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Le Chatelier’s Principle and Equilibrium Constant MCQs for Class 11 Chemistry
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Introduction
Mastering the concepts of Le Chatelier’s Principle and Equilibrium Constant is essential for every CBSE Class 11 Chemistry student. This online MCQ practice test has been carefully curated as per the latest NCERT syllabus, ensuring that you strengthen your understanding of chemical equilibrium — one of the most fundamental topics in Physical Chemistry (Chapter 7: Equilibrium).
Through this interactive quiz, you can test your conceptual clarity on how equilibrium systems respond to changes in concentration, pressure, and temperature, and how the equilibrium constant (Kc and Kp) governs reaction direction and extent.
Each question includes detailed feedback and explanations to help you analyze your answers instantly. Ideal for CBSE Board exam preparation and competitive entrance exams like NEET and JEE (Main), this quiz helps you build accuracy and speed in applying the principles of equilibrium.
Highlight: These MCQs are designed strictly as per the NCERT Class 11 Chemistry syllabus, making them perfect for CBSE Board standards.
Sample MCQs (with Answers & Explanations)
Q1. According to Le Chatelier’s principle, if the temperature of an endothermic reaction is increased, the equilibrium will shift towards —
A) Reactants
B) Products
C) No change
D) Catalyst side
Answer: B) Products
Explanation: Increasing temperature favors the endothermic direction, shifting equilibrium toward product formation.
Q2. For the reaction N₂(g) + 3H₂(g) ⇌ 2NH₃(g), an increase in pressure will —
A) Favor formation of NH₃
B) Favor dissociation of NH₃
C) No effect
D) Decrease Kp
Answer: A) Favor formation of NH₃
Explanation: Pressure increase favors the side with fewer moles of gas. Here, the right side has fewer moles (2 vs 4).
Q3. The equilibrium constant (Kc) of a reaction depends on —
A) Concentration of reactants
B) Catalyst used
C) Temperature only
D) Pressure of system
Answer: C) Temperature only
Explanation: Kc is temperature-dependent; catalysts or concentration changes do not affect its value.
Q4. In the equilibrium H₂(g) + I₂(g) ⇌ 2HI(g), if HI is removed continuously —
A) Equilibrium shifts right
B) Equilibrium shifts left
C) Kc decreases
D) No change
Answer: A) Equilibrium shifts right
Explanation: Removing product shifts equilibrium toward product side to replace what’s removed.
Q5. If Kp = Kc(RT)^Δn, and Δn = 0, then —
A) Kp = Kc
B) Kp > Kc
C) Kp < Kc
D) Kp = 0
Answer: A) Kp = Kc
Explanation: When Δn = 0, (RT)^0 = 1, hence Kp = Kc.