2.3.2 Le Chatelier's Principle

• At chemical equilibrium, the concentrations of reactants and products remain constant.


  True
• Increasing the temperature in a system at equilibrium favors the reaction that absorbs heat.
• An increase in the concentration of reactants in a chemical system at equilibrium will cause a shift to produce more products.
• Match the condition change with the system's response according to Le Chatelier's Principle:

  Add reactants ↔️ Produce more products

  Increase temperature ↔️ Favor endothermic reaction

  Increase pressure ↔️ Shift to side with fewer gas moles
• Increasing temperature in a system at equilibrium favors the exothermic reaction.

  False
• What is the role of a catalyst in chemical equilibrium?

  Accelerates reaction rates
• What happens to equilibrium when the concentration of products is decreased?

  Shifts towards product formation
• Le Chatelier's Principle states that changes in pressure can affect equilibrium, especially in reactions involving gases.
• At chemical equilibrium, the concentrations of reactants and products remain constant.

  True
• Increasing pressure in a system at equilibrium shifts the equilibrium towards the side with fewer moles of gas.
• What happens to the equilibrium of a gas-phase reaction when pressure is increased, according to Le Chatelier's Principle?

  Shifts towards fewer moles
• For an endothermic reaction, increasing temperature favors the product side to absorb heat.


  True
• What happens to the equilibrium of a gas-phase reaction when pressure is decreased, according to Le Chatelier's Principle?

  Shifts towards more moles
• Removing carbon dioxide (CO2) from the reaction of carbon and oxygen shifts the equilibrium to produce more CO
• What happens to the equilibrium of the Haber process when pressure is increased, according to Le Chatelier's Principle?

  Shifts towards products
• Le Chatelier's Principle allows industries to optimize chemical processes for higher yield and efficiency.


  True
• Chemical equilibrium is a state where the forward and reverse reaction rates in a reversible chemical reaction are equal
• When the temperature of a chemical system at equilibrium is increased, the system shifts to the direction of the endothermic reaction.
• What happens to the equilibrium when the concentration of reactants is increased?

  Shifts to produce products
• What happens to the equilibrium when the pressure is increased in a system with fewer moles of gas on the product side?

  Shifts to produce products
• What is the definition of chemical equilibrium?

  Equal forward and reverse rates
• Increasing temperature in a chemical system at equilibrium favors the endothermic reaction.
• Increasing pressure in a system at equilibrium favors the side with more gas molecules.

  False
• Increasing the concentration of reactants in a system at equilibrium shifts the equilibrium towards reactant formation.

  False
• What happens to an endothermic reaction when temperature is increased?

  Shifts towards product side
• What is chemical equilibrium?

  Equal forward and reverse rates
• What happens to equilibrium when temperature is increased in an exothermic reaction?

  Shifts towards reactants
• For endothermic reactions, increasing temperature shifts the equilibrium towards the products
• What happens to the equilibrium of an exothermic reaction when temperature is increased?

  Shifts towards reactants
• According to Le Chatelier's Principle, changes in pressure affect equilibrium in reactions involving gases
• How does adding more ammonia (NH3) to the Haber process affect the equilibrium according to Le Chatelier's Principle?

  Shifts to produce more NH3
• Increasing the temperature in an exothermic reaction reduces heat production and shifts the equilibrium towards the reactants.


  True
• The Haber-Bosch process uses excess reactants to maximize ammonia production
• What is Le Chatelier's Principle?

  Counteract change to equilibrium
• Increasing the pressure in a system at equilibrium favors the side with fewer moles of gas.


  True
• Steps for applying Le Chatelier's Principle

  1️⃣ Identify the change

  2️⃣ Determine the system's response

  3️⃣ Re-establish equilibrium
• Removing a product from a system at equilibrium will shift the equilibrium to produce more of that product.


  True
• What does Le Chatelier's Principle state?

  Counteract change to re-establish equilibrium
• What happens to equilibrium when reactants are added to a system?

  Shifts towards products
• Changing the concentration of reactants or products in a system at equilibrium will shift the equilibrium to counteract the change.