Reversible Reactions

• What are reversible reactions?

  Reactions that can go backward.
• What do reversible reactions reach?

  They reach equilibrium.
• What do the products of a reversible reaction do?

  They can react to form reactants again.
• In the equation A + B ⇌ C + D, what are C and D?

  Products of the reaction.
• What happens to the forward reaction rate at equilibrium?

  It slows down.
• What happens to the backward reaction rate at equilibrium?

  It remains the same as the forward rate.
• What occurs to the concentrations of reactants and products at equilibrium?

  They reach a balance and do not change.
• What does a dynamic equilibrium mean?

  Both forward and backward reactions occur simultaneously.
• What is the effect of increasing reactant concentration on the forward reaction?

  It speeds up the forward reaction.
• What happens to the backward reaction when product concentration increases?

  It speeds up the backward reaction.
• What is the relationship between temperature and equilibrium position?

  Temperature changes can shift equilibrium position.
• What factors affect the position of equilibrium?

  Temperature, pressure, and concentration.
• What is required for equilibrium to be reached?

  A closed system.
• What does a closed system mean in the context of equilibrium?

  No substances can enter or leave the system.
• How does the concentration of reactants affect the equilibrium position?

  Higher concentrations shift equilibrium to products.
• What happens to the equilibrium position if the temperature is increased in an exothermic reaction?

  It shifts to the left, favoring reactants.
• What happens to the equilibrium position if the temperature is decreased in an endothermic reaction?

  It shifts to the left, favoring reactants.
• What is the effect of pressure on gaseous equilibria?

  Increased pressure shifts equilibrium to fewer moles.
• What does the term "dynamic equilibrium" imply about the reactions?

  Reactions continue to occur at equal rates.
• What is the significance of the position of equilibrium in a chemical reaction?

  It determines the concentrations of reactants and products.
• What does it mean if the equilibrium position lies to the right?

  Products are favored over reactants.
• What is the relationship between the concentrations of reactants and products at equilibrium?

  They remain constant over time.
• What does it mean for a reaction to be at equilibrium?

  The rates of forward and backward reactions are equal.
• How does the concentration of products affect the equilibrium position?

  Higher concentrations shift equilibrium to reactants.
• What is the effect of adding an inert gas to a reaction at equilibrium?

  It does not affect the equilibrium position.
• What is the role of catalysts in reversible reactions?

  They speed up both forward and backward reactions equally.
• What does the equilibrium constant indicate?

  The ratio of concentrations of products to reactants.
• What happens to the equilibrium constant if the temperature changes?

  It changes depending on the reaction type.
• What is the general form of the equilibrium constant expression?

  K = [products] / [reactants].
• What does a large equilibrium constant indicate?

  Products are favored at equilibrium.
• How does the position of equilibrium relate to the extent of a reaction?

  A position far to the right indicates a complete reaction.
• What is the effect of dilution on equilibrium?

  It can shift the equilibrium position.
• What does it mean if the equilibrium constant is less than one?

  Reactants are favored over products.
• What is the significance of Le Chatelier's principle?

  It predicts how equilibrium shifts with changes.
• How does the addition of a reactant affect equilibrium?

  It shifts equilibrium toward products.
• What is the effect of removing a product from a reaction at equilibrium?

  It shifts equilibrium toward products.
• What does it mean for a reaction to be at dynamic equilibrium?

  Reactions continue to occur without net change.
• What is the relationship between reaction rates and equilibrium?

  Equilibrium occurs when reaction rates are equal.
• What is the effect of temperature on an exothermic reaction at equilibrium?

  Increasing temperature shifts equilibrium left.
• What happens to the equilibrium position if the pressure is increased in a reaction with more moles of gas?

  It shifts to the side with fewer moles.