11th Chemistry Equilibrium chapter wise mcq quiz for 2026 exam

Test your understanding of chemical equilibrium with our free, chapter-wise MCQ quiz for 11th grade Chemistry. Improve your exam preparation and concept clarity.

Test Chemistry Equilibrium chapter wise MCQ

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Time: 10 Minutes for 10 Question.

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11th Chemistry: Equilibrium

1 / 10

1. Which experiment demonstrates the dynamic nature of chemical equilibrium?

Electrolysis of water

Synthesis of ammonia using Haber’s process with D2 instead of H2

Decomposition of hydrogen peroxide

Combustion of hydrocarbons

2 / 10

2. What is the state of a chemical reaction when the rates of the forward and reverse reactions are equal?

Static equilibrium

Dynamic equilibrium

Thermodynamic equilibrium

Kinetic equilibrium

3 / 10

3. In the solid-liquid equilibrium of ice and water at 273 K and 1 atm pressure, which statement is true?

The mass of ice decreases over time.

The mass of water increases over time.

The mass of ice and water remain constant over time.

The temperature of the system changes.

4 / 10

4. Which experiment demonstrates the dynamic nature of chemical equilibrium?

Electrolysis of water

Synthesis of ammonia using Haber’s process with D2 instead of H2

Decomposition of hydrogen peroxide

Combustion of hydrocarbons

5 / 10

5. Which of the following best describes homogeneous equilibria?

Equilibrium in a single phase

Equilibrium involving multiple phases

Equilibrium that only involves gases

Equilibrium that only involves liquids

6 / 10

6. Which of the following conditions is necessary for equilibrium in a physical process?

Open system

Closed system at a given temperature

Constant pressure

Constant volume

7 / 10

7. If K_c​ is very large (greater than 10³), which of the following statements is true?

The reaction hardly proceeds

Reactants predominate over products

The reaction is at equilibrium

The reaction proceeds nearly to completion

8 / 10

8. Which of the following is an example of equilibrium involving a phase transformation process?

Combustion of methane

Dissolution of sugar in water

Melting of ice to water

Oxidation of iron

9 / 10

9. What does a high value of the equilibrium constant (Kc) suggest about a reaction?

The reaction proceeds rarely.

The reaction proceeds nearly to completion.

The concentrations of reactants are high.

The reaction is very slow.

10 / 10

10. For the reaction A + B ⇌ C + D at equilibrium, what is true about the concentrations of reactants and products?

They are always equal.

They remain constant over time.

They change continuously.

They are zero.

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View Chapter wise MCQ Quiz of 11th Chemistry

Chapter of 11th Chemistry Chapter Wise MCQ

Unit 1 Some Basic Concepts of Chemistry
1.1 Importance of Chemistry
1.2 Nature of Matter
1.3 Properties of Matter and their Measurement
1.4 Uncertainty in Measurement
1.5 Laws of Chemical Combinations
1.6 Dalton’s Atomic Theory
1.7 Atomic and Molecular Masses
1.8 Mole Concept and Molar Masses
1.9 Percentage Composition
1.10 Stoichiometry and Stoichiometric Calculations

Unit 2 Structure of Atom
2.1 Discovery of Sub-atomic Particles
2.2 Atomic Models
2.3 Developments Leading to the Bohr’s Model of Atom
2.4 Bohr’s Model for Hydrogen Atom
2.5 Towards Quantum Mechanical Model of the Atom
2.6 Quantum Mechanical Model of Atom

Unit 3 Classification of Elements and Periodicity in Properties
3.1 Why do we Need to Classify Elements ?
3.2 Genesis of Periodic Classification
3.3 Modern Periodic Law and the Present Form of the Periodic Table
3.4 Nomenclature of Elements with Atomic Numbers > 100
3.5 Electronic Configurations of Elements and the Periodic Table
3.6 Electronic Configurations and Types of Elements: s-, p-, d-, f- Blocks
3.7 Periodic Trends in Properties of Elements

Unit 4 Chemical Bonding and Molecular Structure
4.1 Kössel-Lewis Approach to Chemical Bonding
4.2 Ionic or Electrovalent Bond
4.3 Bond Parameters
4.4 The Valence Shell Electron Pair Repulsion (VSEPR) Theory
4.5 Valence Bond Theory
4.6 Hybridisation
4.7 Molecular Orbital Theory
4.8 Bonding in Some Homonuclear Diatomic Molecules
4.9 Hydrogen Bonding

Unit 5 Thermodynamics
5.1 Thermodynamic Terms
5.2 Applications
5.3 Measurement of ÄU and ÄH: Calorimetry
5.4 Enthalpy Change, ÄrH of a Reaction – Reaction Enthalpy
5.5 Enthalpies for Different Types of Reactions
5.6 Spontaneity
5.7 Gibbs Energy Change and Equilibrium

Unit 6 Equilibrium
6.1 Equilibrium in Physical Processes
6.2 Equilibrium in Chemical Processes – Dynamic Equilibrium
6.3 Law of Chemical Equilibrium and Equilibrium Constant
6.4 Homogeneous Equilibria
6.5 Heterogeneous Equilibria
6.6 Applications of Equilibrium Constants
6.7 Relationship between Equilibrium Constant K, Reaction Quotient Q and Gibbs Energy G
6.8 Factors Affecting Equilibria
6.9 Ionic Equilibrium in Solution
6.10 Acids, Bases and Salts
6.11 Ionization of Acids and Bases
6.12 Buffer Solutions
6.13 Solubility Equilibria of Sparingly Soluble Salts

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