Understanding Chemical Equilibrium and Le Chatelier's Principle

What is chemical equilibrium?

• A state where reactants and products concentrations remain constant over time.

• A state where only reactants are present.

• A state where only products are present.

• A state where the reaction stops completely.

According to Le Chatelier's principle, what happens if the concentration of a reactant is increased?

• The system shifts to consume the added reactant, favoring the forward reaction.

• The system shifts to produce more reactants.

• The system remains unchanged.

• The system shifts to favor the reverse reaction.

How does increasing temperature affect an exothermic reaction at equilibrium?

• It shifts the equilibrium to the left, favoring the reactants.

• It shifts the equilibrium to the right, favoring the products.

• It has no effect on the equilibrium.

• It causes the reaction to stop.

What happens to the equilibrium position when the volume of a gas mixture is decreased?

• The equilibrium shifts towards the side with fewer gas molecules.

• The equilibrium shifts towards the side with more gas molecules.

• The equilibrium remains unchanged.

• The equilibrium shifts randomly.

Why does adding an inert gas not affect the equilibrium position?

• Because it does not participate in the reaction.

• Because it increases the pressure.

• Because it decreases the volume.

• Because it changes the temperature.