6.2 Reversible Reactions + Dynamic Equilibrium

• What are reversible reactions?

  Reversible reactions are chemical reactions where products can react to form the original reactants.
• How can the direction of a reversible reaction be changed?

  The direction can be changed by altering the conditions, such as temperature.
• What symbol is used to represent a reversible reaction?

  The symbol used is ⇌.
• What is an example of a reversible reaction?

  An example is the Haber Process: hydrogen + nitrogen ⇌ ammonia.
• What happens to the energy in a reversible reaction that is endothermic one way?

  If a reversible reaction is endothermic one way, it is exothermic in the opposite direction.
• How much energy is transferred in a reversible reaction?


  The same amount of energy is transferred each way, with one direction losing energy and the other gaining it.
• What is equilibrium in the context of reversible reactions?

  Equilibrium is reached when reactions occur at exactly the same rate in each direction in a closed system.
• What do the relative amounts of substances at equilibrium depend on?

  The relative amounts depend on the conditions of the reaction.
• What does Le Chatelier's principle state about changes in equilibrium?

  It states that if a change is made to any of the conditions, the system responds to counteract the change.
• What happens if the concentration of one of the reactants or products is changed?

  The system is no longer at equilibrium, and concentrations will change until equilibrium is reached again.
• What occurs when the concentration of reactants is increased?

  The position of equilibrium shifts towards products, producing more product until equilibrium is reached again.
• What occurs when the concentration of products is increased?

  The position of equilibrium shifts towards reactants, producing more reactant until equilibrium is reached again.
• What happens to equilibrium when temperature is increased?

  Equilibrium moves in the direction of the endothermic reaction.
• What happens to equilibrium when temperature is decreased?

  Equilibrium moves in the direction of the exothermic reaction.
• How does temperature affect the yield of a reaction based on its exothermic or endothermic nature?

  • An increase in temperature decreases yield for exothermic reactions.
  • An increase in temperature increases yield for endothermic reactions.
  • A decrease in temperature increases yield for exothermic reactions.
  • A decrease in temperature decreases yield for endothermic reactions.
• What effect does an increase in pressure have on gaseous reactions?

  An increase in pressure favors the reaction that produces the least number of molecules.
• What happens to equilibrium when pressure is increased?

  Equilibrium shifts to the side of the equation with fewer moles of gas.
• What happens to equilibrium when pressure is decreased?

  Equilibrium shifts to the side of the equation with more moles of gas.
• How does pressure affect the yield of a reaction based on the volume of gas produced?

  • An increase in pressure decreases yield if the reaction produces a larger volume of gas.
  • An increase in pressure increases yield if the reaction produces a smaller volume of gas.
  • A decrease in pressure increases yield if the reaction produces a larger volume of gas.
  • A decrease in pressure decreases yield if the reaction produces a smaller volume of gas.