Chemical Equilibrium - NEET Previous Year Questions with Complete Solutions

The relation is Kp = Kc × (RT)^Δn, where R is the gas constant (0.0821 L·atm/mol·K), T is the temperature in Kelvin, and Δn is the difference in moles of gaseous products minus gaseous reactants. When Δn = 0, Kp equals Kc.

Chemical Equilibrium is moderately difficult. The conceptual part (Le Chatelier's principle, direction of reaction) is straightforward with NCERT. The numerical part (Kc, Kp, degree of dissociation) requires practice with ICE tables. Students who practise 30–40 PYQs from this chapter consistently score full marks on exam day.

NTA typically asks 2–4 questions from Chemical Equilibrium and Ionic Equilibrium in NEET-UG every year. This translates to 8–16 marks. Given the consistent weightage since 2010, this chapter is non-negotiable for any student targeting 160+ in Chemistry.

If an inert gas is added at constant volume, equilibrium does NOT shift — partial pressures of reactants and products remain unchanged. If inert gas is added at constant pressure, total pressure increases, so the system effectively reduces partial pressures of all species — equilibrium shifts toward the side with more moles of gas.

Start with NCERT Class 11 Chapter 7 (Equilibrium) — read every line. Then solve NCERT examples and exercises. After that, work through NEET PYQs year-by-year. Finally, take timed mock tests. The NCERT Solutions for Class 11 help cross-check your understanding of NCERT problems before moving to PYQs.

Yes, Le Chatelier's Principle appears in NEET almost every year — either as a direct conceptual question or as part of an application-based question on industrial processes like the Haber process. Understanding the effect of temperature, pressure, and concentration changes on equilibrium position is essential.