6.2 Reversible reactions and dynamic equilibrium

• At equilibrium, the rate of the forward reaction equals the rate of the reverse reaction


  True
• What is the reverse reaction in a reversible reaction?

  Products form reactants
• Order the steps in a reversible reaction at equilibrium:

  1️⃣ Reactants → Products

  2️⃣ Products → Reactants

  3️⃣ Rate of forward reaction = Rate of reverse reaction

  4️⃣ Concentrations of reactants and products remain constant
• What is dynamic equilibrium?

  Forward and reverse reactions occur at the same rate
• At equilibrium, the concentrations of reactants and products remain constant


  True
• What is dynamic equilibrium?

  Forward and reverse reactions occur at the same rate
• Order the steps in a reversible reaction:

  1️⃣ Reactants form products

  2️⃣ Products form reactants

  3️⃣ Equilibrium is reached
• Match the key aspect of dynamic equilibrium with its description:

  Rate of Reaction ↔️ Forward rate = Reverse rate

  Concentrations ↔️ Remain constant

  Nature ↔️ Not static, reactions continue
• Dynamic equilibrium is static, meaning no reactions are occurring.

  False
• An increase in temperature for an exothermic reaction shifts equilibrium towards reactants.


  True
• How does increasing temperature affect the equilibrium of an exothermic reaction?

  Shifts towards reactants
• What happens to the equilibrium in the reaction N2(g) + 3H2(g) ⇌ 2NH3(g) when pressure is decreased?

  Shifts towards reactants
• At equilibrium in a reversible reaction, the rates of the forward and reverse reactions are equal.


  True
• Match the reaction type with its description:

  Forward Reaction ↔️ Reactants → Products

  Reverse Reaction ↔️ Products → Reactants
• In a reversible reaction, reactants always form products.


  True
• Match the reaction direction with its description:

  Forward Reaction ↔️ Reactants → Products

  Reverse Reaction ↔️ Products → Reactants
• What occurs in a reversible reaction at dynamic equilibrium?

  Forward and reverse rates are equal
• What happens to equilibrium when the concentration of reactants is increased?

  Shifts toward products
• What do catalysts lower to speed up a reaction?

  Activation energy
• What is a reversible reaction?

  Products form original reactants
• In a reversible reaction, there are two reactions that can occur


  True
• At equilibrium, the rates of the forward and reverse reactions are equal


  True
• In a closed system at equilibrium, the rate of the forward reaction equals the rate of the reverse reaction


  True
• In dynamic equilibrium, both the forward and reverse reactions are continuously happening
• In a closed system, matter or energy can enter or leave the system.

  False
• In an exothermic reaction, increasing temperature shifts the equilibrium towards the reactants.


  True
• In a closed system at equilibrium, the rate of the forward reaction equals the rate of the reverse
• In dynamic equilibrium, the forward reaction rate equals the reverse reaction rate
• In Le Chatelier's principle, a change in concentration causes a shift to consume excess or produce deficient substances
• Compressing a gaseous system at equilibrium shifts it towards the side with fewer gas molecules
• Increasing pressure in a system with gases at equilibrium shifts the equilibrium towards the side with fewer gas molecules
• What is a reversible reaction?

  Products form original reactants
• What is the reverse reaction in N2(g) + 3H2(g) ⇌ 2NH3(g)?

  2NH3(g) → N2(g) + 3H2(g)
• What is the term for the reaction that occurs in the forward direction in a reversible reaction?

  Forward reaction
• What is a reversible reaction?

  Reaction in both directions
• In a closed system at equilibrium, the concentrations of reactants and products remain constant.


  True
• What does Le Chatelier's principle state?

  System opposes change
• In the exothermic Haber process, lower temperatures favor ammonia production.

  True
• Match the factor with its effect on equilibrium:

  Temperature ↔️ Shifts based on exothermic or endothermic

  Pressure ↔️ Shifts to fewer gas molecules

  Concentration ↔️ Shifts to balance
• At equilibrium, the concentrations of reactants and products remain constant