6.2 Reversible reactions and dynamic equilibrium

• In a reversible reaction, the products can react to form the original reactants
• For a reaction to be reversible, the products must be able to form the original reactants
• At equilibrium, the forward and reverse reactions occur at equal rates.


  True
• Match the reaction type with its direction:

  Forward reaction ↔️ Reactants → Products

  Reverse reaction ↔️ Products → Reactants
• Steps describing Le Chatelier's Principle:

  1️⃣ Reaction in dynamic equilibrium

  2️⃣ Stress applied (concentration, temperature, pressure)

  3️⃣ Equilibrium shifts to relieve stress

  4️⃣ New equilibrium is established
• What happens to the equilibrium when the concentration of reactants is increased?

  Shifts towards products
• What is Le Chatelier's Principle?

  Equilibrium shifts to relieve stress
• An increase in pressure in a reversible reaction shifts the equilibrium towards fewer gas molecules
• At equilibrium in a reversible reaction, the concentrations of reactants and products remain constant.


  True
• In dynamic equilibrium, the net change in reactant and product concentrations is zero.


  True
• Decreasing the temperature in a system favors the exothermic reaction.
• At equilibrium in a reversible reaction, the forward and reverse reactions occur at the same rate.


  True
• A reversible reaction can occur in both the forward and reverse directions.


  True
• What is one condition for a reaction to be reversible?

  Products form reactants
• What is the relationship between the rates of the forward and reverse reactions at equilibrium?

  They are equal
• At dynamic equilibrium, there is no net change in the concentrations of reactants and products.


  True
• What is the effect of increasing pressure on a reaction with fewer gas molecules on the product side?

  Shifts towards products
• Which type of reaction is favored by an increase in temperature in a system at equilibrium?

  Endothermic reaction
• What is the state of equilibrium in a reversible reaction?

  Forward rate equals reverse rate
• Dynamic equilibrium occurs when the forward and reverse reactions proceed at the same rate
• Increasing the concentration of reactants in a system at equilibrium shifts the reaction towards the products.


  True
• High pressure favors ammonia production in the Haber process due to fewer gas molecules on the product side.


  True
• What is a reversible reaction?

  Products form original reactants
• What happens to the concentrations of reactants and products at equilibrium in a reversible reaction?

  They remain constant
• Steps describing the conditions for a reversible reaction:

  1️⃣ Products can form original reactants

  2️⃣ Reaction occurs in both directions

  3️⃣ Forward and reverse rates are equal at equilibrium
• A reversible reaction occurs in both the forward and reverse
• What is dynamic equilibrium in a reversible reaction?

  Forward and reverse rates are equal
• Le Chatelier's Principle states that a system in dynamic equilibrium will shift to relieve stress
• Increasing the temperature in a reversible reaction will favor the endothermic reaction.


  True
• Increasing the concentration of reactants in a reversible reaction shifts the equilibrium towards the products.


  True
• A reversible reaction can occur in both the forward and reverse directions.


  True
• What is one condition for a reaction to be reversible?

  Products form original reactants
• What happens to the equilibrium of a system when subjected to a change in concentration, temperature, or pressure?

  It shifts to relieve stress
• What is one application of Le Chatelier's Principle in industry?

  Haber process for ammonia