactant.
Step 5: The system shifts the equilibrium position to the right, which means it will produce more products to balance the increased reactant concentration.
Step 6: As a result, the formation of products is favored, leading to an increase in their concentration.

Le Chatelier's Principle – A principle stating that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change.