Chemical Equilibrium — Chapter Summary
Maharashtra Board · Class 11 · Chemistry
Summary of Chemical Equilibrium for Maharashtra Board Class 11 Chemistry. Part of the Maharashtra Board Class 11 Chemistry syllabus.
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Overview
Chemical equilibrium is a fundamental concept in chemistry that describes the state when forward and reverse reactions occur at equal rates. This chapter explores reversible reactions, equilibrium constants, and factors affecting equilibrium. Understanding equilibrium is crucial for predicting react
Key Concepts
Irreversible reactions proceed in one direction
Irreversible reactions proceed in one direction only (A + B → C + D), while reversible reactions can proceed in both directions (A + B ⇌ C + D). Examp
At equilibrium
At equilibrium, forward and reverse reaction rates are equal, resulting in constant concentrations of all species. The system appears static but react
For reaction aA + bB ⇌
For reaction aA + bB ⇌ cC + dD, the equilibrium constant Kc = [C]ᶜ[D]ᵈ/[A]ᵃ[B]ᵇ. This ratio remains constant at a given temperature. For gases, Kp use
Homogeneous equilibrium involves all species
Homogeneous equilibrium involves all species in same phase (H₂(g) + I₂(g) ⇌ 2HI(g)). Heterogeneous equilibrium involves multiple phases (CaCO₃(s) ⇌ Ca
Reaction quotient Q has same form
Reaction quotient Q has same form as K but uses any concentrations, not just equilibrium ones. If Q < K: forward reaction favored; Q = K: at equilibri
Learning Objectives
- Distinguish between reversible and irreversible reactions with examples
- Understand the concept of dynamic equilibrium in physical and chemical processes
- Apply the law of mass action to write equilibrium constant expressions
- Calculate equilibrium constants (Kc and Kp) and predict reaction directions
- Analyze factors affecting equilibrium using Le Chatelier's principle
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Sources & Official References
Content is aligned to the official syllabus. Refer to the board website for the latest curriculum.
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