C5.3.2 Le Chatelier's Principle

• Le Chatelier's Principle states that a system at equilibrium will shift to counteract any changes in concentration, pressure, or temperature.

  True
• Order the changes to pressure and their effects on equilibrium systems according to Le Chatelier's Principle.

  1️⃣ Increase in pressure

  2️⃣ Shifts to the side with fewer gas molecules

  3️⃣ Decrease in pressure

  4️⃣ Shifts to the side with more gas molecules
• Understanding Le Chatelier's Principle allows us to predict how a chemical system at equilibrium will respond to changes in its conditions.


  True
• If the concentration of a product in an equilibrium system is increased, the system will shift to consume more products
• If the concentration of a product is increased in an equilibrium system, the system shifts to consume more products.
• Match the concentration change with the system's response:

  Increase in reactant concentration ↔️ Shifts to produce more products

  Increase in product concentration ↔️ Shifts to consume more products
• If the temperature of a chemical system at equilibrium is decreased, the system will shift to the exothermic direction.
• Order the steps to predict how pressure changes affect equilibrium using Le Chatelier's Principle:

  1️⃣ Increase in pressure

  2️⃣ System shifts to the side with fewer gas molecules

  3️⃣ New equilibrium is established
• Le Chatelier's Principle applies only to changes in concentration and temperature.

  False
• Match the factor change with the system's response:

  Increase in pressure ↔️ Shifts to fewer gas molecules

  Decrease in temperature ↔️ Shifts to exothermic direction
• The equilibrium system always adjusts to offset changes and maintain balance.

  True
• If the concentration of a reactant in an equilibrium system is increased, the system will shift to produce more products
• Decreasing the temperature in the endothermic reaction N2O4(g) ⇌ 2NO2(g) would favor the formation of N2O4.


  True
• Match the pressure change with the system's response in a chemical equilibrium:

  Increase in pressure ↔️ Shifts to fewer gas molecules

  Decrease in pressure ↔️ Shifts to more gas molecules
• What does a catalyst do to the activation energy of a reaction?

  Lowers it
• What catalyst is used in the Haber process to produce ammonia?

  Iron
• Chemical equilibrium is the dynamic state where the rate of the forward reaction equals the rate of the reverse reaction, resulting in no net change in the concentrations of reactants and products
• If the concentration of a reactant in an equilibrium system is increased, the system will shift to produce more products
• If the temperature of an equilibrium system is increased, the system will shift to the endothermic direction.
• Match the factor change with the system's response according to Le Chatelier's Principle.

  Increase in reactant concentration ↔️ Shifts to produce more products

  Increase in pressure ↔️ Shifts to the side with fewer gas molecules

  Decrease in temperature ↔️ Shifts to the exothermic direction
• According to Le Chatelier's Principle, what happens to an equilibrium system if the concentration of a reactant is increased?

  Shifts to produce products
• A chemical system at equilibrium will always try to offset changes to maintain equilibrium.


  True
• According to Le Chatelier's Principle, what happens to an equilibrium system if the temperature is increased and the reaction is endothermic?

  Shifts to absorb heat
• Decreasing the temperature of an endothermic reaction favors the reverse reaction.


  True
• What is chemical equilibrium defined as?

  Dynamic state with equal rates
• An increase in reactant concentration causes the system to shift to produce more products.
• What is the effect of decreasing the pressure on an equilibrium system?

  Shifts to more gas molecules
• What does a system at equilibrium always try to offset according to Le Chatelier's Principle?

  Change in concentration
• What type of reaction is favored by increasing temperature in an equilibrium system?

  Endothermic
• Increasing the pressure of a system at equilibrium will cause it to shift towards the side with fewer gas molecules
• What product is favored in the reaction N2(g) + 3H2(g) ⇌ 2NH3(g) when the pressure is increased?

  NH3
• Adding a catalyst to a chemical system at equilibrium changes the equilibrium position.

  False
• Applying Le Chatelier's Principle in industrial processes can lead to increased product yield
• The Contact process uses vanadium pentoxide as a catalyst to produce sulfuric acid.

  True