Chemistry Chapter on Reversible and Irreversible Processes

Reversible and Irreversible Processes

• Reversible Processes: Reactions where products can convert back into reactants under the same conditions, e.g., formation of NH₃, HI, SO₂.

• These processes do not proceed to completion, allowing for the possibility of reverse reactions.

• Irreversible Processes: Reactions where products do not revert to reactants, e.g., 2KClO₃ → 2KCl + 3O₂.

• These processes typically go to completion, often seen in precipitation and gas evolution reactions.

Types of Equilibria

• Physical Equilibrium: Involves the phase changes between states of matter without altering the chemical composition, e.g., H₂O(s) ⇌ H₂O(l).
• Chemical Equilibrium: Involves a balance between forward and reverse reactions of chemical species, e.g., PCl₅(g) ⇌ PCl₃(g) + Cl₂(g).
• Ionic Equilibrium: Describes the equilibrium established between a weak acid/base and its ions in solution, e.g., CH₃COOH(aq) ⇌ CH₃COO⁻(aq) + H⁺(aq).

Physical Equilibrium Characteristics

• Solid to Liquid: When a solid melts to form a liquid, the melting point remains constant under a specific pressure, e.g., H₂O(s) ⇌ H₂O(l).
• Liquid to Vapor: At a specific temperature, the vapor pressure is established as liquid turns to gas, e.g., H₂O(l) ⇌ H₂O(g).
• Solute to Solution: The concentration of a solid solute dissolved in a solvent becomes constant at a given temperature, e.g., Sugar(s) ⇌ Sugar(solution).
• Gas to Aqueous: The concentration of a gas in an aqueous solution stabilizes at a constant value at a given temperature, e.g., CO₂(g) ⇌ CO₂(aq).

Explore the concepts of reversible and irreversible processes in chemical reactions. This quiz will help you understand how products can revert to reactants under certain conditions and the types of equilibria that arise in different reactions. Test your knowledge on key examples and definitions related to this critical area of chemistry.