Bihar Board - Class 11 - Chemistry - Chapter 7: Equilibrium Handwritten Notes

The "Equilibrium" chapter focuses on the dynamic balance between opposing processes in chemical and physical systems. It introduces the concept of reversible reactions and the conditions under which equilibrium is established. This chapter also explains how external factors like temperature and pressure influence equilibrium.

Key Points:

1. Dynamic Equilibrium:

   • A state where the forward and reverse reactions occur at the same rate, resulting in no net change in the concentration of reactants and products.

2. Types of Equilibria:

   • Physical Equilibrium: Involves changes in physical state (e.g., liquid-vapor equilibrium in water).
   • Chemical Equilibrium: Involves chemical reactions where reactants and products coexist in balance.

3. Law of Chemical Equilibrium (Le Chatelier’s Principle):

   • The equilibrium constant ($$KK) expresses the ratio of product concentrations to reactant concentrations, each raised to their stoichiometric coefficients.
   • Le Chatelier's Principle predicts how a system at equilibrium reacts to changes in concentration, temperature, or pressure.

4. Factors Affecting Equilibrium:

   • Concentration: Adding more reactant shifts the equilibrium toward the products, and vice versa.
   • Temperature: Endothermic reactions are favored by heat, while exothermic reactions are favored by cooling.
   • Pressure: In gaseous equilibria, increasing pressure favors the side with fewer gas molecules.

5. Acid-Base Equilibrium:

   • The concept of $$pHpH, $$pKapKa, and $$pKbpKb are introduced to describe acid and base strength.
   • Equilibrium in acid-base reactions is governed by the dissociation constants ($$KaKa and $$KbKb).

6. Ionic Equilibrium:

   • Explains the dissociation of salts, acids, and bases in water.
   • Concepts like solubility product ($$KspKsp) and common ion effect are covered.

7. Applications of Equilibrium:

   • Predicting the extent of reactions.
   • Designing industrial processes like the Haber process for ammonia synthesis.

Conclusion:

The "Equilibrium" chapter is fundamental for understanding the balance of reactions and the factors influencing it. It highlights the dynamic nature of chemical and physical processes, equipping students to predict and control outcomes in various systems. Mastery of equilibrium concepts is crucial for advanced studies in chemistry and practical applications in industries.

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