Le Chatelier's Principle and Equilibrium

What is a characteristic of reversible reactions?

• They only occur in one direction.

• They happen at different rates.

• They can reach equilibrium.

• They produce only reactants.

What happens to the reaction rates when a reversible reaction reaches equilibrium?

• The forward reaction stops.

• The reverse reaction stops.

• Both reactions continue at the same rate.

• Both reactions stop completely.

Which gas is a reactant in the formation of ammonia (NH₃) in a reversible reaction?

• Oxygen (O₂)

• Hydrogen (H₂)

• Carbon dioxide (CO₂)

• Nitric oxide (NO)

When does the reverse reaction begin according to the diagram?

• At the start of the reaction.

• When products are formed.

• When dynamic equilibrium is established.

• When the rate of forward reaction is high.

What is the chemical formula for the reactants in the dynamic equilibrium of ammonia synthesis?

• N₂ + 3H₂

• 2NH₃

• H₂O + CO₂

• CH₄ + O₂

What is the significance of the double arrow in the chemical equation for dynamic equilibrium?

• It indicates a one-way reaction

• It indicates a reversible reaction

• It indicates no reaction

• It indicates a completed reaction

What is Le Chatelier's Principle primarily concerned with?

• The speed of chemical reactions

• The equilibrium of chemical reactions

• The energy of chemical reactions

• The color change in chemical reactions

How does a system respond to a change in concentration according to Le Chatelier's Principle?

• By increasing temperature

• By shifting the reaction

• By changing color

• By decreasing pressure

What is the result of adding a catalyst to a reaction at equilibrium?

• It changes the equilibrium constant

• It speeds up the reaction without changing equilibrium

• It decreases the reaction rate

• It increases the reaction temperature

What is the effect of increasing pressure on reactants in a reaction?

• Reactants will collide less frequently and make fewer products

• Reactants will stop colliding and no products will be made

• Reactants will collide more frequently and will make more products

• Reactants will remain unchanged