2.6.1 Reversible Reactions and Equilibrium

• What is a reversible reaction?

  Reaction in both directions
• Reversible reactions do not go to completion
• The equilibrium state is reached when the rates of the forward and reverse reactions are equal
• Match the feature with the type of reaction:

  Equal forward and reverse rates ↔️ Equilibrium State

  Reactants are entirely consumed ↔️ Reaction Going to Completion
• Increasing the concentration of reactants shifts the equilibrium to favor the products
• Dynamic equilibrium is a static process.

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

  They remain constant
• What is an example of a reversible reaction?

  $N_{2}(g) +$$3H_{2}(g) \rightleftharpoons 2NH_{3}(g)$
• What type of reaction does an increase in temperature favor in equilibrium?

  Endothermic reaction
• In the Haber Process, what conditions favor ammonia formation?

  High pressure, moderate temperature
• In the Haber Process, high pressure and moderate temperature favor the formation of ammonia
• Reversible reactions reach a state of dynamic equilibrium.


  True
• Reversible reactions reach dynamic equilibrium, unlike irreversible reactions.


  True
• What happens to the concentrations of reactants and products at equilibrium?

  Remain constant
• What does Le Chatelier's Principle state?

  System counteracts disturbances
• What effect does increasing pressure have on equilibrium in a system with unequal gas molecules on each side?

  Favors side with fewer molecules
• What is the characteristic of a reaction that goes to completion?

  Reactants are entirely consumed
• Match the features with the correct reaction type:

  Equal forward and reverse rates ↔️ Equilibrium State

  Reactants are entirely consumed ↔️ Reaction Going to Completion
• An irreversible reaction goes to completion
• Le Chatelier's Principle states that a system at equilibrium will shift to counteract any change in conditions.


  True
• Equilibrium shifts aim to re-establish the original conditions of the system.


  True
• Match the factors affecting equilibrium with their effects:

  Concentration ↔️ Shifts equilibrium to favor products

  Pressure ↔️ Favors the side with fewer gas molecules

  Temperature ↔️ Favors the endothermic reaction
• What is the effect of excess alcohol in esterification on the equilibrium position?

  Favors product formation
• What is the key difference between reversible and irreversible reactions in terms of direction?

  Both forward and reverse vs. Only forward
• Give an example of a reversible reaction.

  $N_{2}(g) +$$3H_{2}(g) \rightleftharpoons 2NH_{3}(g)$
• At equilibrium, the forward and reverse reactions stop completely.

  False
• Le Chatelier's Principle applies only to systems at equilibrium.


  True
• Sequence the effects of changes on equilibrium according to Le Chatelier's Principle:

  1️⃣ Increase in concentration of reactants

  2️⃣ Equilibrium shifts to favor products
• In reversible reactions, the equilibrium state is reached when the rates of the forward and reverse reactions are equal
• Arrange the following reaction types based on their completion status:

  1️⃣ Irreversible reaction

  2️⃣ Reversible reaction
• Match the features with the correct reaction type:

  Equal forward and reverse rates ↔️ Equilibrium State

  Reactants are entirely consumed ↔️ Reaction Going to Completion
• An increase in the concentration of reactants shifts the equilibrium to favor the products
• The position of dynamic equilibrium can be influenced by changes in concentration, pressure, and temperature
• Adding nitrogen in the Haber Process increases ammonia production.


  True