2.6.2 Factors Affecting Equilibrium

• What is Le Chatelier's Principle?

  Equilibrium shifts to counteract change
• In dynamic equilibrium, the forward and reverse reactions occur at the same rate
• What is dynamic equilibrium in a chemical system?

  Forward and reverse reactions occur at the same rate
• Static equilibrium occurs when there is no reaction taking place.


  True
• Each factor in Le Chatelier's Principle influences equilibrium to minimize the effect of change.


  True
• Le Chatelier's Principle states that a system in equilibrium will shift to counteract any applied change.

  True
• What are the three main factors affecting equilibrium according to Le Chatelier's Principle?

  Concentration, pressure, temperature
• Increasing the concentration of reactants in an equilibrium system shifts the equilibrium forward
• What principle governs the effect of temperature on equilibrium?

  Le Chatelier's Principle
• The role of pressure in reversible reactions is to shift the equilibrium towards fewer gas molecules
• Match the factor with its effect on equilibrium shift:

  Concentration ↔️ Shifts away from added reactants/products

  Pressure ↔️ Shifts towards fewer gas molecules

  Temperature ↔️ Shifts towards heat absorption
• How does changing the concentration of reactants or products affect equilibrium position?

  It shifts the equilibrium
• Dynamic equilibrium results in no net change in reactant and product concentrations.


  True
• In dynamic equilibrium, there is no net change in concentrations
• What is Le Chatelier's Principle?

  A system shifts to counteract change
• Match the factor with its effect on equilibrium shift:

  Concentration ↔️ Shifts away from added substances

  Pressure ↔️ Shifts towards fewer gas molecules

  Temperature ↔️ Shifts towards heat absorption
• Changing the concentration of reactants or products shifts equilibrium according to Le Chatelier's Principle.

  True
• Increasing the temperature in an exothermic reaction shifts the equilibrium towards the reactants
• What happens to equilibrium if you increase the pressure in a reaction with fewer gas molecules on the product side?

  Shifts towards products
• What is the primary role of a catalyst in a chemical reaction?

  Lowers activation energy
• What is dynamic equilibrium in a chemical system?

  Forward and reverse rates are equal
• What is static equilibrium?

  No change or movement
• Each factor influences equilibrium to minimize the effect of the change.

  True
• Arrange the effects of concentration changes on equilibrium shifts:

  1️⃣ Increase reactants: Shifts forward

  2️⃣ Decrease reactants: Shifts backward

  3️⃣ Increase products: Shifts backward

  4️⃣ Decrease products: Shifts forward
• In static equilibrium, there is no reaction taking place.
• What is dynamic equilibrium in a chemical system?

  Forward and reverse reactions occur at the same rate
• Static equilibrium occurs when there is no reaction taking place.

  True
• Increasing the temperature in an endothermic reaction shifts the equilibrium towards the products
• What happens to equilibrium if you add more reactants?

  Shifts towards products
• Order the effects of concentration changes on equilibrium from reactant increase to product decrease:

  1️⃣ Increase reactants: Equilibrium shifts forward

  2️⃣ Decrease reactants: Equilibrium shifts backward

  3️⃣ Increase products: Equilibrium shifts backward

  4️⃣ Decrease products: Equilibrium shifts forward
• What happens to the equilibrium in an endothermic reaction if you increase the temperature?

  Shifts towards products
• Decreasing the pressure in a reversible reaction shifts the equilibrium towards the side with more gas molecules
• One key benefit of using catalysts is a lower reaction temperature
• Increasing pressure in a reversible reaction shifts the equilibrium towards fewer gas molecules
• What happens to the equilibrium in the reaction N₂ (g) + 3H₂ (g) ⇌ 2NH₃ (g) if you decrease the concentration of H₂?

  Shifts towards reactants
• The direction of equilibrium shift depends on whether the forward reaction is exothermic or endothermic.


  True
• In the reaction N₂ (g) + 3H₂ (g) ⇌ 2NH₃ (g), increasing the pressure shifts the equilibrium towards the right.

  True
• The Haber-Bosch process uses iron oxide as a catalyst to produce ammonia.

  True