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Chemical Equilibrium is a core chapter of Physical Chemistry and holds significant importance in the NEET examination. Questions from this chapter are often formula-based, numerical, and concept-driven, making it one of the most scoring topics for students who understand the fundamentals clearly. In Chemical Equilibrium, students learn about reversible reactions, equilibrium constants, Le Chatelier’s Principle, and the relationship between concentration, pressure, and temperature. At studentbro.in, this chapter is explained in a student-friendly and NEET-focused manner, ensuring better conceptual clarity and faster revision.
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Chemical Equilibrium is the state of a reversible reaction where the rate of the forward reaction becomes equal to the rate of the backward reaction. At equilibrium, the concentration of reactants and products remains constant, though reactions continue dynamically. Example: N₂ + 3H₂ ⇌ 2NH₃ This concept forms the base of several advanced topics like Ionic Equilibrium and Electrochemistry.
The Law of Mass Action states that the rate of a chemical reaction is proportional to the product of the active masses (concentrations) of the reactants. For a reaction: aA + bB ⇌ cC + dD Equilibrium Constant (Kc): Kc = [C]ᶜ[D]ᵈ / [A]ᵃ[B]ᵇ This formula is extremely important for NEET numerical problems.
Kc is expressed in terms of molar concentration. Kp is expressed in terms of partial pressure (used in gaseous reactions). Kp = (Partial pressure of products) / (Partial pressure of reactants)
One of the most frequently asked NEET formulas: Kp = Kc (RT)ⁿ Where: R = Gas constant T = Temperature in Kelvin n = Difference between moles of gaseous products and reactants
• Remains constant at constant temperature • Independent of initial concentration • Large K → product favored reaction • Small K → reactant favored reaction • Solids and pure liquids are excluded These points are often tested in NEET conceptual questions.
Reaction Quotient helps predict the direction of a reaction. Q = [Products] / [Reactants] • Q < K → Reaction proceeds forward • Q > K → Reaction proceeds backward • Q = K → System is at equilibrium
Le Chatelier’s Principle states that any change imposed on a system at equilibrium causes the system to adjust itself to counteract the change. Effect of Concentration: Increase in reactants → Forward shift Effect of Pressure: Increase in pressure → Favors fewer moles of gas Effect of Temperature: Endothermic reaction → Increase in temperature favors products
Homogeneous Equilibrium: All reactants and products are in the same phase. Heterogeneous Equilibrium: Reactants and products are in different phases. Solids and liquids are excluded from equilibrium expressions.
Degree of dissociation represents the fraction of molecules dissociated. α = Moles dissociated / Initial moles This concept is essential for NEET numerical questions involving equilibrium.
Chemical Equilibrium lays the foundation for Ionic Equilibrium, which deals with acids, bases, and salts. pH = −log[H⁺] pOH = −log[OH⁻] pH + pOH = 14
• Appears every year in NEET • High scoring chapter • Strong formula-based weightage • Helps in understanding Ionic Equilibrium
✔ NEET-focused content ✔ Clear explanations ✔ Formula-oriented approach ✔ Easy revision material ✔ Trusted by NEET aspirants
Chemical Equilibrium is one of the most important and scoring chapters in NEET Chemistry. With a strong understanding of equilibrium formulas, constants, and principles, students can easily solve both conceptual and numerical questions. Regular revision and practice from studentbro.in will help NEET aspirants build confidence and achieve higher scores in Chemistry.
